88:I[170619,["$2","$3","$4","$5","$6","$7","$8","$9","$a","$b","$c","$d","$e","$f","$10","$11","$12","$13","$14","$15","$16","$17","$18","$19","$1a","$59","$5a","$5b","$5c","$7a","$7b","$7c","$7d","$7e","$7f","$80","$81","$82","$83","$84"],"PreviewShell"] 89:T38c4,

Active Monitoring Checklist

Teacher Resource: Partial Pressure Parade (60m Lesson)

Current Lesson

Partial Pressure Parade

Monitoring Objective

Circulate to verify conceptual shifts from individual gas behavior to mixed system behavior. Ensure students use Sentence Stems for reasoning and correctly apply the Ptotal = P1 + P2... additive logic.

Lesson Phase / Task	Student "Look-Fors" (Evidence)	Scaffolding Probes / Prompts
Phase 1 (0-5m) Stop & Jot: Tank A/B	Correctly sums Tank A + Tank B. Identifies that volume is constant.	"If we added a third tank of helium, what would happen to the total force on the walls?"
Phase 2 (5-15m) Reading Chunk 1: Dalton	Uses word "independent" or "no interference." Draws particles spaced apart.	"Are the Nitrogen particles pushing the Oxygen particles out of the way, or ignoring them?"
Reading Chunk 2: Scuba	Recognizes doubling total P doubles partial P. Links mole % to pressure contribution.	"If a tank is 20% Oxygen, does that percentage change as you dive deeper? What about the actual pressure?"
Reading Chunk 3: Water	Identifies water vapor as "contamination." Recognizes need to subtract vapor P.	"Why can't we just measure the total gas? What is hiding inside that tube besides our product?"
Phase 3 (15-30m) Gas Collection Lab	Reads meniscus at eye level. Records water temp immediately. Matches temp to the Vapor P chart.	"If the water was ice cold, would the 'vapor contamination' be higher or lower?"

Misconception Alert

Students often try to add the vapor pressure to the total pressure instead of subtracting it from the total to find the dry gas. Watch for "P_dry = P_total + P_H2O" errors.

Teacher Talk

"Listen for students using 'Mole Fraction' correctly—it's a share of the whole, not a unit of pressure itself."

Phase 4-6: Application & Mastery

Station Rotation (30-50m)

Station	Key Mastery "Look-Fors"	Intervention Question
1: Mixture Model	Correctly uses Ideal Gas Law to find O2 pressure before adding to N2.	"Can you just add the moles, or do you have to find the pressures first?"
2: Atmospheric Ratios	Correctly multiplies 0.21 atm by 0.20 (20%) for partial O2.	"Does Nitrogen push Oxygen out of the mix when you go deeper, or just squeeze it?"
3: Water Trap	Converts mmHg to atm correctly (div by 760) before subtracting.	"Can we subtract mmHg from atm directly? Why not?"
4: Fraction & Partiality	Uses Total Moles (sum of both gases) in the denominator for mole fraction ($\chi$).	"Is the mole fraction 0.30/1.20 or 0.30/1.50? Why do we include both?"

PHASE 5

Vocab Speed Run

Observation: Are students confusing "Partial Pressure" with "Vapor Pressure"?

Dalton's Law identification

Correct Mole Fraction units (None!)

PHASE 6

Final Mastery

Check Exit Tickets for: "Cumulative force" or "Sum of collisions" reasoning.

Must include: Ptotal > Pany_individual

Circulation Notes / Intervention Groups

Needs Reteach (Math Correction)

Ready for Extension (Mole Fractions)

High-Leverage Move

"Praise the use of units during Station 3 conversions!"

Efficiency Target

5m Rotation Pace

8a:T1f0d,

Pressure Poster Workshop

Partial Pressure Parade Design Brief

NAME: ________________________________

DATE: ________________________________

The Mission: Visualizing Invisible Forces

Our classroom Word Wall needs an upgrade. Your task is to design a high-impact, scientific display card for one of the key concepts from the Partial Pressure Parade. Your design must bridge the gap between macroscopic data (what we measure) and microscopic behavior (what particles are actually doing).

Phase 1: Choose Your Concept

Dalton's Law

Partial Pressure

Mole Fraction

Vapor Pressure

Wet vs. Dry Gas

Total Pressure

Phase 2: The Blueprint (Drafting)

The Scientific Pitch (Concise Definition):

The Math Path (Formula/Variables):

The Reality Anchor (One real-world application/connection):

CONCEPT NAME

Write your chosen concept above

Particle Model View

Visualize collisions, gas mixtures, or boundaries

Definition

Formula & Variables

Real-World Logic

Pressure Power Unit | Word Wall Expansion

Design Lab 05

8b:T1c60,

Pressure Parade

Reading Passage

Name: ____________________________________

Date: _____________________________________

The Power of the Sum

John Dalton discovered that in a mixture of non-reacting gases, the Total Pressure is equal to the sum of the pressures of each individual gas. We call these individual pressures Partial Pressures. This happens because gas particles act independently—they hit the container walls without being affected by the other types of particles in the mix.

\[ P_{total} = P_1 + P_2 + P_3 + ... \]

STOP AND JOT

Explain why total pressure is a simple addition problem using particle behavior:

"The total is a sum because gas particles act _________________________________________________________________________________."

Scuba & Moles

Scuba divers use specific mixtures of gas because high partial pressures of Oxygen can be dangerous. To find the pressure of one specific gas in a mix, we use the Mole Fraction ($\chi$)—the ratio of moles of that gas to the total moles. If Oxygen makes up 21% of the moles, it provides 21% of the total pressure.

THINK PAIR AND SHARE

"If a diver goes deeper and the total pressure doubles, what happens to the partial pressure of Nitrogen if the mixture percentage stays the same?"

• "Since the mole fraction is constant, the partial pressure would __________________ because..."

• "I agree/disagree because doubling the total pressure causes __________________..."

The Water Trap

In chemistry labs, we often collect gas by bubbling it through water. However, some water always evaporates and mixes with our gas. We call this Vapor Pressure. To find the pressure of just the dry gas, we must subtract the water vapor pressure from the total atmospheric pressure.

\[ P_{total} = P_{dry\ gas} + P_{water\ vapor} \]

STOP AND JOT

Why is temperature key when collecting gas over water?

"Temperature is key because higher temperature leads to _______________________________________ vapor pressure..."

Comprehension Check

Scenario 1

A mixture has P_Argon = 1.2 atm and P_Helium = 0.8 atm. Total Pressure = 3.0 atm. Find P_Neon.

Scenario 2

Why must you convert vapor pressure units to match the total pressure units?

8c:T247f,

Law Legend Card Sort

Partial Pressure Parade Activity • Student Handout

12 Scenarios • 3 Categories

Boyle's Law

$P_1V_1 = P_2V_2$

Constant Temp

Charles's Law

$\frac{V_1}{T_1} = \frac{V_2}{T_2}$

Constant Pressure

Dalton's Law

$P_{total} = P_1 + P_2 + P_3 + ...$

Partial Pressures

A deep-sea diver surfaces too quickly and the gas volume in their lungs expands as the external pressure drops.

Scenario 01

A technician calculates the total pressure of a gas cylinder by adding the individual pressures of Nitrogen, Oxygen, and Argon.

Scenario 02

A car tire appears slightly flat on a cold winter morning because the lower temperature caused the gas volume to decrease.

Scenario 03

Bubbles blown by a fish get significantly larger as they float toward the surface where the water pressure is lower.

Scenario 04

A student uses a chart to find the "dry pressure" of Oxygen by subtracting the vapor pressure of water from the total pressure.

Scenario 05

A balloon placed in a hot car expands in size because the increasing temperature forces the gas particles to occupy more space.

Scenario 06

When you push down on the handle of a bicycle pump, the internal volume decreases and the pressure pushes the air into the tire.

Scenario 07

A deep-sea diver breathes "Trimix," a blend of Helium, Oxygen, and Nitrogen gases combined in a single pressurized tank.

Scenario 08

Liquid nitrogen is poured onto a birthday balloon, causing the gas inside to cool down and the balloon to shrivel instantly.

Scenario 09

A bag of potato chips appears "puffed up" and tightly inflated when taken on a plane where the cabin pressure is lower than sea level.

Scenario 10

A welder uses a gas cylinder containing a mixture of 75% Argon and 25% $CO_2$ to protect the weld from the atmosphere.

Scenario 11

A syringe plunger moves outward when the air inside is heated by the sun, increasing the volume of the trapped gas.

Scenario 12

8d:T1d6e,

Active Monitoring Checklist

Teacher Resource: Pressure Parade Reading Passage

Activity Phase

Literacy / Concept Intro

Monitoring Objective

Circulate during the Pressure Parade Chunked Reading. Focus on students' ability to link particle independence to the summing of pressures and their conceptual understanding of how vapor pressure "contaminates" dry gas samples. Use these prompts to redirect and push thinking.

Chunk & CFU	Student "Look-Fors" (Evidence of Mastery)	Scaffolding Questions / Redirects
Chunk 1: Power of Sum CFU: Stop and Jot	Calculates total (5.5 atm) correctly. Explains that particles act independently. Links addition to "Partial Pressures".	"If the Oxygen particles hit the walls, and the Nitrogen particles hit the same walls, why wouldn't we add them?"
Chunk 2: Scuba science CFU: Think-Pair-Share	Connects "mole fraction" to "percentage of the mix." Reasoning: If Total P doubles, and % O₂ is constant, Partial P O₂ also doubles.	"If the tank is 20% Oxygen at the surface, and 20% Oxygen at depth, how does the 'hit' force change if the total pressure is higher?"
Chunk 3: Water Trap CFU: Stop and Jot	Identifies that water evaporates into the gas. Notes that Vapor Pressure changes with Temperature. Recognizes the subtraction rule.	"If the lab is very hot today, will there be MORE or LESS water vapor in your sample compared to a cold day?"

Struggle Spots

Mole Fraction Confusion: Students may try to add moles to pressure directly. Remind them: Ratio first, then Pressure.

Vapor Pressure: Students often forget to subtract. Ask: "Is this gas PURE or WET?"

Mastery Checkpoint

Ask a student randomly:

"Why is 'collected over water' a problem for finding the pressure of a pure gas?"

8e:T17b4,

Partial Pressure Station Pack

Based on POGIL Models 1-4

The Mixture Model

Source: Model 1

Examine the three tanks. Notice that Tank C is just Tank A and B combined. Complete the table on your handout.

Math Mission

Use the Ideal Gas Law to calculate $P$ for each gas. Use $R = 0.0821 \frac{L \cdot atm}{mol \cdot K}$.

Atmospheric Ratios

Source: Model 2 & Q10

Draw air as a particulate mixture. Then, solve the Scuba Rescue problem where oxygen pressure drops by 80%!

Scuba Hint

If Oxygen drops by 80%, only 20% remains. Multiply the original pressure by 0.20.

The Water Trap

Source: Model 3 & Q18

When gas is collected over water, it gets "wet" with water vapor. You must subtract the water's pressure to find the "dry" gas pressure.

Lookup Table

Check the chart for the vapor pressure at 24°C. Convert it to atm before doing your math!

Fraction & Partiality

Source: Model 4

Examine the Helium, Argon, and Krypton mix. Look at how "Mole Fraction" connects to "Partial Pressure."

Discovery Hint

Try dividing the pressure of Helium by the total pressure. Does it match the fraction?

8f:T584a,

Chemistry Unit: Pressure Power

Partial Pressure Parade

March 26, 2026 60 Minute Session

Bellringer: STOP AND JOT

5:00

Tank A has 2.0 atm of Oxygen.
Tank B has 3.5 atm of Nitrogen.

What happens to the pressure when they are combined into a third tank? Why?

Sentence Stem:

"The total pressure will be ___________ because Dalton's Law states that ______________________."

Mixing Independent Particles

Chunk 2: Think Pair Share

Reading Follow-Along

"If a diver goes deeper and the total pressure doubles, what happens to the partial pressure of Nitrogen if the mixture percentage doesn't change?"

Discussion Stems:

• "Since the mole fraction is fixed, the pressure would..."
• "I agree/disagree because multiplying the total by ____..."

Depth Danger

Partial pressure increases with depth even if the mix stays the same!

Chunk 3: STOP AND JOT

The "Wet" Gas Logic

Why is it necessary to look up the temperature of the water before calculating the pressure of a gas collected over water?

Sentence Stem:

"It is necessary to know the temperature because vapor pressure __________________________________."

The Formula

\[ P_{total} = P_{gas} + P_{H_2O} \]

Water vapor pressure is added to your sample from evaporation!

Vocab Speed Run

5:00

Partial Pressure

Mole Fraction

Vapor Pressure

1. Ratio of moles of one gas to the total moles.

2. Pressure of a single gas in a mixture.

3. Pressure of water gas from evaporation.

Alka-Seltzer Bubbles

We are collecting $CO_2$ over water. But wait... is it just $CO_2$ inside your collection bottle?

Lab Goal: Correct for Vapor Pressure to find the pure gas pressure.

Lab: Gas Capture

15:00

The Mission:

1 Fill & invert bottle in water bath.
2 Connect tube to reaction flask.
3 Drop tablet & seal immediately!
4 Measure Temp & Atmospheric Pressure.

Correcting Your Data:

\[ P_{gas} = P_{atm} - P_{H_2O} \]

Subtract the Vapor Pressure from the table based on your water temperature!

Partial Pressure Parade: Active Stations

ROTATION TIMER:

5:00

Particle Artist

Draw "Dry Air." Use different shapes for Nitrogen, Oxygen, and Argon.

N: 78% | O: 21% | Ar: 1%

SCUBA Rescue

Solve Q10. What is the partial pressure of O₂ at the surface vs depth?

Use Dalton's Sum!

Fraction Duel

Derive the Mole Fraction formula ($\chi_i$) and apply it to Helium mix.

Ratio: n_i / n_total

Vapor Hunter

Find partial pressure of $CO_2$ at 24°C and 1.02 atm total.

Lookup & Subtract!

Card Sort Race

10:00

Sort your 12 scenario cards into these categories:

Boyle's Law

Charles's Law

Dalton's Law

GO! GO! GO!

100% Accuracy = Lab Bonus Point!

Final Checklist

5:00

Mastery Check

1. The One-Sentence Rule:

Explain why the total pressure of a gas mixture is always greater than any of its individual partial pressures.

2. Quick Math:

Total Pressure = 2.5 atm.
He accounts for 1.8 atm.
What is Ar?

Pass POGILs and Lab Reports forward!

90:T1b2e,

Bubble Bound Lab

Investigating Dalton's Law: Collecting Gas Over Water

Name:

Date:

Mission Objective:

Collect Carbon Dioxide ($CO_2$) gas produced by an Alka-Seltzer reaction using water displacement. Use Dalton's Law of Partial Pressures to calculate the pressure of the dry gas by correcting for water vapor pressure.

Part 1: Lab Data Collection

Experimental Readings

Atmospheric Pressure ($P_{total}$): __________ atm

Water Temperature ($T$): __________ $^\circ C$

Volume of Gas Collected ($V$): __________ mL

Vapor Pressure Lookup

Temp ($^\circ C$)	Pressure (mmHg)
20	17.5
21	18.7
22	19.8
23	21.1
24	22.4

Reference: Model 3 of POGIL Packet

Part 2: Dalton's Correction

A. Convert Water Vapor Pressure to atm

Calculation: $\text{mmHg} \div 760 = \text{atm}$

B. Calculate Pressure of DRY $CO_2$

$P_{dry} = $ ____________ atm

Equation: $P_{total} - P_{H2O}$

Part 3: Deep Dive Analysis

1. Based on your results, if we forgot to subtract the water vapor pressure, would our calculated number of moles of $CO_2$ be too high or too low? Explain why.

2. Particle Challenge: In the box below, draw a particulate model of the gas inside your collection bottle. Use different symbols for $CO_2$ and $H_2O$ molecules.

Sketch Particulate Mixture Here

$CO_2$

$H_2O$

91:T5851,

Chemistry Unit: Pressure Power

Partial Pressure Parade

March 26, 2026 60 Minute Session

Bellringer: STOP AND JOT

5:00

Tank A has 2.0 atm of Oxygen.
Tank B has 3.5 atm of Nitrogen.

What happens to the pressure when they are combined into a third tank? Why?

SENTENCE STEM:

"The total pressure will be ___________ because Dalton's Law states that ______________________."

Mixing Independent Particles

Chunk 2: THINK PAIR SHARE

Reading Activity

"If a diver goes deeper and the total pressure doubles, what happens to the partial pressure of Nitrogen if the mixture percentage doesn't change?"

SENTENCE STEMS:

• "Since the mole fraction is fixed, the pressure would..."
• "I agree/disagree because multiplying the total by ____..."

Depth Danger

Partial pressure increases with depth even if the mix stays the same!

Chunk 3: STOP AND JOT

The "Wet" Gas Logic

Why is it necessary to look up the temperature of the water before calculating the pressure of a gas collected over water?

SENTENCE STEM:

"It is necessary to know the temperature because vapor pressure ______________________."

The Correction Formula

\[ P_{gas} = P_{atm} - P_{H_2O} \]

Standard Temperature & Pressure (STP) doesn't apply to "wet" gases!

Vocab Speed Run

5:00

Partial Pressure

Mole Fraction

Vapor Pressure

1. Ratio of moles of one gas to the total moles.

2. Pressure of a single gas in a mixture.

3. Pressure of water gas from evaporation.

Alka-Seltzer Bubbles

We are collecting $CO_2$ over water. But wait... is it just $CO_2$ inside your collection bottle?

Lab Goal: Correct for Vapor Pressure to find the pure gas pressure.

Lab: Gas Capture

15:00

The Mission:

1 Fill & invert bottle in water bath.
2 Connect tube to reaction flask.
3 Drop tablet & seal immediately!
4 Measure Temp & Atmospheric Pressure.

Correcting Your Data:

\[ P_{gas} = P_{atm} - P_{H_2O} \]

Subtract the Vapor Pressure from the table based on your water temperature!

Partial Pressure Parade: Active Stations

ROTATION TIMER:

5:00

Particle Artist

Draw "Dry Air." Use different shapes for Nitrogen, Oxygen, and Argon.

N: 78% | O: 21% | Ar: 1%

SCUBA Rescue

Solve Q10. What is the partial pressure of O₂ at the surface vs depth?

Use Dalton's Sum!

Fraction Duel

Derive the Mole Fraction formula ($\chi_i$) and apply it to Helium mix.

Ratio: n_i / n_total

Vapor Hunter

Find partial pressure of $CO_2$ at 24°C and 1.02 atm total.

Lookup & Subtract!

Card Sort Race

10:00

Sort your 12 scenario cards into these categories:

Boyle's Law

Charles's Law

Dalton's Law

GO! GO! GO!

100% Accuracy = Lab Bonus Point!

Final Checklist

5:00

Mastery Check

1. The One-Sentence Rule:

Explain why the total pressure of a gas mixture is always greater than any of its individual partial pressures.

2. Quick Math:

Total Pressure = 2.5 atm.
He accounts for 1.8 atm.
What is Ar?

Pass POGILs and Lab Reports forward!

92:T15f5,

Teacher Cheat Sheet

Partial Pressure Parade • Answer Key & Facilitation Guide

Official Reference

Law Legend Card Sort Keys

Boyle's Law

01: Diver Lungs (P vs V)
04: Fish Bubbles (P vs V)
07: Bicycle Pump (V vs P)
10: Chip Bag on Plane (P vs V)

Charles's Law

03: Cold Winter Tire (T vs V)
06: Hot Car Balloon (T vs V)
09: Liquid Nitrogen (T vs V)
12: Syringe in Sun (T vs V)

Dalton's Law

02: Gas Cylinder Addition
05: "Dry Pressure" Oxygen
08: SCUBA "Trimix" Blend
11: Welding Gas Mixture

Station Rotation Math Solutions

Station 2: SCUBA Rescue (Q10)

Part A (Initial):

$P_{tot} = 0.65 + 0.38 = \mathbf{1.03 \text{ atm}}$

Part B (Dive Drop):

$P_{O2(new)} = 0.65 \times 0.20 = \mathbf{0.13 \text{ atm}}$

Station 3: Mole Fraction (Model 4)

Equation: $X_i = \frac{n_i}{n_{total}}$ and $P_i = X_i \times P_{total}$

Students should notice that $0.35 \text{ atm} \div 2.80 \text{ atm} = 0.125$.

Lab: Bubble Bound Analysis

Q1: Forgotten Vapor Correction

"If we forget to subtract $P_{H2O}$, the pressure of the gas would appear higher than it actually is. Since moles are directly proportional to pressure (Ideal Gas Law), our calculated moles of $CO_2$ would be artificially high."

Q2: Particle Sketch Logic

"The bottle should show mostly $CO_2$ molecules with some $H_2O$ molecules scattered throughout, as both are contributing to the total pressure measured."

93:T39b1,

The Mixture Model

Dalton's Law of Partial Pressures

Background

Each gas in a mixture acts independently. The Total Pressure is found by adding up each individual gas's contribution.

Environment Data:

Volume (V) 10.0 L
Temp (T) 298 K
R-Value 0.0821

1. Calculate the pressure of 0.50 moles of Oxygen:

$P = \frac{(0.50) (0.0821) (298)}{10.0}$

Result in atm

2. If Nitrogen is also in the container at 1.25 atm, find the Total Pressure:

+ 1.25 =

Total Pressure (atm)

Atmospheric Ratios

Mole Fractions in Mixtures

Scuba divers breathe gas mixtures where the partial pressure of Oxygen must stay within safe limits. If total pressure increases, individual pressures increase proportionately.

Particle Sketch Area

Sketch 10 particles (8 N, 2 O)

"A nitrox tank has a total pressure of 1.00 atm. Oxygen accounts for 0.21 atm. After a dive, the oxygen partial pressure has decreased by 80%."

Remaining O₂ %

100% - 80% = ____ %

Multiplier

0.____

Final Partial Pressure Calculation:

0.21 × =

Atmospheres (atm)

The Water Trap

Vapor Pressure Corrections

When collecting gas over water, some water evaporates and mixes with it. Subtract the water vapor pressure (P_H₂O) to find the pressure of the pure gas.

Vapor Pressure Reference

22.0 °C	19.8 mmHg
24.0 °C	22.4 mmHg
26.0 °C	25.2 mmHg

1. Convert 24°C Vapor Pressure (22.4 mmHg) to atm:

22.4÷760=

2. Final Calculation (Barometer = 1.02 atm):

1.02−=

Pure Dry Pressure (atm)

Fraction & Partiality

Mole Fractions vs Partial Pressures

Mole Fraction ($\chi$) is the proportion of a mixture made of one type of gas. If a gas is 10% of the moles, it exerts 10% of the total pressure.

Governing Formula

P_gas = ($\chi$_gas) × P_total

1. Find Mole Fraction ($\chi$) for 0.30 moles in 1.50 total moles:

$\chi$ =

0.301.50

=________

2. If Total Pressure is 2.80 atm, calculate Partial Pressure:

$\times$2.80=

Partial Pressure (atm)

94:T22a3,

Pressure Parade

Chunked Reading Passage

Name: ____________________________________

Date: _____________________________________

CHUNK 1

The Power of the Sum

\[ P_{total} = P_1 + P_2 + P_3 + ... \]

STOP AND JOT

Why is the total pressure a simple sum? Explain in one sentence.

SENTENCE STEMS:

"The total is a sum because gas particles act ________..."

CHUNK 2

Scuba & Moles

THINK PAIR AND SHARE

"If a diver goes deeper and the total pressure doubles, what happens to the partial pressure of Nitrogen if the mixture percentage stays the same?"

SENTENCE STEMS:

• "Since the mole fraction is constant, the partial pressure would ________..."

• "I agree/disagree because doubling the total pressure causes ________..."

CHUNK 3

The Water Trap

\[ P_{total} = P_{dry\ gas} + P_{water\ vapor} \]

Vapor pressure changes based on the water's temperature!

STOP AND JOT

Why is temperature key when collecting gas over water?

SENTENCE STEMS:

"Temperature is key because higher temperature leads to ________ vapor pressure..."

Identity Verification Check

Scenario 1

Calculation Required:

A mixture has P_Ar = 1.2 atm and P_He = 0.8 atm. Total P = 3.0 atm. Find P_Ne.

Scenario 2

Unit Check:

Why must you convert vapor pressure to 'atm' before subtracting it from 1.02 atm?

95:T3dde,

Station Parade Report

Partial Pressure Parade • Scaffolded Student Rotation Guide

Name:

Date:

The Mixture Model

V = 10.0 L T = 298 K R = 0.0821

A. Solve for Tank A (Oxygen):

Equation: P = (nRT) / V

$P = \frac{($ $) (0.0821) (298)}{10.0} = $ atm

B. Tank C (Combined Mixture):

Ptotal = P1 + P2

+ = atm

Atmospheric Ratios

Scuba Mission

1. Initial System Total:

0.65 atm + 0.38 atm = atm

2. Final Remaining Oxygen:

0.65 atm $\times$ 0.20 = atm

Air Particle Model Drawing

N: 78% O: 21% Ar: 1%

The Water Trap

A. Vapor Pressure Correction:

Step 1: Lookup at 24°C

Pressure: mmHg

Step 2: Convert Units

$\div$ 760 = atm

B. Find Pressure of Dry Gas:

Pdry = Ptotal - Pwater

0.989 atm $-$ =

atm

Fraction & Partiality

A. Mole Fraction Formula:

Xi =

moles of species

total moles

B. Verify Krypton Pressure:

Method: Ratio

PKr = (Xi) $\times$ (Ptotal)
$\times$ 2.80 =

Method: Sum

PKr = 2.80 $-$ (Sum of Others)
2.80 $-$ 1.05 =

Synthesis Phase

Vocab Check

Partial Pressure

Definition ID:

Mole Fraction

Definition ID:

Vapor Pressure

Definition ID:

Exit Ticket: The One-Sentence Rule

Explain why the total pressure of a gaseous mixture is always higher than any of its individual component pressures:

Hand in your completed Parade Report

Calibration Center

Standard Measurement Conversion Tool

Temperature: Celsius to Kelvin

Kelvin = Celsius + 273

Quick Case:

25.0 °C + = K

Pressure: mmHg to atmospheres

1 atm = 760 mmHg

Quick Case:

760 mmHg $\div$ = atm

96:T316b,

Station Parade Report

Partial Pressure Parade • Student Rotation Evidence

Name:

Date:

The Mixture Model

Step A: Oxygen Pressure (0.50 moles)

$P = \frac{(0.50) (0.0821) (298)}{10.0} = $ atm

Step B: Total Pressure Sum

+ 1.25 = atm

Dalton's Law: Particles hit the walls independently!

Atmospheric Ratios

Scuba Survival Calculation

Remaining Oxygen Share (20% of 0.21 atm):

0.21 atm $\times$ 0.20 =

Particle Mixture Sketch

Draw circles for N and squares for O

The Water Trap

Conversion Sandbox

22.4 $\div$ 760 = atm

Finding Pure Dry Gas Pressure

1.02 atm $-$ =

atm

Fraction & Partiality

Step A: Mole Fraction Ratio

$\chi$ =

0.30 1.50

= ________

Step B: Partial Pressure Product

$\times$ 2.80 =

Synthesis Phase

Vocab Speed Log

Partial Pressure

Matching Letter:

Mole Fraction

Matching Letter:

Vapor Pressure

Matching Letter:

Exit Ticket: The One-Sentence Rule

"Explain why the total pressure of a gaseous mixture is always higher than any of its individual component pressures:"

Final Rotation Check-In

Calibration Toolkit

Essential Gas Law Measurement Conversion

Temperature Pivot

Kelvin = °Celsius + 273.15

Pressure Standard

1.00 atm = 760 mmHg

97:T20d2,

Partial Pressure Parade

Lesson Plan • Chemistry Unit: Pressure Power

60 Minute Session

Date: 03/26/2026

Essential Question

How do individual gases in a mixture contribute to the total pressure of a system, and how can we mathematically isolate a single gas species?

Learning Objectives

Define partial pressure and mole fraction using Dalton's Law.
Calculate partial pressure given total pressure and mole quantities.
Correct for vapor pressure in gas collection over water lab scenarios.

Materials Needed

Chunked Reading Passage
Active Monitoring Checklist
Station Cards (1-4)
Alka-Seltzer, Flasks, Water Troughs

Instructional Sequence (60m)

Stop and Jot Bellringer

0:00 - 0:05

Students enter and solve the "Tank A/B" pressure prompt using the Stop and Jot strategy. Focus on additive reasoning.

Chunked Reading & Discussion

0:05 - 0:15

Guided reading of the Chunked Passage. Students use Think-Pair-Share for Chunk 2 (Scuba) and Sentence Stems for Chunk 3 (Water Trap). Teacher circulates with Monitoring Checklist.

Gas Collection over Water

0:15 - 0:30

Rapid lab execution. Students collect bubbles and measure temperature to prepare for the "wet" gas correction calculation.

Station Rotation Parade

0:30 - 0:50

Four-station rotation. 5 minutes per station. Students use station cards to practice Scuba math, Vapor pressure, and Mole fractions.

Vocab Speed Run

0:50 - 0:55

High-energy check for vocabulary terms encountered during the lesson.

Final Mastery Verification

0:55 - 1:00

Final synthesis questions on the reading passage. Collect all student evidence.

Teacher Facilitation Tips

Literacy Scaffolding:

During Chunk 2 (Scuba), ensure students are looking for the "doubling" relationship. If total pressure doubles, the "share" of each gas doubles too. Use the sentence stems to force scientific reasoning over simple guessing.

Station Management:

Set a physical timer at the front for the 5-minute rotations. Station 3 (Water Trap) usually takes the longest; prioritize the conversion step (mmHg to atm) for these students.

98:T19ef,

The Mixture Model

Dalton's Law of Partial Pressures

Station ID

ST-01

The Concept

John Dalton discovered that individual gas particles in a container behave independently. They hit the walls and create pressure without being slowed down or affected by other types of particles in the mixture.

P_total = P₁ + P₂ ...

Environment Data:

Volume (V) 10.0 L
Temp (T) 298 K
R-Constant 0.0821

Step A: Isolate Gas 1

Use the Ideal Gas Law to calculate the partial pressure of 0.50 moles of Oxygen:

$P = \frac{($ 0.50 $) (0.0821) (298)}{10.0}$

Calculate your result in atmospheres (atm)

Step B: Sum to Total

If a second gas (Nitrogen) is added to the same container with a pressure of 1.25 atm, what is the Total Pressure?

+ 1.25 =

Total Mixture Pressure (atm)

99:T2aa7,

GAS LAB EXPLORER

Relationships Between Gas Variables

Name: ____________________________________

Date: _________________ Block: _________

Investigation Goal

How do pressure and temperature affect the volume of a trapped gas?

Part I: Pressure vs. Volume (Boyle's Law)

Add varying masses (books) to the top of a sealed syringe and record the change in volume of the air inside.

Trial #	Mass Added (# books)	Estimated Pressure
1 (Initial)	0 Books	Atmospheric
2	2 Books	Atm. + 2 units
3	4 Books	Atm. + 4 units
4	6 Books	Atm. + 6 units

Graph: Volume vs. Pressure

Volume (mL)

Pressure (# of Books)

Analysis: Based on your graph, describe the mathematical relationship between pressure and volume. Is it linear or inverse?

Part II: Temp vs. Volume (Charles's Law)

Experimental data for dry air. Convert all Celsius temperatures to Kelvin: K = °C + 273.15

Bath Type	Temp (°C)	Volume (mL)
Salt Ice Water	-10.0°C	15.0 mL
Ice Water	0.0°C	15.6 mL
Room Temperature	22.0°C	16.8 mL
Hot Water	80.0°C	20.1 mL

Particle-Level Model

Draw the arrangement and relative speed of the gas particles. Use longer "Whoosh" marks for faster particles!

Cold Gas (-10°C)

Hot Gas (80°C)

1. Explain the concept of Absolute Zero. What would happen to the volume of an ideal gas at 0 Kelvin?

2. Why is Kelvin preferred over Celsius for gas laws? Consider what happens to the math if temperature is 0°C.

Gas Lab Explorer

STU-713773-CHEM

9a:T22d9,

Pressure Power Word Wall

Vocabulary connected to the Gas Lab Explorer Activity

Variable: P

Pressure

The force of gas particles hitting the walls of their container.

Lab Explorer Link:

"Adding more books to the syringe increased the pressure, forcing particles closer together."

Variable: V

Volume

The amount of 3D space a gas occupies (usually in mL or Liters).

Lab Explorer Link:

"We measured the mL of space inside the syringe as the plunger moved up and down."

Variable: T

Temperature

The measure of the average kinetic energy (speed) of gas particles.

Lab Explorer Link:

"In the water baths, hot gas particles moved faster than cold gas particles."

Inverse

A relationship where one variable goes UP while the other goes DOWN.

Lab Explorer Link:

"Pressure and Volume are inverse. More pressure = less volume in the syringe."

Direct

A relationship where both variables go UP or DOWN together.

Lab Explorer Link:

"Temperature and Volume are direct. Hotter gas = more volume (the balloon grew)."

K.M.T.

Kinetic Molecular Theory

The idea that gas particles are constantly moving in random, straight lines.

Lab Explorer Link:

"We drew 'whoosh marks' to show the kinetic energy of the moving particles."

Absolute Zero

0 Kelvin. The theoretical temperature where all particle motion stops.

Lab Explorer Link:

"At 0 K, the gas volume would mathematically drop to zero as particles stop moving."

Collision

When gas particles hit each other or the container walls, creating pressure.

Lab Explorer Link:

"Smaller volume = more collisions with the syringe walls = higher pressure."

Variable: n

Moles

A measurement of the quantity (number) of gas particles present.

Lab Explorer Link:

"Since the syringe was sealed, the number of moles (n) stayed constant."

Add Your Own Term

9b:T1922,

Marshmallow Mission

Boyle's Law Pressure Probe

Name: ____________________________________

Date: _____________________________________

The Objective

Marshmallows are mostly air trapped in sugar pockets. By changing the pressure inside a sealed syringe, we can observe the direct effect of pressure on volume. Follow the steps below to investigate.

Equipment

1x 60mL Plastic Syringe
1x Syringe Tip Cap (or your thumb)
1x Mini Marshmallow

Initial Prediction

If I seal the syringe and pull the plunger out (increasing the space for air), the marshmallow will:

If I seal the syringe and push the plunger in (decreasing the space), the marshmallow will:

Data Collection

Action A

Pull Plunger Out

Observation: Describe the marshmallow's size and texture.

Particle Model: Show the air particles around the marshmallow.

Marshmallow

Action B

Push Plunger In

Observation: Describe the marshmallow's size and texture.

Particle Model: Show the air particles around the marshmallow.

Marshmallow

Mission Debrief

1. Relationship Analysis:

When you pushed the plunger in, you decreased the volume available for the air. This caused the pressure to increase. What happened to the volume of the marshmallow? Is this relationship direct or inverse?

2. The KMT Connection:

Explain why the marshmallow expanded when you pulled the plunger out. Think about the frequency of air particle collisions against the outside of the marshmallow sugar pockets.

9c:T767f,

Pressure Power

The Behavior of Gases

Engage: Balloon in a Bottle

The Mystery

Watch as a balloon is placed over the mouth of an empty glass bottle. The bottle is then heated on a hot plate.

What do you predict will happen to the balloon?

Observation Deck

Draw or describe the result in your lab notebook

Essential Questions

How do changes in pressure, volume, and temperature affect gas behavior?

How can we use mathematical models to predict these changes accurately?

What happens to gas particles at the molecular scale when variables change?

Lab Part I: Pressure & Volume

The Setup

Sealed syringe with trapped air

The Action

Adding mass to the plunger

The Measure

Record volume changes (mL)

Safety Warning

Keep syringe cap secure. Balance weights carefully. Never point the plunger toward eyes or faces.

Boyle's Law

$ P_1 V_1 = P_2 V_2 $

For a fixed amount of gas at constant temperature, the volume increases as the pressure decreases.

Inverse Relationship

Lab Part II: Temp & Volume

We will observe how air in a syringe responds to different environment temperatures:

Ice Salt Bath (~ -10°C)

Ice Water (~ 0°C)

Ambient Air (~ 22°C)

Hot Water Bath (~ 80°C)

Crucial Rule

KELVIN (K)

Temperature must be in Kelvin for calculations!

Charles's Law

\[ \frac{V_1}{T_1} = \frac{V_2}{T_2} \]

The volume of a gas is directly proportional to its Kelvin temperature at constant pressure.

Direct Relationship

Gay-Lussac's Law

\[ \frac{P_1}{T_1} = \frac{P_2}{T_2} \]

The pressure is directly proportional to the Kelvin temperature at constant volume.

Pressure Cooker Logic

Volume stays constant

Heat ↑ Pressure ↑

The Combined Gas Law

\[ \frac{P_1 V_1}{T_1} = \frac{P_2 V_2}{T_2} \]

Syncs Boyle's, Charles's, and Gay-Lussac's laws to account for all three variables changing at the same time.

The Molecular View (KMT)

Random Motion

Particles move constantly and randomly in straight paths.

Wall Collisions

Pressure comes from particles hitting the container walls.

Kinetic Energy

Temperature measures the average kinetic energy (speed).

"Heat it up → Particles go faster → Hit walls harder and more often."

Your Turn: Model It!

In your groups, develop a visual model showing how gas particles behave in a syringe when:

T is constant, Volume is halved

P is constant, Temp is doubled

Volume is constant, Temp is increased

Checklist

Clear particle diagrams
"Whoosh" marks for speed/KE
Accurate wall collision count
Labeled P, V, and T values

VOCAB SPEED SHOWDOWN

Set 1: Shout the definition or sketch the model!

Pressure

Volume

Temperature

Moles (n)

Boyle's Law

Charles's

Gay-Lussac

Combined

Kinetic E

Abs. Zero

Kelvin (K)

Ideal Gas

Partial P

STP

Diffusion

Effusion

60 Seconds

High Speed

VOCAB SPEED SHOWDOWN

Set 2: Challenge Level!

Dalton's

Gas Const (R)

Avogadro

Real Gas

Elastic Col.

Pascal (Pa)

Atmosphere

KMT

Molar Vol

Graham's

Barometer

Mole Frac

Manometer

Torr

mmHg

Vacuum

60 Seconds

Mastery

9d:T22a2,

Boyle's Law: The Squeeze

Scaffolded Practice & Roleplay

Name: ____________________________________

Roleplay: The Crowded Party

Imagine you and 10 friends are "gas particles" in a large gymnasium (High Volume). You are running around in straight lines. Suddenly, the walls begin to close in until you are all trapped in a small walk-in closet (Low Volume).

1. Wall Collisions

In which room (Gym or Closet) will you hit the walls MORE often?

2. Pressure Connection

If "hitting walls" = Pressure, which room has higher pressure?

3. The Relationship

As Volume decreases, Pressure ____________________. This is an ____________________ relationship.

Drawing the Lab

Based on your Gas Lab Explorer observations, draw the gas particles inside the syringe for both trials. Use 6 particles per syringe.

Trial A: No Books (Low Pressure)

Volume is High. Particles are far apart.

Trial B: 6 Books (High Pressure)

Volume is Low. Particles are crowded.

The Formula

P₁V₁ = P₂V₂

Golden Rule:

Temperature (T) and Moles (n) must stay constant!

Problem 1: The Deep Sea Diver

Guided

A bubble of air underwater has a volume of 10.0 mL at a pressure of 4.0 atm. As the bubble rises to the surface, the pressure drops to 1.0 atm. What is the new volume?

P1 (Initial P)

4.0 atm

V1 (Initial V)

10.0 mL

P2 (Final P)

1.0 atm

V2 (Final V)

Show your calculation below:

Problem 2: The Marshmallow Smasher

Intermediate

Inside a vacuum chamber, a marshmallow occupies 50 mL of space at 101 kPa. If the volume is compressed to 20 mL, what is the new internal pressure?

Predict:

P will increase P will decrease

Identify Variables & Solve:

Vocabulary Check:

"When the diver's bubble rose, the pressure decreased, which caused the volume to increase. This demonstrates the relationship of Boyle's Law."

9e:T155f,

Marshmallow Mission

Teacher Answer Key & Facilitation Guide

Reference Only

Initial Predictions

Plunger Out

"The marshmallow will expand / get bigger."

Plunger In

"The marshmallow will shrink / shrivel up."

Expected Observations

Action A: Pull Out

Observation: The marshmallow expands significantly. It looks "puffy" or like it's growing.

Particle Model Logic:

Students should draw air particles more spread out. With lower pressure outside the marshmallow, the air trapped inside the sugar bubbles pushes outward more effectively.

Action B: Push In

Observation: The marshmallow shrivels and shrinks. It looks wrinkled and much smaller than its original size.

Particle Model Logic:

Students should draw air particles crowded together. The increased pressure from the compressed air in the syringe pushes harder on the marshmallow, crushing the air pockets inside.

Debrief Solutions

1. Relationship Analysis:

The volume of the marshmallow decreased as the pressure increased. This is an inverse relationship (Boyle's Law).

2. The KMT Connection:

When the plunger is pulled out, the air particles in the syringe occupy a larger volume, resulting in fewer collisions per square inch against the marshmallow's surface (lower pressure). The air trapped inside the marshmallow pockets now collides more frequently than the outside air, pushing the sugar walls outward until the internal and external pressures equalize.

9f:T253d,

Boyle's Law: The Squeeze

Practice & Roleplay Exploration

Name: ____________________________________

Roleplay: The Party Crush

The Scene: You and 10 classmates are "Gas Particles."

Trial 1: Large Room

Spread out and move in straight lines. How often are you bumping into the walls?

Trial 2: The Corner

Move to a 3x3 square corner. Move at the SAME speed. Do you hit the walls more or less?

Observation: When Volume (space) decreased, the Pressure (wall hits) ____________________.

Syringe Modeling

Draw 5 gas particles in each syringe. Use "whoosh marks" (lines) to show they are moving at the SAME speed in both.

High Volume / Low Pressure

Large space = Infrequent collisions.

Low Volume / High Pressure

Small space = Frequent collisions.

Boyle's Law Formula

P₁V₁ = P₂V₂

Conditions:

Temperature & Moles are CONSTANT

1 The Weather Balloon

A weather balloon contains 500 L of Helium at sea level (1.0 atm). As it rises, the pressure drops to 0.25 atm. What is the new volume?

Step 1

List Variables

1.0 atm

500 L

0.25 atm

Step 2: Substitute into Formula

(1.0) * (500) = (0.25) * (V2)

Step 3: Solve for V2

V2 = _________ L

2 The Submarine Window

An air pocket in a submarine has a volume of 10 mL at a pressure of 100 kPa. If a leak increases the pressure to 500 kPa, what is the final volume?

Show Work (P1V1 = P2V2):

a0:T1da7,

Boyle's Law: The Squeeze

Teacher Answer Key

Roleplay: The Party Crush Key

Trial 1: Large Room

Answer: Infrequent collisions / Low Pressure.

Trial 2: The Corner

Answer: Frequent collisions / High Pressure.

Observation: When Volume (space) decreased, the Pressure (wall hits) INCREASED.

Syringe Modeling Key

High Volume / Low Pressure

Particles should be far apart with same length marks.

Low Volume / High Pressure

Particles crowded in the bottom; same energy.

Boyle's Law Formula

P₁V₁ = P₂V₂

1. The Weather Balloon Key

1.0 atm

500 L

0.25 atm

2000 L

(1.0 atm) * (500 L) = (0.25 atm) * V2
500 = 0.25 * V2
V2 = 500 / 0.25 = 2000 L

2. The Submarine Window Key

100 kPa

10 mL

500 kPa

2 mL

(100 kPa) * (10 mL) = (500 kPa) * V2
1000 = 500 * V2
V2 = 1000 / 500 = 2 mL

a1:T21ee,

Charles's Law: The Tug

Scaffolded Practice & Roleplay

Name: ____________________________________

Roleplay: The Particle Dance

Imagine you are a gas particle in a balloon. The temperature outside is the "tempo" of the music.

1. The Arctic (Slow Tempo)

The music is slow. You are barely moving. Are you pushing on the walls of the balloon very hard?

2. The Beach (Fast Tempo)

The music is fast! You are bouncing off the walls with high energy. What happens to the size of the balloon?

3. The Relationship

As Temperature increases, Volume ____________________. This is a ____________________ relationship.

Drawing the Balloon

Based on your Gas Lab Explorer observations, draw the gas particles and the size of the balloon. Show particle speed using "whoosh marks" (lines behind the dots).

Trial A: Ice Water Bath

Low Energy = Small Volume.

Trial B: Boiling Water Bath

High Energy = Large Volume.

The Formula

V₁ / T₁ = V₂ / T₂

CRITICAL RULE:

K = °C + 273.15

You MUST use Kelvin!

Problem 1: The Liquid Nitrogen Balloon

Guided

A balloon has a volume of 3.0 L at room temperature (25°C). It is dipped in liquid nitrogen, and the temperature drops to -196°C. What is the new volume?

Step 0: Convert Temperatures to Kelvin!

T1: 25 + 273.15 = 298.15 K

T2: -196 + 273.15 =

3.0 L

T1 (in K)

298.15 K

Show your cross-multiplication below:

Problem 2: The Sunny Car

Independent

A sealed bag of chips has a volume of 250 mL in an air-conditioned car at 20°C. The car is parked in the sun, and the temp inside rises to 55°C. What is the new volume?

Calculate Kelvin first, then solve for V2:

a2:T1f49,

Charles's Law: The Tug

Practice & Roleplay Exploration

Name: ____________________________________

Roleplay: The Particle Dance

The Scene: You are a "Gas Particle" inside a flexible balloon. The music tempo represents Temperature.

Trial 1: Slow Waltz (Cold)

Move very slowly. Are you pushing the balloon walls outward very much?

Trial 2: Fast Techno (Hot)

Jump and move fast! Do you push the walls further out now?

Observation: When Temperature increased, the Volume (balloon size) ____________________.

Balloon Modeling

Draw the balloon size and the particles inside. Use "whoosh marks" to show High Speed vs Low Speed.

Cold Gas (Liquid Nitrogen)

Low Kinetic Energy = Small Volume.

Hot Gas (Sunlight)

High Kinetic Energy = Large Volume.

Charles's Law Formula

V₁ / T₁ = V₂ / T₂

Must Convert T to Kelvin!

K = °C + 273.15

1 The Frozen Balloon

A balloon with a volume of 2.0 L at 25°C is placed in a freezer at -5°C. What is the new volume of the balloon?

Step 1: Kelvin Conversion (Critical!)

T1 = 25 + 273 = 298 K

T2 = -5 + 273 = _______ K

2.0 L

T1 (K)

298 K

T2 (K)

_______

Show Cross-Multiplication (V1 * T2 = V2 * T1):

2 The Hot Air Balloon

A hot air balloon starts with 1000 L of air at 20°C. The pilot heats the air to 80°C. What is the new volume?

Convert T to K, Setup, and Solve:

a3:T1a01,

Charles's Law: The Tug

Teacher Answer Key

Roleplay: The Particle Dance Key

Trial 1: Slow Waltz (Cold)

Answer: No, the pressure is lower, so the balloon stays small.

Trial 2: Fast Techno (Hot)

Answer: Yes, the increased speed pushes the walls out further.

Observation: When Temperature increased, the Volume (balloon size) INCREASED.

Balloon Modeling Key

Cold Gas (Liquid Nitrogen)

Balloon is tiny; particles have no/short marks.

Hot Gas (Sunlight)

Balloon is large; particles have long "whoosh" marks.

Charles's Law Formula

V₁ / T₁ = V₂ / T₂

1. The Frozen Balloon Key

Step 1: Kelvin Conversion Key

T1 = 25 + 273 = 298 K

T2 = -5 + 273 = 268 K

2.0 L

298 K

268 K

~1.80 L

2.0 L / 298 K = V2 / 268 K
V2 = (2.0 * 268) / 298
V2 = 536 / 298 = 1.7986... ≈ 1.80 L

2. The Hot Air Balloon Key

T1 = 20 + 273 = 293 K
T2 = 80 + 273 = 353 K
1000 L / 293 K = V2 / 353 K
V2 = (1000 * 353) / 293
V2 = 353,000 / 293 ≈ 1204.78 L

a4:T2047,

Gay-Lussac: The Punch

Scaffolded Practice & Roleplay

Name: ____________________________________

Roleplay: Particle Bumper Cars

Imagine you are in a bumper car arena. The walls are made of solid steel and **cannot move** (Constant Volume).

1. Low Heat (Slow Cars)

The cars are moving slowly. When you hit a wall, is it a loud bang or a soft tap?

2. High Heat (Fast Cars)

The cars are zooming! You hit the walls more often and much harder. What happens to the "Pressure" on the walls?

3. The Relationship

As Temperature increases in a rigid container, Pressure ____________________. This is a ____________________ relationship.

Drawing the Rigid Tank

Draw the gas particles in these two rigid containers (Volume stays the same!). Draw the needle on the **Pressure Gauge** to show the change.

A: Room Temp Tank (293 K)

Low Temp = Low Pressure.

B: Blowtorch Tank (600 K)

High Temp = High Pressure.

The Formula

P₁ / T₁ = P₂ / T₂

Danger Zone:

V must be CONSTANT!

Always use Kelvin (K) for T.

Problem 1: The Pressure Cooker

Guided

A pressure cooker is sealed at 1.0 atm and room temperature (20°C). The water inside boils and reaches 120°C. What is the pressure inside the cooker?

Initial State (1)

P1 = 1.0 atm

T1 = 20 + 273.15 = 293.15 K

Final State (2)

P2 = ?

T2 = 120 + 273.15 = ________ K

Setup your equation and solve for P2:

Problem 2: The Aerosol Can Warning

Real-World

"WARNING: Store below 50°C. Contents under pressure. May explode if heated."

An aerosol can has a pressure of 3.0 atm at 25°C. If the can is thrown into a fire (600°C), what will the pressure become? (Assume the can holds its shape until it bursts).

Identify Variables (Convert T to K) & Solve:

a5:T1bbb,

GAS MASTER CHART

Quick Reference Guide

BOYLE'S LAW

Volume vs Pressure

$ P_1 V_1 = P_2 V_2 $

Key Takeaway: INVERSE relationship. If pressure goes UP, volume goes DOWN. (Temp constant)

CHARLES'S LAW

Volume vs Temp

\[ \frac{V_1}{T_1} = \frac{V_2}{T_2} \]

Key Takeaway: DIRECT relationship. If temperature goes UP, volume goes UP. (Pressure constant)

GAY-LUSSAC'S LAW

Pressure vs Temp

\[ \frac{P_1}{T_1} = \frac{P_2}{T_2} \]

Key Takeaway: DIRECT relationship. If temperature goes UP, pressure goes UP. (Volume constant)

THE COMBINED LAW

P, V, & T

\[ \frac{P_1 V_1}{T_1} = \frac{P_2 V_2}{T_2} \]

Key Takeaway: Useful when all three variables change. Remeber: Temp MUST be in Kelvin!

Variables

P = PRESSURE (atm, mmHg, kPa)
V = VOLUME (L, mL)
T = TEMPERATURE (Kelvin ONLY)
n = NUMBER OF MOLES

Temperature Fix

K = °C + 273.15

No Negative Numbers in Gas Math!

Ideal Standard (STP)

TEMP = 0°C (273.15 K)
PRESSURE = 1.00 atm
101.3 kPa // 760 mmHg

Boyle's Graph

Inverse Curve

Charles's Graph

Direct Linear

Gay-Lussac's Graph

Direct Linear

a6:T3911,

Mixed Law Medley

Pressure, Volume, and Temperature Integration

Name:

Date:

Formula Bank

Boyle's Law

$P_1V_1 = P_2V_2$

Charles's Law

$\frac{V_1}{T_1} = \frac{V_2}{T_2}$

Gay-Lussac's Law

$\frac{P_1}{T_1} = \frac{P_2}{T_2}$

Combined Law

$\frac{P_1V_1}{T_1} = \frac{P_2V_2}{T_2}$

Pro-Tips & Conversions

Temperature: Always use Kelvin! ($K = ^\circ C + 273$)
Constants: Identify which variable doesn't change first.
Isolate: Rearrange your formula before plugging in numbers.

Mission Instructions:

Complete each scenario by identifying variables, choosing the correct law, and showing your mathematical steps. Check your results against the Answer Bank at the end of page 2!

A flexible syringe contains 50.0 mL of air at 1.20 atm. If the plunger is compressed to a volume of 20.0 mL at constant temperature, what is the new pressure inside the syringe?

Variables List

$P_1$: ____ $P_2$: ____ $V_1$: ____ $V_2$: ____

Identify Law

Boyle's

Charles's

Combined

Constant

Mathematical Solve & Final Answer

A birthday balloon has a volume of 2.50 L at a room temperature of $22.0^\circ C$. If the balloon is taken outside into the winter air where the temperature is $-5.0^\circ C$, what will be its new volume? (Pressure remains constant).

Temp Conversion

$T_1$: 22.0 + 273 = ____ K

$T_2$: -5.0 + 273 = ____ K

Variables

$V_1$: ____ $V_2$: ____

Equation Choice

_____________

Mathematical Solve & Final Answer

Mixed Law Medley (Page 2)

Student Name: ________________________

A rigid steel tank contains gas at a pressure of 150 kPa when the temperature is $25.0^\circ C$. If the tank is heated to $150.0^\circ C$, what will be the new pressure inside the tank?

Variable Map

$P_1$: __________

$T_1$: __________ K

Target

$P_2$: ???

$T_2$: __________ K

Law Applied

Gay-Lussac's

Mathematical Solve & Final Answer

A weather balloon is released from the surface where the pressure is 101.3 kPa, the volume is 15.0 L, and the temperature is $20.0^\circ C$. It rises to where the pressure is 45.0 kPa and the temperature is $-30.0^\circ C$. What is its new volume?

Initial State ($P_1, V_1, T_1$)

P: ______ V: ______ T: ______ K

Final State ($P_2, V_2, T_2$)

P: ______ V: ??? T: ______ K

Isolate $V_2$ and Solve

Challenge: The Pressure Cooker

ANALYSIS

A pressure cooker contains steam at 1.00 atm and $100^\circ C$. The lid bursts at 3.50 atm. If the temperature hits $250^\circ C$, will it burst? Show proof.

Constants Check

Which variable is constant?

Comparison

Compare $P_{calc}$ to 3.50 atm.

Show Mathematical Proof

a7:T1426,

KITCHEN CHEMISTRY

Pressure Cookers & Gay-Lussac's Law

Name: ____________________________________

The System

Sealed Pressure Cooker

V = CONSTANT

The Phenomenon

Standard pots boil water at 100°C. However, a pressure cooker uses a sealed lid to trap steam, allowing the internal pressure to rise. As the pressure increases, the boiling point of the water increases, allowing food to cook much faster.

Guiding Question:

How does temperature affect the pressure of a gas trapped inside a fixed-volume container?

CLAIM

State your answer to the guiding question.

EVIDENCE

Provide data or observations to support your claim.

Observation 1: Heating

Observation 2: Gauge Reading

REASONING

Connect your evidence to the scientific principle (KMT).

1. Explain how kinetic energy changes with temperature...

2. Explain how collision frequency and force change...

3. Use Gay-Lussac's Law to conclude...

Safety Connection

If the temperature of a pressure cooker exceeds its safety limits, the pressure will rise until the structural integrity of the pot fails. This is why every pressure cooker has a "relief valve" to release gas and lower pressure safely.

a8:T2215,

Gay-Lussac's Law: The Punch

Practice & Roleplay Exploration

Name: ____________________________________

Roleplay: Bumper Cars

The Scene: You are in a bumper car arena. The walls are made of steel and cannot move (Constant Volume).

Trial 1: Low Heat (Slow Cars)

You move slowly. When you hit the steel wall, is the impact force high or low?

Trial 2: Blowtorch (Fast Cars)

You zoom fast! You hit the walls more often and harder. What happened to the pressure?

Observation: In a rigid container, as Temperature increased, Pressure ____________________.

Gauge Modeling

The container volume stays the same! Draw the particles and move the Pressure Gauge needle to show the change.

A: Tank at Room Temp (293 K)

Low Temp = Low Gauge Pressure.

B: Tank in Fire (600 K)

High Temp = High Gauge Pressure.

Gay-Lussac Formula

P₁ / T₁ = P₂ / T₂

Caution:

Use KELVIN only!

1 The Pressure Cooker

A pressure cooker is sealed at 1.0 atm and 20°C. The temperature rises to 120°C. What is the new pressure?

Step 1: Kelvin Conversion

T1 = 20 + 273 = 293 K

T2 = 120 + 273 = _______ K

1.0 atm

T1 (K)

293 K

T2 (K)

_______

Show Algebra (P1 * T2 = P2 * T1):

2 The Aerosol Can

An aerosol can has a pressure of 3.0 atm at 25°C. If the temperature is increased to 300°C, what is the new pressure?

Convert T to K, Setup, and Solve:

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Answer Key

Mixed Law Medley • Teacher Reference Only

Official Key

Boyle's Law Calculation

Mapping

$P_1 = 1.20 \text{ atm}$, $V_1 = 50.0 \text{ mL}$

$P_2 = ?$, $V_2 = 20.0 \text{ mL}$

Law: Boyle's Law

Constant: Temperature

Solution Pathway

$P_1V_1 = P_2V_2$
$(1.20)(50.0) = P_2(20.0)$
$60.0 = P_2(20.0)$
$P_2 = 3.00 \text{ atm}$

Charles's Law Calculation

Mapping

$V_1 = 2.50 \text{ L}$, $T_1 = 22.0 + 273 = 295 \text{ K}$

$V_2 = ?$, $T_2 = -5.0 + 273 = 268 \text{ K}$

Law: Charles's Law

Solution Pathway

$\frac{V_1}{T_1} = \frac{V_2}{T_2} \rightarrow V_2 = \frac{V_1T_2}{T_1}$
$V_2 = \frac{(2.50)(268)}{295}$
$V_2 = \frac{670}{295}$
$V_2 = 2.27 \text{ L}$

Gay-Lussac's Law Calculation

Mapping

$P_1 = 150 \text{ kPa}$, $T_1 = 25.0 + 273 = 298 \text{ K}$

$P_2 = ?$, $T_2 = 150.0 + 273 = 423 \text{ K}$

Law: Gay-Lussac's Law

Solution Pathway

$\frac{P_1}{T_1} = \frac{P_2}{T_2} \rightarrow P_2 = \frac{P_1T_2}{T_1}$
$P_2 = \frac{(150)(423)}{298}$
$P_2 = \frac{63450}{298}$
$P_2 = 213 \text{ kPa}$

Answer Key (Page 2)

Combined Gas Law Calculation

Mapping

$P_1 = 101.3 \text{ kPa}, V_1 = 15.0 \text{ L}, T_1 = 293 \text{ K}$

$P_2 = 45.0 \text{ kPa}, V_2 = ?, T_2 = 243 \text{ K}$

Solution Pathway

$\frac{P_1V_1}{T_1} = \frac{P_2V_2}{T_2} \rightarrow V_2 = \frac{P_1V_1T_2}{P_2T_1}$
$V_2 = \frac{(101.3)(15.0)(243)}{(45.0)(293)}$
$V_2 = \frac{369238}{13185}$
$V_2 = 28.0 \text{ L}$

Challenge: Pressure Cooker

Constant

Volume ($V$) is constant in a rigid cooker.

Mapping

$P_1 = 1.00 \text{ atm}, T_1 = 373 \text{ K}$

$P_2 = ?, T_2 = 523 \text{ K}$

The Proof

$P_2 = \frac{(1.00)(523)}{373} = 1.40 \text{ atm}$

Verdict: Will NOT burst.

Calculated pressure (1.40 atm) is much lower than the 3.50 atm limit.

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Gay-Lussac's Law: The Punch

Teacher Answer Key

Roleplay: Bumper Cars Key

Trial 1: Low Heat (Slow Cars)

Answer: Soft tap / Low force impact.

Trial 2: Blowtorch (Fast Cars)

Answer: Pressure increased significantly due to speed and frequency.

Observation: In a rigid container, as Temperature increased, Pressure INCREASED.

Gauge Modeling Key

A: Tank at Room Temp (293 K)

Needle should point to the left/low pressure.

B: Tank in Fire (600 K)

Needle should point to the right/high pressure.

Gay-Lussac Formula

P₁ / T₁ = P₂ / T₂

1. The Pressure Cooker Key

Step 1: Kelvin Conversion Key

T1 = 20 + 273 = 293 K

T2 = 120 + 273 = 393 K

1.0 atm

293 K

393 K

~1.34 atm

1.0 atm / 293 K = P2 / 393 K
P2 = (1.0 * 393) / 293
P2 = 393 / 293 ≈ 1.34 atm

2. The Aerosol Can Key

T1 = 25 + 273 = 298 K
T2 = 300 + 273 = 573 K
3.0 atm / 298 K = P2 / 573 K
P2 = (3.0 * 573) / 298
P2 = 1719 / 298 ≈ 5.77 atm

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Law Lab Classifier

Identification & Mathematical Modeling

Name: ____________________________________

Date: _________________ Period: _________

Boyle's Law

Constant: Temp (T)

P vs. V (Inverse)

Charles's Law

Constant: Pressure (P)

V vs. T (Direct)

Gay-Lussac's

Constant: Volume (V)

P vs. T (Direct)

A scuba tank holds 15 L of air at 200 atm. If all the air is released into a giant 3000 L balloon at the same temperature, what is the new pressure?

Step A: Identify & Classify

Constant:

Law Name:

Step B: Solve It

Show setup and final answer (with units):

A research balloon has a volume of 5.0 L at 20°C. It is carried into the upper atmosphere where the temperature is -40°C. Assuming pressure is held constant, what is the new volume?

Step A: Identify & Classify

Constant:

Law Name:

Step B: Solve It

Remember Kelvin! K = °C + 273.15

An aerosol can is at 1.5 atm at a room temperature of 25°C. If the can is heated to 400°C, what will be the final internal pressure? (The can's volume does not change).

Step A: Identify & Classify

Constant:

Law Name:

Step B: Solve It

A tire has a pressure of 32 psi at 20°C. After a long drive, the friction heats the tire air to 50°C. If the volume of the tire is constant, what is the new pressure?

Step A: Identify & Classify

Constant:

Law Name:

Step B: Solve It

A sample of air occupies 2.5 L at 1.0 atm. If it is compressed into a 0.5 L container at constant temperature, what is the pressure inside the smaller container?

Step A: Identify & Classify

Constant:

Law Name:

Step B: Solve It

Classification Strategy

"To choose the right law, I always look for the variable that DOES NOT change. If the container is rigid, I know volume is constant. If the syringe is sealed and moved to a bath, I know moles are constant..."

Write your own tip for identifying gas laws in word problems:

LAB-IDENT-77

PRESSURE POWER UNIT

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Law Lab Classifier

Teacher Answer Key

1. Scuba Tank (15L, 200atm) → Balloon (3000L). Constant Temp.

Identification Key

Constant: Temperature (T)

Law: BOYLE'S LAW

P1V1 = P2V2
(200 atm)(15 L) = P2(3000 L)
3000 = 3000 * P2
P2 = 1.0 atm

2. Balloon (5.0L, 20°C) → Upper Atmosphere (-40°C). Constant Pressure.

Identification Key

Constant: Pressure (P)

Law: CHARLES'S LAW

T1 = 293.15 K | T2 = 233.15 K
V1/T1 = V2/T2
5.0 / 293.15 = V2 / 233.15
V2 = (5.0 * 233.15) / 293.15
V2 ≈ 3.98 L

3. Aerosol Can (1.5atm, 25°C) → Heat (400°C). Constant Volume.

Identification Key

Constant: Volume (V)

Law: GAY-LUSSAC'S LAW

T1 = 298.15 K | T2 = 673.15 K
P1/T1 = P2/T2
1.5 / 298.15 = P2 / 673.15
P2 = (1.5 * 673.15) / 298.15
P2 ≈ 3.39 atm

4. Tire (32 psi, 20°C) → Drive (50°C). Constant Volume.

Identification Key

Constant: Volume (V)

Law: GAY-LUSSAC'S LAW

T1 = 293.15 K | T2 = 323.15 K
32 / 293.15 = P2 / 323.15
P2 = (32 * 323.15) / 293.15
P2 ≈ 35.27 psi

5. Sample (2.5L, 1.0atm) → Container (0.5L). Constant Temp.

Identification Key

Constant: Temperature (T)

Law: BOYLE'S LAW

(1.0 atm)(2.5 L) = P2(0.5 L)
2.5 = 0.5 * P2
P2 = 2.5 / 0.5
P2 = 5.0 atm

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PEER REVIEW PRO

Combined Gas Law Modeling Rubric

Scoring Guide

Reviewer: ________________________________

Model Author: ____________________________

Review Mission

Evaluate how well your peers have modeled the relationships between pressure, volume, and temperature using Kinetic Molecular Theory (KMT). Provide constructive feedback to help them improve their scientific communication.

Criterion	Expert (4 pts)	Developing (3 pts)	Novice (1-2 pts)
KMT Accuracy Do particle size, count, and speed match the scenario?	Particle count is constant. Speed ("whooshes") and spacing perfectly reflect the temperature and volume changes.	Particles are present, but speed or spacing is slightly inconsistent with the scenario variables.	Particle count changes (leaks), or speed/spacing contradicts the laws being modeled.
Collision Logic Is pressure visually represented as collisions?	Clear visual evidence of particles hitting container walls. High pressure = many hits; Low = few hits.	Some collisions shown, but the relationship between frequency and pressure is vague.	No clear collisions shown, or pressure is not linked to particle interaction with the walls.
Variable Clarity Are P, V, and T clearly defined for each state?	Initial and final values for P, V, and T are explicitly labeled. Change direction is clear.	Most variables are labeled, but some units or directions of change are missing.	Labels are missing, disorganized, or incorrect. Variables are not defined.
Scientific Rationale Is the mathematical relationship explained?	Succinct written explanation uses the correct gas law names and explains the 'why' using KMT.	Correct gas law identified, but the KMT explanation is weak or incomplete.	Incorrect law identified, or no written explanation provided.

Glow (What was done well?)

Grow (Actionable Improvement)

Total Score Calculation

_____ / 16

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Ideal Identity

Chunked Reading Passage

Name: ____________________________________

Date: _____________________________________

CHUNK 1

The Perfect Gas Myth

In chemistry, we often talk about an Ideal Gas. But here's the secret: an ideal gas doesn't actually exist. It is a mathematical model—a "perfect" version of a gas that follows the rules of the Kinetic Molecular Theory (KMT) perfectly at all temperatures and pressures. Scientists use this model because it makes the math much simpler, and for most gases we encounter in daily life, the model is "close enough" to the truth.

"An ideal gas is a gas that perfectly fits all the assumptions of the kinetic-molecular theory."

The 5 Assumptions

1. Gases consist of large numbers of tiny particles.
2. Collisions are elastic (no energy lost).
3. Particles move in continuous, rapid, random motion.
4. There are no forces of attraction between particles.
5. The particles themselves have zero volume.

STOP AND JOT

In your own words, why do scientists use the "Ideal Gas" model if ideal gases aren't real?

Sentence Stem:

"Scientists use this model because it ___________________________________________________________________________________."

CHUNK 2

Where Reality Breaks the Rules

Issue #1: Sticky Particles

KMT assumes gas particles don't care about each other. In reality, every atom and molecule has some level of attraction (intermolecular forces). When particles slow down, these tiny "sticky" forces pull them together, eventually causing the gas to condense into a liquid.

Issue #2: Physical Volume

KMT assumes particles have no size. But atoms are matter! They occupy physical space. In a very small container, the volume of the particles themselves becomes significant, leaving less "empty space" than the model predicts.

THINK PAIR AND SHARE

"If we had a gas made of very 'sticky' (polar) particles like water vapor, would it act more or less ideal than Helium? Why?"

Sentence Stems for Discussion:

• "I think water vapor would act more / less ideal because..."

• "I agree/disagree because particles with high attraction tend to..."

CHUNK 3

The "Ideal" Escape

The Golden Rule of Gas Math

Real gases behave most like ideal gases when they are at
HIGH TEMPERATURE and LOW PRESSURE.

Why High Temp?

Particles zip past so fast that attractions don't have time to "grab" them.

Why Low Pressure?

Particles are so far apart that their individual size is basically zero compared to the space.

STOP AND JOT

Explain the relationship between temperature and ideal behavior:

Sentence Stem:

"To keep a gas behaving 'ideally,' we should increase/decrease the temperature because ___________________________________________________________________________________."

Identity Verification Check

Mastery Question 1

Which KMT assumption is violated when a gas turns into a solid or liquid?

Mastery Question 2

Under which set of conditions would Oxygen gas deviate MOST from ideal behavior?

The Ultimate Choice

Pair A: Heat Choice

He at 500K

He at 100K

Pair B: Pressure Choice

Ne at 1 atm

Ne at 50 atm

Pair C: Molecule Choice

H₂O (Polar)

H₂ (Nonpolar)

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Active Monitoring Checklist

Teacher Resource: Ideal Identity Reading Passage

Lesson Phase

Guided Practice / Literacy

Monitoring Objective

Circulate during the Chunked Reading. Focus on identifying students who struggle to articulate why a gas is non-ideal (Intermolecular Forces vs. Particle Volume) and provide immediate scaffolding using the provided sentence stems.

Reading Chunk	Student "Look-Fors" (Evidence of Mastery)	Scaffolding Question / Prompt
Chunk 1: The Myth	Students explain that "Ideal" means "Perfect/Model" not "Real". Stop and Jot highlights that the model is for simpler math.	"If a gas is 'ideal', does it follow all the rules of KMT, or just some?"
Chunk 2: Reality Gap	Students mention "stickiness" or "attraction" as a violation. Think-Pair-Share distinguishes between Polar (less ideal) and Nonpolar (more ideal) molecules.	"Think about the magnets. Do gas particles have tiny magnets inside them that pull them together?"
Chunk 3: Golden Rule	Students identify High T / Low P as ideal conditions. Stop and Jot 2 links speed (High T) to overcoming attractions.	"If the particles are zipping past each other like race cars, do they have time to stick together?"

Common Misconceptions

Thinking "Ideal" means "Better": Clarify that ideal gases are just simpler models, not "higher quality" gases.

Mixing up conditions: Many students think Low Temp is ideal. Remind them: Cold = Slow = Sticky.

Mastery Checkpoint

By the end of the rotation, 100% of students should be able to answer:

"Why does a gas stop behaving ideally when it gets very cold and very crowded?"

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SYRINGE MODELS

Developing Models for the Combined Gas Law

Name: ____________________________________

Scientific Modeling Task

In each scenario below, draw the Initial State and the Final State of the gas particles inside the syringe. Use the provided variables to guide your diagrams.

Scenario: Temperature is Constant, Volume is Halved

Initial State (V = 20 mL, P = 1 atm)

Final State (V = 10 mL, P = ???)

Scientific Explanation (Link KMT to Pressure):

Scenario: Pressure is Constant, Temperature is Doubled

Initial State (T = 300 K, V = 10 mL)

Final State (T = 600 K, V = ???)

Scientific Explanation (Link KMT to Volume):

Scenario: Volume is Constant, Temperature is Increased

Initial State (V = 15 mL, T = 273 K)

Final State (V = 15 mL, T = 400 K)

Scientific Explanation (Link KMT to Pressure):

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Ideal Identity

Teacher Answer Key

Reference Only

1. Why is the "Ideal Gas" considered a model rather than a reality?

It is a mathematical model used to simplify calculations. In reality, no gas follows all KMT assumptions perfectly (particles have volume and exert attractive forces), but the ideal model is "close enough" for most conditions.

2. Conditions for Deviation

Real gases deviate from ideal behavior at Low Temperature and High Pressure.

3. Violated Assumption

The assumption that there are no forces of attraction between particles. When a gas turns to liquid, attractions have pulled the particles together.

Ultimate Choice Key (More Ideal)

Pair A

He at 500K

Reason: High Temp (faster motion overcomes attractions)

Pair B

Ne at 1 atm

Reason: Low Pressure (particles are far apart)

Pair C

H₂ (gas)

Reason: Non-polar and smaller (weaker attractions)

Quick Reference: Ideal vs. Real

Feature	Ideal Gas (Model)	Real Gas (Actual)
Volume	Particles have zero volume.	Particles occupy physical space.
Attraction	No intermolecular forces.	Small attractive forces exist.
Collisions	Perfectly elastic (no energy lost).	Nearly elastic (tiny energy loss).

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Ideal Equation Engine

Mathematical Modeling: $PV = nRT$

Name: ____________________________________

Date: _____________________________________

The Formula

PV = nRT

Variable Calibration

Pressure

atm

Volume

Liters (L)

Amount

moles (mol)

Temp

Kelvin (K)

Constant R = 0.0821 $\frac{L \cdot atm}{mol \cdot K}$

T(K) = °C + 273.15

Unit Pre-Check

Celsius to Kelvin

25°C = ________ K

-10°C = ________ K

mL to Liters

500 mL = ________ L

1,250 mL = ________ L

Grams to Moles

Use He = 4.00 g/mol

8.0 g He = ________ mol

Guided Mission 1: The Weather Balloon

"A high-altitude weather balloon contains 15.0 moles of Helium. If the pressure at that altitude is 0.45 atm and the temperature is -20°C, what is the volume of the balloon?"

Step 1: Variables

P = 0.45 atm V = ??? n = 15.0 mol R = 0.0821 T = -20°C → ________ K

Step 2: Algebra & Solution

Rearrange the formula to solve for V:

V = __________________

Final Calculation

Mission Parameters

A scuba tank with a volume of 12.0 L is filled with 80.0 moles of air at 25°C. What is the pressure (in atm) inside the tank?

Analyze Variables

P = ________

V = ________

n = ________

T = ________ (Kelvin)

Work & Solution

A sample of Carbon Dioxide gas occupies a volume of 2.50 L at 350 K and 1.25 atm. How many moles of CO₂ are present in the sample?

Analyze Variables

P = ________

V = ________

n = ________

T = ________

Work & Solution

Level 2 Challenge

The Oxygen Tank Problem

A 5.0 L container holds 16.0 grams of Oxygen gas (O₂). If the pressure is 2.5 atm, what is the temperature of the gas in Kelvin? (Note: O₂ molar mass = 32.0 g/mol. You must convert grams to moles first!)

Pre-Calculation (n)

Ideal Gas Law Work

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Ideal Equation Engine

Teacher Answer Key

Reference Only

Unit Pre-Check Solutions

Celsius to Kelvin

25°C = 298 K

-10°C = 263 K

mL to Liters

500 mL = 0.5 L

1,250 mL = 1.25 L

Grams to Moles

8.0 g He = 2.0 mol

Guided Mission 1: Weather Balloon

Solve for V: $V = \frac{nRT}{P}$

Variables:

T = 253 K (-20 + 273)

n = 15.0 mol

Calculation:

$V = \frac{(15.0)(0.0821)(253)}{0.45}$

V = 692.6 L

2. Scuba Tank Pressure

Solve for P: $P = \frac{nRT}{V}$

Variables:

n = 80.0 mol, V = 12.0 L

T = 298 K

Calculation:

$P = \frac{(80.0)(0.0821)(298)}{12.0}$

P = 163.1 atm

3. CO₂ Moles

Solve for n: $n = \frac{PV}{RT}$

Variables:

P = 1.25 atm, V = 2.50 L

T = 350 K

Calculation:

$n = \frac{(1.25)(2.50)}{(0.0821)(350)}$

n = 0.109 mol

4. Challenge: Oxygen Temp

Step 1: Grams to Moles

$16.0g \cdot \frac{1 mol}{32.0g} = 0.50 mol$

Step 2: Solve for T

$T = \frac{PV}{nR}$

Calculation:

$T = \frac{(2.5)(5.0)}{(0.50)(0.0821)}$

T = 304.5 K

(31.35°C)

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GAS GLOSSARY CARDS

Vocabulary Review & Sorting Game

Concept

Boyle's Law

The inverse relationship between pressure and volume at a constant temperature.

$ P_1 V_1 = P_2 V_2 $

Concept

Charles's Law

The direct relationship between temperature and volume at a constant pressure.

\[ \frac{V_1}{T_1} = \frac{V_2}{T_2} \]

Concept

Gay-Lussac

The direct relationship between temperature and pressure at a constant volume.

\[ \frac{P_1}{T_1} = \frac{P_2}{T_2} \]

Theory

KMT

Kinetic Molecular Theory: Explains that gas particles are in constant, random motion.

Variable

Absolute Zero

The theoretical temperature where all particle motion stops (0 Kelvin).

-273.15°C

Formula

Combined Law

Expresses the relationship between P, V, and T for a fixed amount of gas.

\[ \frac{P_1 V_1}{T_1} = \frac{P_2 V_2}{T_2} \]

Cut along solid lines to create study cards

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Formula Finder

Gas Law Mnemonics & Mastery

Name:

Date:

Part 1: Video Check-In

Watch the video "Mnemonic for Gas Laws" and answer the following questions to unlock the mnemonic secret!

1. What is the full mnemonic phrase shared in the video?

Can These Girls Play Basketball Very Well?

Can These Guys Possibly Be Victorious?

Could They Go Past Big Valleys?

2. In the mnemonic triangle, what does "Possibly" stand for?

Particles

Pressure

Product

3. When letters are side-by-side in the triangle, what math operation do you use?

Multiplication (e.g., $ P \times V $)

Division (e.g., $ V / T $)

Addition (e.g., $ P + T $)

Part 2: Mnemonic Maker

Create your own Formula Finder Triangle below. Follow these steps from the video:

1 Draw a large triangle and divide it into three sections.
2 Write the mnemonic letters (C, T, G, P, B, V) clockwise starting from the bottom right corner.
3 Place the variables ($ P $, $ V $, $ T $) inside the corner pieces.

Draw Triangle Here

Part 3: The Scramble

Mission Instructions:

1. Identify the law first. 2. Convert all temperatures to Kelvin ($ K = ^\circ C + 273 $). 3. Solve for the missing variable.

Problem 01 The Balloon Blast

A balloon contains $ 2.0\text{ L} $ of air at $ 298\text{ K} $. If the temperature is increased to $ 350\text{ K} $ at constant pressure, what is the new volume?

Gas Law

Show Your Work

Problem 02 The Scuba Squeeze

A diver's tank has a volume of $ 10\text{ L} $ at $ 1.0\text{ atm} $. If the pressure increases to $ 3.0\text{ atm} $ at constant temperature, what is the new volume?

Gas Law

Show Your Work

Problem 03 The Pressure Cooker

A sealed container at $ 100\text{ kPa} $ is heated from $ 20^\circ\text{C} $ to $ 120^\circ\text{C} $. Volume is constant. Find the final pressure.

Gas Law

Show Your Work

Problem 04 Tire Troubles

A car tire has a pressure of $ 32\text{ psi} $ at $ 15^\circ\text{C} $. After a long drive, the temperature rises to $ 45^\circ\text{C} $. What is the new pressure? (V is constant)

Gas Law

Show Your Work

Problem 05 Piston Push

A piston compresses $ 500\text{ mL} $ of gas at $ 760\text{ mmHg} $ down to $ 100\text{ mL} $. If T is constant, find the new pressure.

Gas Law

Show Your Work

Problem 06 Winter Woes

A soccer ball inflated to $ 2.5\text{ L} $ at $ 25^\circ\text{C} $ is taken outside where it's $ -5^\circ\text{C} $. At constant pressure, what is its new volume?

Gas Law

Show Your Work

Problem 07 Spray Can Caution

An aerosol can has a pressure of $ 3.0\text{ atm} $ at $ 20^\circ\text{C} $. It is thrown into a fire ($ 600^\circ\text{C} $). If it bursts at $ 8.0\text{ atm} $, will it explode?

Gas Law

Show Your Work

Problem 08 Mountain Meditations

A bag of chips has $ 150\text{ mL} $ of air at sea level ($ 1.0\text{ atm} $). On a mountain, the pressure is $ 0.7\text{ atm} $. New volume? (T constant)

Gas Law

Show Your Work

Problem 09 Laboratory Leak

A gas syringe contains $ 50\text{ mL} $ at $ 100^\circ\text{C} $. It is cooled until the volume is $ 25\text{ mL} $ (constant pressure). What is the final temperature in $ ^\circ C $?

Gas Law

Show Your Work

Problem 10 Deep Sea Discovery

A bubble rises from the bottom of a lake ($ 5.0\text{ atm} $, $ 10\text{ mL} $) to the surface ($ 1.0\text{ atm} $). If T is constant, what is its volume at the surface?

Gas Law

Show Your Work

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Atmospheric Incident Report

Self-Guided Field Activity // Unit: Gas Law Investigation

Investigator:

Badge #:

Case Study Reference Guide

Boyle's Law (P vs V)

Inverse Relationship

Pressure UP = Volume DOWN. Particles get squeezed into smaller space.

Charles's Law (V vs T)

Direct Relationship

Temp UP = Volume UP. Particles hit harder/faster, pushing walls outward.

Gay-Lussac (P vs T)

Direct Relationship

Temp UP = Pressure UP. (In rigid containers like cans). Explosion risk!

CASE #01

The "Pop" in the Pines

"I was camping in the high mountains where air pressure is thin. I sealed my water bottle tightly before driving down to the valley at sea level (high pressure). When I parked, my bottle was crushed flat like a soda can!"

Changing Variables

Correct Gas Law

Evidence Interpretation (Explain why the bottle crushed)

Particle Map: Inside Bottle

Mountain

Sea Level

Draw 8 particles in each. Change the spacing.

CASE #02

The Winter Morning "Flat"

"I checked my car's tire pressure on a hot summer day. Six months later, a cold front hit. My tires looked low and the dashboard alarm went off—but there are NO leaks in the tires. Where did the pressure go?"

Variables Involved:

Check the investigator's logic (Circle one):

Directly Proportional

Inversely Proportional

Microscopic Description (Particle Speed & Collisions)

Determination

Law Applied

CASE #03

The Floating Fiesta Failure

"We filled party balloons in a cold garage. As soon as we brought them into the heated party room, they began to swell. Suddenly—BANG! The balloons exploded before the guests even arrived."

Data Log

Temperature

Cold Hot

Volume

Investigator's Conclusion (Use KMT Logic)

Explain why the balloons burst. Mention particles, speed, and collisions with the container wall...

Forensic Forecast

Complete the table based on your investigation skills. Circle the final outcome.

Incident Scenario	Pressure Prediction	Volume Prediction
Heating an aerosol can over a fire.	INCREASE / DECREASE	NO CHANGE
Pulling UP on a syringe plunger.	INCREASE / DECREASE	INCREASE / DECREASE
Putting a gas cylinder in a freezer.	INCREASE / DECREASE	NO CHANGE

Critical Evidence Challenge

A rookie says: "If I double the temperature from 20°C to 40°C, the gas pressure will also double exactly."

Prove them wrong. Why must gas law investigations use Kelvin instead of Celsius?

Bureau of Gas Law Investigation // Incident Report Form GL-102

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Word Wall Workshop

Vocabulary Application & Concept Mapping

Name: ____________________________________

Activity 1: The Triple Threat Match

Use the Word Wall cards to match the Law with its "Constant" (what stays the same) and its "Relationship" type.

Gas Law	The Constant	Mathematical Relationship
Boyle's Law	________________________	________________________
Charles's Law	________________________	________________________
Gay-Lussac's Law	________________________	________________________

Activity 2: Snapshot Scenarios

Read each scenario. Identify the TWO primary Word Wall terms involved and circle the correct relationship.

Scenario A

A mountain climber takes a bag of chips up a summit. As the air pressure decreases, the bag puffs up and looks like it's about to pop.

Term 1: _________________

Term 2: _________________

Direct Inverse

Scenario B

A student leaves a basketball outside on a freezing winter night. In the morning, the ball is flat and has very little bounce.

Term 1: _________________

Term 2: _________________

Direct Inverse

Activity 3: KMT Storytellers

Complete the scientific explanation using at least 4 terms from the Word Wall.

When we used the blowtorch on the rigid metal tank during the lab, the gas particles gained massive amounts of ________________________. This caused them to move at a much higher speed. According to the ________________________________________________, these particles began to have more frequent and more forceful ________________________ with the metal walls. Because the tank was a fixed size, the ________________________ remained constant, but the ________________________ inside the tank skyrocketed!

Activity 4: Visual Remix

Choose ONE term from the Word Wall. Redesign its icon to better show its meaning in a laboratory setting.

Draw Your New Icon Here

Term: ________________________

Explain Your Design:

Why does this image help a student understand the science better than the original Word Wall icon?

Word Wall Activity Guide

CHEM-VOCAB-09

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Gas Law Shuffle

Sorting Activity & Challenge

Name: ____________________________________

Date: _____________________________________

Mission Parameters

Cut out the 18 cards below and on the next page. Scramble them well! Your mission is to organize them into three distinct columns—one for Boyle's, Charles's, and Gay-Lussac's. Once matched, call your instructor for verification before recording the data in your Mastery Log.

Mathematical Model

$\frac{P_1}{T_1} = \frac{P_2}{T_2}$

Law Identity

Boyle's Law

The Constant

Pressure (P)

(n is also constant)

Data Profile

P V

Law Identity

Gay-Lussac's Law

Relationship Type

Direct

As Temperature rises, Volume expands.

The Constant

Temperature (T)

(n is also constant)

Field Application

A balloon shrivels up when placed in a freezer and expands when brought back to room temp.

Mathematical Model

$P_1V_1 = P_2V_2$

Law Identity

Charles's Law

The Constant

Volume (V)

(n is also constant)

Relationship Type

Inverse

As pressure increases, volume decreases.

Field Application

The pressure inside a car tire increases significantly after a long drive on hot asphalt.

Mathematical Model

$\frac{V_1}{T_1} = \frac{V_2}{T_2}$

Data Profile

P T

Data Profile

V T

Relationship Type

Direct

As heat is added, pressure rises in a fixed volume.

Field Application

Using a syringe or bicycle pump; decreasing the space makes the air push back harder.

Mastery Log

Transfer your verified sorting results into the table below.

Law Identity	Formula	Constant	Relationship

The KMT Connection

Choose one of the laws you sorted and explain its relationship using Kinetic Molecular Theory (particles, collisions, and speed).

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Gas Law Gear

Unit Assessment Strategy & Reference

Name: __________________________

Date: ___________

KMT & Particle Logic

1. Temp ($T$) = Average Kinetic Energy. Higher temp = faster particles = more collisions.
2. Pressure ($P$) is caused by collisions with walls. No collisions = No pressure.
3. Rigid Containers: Volume ($V$) is constant. Cans/Tanks can explode if heated!
4. Flexible Containers: Volume ($V$) changes to match external pressure. (Balloons).

Survival Tools

Temp (Must be K)

$K = ^\circ C + 273$

Pressure Units

$1\text{ atm} = 101.3\text{ kPa}$

$760\text{ mmHg} = 760\text{ torr}$

Volume Units

$1000\text{ mL} = 1\text{ L}$

Standard (STP)

$0^\circ C$ and $1\text{ atm}$

The Gas Law Toolbox Changing States?

Boyle's (Inverse)

$P_1V_1 = P_2V_2$

Pressure $\uparrow$ then Volume $\downarrow$

Charles's (Direct)

$\frac{V_1}{T_1} = \frac{V_2}{T_2}$

Temp $\uparrow$ then Volume $\uparrow$

Combined Law

$P_1V_1T_2 = P_2V_2T_1$

Use when $P, V$, and $T$ all change.

Dalton's (Mixtures)

$P_{\text{tot}} = P_1 + P_2 \dots$

Over Water:
$P_{\text{gas}} = P_{\text{tot}} - P_{\text{vap}}$

Ideal Gas Law

PV=nRT

Single State Only

R Values:

$0.0821$ (atm) | $8.314$ (kPa)

*Volume MUST be in LITERS!

Gas Stoichiometry Roadmap

Grams

START (A)

Moles A

$g \to mol$
MM Molar Mass

Moles B

MOLE RATIO
Coefficients

Liters

$mol \to L$
22.4 L (STP)

The Tactical Set-up (Tracks)

Multiply Top | Divide Bottom

Given $g$ (A)

1 mol (A)

Molar Mass $g$

COEFF mol (B)

COEFF mol (A)

22.4 L (B)

1 mol (B)

Target

LITERS (B)

The "Which Law?" Quiz

• Changing $P, V$, or $T$? Use Combined Law.
• Only ONE set of conditions? Use $PV=nRT$.
• Dealing with mixtures? Use Dalton's Law.
• Reaction involved? Use the Stoich Roadmap!

The Grade Killers

1. Forgetting to convert Celsius to Kelvin.
2. Using $mL$ instead of $L$ in the Ideal Gas Law.
3. Not balancing the equation before Stoichiometry.

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Stoich Mission Manual

Tactical Briefing: Gas Stoichiometry Operations

Codename:

Date:

Mission: Solve Gas Reactions

T: STP vs Non-STP

Tools: PV=nRT & 22.4L

The STP Shortcut (Molar Volume)

In chemistry, "Standard Temperature and Pressure" (STP) is defined as 0°C (273.15 K) and 1.00 atm. Under these specific conditions, Avogadro's Law tells us that 1 mole of any gas occupies exactly 22.4 Liters. This is called the Molar Volume.

Tactical Note: This is a massive timesaver! If you see "at STP," you can skip the Ideal Gas Law and just use 22.4 L/mol as a conversion factor in your dimensional analysis.

Stop and Jot

Why is it dangerous to use the "22.4 L/mol" shortcut if the reaction is taking place at 25°C? Explain using the relationship between Temperature and Volume.

The Non-STP Bridge (PV=nRT)

Most real-world reactions don't happen at freezing point (0°C). When conditions are Non-STP, the "22.4 L" shortcut breaks. Instead, we use the Ideal Gas Law ($PV=nRT$) to bridge the gap between the mole-ratios of stoichiometry and the physical volume of the gas.

Scenario A: Start with grams $\rightarrow$ Find Moles $\rightarrow$ Use Stoich for Gas Moles $\rightarrow$ Use $PV=nRT$ to find Volume.
Scenario B: Start with Gas Volume $\rightarrow$ Use $PV=nRT$ to find Moles $\rightarrow$ Use Stoich for other moles $\rightarrow$ Convert to Mass.

Think-Pair-Share

Discuss with a partner: In $PV=nRT$, which variable connects directly to the coefficients in a balanced chemical equation? Why is that variable the "common currency" of chemistry?

Partner Discussion Notes:

The Volume-Volume Shortcut

If all gases in a reaction are at the same temperature and pressure, there is an ultimate shortcut! Because volume is directly proportional to moles (Avogadro), the mole ratios in the equation are the exact same as the volume ratios. If the equation says 2 moles of $H_2$ react with 1 mole of $O_2$, then 2 Liters of $H_2$ react with 1 Liter of $O_2$.

Sentence Stems

"If the Temperature and Pressure are constant for both reactant and product, I can use the _________________________ as a direct conversion factor for _________________________."

"This is simpler than PV=nRT because I don't need to calculate _________________________ first."

Live-Fire Missions

Level 1: Volume Shortcut High Support

Mission: 10.0 L of hydrogen gas ($H_2$) reacts with excess oxygen to produce water vapor at constant temperature and pressure. How many Liters of $O_2$ are consumed?
Equation: $2H_2(g) + O_2(g) \rightarrow 2H_2O(g)$

10.0 L

$H_2$

L $O_2$ L $H_2$

L $O_2$

Level 2: Mole-to-Volume STP Standard Support

Mission: If 3.50 moles of Nitrogen gas ($N_2$) reacts with hydrogen at STP, what volume of Ammonia ($NH_3$) is produced?
Equation: $N_2(g) + 3H_2(g) \rightarrow 2NH_3(g)$

3.50 mol $N_2$

2 mol $NH_3$

22.4 L $NH_3$

1 mol $N_2$

1 mol $NH_3$

Level 3: Mass-to-Volume STP Mission Support

Mission: 12.0 grams of Magnesium reacts with HCl to produce Hydrogen gas at STP. Find the volume of $H_2$ produced.
$Mg(s) + 2HCl(aq) \rightarrow MgCl_2(aq) + H_2(g)$

12.0 g Mg

mol Mg

mol $H_2$

22.4 L $H_2$

MM Mg

Ratio Mg

1 mol $H_2$

Volume:

Level 4: Mass-to-Volume Non-STP Operational Support

Mission: 50.0g of $KClO_3$ decomposes to produce Oxygen gas at 300 K and 1.50 atm. Find the volume of $O_2$.
$2KClO_3(s) \rightarrow 2KCl(s) + 3O_2(g)$ (MM: 122.5 g/mol)

Step 1: Railroad to Moles of $O_2$ (the target gas)

50.0g $KClO_3$

1 mol $KClO_3$

Ratio $O_2$

MM $KClO_3$

Ratio $KClO_3$

Moles $O_2$ (n):

Step 2: Apply Ideal Gas Law to Find Volume

VARIABLES P=_____ n=_____ T=_____

SETUP $V = nRT/P$

FINAL VOLUME:

Level 5: Volume-to-Mass Non-STP Elite Ops

Mission: 750 mL of $H_2$ is collected at 25°C and 740 torr. What mass of Zinc was used?
$Zn(s) + 2HCl(aq) \rightarrow ZnCl_2(aq) + H_2(g)$ (MM Zn: 65.38 g/mol)

Step 1: Get $n$ of $H_2$

P (atm):

V (L):

T (K):

n = ________ mol $H_2$

Step 2: Railroad to Mass of $Zn$

mol $H_2$

Ratio $Zn$

MM $Zn$

Ratio $H_2$

1 mol $Zn$

FINAL MASS (g Zn):

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Stoich Squad

Mission: Gas Stoichiometry Review

Name:

Date:

STP Constant

1 mol = 22.4 L

Shortcut

Vol Ratio = Mol Ratio

Gas Constant

R = 0.0821 atm·L

Volume to Volume

Shortcut: Use coefficients directly if T and P are constant.

1. What volume of fluorine gas is needed to prepare 50.0 mL of chlorine gas?

2KCl(aq) + F2(g) → 2KF(aq) + Cl2(g)

Workspace

Final Answer

_____ mL F₂

2. What volume of NH₃ gas is needed to produce 10.0 liters of N₂ at the same P and T?

2NH3(g) → N2(g) + 3H2(g)

Show Your Ratio Logic

Mass to Volume at STP

Standard Temperature and Pressure: 1 mole = 22.4 L

3. Calculate the volume of chlorine gas at STP required to react with 3.50 g of silver metal.

2Ag(s) + Cl2(g) 2AgCl(s)

Step 1: Grams Ag → Mols Ag

Step 2: Mol Ag → Mol Cl2

Step 3: Mol Cl2 → Liters

Modular Stoich Calculation Space

4. Calculate the mass of iron that must be used to obtain 0.500 L of hydrogen at STP.

3Fe(s) + 4H2O(l) → Fe3O4(s) + 4H2(g)

5. How many liters of oxygen will be produced at STP if 1.25 kg of potassium chlorate decomposes completely?

2KClO3(s) → 2KCl(s) + 3O2(g)

Warning: Convert kg to grams first!

The Ideal Journey

When conditions aren't STP, use $PV = nRT$ to find volume.

6. What volume of H₂ gas is produced at 23.5°C and 779 torr when 0.2281 g of Mg reacts with excess HCl?

Mg(s) + 2HCl(aq) → MgCl2(aq) + H2(g)

Part A: Moles H₂ (Stoich)

Part B: Units Check (Kelvin & Atm)

Temp (K) __________

Press (atm) __________

Final Step: PV = nRT

7. How many grams of CaCO₃ are needed to form 3.45 L of CO₂ at 740 mmHg and 121°C?

CaCO3(s) → CO2(g) + CaO(s)

Hint: Find moles of CO₂ first using the Ideal Gas Law!

8. How many liters of chlorine gas will be needed to make 75.0 grams of C₂H₂Cl₄ at 1.90 atm and 30°C?

2Cl2(g) + C2H2(g) → C2H2Cl4(g)

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Gas Gauntlet

Behavior of Gases Study Guide

Name: __________________________________

Date: ___________________________________

1. Particle Power (KMT & Temperature)

Temperature: Measures average kinetic energy. If Temp ↑, particles move faster and hit walls with more force.

Absolute Zero: 0 Kelvin. Theoretical temperature where all molecular motion stops.

Review Set 1

1. When a cup of coffee cools from 140°F to 120°F, what happens to the molecules? (Select TWO)

Gain kinetic energy

Molecule's motion slows down

Molecules move closer together

Molecules gain thermal energy

2. How does the kinetic energy of gas particles change as the Kelvin temperature is doubled?

3. Explain why scent molecules from a heated air freshener fill a room faster than cold ones.

2. Relationship Logic (The Laws)

Boyle's Law

INVERSE

Pressure up, Volume down.

Charles's Law

DIRECT

Temp up, Volume up.

Gay-Lussac's

DIRECT

Temp up, Pressure up.

Review Set 2

4. A standard balloon pressure decreases. What happens to the helium gas? (Select TWO)

□ Helium expands to a greater volume

□ Moles of helium will remain constant

□ The helium particles will move faster

□ Volume of gas will decrease

5. A rigid cylinder tank is being filled with gas. Why does the pressure increase?

A. Particles move slower

B. More collisions with the container walls

C. Particles get physically larger

6. When liquid nitrogen (77 K) is poured over a room temp balloon (298 K), the balloon shrinks. Which law is this?

3. Dalton's mixtures (Partial Pressure)

Total Pressure: $P_{total} = P_1 + P_2 + P_3...$

Gas over Water: To find the pressure of the "dry" gas, you must subtract the water vapor pressure from the barometric total. $P_{gas} = P_{total} - P_{H_2O}$

Review Set 3

7. Nitrogen is collected over water at 40.0°C. If total pressure is 99.42 kPa and water vapor pressure is 7.38 kPa, find the nitrogen pressure.

Work Space

8. A tank has 3 gases. Gas A = 20 kPa, Gas B = 50 kPa. Total Pressure = 110 kPa. What is Gas C?

9. True/False: Gases in a mixture all have the same average kinetic energy if they are at the same temperature.

True

False

4. Math Mastery (Quantitative)

One Snapshot

$PV = nRT$

The Big Change

$\frac{P_1V_1}{T_1} = \frac{P_2V_2}{T_2}$

Always check units: Kelvin is a must!

Review Set 4

10. 3.61 moles of gas are in a 1500 mL container at 100°C. Find pressure in atm.

Remember: mL → L and °C → K

11. A 40.0 mL gas sample at 7.0°C and 1.50 atm is changed to 3.0°C and 1.75 atm. What is the new volume?

Work Space

12. A bag with 250 mL of air at 101 kPa is moved to an altitude where pressure is 85 kPa. Find the new volume.

5. Reaction Math (Stoichiometry)

STP Shortcuts

1 mol = 22.4 Liters

(Only at 0°C and 1 atm)

Pathfinder

Grams $\rightarrow$ Moles $\rightarrow$ Ratio $\rightarrow$ Volume

Review Set 5

13. Equation: $C_3H_8(g) + 5O_2(g) \rightarrow 3CO_2(g) + 4H_2O(g)$

Which setup finds the volume of $CO_2$ at STP from 22 g of $C_3H_8$? (Molar mass = 44 g/mol)

22g $C_3H_8$ × $\frac{1 \text{ mol } C_3H_8}{44\text{g } C_3H_8}$ × $\frac{3 \text{ mol } CO_2}{1 \text{ mol } C_3H_8}$ × $\frac{22.4 \text{ L } CO_2}{1 \text{ mol } CO_2}$

22g $C_3H_8$ × $\frac{1 \text{ mol } C_3H_8}{44\text{g } C_3H_8}$ × $\frac{22.4 \text{ L } CO_2}{1 \text{ mol } CO_2}$

14. $4NH_3(g) + 5O_2(g) \rightarrow 4NO(g) + 6H_2O(\ell)$

If 128 g $O_2$ reacts at STP, what volume of NO is produced? (MM $O_2$ = 32 g/mol)

Step 1: Grams $\rightarrow$ Moles

Step 2: Mole Ratio

15. What is the volume of 2.0 moles of Neon gas at STP?

___________________ Liters

Mastery Achieved

15 Targeted Review Questions Completed.

Pressure Power Unit

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Answer Key

Formula Finder Worksheet

Teacher Reference Only

Part 1: Video Check

1. Mnemonic Phrase:

"Can These Guys Possibly Be Victorious?"

2. "Possibly" stands for:

Pressure

3. Side-by-side math:

Multiplication ($ P \times V $)

Part 2: Mnemonic Maker

Top Corner: Temperature ($ T $)

Bottom Left: Pressure ($ P $)

Bottom Right: Volume ($ V $)

Left Side (P & T): Gay-Lussac's Law ($ P/T $)

Right Side (V & T): Charles's Law ($ V/T $)

Bottom Side (P & V): Boyle's Law ($ P \times V $)

Part 3: The Scramble Solutions

01. The Balloon Blast (Charles's Law)

$ V_1/T_1 = V_2/T_2 $

$ 2.0 / 298 = V_2 / 350 \implies V_2 = (2.0 \times 350) / 298 \approx \mathbf{2.35\text{ L}} $

02. The Scuba Squeeze (Boyle's Law)

$ P_1 V_1 = P_2 V_2 $

$ 1.0 \times 10 = 3.0 \times V_2 \implies V_2 = 10 / 3.0 \approx \mathbf{3.33\text{ L}} $

03. The Pressure Cooker (Gay-Lussac's Law)

$ P_1/T_1 = P_2/T_2 $; $ T_1 = 293\text{ K}, T_2 = 393\text{ K} $

$ 100 / 293 = P_2 / 393 \implies P_2 = (100 \times 393) / 293 \approx \mathbf{134.13\text{ kPa}} $

04. Tire Troubles (Gay-Lussac's Law)

$ T_1 = 288\text{ K}, T_2 = 318\text{ K} $

$ 32 / 288 = P_2 / 318 \implies P_2 = (32 \times 318) / 288 \approx \mathbf{35.33\text{ psi}} $

05. Piston Push (Boyle's Law)

$ 760 \times 500 = P_2 \times 100 \implies P_2 = 380000 / 100 = \mathbf{3800\text{ mmHg}} $

06. Winter Woes (Charles's Law)

$ T_1 = 298\text{ K}, T_2 = 268\text{ K} $

$ 2.5 / 298 = V_2 / 268 \implies V_2 = (2.5 \times 268) / 298 \approx \mathbf{2.25\text{ L}} $

07. Spray Can Caution (Gay-Lussac's Law)

$ T_1 = 293\text{ K}, T_2 = 873\text{ K} $

$ 3.0 / 293 = P_2 / 873 \implies P_2 = (3.0 \times 873) / 293 \approx \mathbf{8.94\text{ atm}} $. Yes, it explodes!

08. Mountain Meditations (Boyle's Law)

$ 1.0 \times 150 = 0.7 \times V_2 \implies V_2 = 150 / 0.7 \approx \mathbf{214.29\text{ mL}} $

09. Laboratory Leak (Charles's Law)

$ T_1 = 373\text{ K} $

$ 50 / 373 = 25 / T_2 \implies T_2 = (25 \times 373) / 50 = 186.5\text{ K} \implies \mathbf{-86.5^\circ\text{C}} $

10. Deep Sea Discovery (Boyle's Law)

$ 5.0 \times 10 = 1.0 \times V_2 \implies V_2 = \mathbf{50\text{ mL}} $

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STATION SCRAMBLE

Final Review Rotation

Boyle's Squeeze

The Prompt: Imagine you are a gas particle inside a balloon that is being squished.

Task: Roleplay the movement of 3 particles. If the volume is halved, how often do you hit the walls? Write your answer on your station tracker.

Focus: Inverse Relationship

Charles's Stretch

The Prompt: A tire's volume is measured in a garage (25°C). Then it goes outside into the winter snow (-5°C).

Task: Convert both temperatures to Kelvin. Predict the volume change (increase or decrease). Use Charles's Law to justify.

Focus: Kelvin & Direct Relation

Lussac's Blast

The Prompt: Look at the provided pressure gauge photo. As the bunsen burner heats the rigid canister, the needle moves from 100 kPa to 200 kPa.

Task: Draw a "Whoosh" diagram for the particles at both pressures. Explain why the canister doesn't change size.

Focus: Constant Volume

Absolute Quest

The Prompt: Use the graph provided at the station. Trace the line back until the volume hits zero.

Task: What is the X-intercept temperature? Why is this temperature "absolute"? Can we ever go below it?

Focus: 0 K Concepts

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Investigator Key

Official Bureau Use Only // Unit: Gas Law Investigation

Teacher Reference

Case #01

The "Pop" in the Pines (Boyle's Law)

Answers:

Variables: Pressure (P) and Volume (V)
Law: Boyle's Law

Interpretation:

As the investigator drives down the mountain, external atmospheric pressure increases. According to Boyle's Law, pressure and volume are inversely proportional. The high pressure at sea level squeezes the gas inside the bottle into a smaller space (volume decreases), crushing the container.

Particle Map:

MOUNTAIN

Sea Level

Case #02

The Winter Morning "Flat" (Gay-Lussac's Law)

Answers:

Variables: Temperature (T) and Pressure (P)
Logic: Directly Proportional

Microscopic Description:

When temperature drops, particles lose kinetic energy and slow down. They strike the tire walls less frequently and with less force, which results in a measurable drop in pressure even though no air was lost.

Determination

Gay-Lussac's Law

Case #03

The Floating Fiesta Failure (Charles's Law)

Data Log Key

Volume

Small Large

Conclusion Key:

As the balloons were moved from the cold garage to the hot room, the gas particles gained kinetic energy and began moving faster. They hit the inside of the balloon with more force, pushing the elastic outward to maintain constant pressure. The volume increased rapidly (Charles's Law) until the material reached its elastic limit and burst.

Forensic Forecast Key

Incident Scenario	Constant	Pressure	Volume
Heating aerosol can	Volume	INCREASE	NO CHANGE
Pulling UP plunger	Temp	DECREASE	INCREASE
Cylinder in freezer	Volume	DECREASE	NO CHANGE

Critical Evidence Key

The rookie is incorrect. Gas calculations must use the Kelvin scale because pressure and volume are proportional to the *total* kinetic energy of particles, which only starts at absolute zero (0K). 20°C is 293K and 40°C is 313K. While 40 is double 20, 313K is NOT double 293K. Therefore, the pressure will only increase by about 6.8%, not 100%.

Key Verified

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Word Wall Workshop

Teacher Answer Key

Activity 1: The Triple Threat Match Key

Gas Law	The Constant	Mathematical Relationship
Boyle's Law	Temperature (T) / Moles (n)	Inverse
Charles's Law	Pressure (P) / Moles (n)	Direct
Gay-Lussac's Law	Volume (V) / Moles (n)	Direct

Activity 2: Snapshot Scenarios Key

Scenario A (Mountain Climber)

Term 1: Pressure

Term 2: Volume

Inverse

Scenario B (Freezing Basketball)

Term 1: Temperature

Term 2: Volume

Direct

Activity 3: KMT Storytellers Key

When we used the blowtorch on the rigid metal tank during the lab, the gas particles gained massive amounts of Kinetic Energy (Temperature). This caused them to move at a much higher speed. According to the Kinetic Molecular Theory (KMT), these particles began to have more frequent and more forceful Collisions with the metal walls. Because the tank was a fixed size, the Volume remained constant, but the Pressure inside the tank skyrocketed!

Activity 4: Teacher Notes

Look for icons that move away from generic symbols (like just a thermometer) toward situational symbols (like particles hitting a wall with force vectors, or a piston compressing particles). Students should show a clear link between the macroscopic variable and microscopic particle behavior.

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Stoich Mission Manual

Teacher Answer Key & Facilitation Guide

Reference Only

Reading CFU Solutions

01 Stop and Jot: Temperature Hazard

At 25°C, the gas is warmer than STP (0°C). Since volume is directly proportional to temperature (Charles's Law), the gas will occupy more than 22.4 Liters per mole. Using the shortcut would lead to an incorrect, too-small volume.

02 Think-Pair-Share: The Mole Connection

The variable is "n" (moles). It is the "common currency" because the balanced equation's coefficients tell us the ratio of moles reacting/produced, regardless of mass or volume.

03 Sentence Stems: Volume Shortcut

"...use the coefficients / mole ratio as a direct conversion factor for volumes."
"...don't need to calculate moles first."

Mission Solutions (Calculations)

Mission 1: Vol-Vol

5.00 L $O_2$

$10.0 \text{ L } H_2 \times (1 \text{ L } O_2 / 2 \text{ L } H_2)$

Mission 2: Mol-Vol STP

156.8 L $NH_3$

$3.50 \text{ mol } N_2 \times (2 \text{ mol } NH_3 / 1 \text{ mol } N_2) \times 22.4 \text{ L/mol}$

Mission 3: Mass-Vol STP

$12.0 \div 24.31 \times 1/1 \times 22.4 = \mathbf{11.06 \text{ L } H_2}$

Mission 4: Mass-Vol Non-STP

Step 1 (n): $50.0\text{g} \div 122.5 \times 3/2 = \mathbf{0.612 \text{ mol } O_2}$

Step 2 (V): $V = (0.612 \times 0.0821 \times 300) / 1.50 = \mathbf{10.05 \text{ L } O_2}$

Mission 5: Vol-Mass Non-STP (Elite Ops)

Part A: The Gas Moles

P = 0.974 atm (740/760)

V = 0.750 L (750 mL)

T = 298 K (25°C + 273)

$n = PV/RT = 0.0298 \text{ mol } H_2$

Part B: The Reaction

Ratio Zn : $H_2$ is 1 : 1

Moles Zn = 0.0298 mol

Mass = $0.0298 \times 65.38 \text{ g/mol}$

Final Answer: 1.95 g Zn

Teacher Facilitation Tips

Scaffolding Transition: Notice how Mission 5 forces students to perform their own unit conversions (mL to L, torr to atm) before using the gas law.
The Shortcut Lock: Ensure students understand that the "22.4 L" rule is a *shortcut* specifically for STP. They should never use it in Mission 4 or 5.
Coloring Activity: Use the coloring page as a review tool. Students should color the "Bridge" a distinct color to emphasize that mole ratios are the only way to switch chemicals.

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Gas Gauntlet

Teacher Answer Key

Reference Only

Section 1: Particle Power Answers

1. Result of average kinetic energy increasing:

Answers: A & C

A: Particles will have an increase in thermal energy.
C: Particles will move faster, increasing collision rates.

2. Air freshener heating explanation:

"Heating the air freshener provides energy to the scent molecules, increasing their average kinetic energy. This causes the molecules to move faster and collide more frequently with air particles, allowing the scent to diffuse and fill the room more quickly."

Section 2: Qualitative Law Answers

3. Bag of chips on plane:

Answer: Pressure ↓, Volume ↑ (Inflates)

Reason: Boyle's Law states an inverse relationship between P and V.

4. Rigid oxygen tank filling:

Answer: Pressure will increase

Reason: Adding more particles to a fixed volume increases collision rates with the walls.

Section 3: Dalton's Law Answers

5. Nitrogen over water calculation:

P_total = 99.42 kPa | P_water = 7.38 kPa
P_gas = P_total - P_water
P_nitrogen = 99.42 - 7.38 = 92.04 kPa

6. Balloon partial pressure:

P_total = 103 kPa | P_CO2 = 40 kPa
P_N2 = 103 - 40 = 63 kPa

Section 4: Master Equation Answers

7. Bag of nuts (Boyle's Law):

P1 = 101 kPa, V1 = 250 mL, P2 = 85 kPa
P1V1 = P2V2
(101)(250) = (85)(V2)
25250 = 85V2
V2 = 297.06 mL

8. Soda bottle sinking (Combined Law):

P1 = 1.50 atm, V1 = 40.0 mL, T1 = 280 K (7 + 273)
P2 = 1.75 atm, V2 = ?, T2 = 276 K (3 + 273)
(P1V1)/T1 = (P2V2)/T2
(1.50 × 40.0) / 280 = (1.75 × V2) / 276
60 / 280 = 1.75V2 / 276
0.214 = 1.75V2 / 276
59.14 = 1.75V2
V2 = 33.80 mL

Section 5: Gas Stoichiometry Answers

9. Setup for Propane combustion:

Answer: Setup A

Reason: Setup A includes the molar mass conversion, the 3:1 mole ratio from the balanced equation, and the 22.4 L/mol molar volume at STP.

10. Ammonia/Oxygen Volume Calculation:

Step 1 (Grams to Moles O2):
128 g O2 / 32 g/mol = 4.0 moles O2

Step 2 (Mole Ratio):
4.0 mol O2 × (4 mol NO / 5 mol O2) = 3.2 moles NO

Step 3 (Molar Volume at STP):
3.2 mol NO × 22.4 L/mol = 71.68 L (Choice B in original assessment)

c3:T183c,

Gas Law Shuffle

Teacher Answer Key

Reference Only

Correct Sorting Matrix

Category	Boyle's Law	Charles's Law	Gay-Lussac's Law
Formula	$P_1V_1 = P_2V_2$	$\frac{V_1}{T_1} = \frac{V_2}{T_2}$	$\frac{P_1}{T_1} = \frac{P_2}{T_2}$
Constant	Temperature (T)	Pressure (P)	Volume (V)
Relationship	Inverse	Direct	Direct
Graph Type	Hyperbola (Curved down)	Linear (Upward slope)	Linear (Upward slope)
Scenario	Syringe / Bicycle Pump	Balloon in Freezer	Tire Pressure on Hot Road

KMT Explanation Exemplars

Boyle's Law (P & V)

When volume decreases, gas particles have less space to move around. This causes them to collide with the walls of the container more frequently. Since pressure is defined by the frequency and force of these collisions, the pressure increases.

Charles's Law (V & T)

As temperature increases, gas particles gain kinetic energy and move faster. To keep the pressure constant (meaning the same collision force against the outside atmosphere), the particles must spread out, which increases the total volume of the container.

Gay-Lussac's Law (P & T)

Increasing temperature makes particles move faster and hit the walls with more force and frequency. Because the volume is fixed (it can't expand), these faster and more frequent collisions result in a measurable increase in pressure.

c4:T3e6e,

Gas Law Gear

Unit Assessment Strategy & Reference

Name: __________________________

Date: ___________

KMT & Particle Logic

1. Temp ($T$) = Average Kinetic Energy. Higher temp = faster particles = more collisions.
2. Pressure ($P$) is caused by collisions with walls. No collisions = No pressure.
3. Rigid Containers: Volume ($V$) is constant. Cans/Tanks can explode if heated!
4. Flexible Containers: Volume ($V$) changes to match external pressure. (Balloons).

Survival Tools

Temp (Must be K)

$K = ^\circ C + 273$

Pressure Units

$1\text{ atm} = 101.3\text{ kPa}$

$760\text{ mmHg} = 760\text{ torr}$

Volume Units

$1000\text{ mL} = 1\text{ L}$

Standard (STP)

$0^\circ C$ and $1\text{ atm}$

The Gas Law Toolbox Mathematical Modeling

Boyle's (Inverse)

$P_1V_1 = P_2V_2$

If Pressure $\downarrow$, Volume $\uparrow$. (Balloons expanding in altitude).

Charles's (Direct)

$\frac{V_1}{T_1} = \frac{V_2}{T_2}$

If Temp $\downarrow$, Volume $\downarrow$. (Liquid Nitrogen cooling a balloon).

Combined Gas Law

$P_1V_1T_2 = P_2V_2T_1$

Use when $P, V$, and $T$ all change. (Soda bottles sinking in water).

Dalton's (Mixtures)

$P_{\text{total}} = \sum P_{\text{parts}}$

Over Water:
$P_{\text{gas}} = P_{\text{total}} - P_{\text{vapor}}$

Ideal Gas Law

PV=nRT

Single State Only

R Constants (Match the units!):

$0.0821$ (atm) | $8.314$ (kPa)

Volume MUST be in LITERS!

Stoichiometry Mission Roadmap

Grams

START (A)

Divide by MM

Moles A

BRIDGE

Mole Ratio

Moles B

COEFFICIENTS

Multiply 22.4

Liters

TARGET (B)

The Mission Set-Up (Railroad Tracks)

Multiply across Top | Divide by Bottom

GIVEN g (A)

1 (Place Holder)

1 mol (A)

Molar Mass $g$

COEFF mol (B)

COEFF mol (A)

22.4 L (B)

1 mol (B)

$=$

Solution

Liters (B)

The Identification Phase

• Combined Law? Look for keywords like "initial", "final", "change", or "dropped into depth".
• Ideal Law? Look for moles ($n$) and only one set of conditions.
• Stoichiometry? Look for two different substances in a reaction.

Critical Failures

1. THE KELVIN TRAP: If you see $^\circ C$, add 273 IMMEDIATELY. Math doesn't work in Celsius.
2. THE UNIT MISMATCH: Ensure $R$ and Pressure share units (both atm or both kPa).

c5:T3cd1,

Stoich Squad: Mission Scaffold

Tactical Guide to Gas Reactions

OPERATIVE: ___________________________

DATE: ___________________________

Mole Ratio Shortcut

A → B

If P & T are constant: Volume Ratio = Coefficient Ratio

The STP Vault

STP

Standard Temp (0°C) & Press (1 atm): 1 mol = 22.4 L

Volume-to-Volume Shortcut

1. What volume of fluorine gas is needed to prepare 50.0 mL of chlorine gas?

2KCl + 1F₂ → 2KF + 1Cl₂

Start With

50.0 mL Cl₂

Ratio From Equation

____ mol F₂

____ mol Cl₂

Target Result

_________ mL F₂

2. How many liters of water vapor can be formed if 1.25 liters of ethylene (C₂H₄) are consumed?

C₂H_4(g) + 3O_2(g) → 2CO_2(g) + 2H₂O_(g)

1.25 L C₂H₄

____ L H₂O

____ L C₂H₄

_________ L H₂O

Mass to Volume at STP

3. Calculate the volume of chlorine gas at STP required to react with 3.50g of silver metal.

2Ag_(s) + 1Cl_2(g) → 2AgCl_(s)

Given

3.50 g Ag

Molar Mass Ag

1 mol Ag

_______ g Ag

Mole Ratio

____ mol Cl₂

____ mol Ag

STP Vol

22.4 L Cl₂

1 mol Cl₂

Solve: (3.50 × 1 × ___ × 22.4) / (___ × ___) = ___________ L Cl₂

4. Calculate the mass of iron needed to obtain 0.500 L of hydrogen at STP.

3Fe + 4H₂O → Fe₃O₄ + 4H₂

0.500 L H₂

1 mol H₂

22.4 L H₂

____ mol Fe

____ mol H₂

____ g Fe

1 mol Fe

The Ideal Gauntlet (Non-STP)

6. What volume of H₂ is produced at 23.5°C and 779 torr when 0.2281 g of Mg reacts with excess HCl?

Phase 1: Get Stoich Moles ($n$)

0.2281 g Mg

1 mol Mg

24.31 g Mg

1 mol H₂

1 mol Mg

$n = $ __________ mol H₂

Phase 2: Variable Unit Check

Pressure ($P$) 779 / 760 = _____ atm

Temperature ($T$) 23.5 + 273 = _____ K

Constant ($R$) 0.0821 L·atm/mol·K

Phase 3: Solve for $V$

$V = \frac{nRT}{P}$

________ Liters

7. How many grams of CaCO₃ are needed to form 3.45 L of CO₂ at 740 mmHg and 121°C?

Step 1: Ideal Gas ($n$)

P = 740 / 760 T = 121 + 273

Show math for n = PV / RT

$n = $ __________ mol CO₂

Step 2: Stoich (Grams)

Convert mol CO₂ → mol CaCO₃ → grams CaCO₃

__________ g CaCO₃

9. How many liters of Cl₂ will be needed to make 75.0 grams of C₂H₂Cl₄ at 1.90 atm and 30°C?

Balanced: 2Cl₂ + C₂H₂ → C₂H₂Cl₄

1. Stoich for $n$ 2. Ideal for $V$

c6:T2b36,

Pressure Power Quiz

Certification Exam: Gas Phase Mechanics

Name:

Date:

I. Phase Foundations

1. According to Kinetic Molecular Theory (KMT), what causes the pressure exerted by a gas inside a container?

The attraction between gas particles and the walls.

Collisions of gas particles with the container walls.

The total volume occupied by the particles themselves.

The gravitational pull on the gas particles.

2. Which gas law describes a relationship that is inversely proportional?

Charles's Law (V & T)

Gay-Lussac's Law (P & T)

Boyle's Law (P & V)

Avogadro's Law (V & n)

II. Particle Visualization

3. A sealed, flexible balloon contains 10 gas particles at room temperature. The balloon is then placed into a freezer. Sketch the "Before" and "After" states, ensuring your model reflects KMT principles.

Before (Room Temp)

After (Freezer)

Annotation: Explain one way your "After" drawing demonstrates a change in kinetic energy.

"A sample of neon gas at 25°C is heated to 50°C. The volume will exactly double."

4. Is this statement correct? Why or why not? (Include reference to the absolute temperature scale).

III. Computational Analysis

Investigator Equation Archive

Boyle's

$ P_1V_1 = P_2V_2 $

Charles's

$ \frac{V_1}{T_1} = \frac{V_2}{T_2} $

Gay-Lussac

$ \frac{P_1}{T_1} = \frac{P_2}{T_2} $

Combined

$ \frac{P_1V_1}{T_1} = \frac{P_2V_2}{T_2} $

Kelvin Conversion: $ K = ^\circ C + 273 $

Show all work, identify variables, and include units for full credit.

5. A gas occupies 4.5 L at a pressure of 1.2 atm. If the volume is compressed to 1.5 L while temperature remains constant, what will be the new pressure?

[5 points]

Known Variables

6. A rigid steel cylinder contains a gas at 300 K and 5.0 atm of pressure. If the cylinder is heated until the pressure reaches 12.0 atm, what is the new temperature in Kelvin?

[5 points]

Known Variables

7. THE CHALLENGE: A weather balloon has a volume of 105 L at 27°C and 1.00 atm. It rises to an altitude where the temperature is -13°C and the pressure is 0.40 atm. What is the new volume of the balloon?

[10 points]

Final Check: Did you convert all temperatures to Kelvin? Did your final answers include units? Re-check Case #7 for temperature signs.

c7:T13e9,

Gas Gauntlet

Teacher Answer Key (14-Point Version)

Reference Only

Section 1: Particle Power

1. Liquid Nitrogen Balloon: Particles lose kinetic energy & Collide less frequently.

2. Triple KE: Pressure would triple (if volume is constant). Triple KE means triple the collision force and frequency against the walls.

Section 2: Relationship Logic

3. Oxygen Tank Filling: B. As moles increase, pressure increases.

4. Warm to Cold: Volume decreases (Charles's Law - Direct relationship between T and V).

5. Particle Models: High Pressure should show many more particles (density) or more/longer motion vectors (speed) than Low Pressure.

Section 3: Dalton's Law

6. PN2 Calculation: P_total (1.0) - P_O2 (0.2) - P_CO2 (0.1) = 0.7 atm.

7. Why subtract vapor pressure? Because water molecules evaporate into the collection container, adding their own pressure to the gas being measured.

8. Dry Nitrogen: 100.0 kPa - 7.38 kPa = 92.62 kPa.

Section 4: Math Power

9. Ideal Gas Law (PV=nRT):

P(5.0) = (0.5)(0.0821)(300)
5P = 12.315
P = 2.46 atm

10. Combined Law (Soda Bottle):

(1.50 × 40.0) / 280 = (1.75 × V2) / 276
60 / 280 = 1.75V2 / 276
V2 = 33.80 mL

11. Boyle's Law (Constant T):

P1V1 = P2V2
(1.0)(1.5) = (P2)(3.0)
1.5 = 3P2
P2 = 0.5 atm

Section 5: Stoichiometry

12. H2O Setup at STP:

Answer: Setup [A] (Grams O2 $\rightarrow$ Moles O2 $\rightarrow$ Moles H2O $\rightarrow$ Liters H2O)

13. Mass of 11.2 L N2 at STP:

11.2 L / 22.4 L/mol = 0.5 mol
0.5 mol × 28 g/mol = 14.0 g

14. Volume of 4.0 moles CO2 at STP:

4.0 mol × 22.4 L/mol = 89.6 L

c8:T4028,

Stoich Squad

Ultimate Mission Scaffold: Gas Reactions

Operative Status

NAME: __________________________

STP Constant

1 mol = 22.4 L

Pressure

1 atm = 760 mmHg

Temperature

K = °C + 273

Gas Constant

R = 0.0821

The Volume Shortcut

Valid only when Temp and Pressure are CONSTANT

1. What volume of fluorine gas (F₂) is needed to prepare 50.0 mL of chlorine gas (Cl₂)?

2 KCl

1 F₂

2 KF

1 Cl₂

GIVEN

50.0 mL

Cl₂

RATIO

_____ mol F₂

_____ mol Cl₂

SOLVE

_______ mL

F₂

2. How many liters of NH₃ gas are needed to produce 10.0 liters of N₂ at the same P and T?

2 NH_3(g) → 1 N_2(g) + 3 H_2(g)

10.0 L N₂

____ mol NH₃

____ mol N₂

_________ L NH₃

The STP Highway

Path: Grams → Moles → Moles → Liters (or vice-versa)

3. Calculate the volume of chlorine gas (Cl₂) at STP required to react with 3.50 g of silver metal.

Molar Mass Ag 107.87 g/mol

2 Ag + 1 Cl₂ → 2 AgCl

3.50 g Ag

1 mol Ag

______ g Ag

____ mol Cl₂

____ mol Ag

22.4 L Cl₂

1 mol Cl₂

= ___________ L Cl₂

4. Calculate the mass of iron (Fe) that must be used to obtain 0.500 L of hydrogen at STP.

3 Fe + 4 H₂O → 1 Fe₃O₄ + 4 H₂

0.500 L H₂

1 mol H₂

22.4 L H₂

____ mol Fe

____ mol H₂

____ g Fe

1 mol Fe

5. Calculate the mass of hydrogen peroxide (H₂O₂) needed to obtain 0.460 L of oxygen gas at STP.

2 H₂O_2(aq) → 2 H₂O_(l) + 1 O_2(g)

Build your own Railroad Tracks here!

The Ideal Gauntlet

The Multi-Phase Mission: $PV = nRT$

6. What volume of H₂ is produced at 23.5°C and 779 torr when 0.2281 g of Mg reacts with excess HCl?

Phase 1: Stoich Moles ($n$)

Mg + 2HCl → MgCl₂ + 1H₂

0.2281 g Mg → mol Mg → mol H₂

$n$ = ____________ mol H₂

Phase 2: Calibration

P (atm) 779 / 760 = _____

T (Kelvin) 23.5 + 273 = _____

Phase 3: Ideal Solve

Rearrange to $V = nRT / P$

Output

_________ Liters

7. How many grams of CaCO₃ are needed to form 3.45 L of CO₂ at 740 mmHg and 121°C?

1 Phase A: Find $n$ (Ideal Gas)

P = 740/760 = _____ atm

T = 121+273 = _____ K

$n$ = ___________ mol CO₂

2 Phase B: Stoich to Grams

mol CO₂ → mol CaCO₃ → grams

___________ grams

c9:T191d,

Stoich Mission Map

The Visual Protocol for Gas Stoichiometry

The Intel

Scan the environment: Is it STP or Non-STP?

STP = 22.4L NON = PV=nRT

Mobilize

Convert whatever you have (grams or Liters) into MOLES.

Mass / Molar Mass

V / 22.4 (if STP)

The Mole Bridge

Use the Coefficients!

This is the ONLY way to cross from Molecule A to Molecule B.

Final Form

Convert your new moles (B) back into Mass or Volume.

x Molar Mass

PV=nRT or 22.4L

Color Code Key

Reactant Data

Product Goal

STP Constants

Follow the path. Color the intel, bridge, and final form. Master the stoichiometry mission.

ca:T2475,

Quiz Answer Key

Teacher Reference // Unit: Pressure Power

Master Copy

I. Phase Foundations Key

1. Pressure cause:

Collisions of gas particles with the container walls.

2. Inversely proportional law:

Boyle's Law (P & V)

II. Visualization Key

Before: Large Volume / High Velocity

After: Small Volume / Low Velocity

Key Evidence: Particles in the "After" state should be moving slower (shorter or no velocity vectors) and be closer together because lower temperature means lower kinetic energy and smaller volume (Charles's Law).

4. Statement Justification:

Incorrect. Volume is directly proportional to absolute temperature (Kelvin), not Celsius. 25°C is 298 K and 50°C is 323 K. Since 323 is not double 298, the volume will not double. A true doubling of temperature would require heating the gas to 596 K (323°C).

III. Computational Key

5. Boyle's Law Problem

Variables

P1 = 1.2 atm

V1 = 4.5 L

V2 = 1.5 L

P2 = ?

P1V1 = P2V2
(1.2 atm)(4.5 L) = P2 (1.5 L)
5.4 = P2 (1.5)
P2 = 5.4 / 1.5
P2 = 3.6 atm

6. Gay-Lussac's Law Problem

Variables

T1 = 300 K

P1 = 5.0 atm

P2 = 12.0 atm

T2 = ?

P1 / T1 = P2 / T2
5.0 atm / 300 K = 12.0 atm / T2
5.0 (T2) = 12.0 (300)
5.0 (T2) = 3600
T2 = 3600 / 5.0
T2 = 720 K

7. Combined Gas Law Challenge

Variables

P1 = 1.0 atm

V1 = 105 L

T1 = 300 K (27+273)

P2 = 0.40 atm

T2 = 260 K (-13+273)

V2 = ?

(P1V1)/T1 = (P2V2)/T2
(1.0 atm * 105 L) / 300 K = (0.40 atm * V2) / 260 K
0.35 = (0.40 * V2) / 260
0.35 * 260 = 0.40 * V2
91 = 0.40 * V2
V2 = 91 / 0.40
V2 = 227.5 L

cb:T6368,

Stoich Squad

Ultimate Mission Scaffold: Gas Reactions

Operative Status

NAME: __________________________

STP Volume

1 mol = 22.4 L

Pressure Conversion

1 atm = 760 torr

Temperature Unit

K = °C + 273

Gas Constant

R = 0.0821

Mission Alpha: The Volume Shortcut

If P and T are constant, Volume Ratios = Mole Ratios

1. What volume of fluorine gas is needed to prepare 50.0 mL of chlorine gas at the same conditions of T and P?

2 KCl + 1 F₂ → 2 KF + 1 Cl₂

50.0 mL

GIVEN

_____ mol F₂

_____ mol Cl₂

_______

mL F₂

2. How many liters of water vapor (H₂O) can be formed if 1.25 liters of ethylene (C₂H₄) are consumed?

1 C₂H₄ + 3 O₂ → 2 CO₂ + 2 H₂O

1.25 L

C₂H₄

_____ mol H₂O

_____ mol C₂H₄

_______

L H₂O

3. What volume of NH₃ gas is needed to produce 10.0 liters of N₂ at the same P and T?

2 NH₃ → 1 N₂ + 3 H₂

10.0 L

N₂

_____ mol NH₃

_____ mol N₂

_______

L NH₃

Mission Beta: The STP Highway

At STP (0°C, 1 atm), go through moles: 1 mol = 22.4 L

4. Calculate the volume of chlorine gas (Cl₂) at STP required to react with 3.50 g of silver metal (Ag).

Silver MM 107.87 g/mol

2 Ag + 1 Cl₂ → 2 AgCl

START

3.50 g Ag

MASS → MOL

1 mol Ag

______ g Ag

RATIO

____ mol Cl₂

____ mol Ag

MOL → VOL

22.4 L Cl₂

1 mol Cl₂

= ___________ L Cl₂

5. Calculate the mass of iron (Fe) that must be used to obtain 0.500 L of hydrogen (H₂) at STP.

3 Fe + 4 H₂O → 1 Fe₃O₄ + 4 H₂

0.500 L H₂

1 mol H₂

22.4 L H₂

____ mol Fe

____ mol H₂

____ g Fe

1 mol Fe

Fe Molar Mass: 55.85 g/mol

6. How many grams of H₂O₂ are needed to obtain 0.460 L of O₂ at STP?

2 H₂O₂ → 2 H₂O + 1 O₂

0.460 L O₂

1 mol O₂

22.4 L O₂

____ mol H₂O₂

____ mol O₂

____ g H₂O₂

1 mol H₂O₂

Mission Gamma: The Ideal Gauntlet

Multi-Phase Ops: Use $PV = nRT$ for non-STP conditions

7. What volume of H₂ is produced at 23.5°C and 779 torr when 0.2281 g of Mg reacts with excess HCl?

Mg + 2 HCl → MgCl₂ + 1 H₂

Mg MM

24.31 g/mol

Phase 1: Finding Moles ($n$)

0.2281 g Mg × (1/24.31) × (1/1)

$n = $ ____________ mol H₂

Phase 2: Calibration

P (atm) 779 / 760 = _____

T (Kelvin) 23.5 + 273 = _____

Phase 3: The Ideal Solve

Solve: $V = \frac{nRT}{P}$

($n$ from P1) × (0.0821) × ($T$ from P2)

($P$ from P2)

= _________ Liters

8. How many grams of CaCO₃ are needed to form 3.45 L of CO₂ at 740 mmHg and 121°C?

CaCO₃ → 1 CO₂ + CaO

CaCO₃ MM

100.09 g/mol

A Phase A: Find $n$ (Ideal Gas)

$n = \frac{PV}{RT}$

INPUTS:

P = 740/760 = _____ atm

V = 3.45 L

T = 121+273 = _____ K

$n$ = ___________ mol CO₂

B Phase B: Stoich to Grams

Moles CO₂ → Moles CaCO₃ → Grams

($n$ from Part A) × (1/1) × (100.09)

= ___________ g

Expert Level Extraction

Combine all skills: stoichiometry and non-STP calculation

Mission 09

9. How many liters of Cl₂ are needed to make 75.0 grams of C₂H₂Cl₄ at 1.90 atm and 30°C?

Mole Ratio

2 Cl₂ : 1 C₂H₂Cl₄

Molar Mass

C₂H₂Cl₄ = 167.84 g/mol

Conditions

1.90 atm | 303 K

PHASE 1: Find moles of Cl₂ (Stoich)

75.0 g → Mols → Mole Ratio → mol Cl₂

$n$ = __________ mol Cl₂

PHASE 2: Find Volume of Cl₂ (Ideal)

Use $V = nRT / P$ with mol from Phase 1

LITERS = __________ L

Stoich Squad Command Mission Successful? [ ] YES [ ] NO

cc:T13a1,

Gas Gauntlet

Teacher Answer Key (15-Point Mastery Version)

Reference Only

Section 1: Particle Power

1. Coffee Cooling: Molecule's motion slows down & Molecules move closer together.

2. Doubled Temp: Kinetic energy doubles (KE is directly proportional to Kelvin temperature).

3. Heated Scent: Higher temp means higher average kinetic energy; molecules move faster and diffuse across the room more quickly.

Section 2: Relationship Logic

4. Balloon Pressure Decrease: Helium expands to a greater volume & Moles of helium will remain constant.

5. Tank Filling: B. More collisions with the container walls.

6. Liquid Nitrogen Balloon: Charles's Law (Volume and Temperature are directly proportional).

Section 3: Dalton's Law

7. Nitrogen pressure: 99.42 kPa - 7.38 kPa = 92.04 kPa.

8. Gas C: 110 kPa - (20 + 50) = 40 kPa.

9. True/False: True (Temperature is the measure of average kinetic energy).

Section 4: Math Power

10. Methane snapshot (PV=nRT):

n = 3.61, V = 1.5 L, T = 373 K
P(1.5) = (3.61)(0.0821)(373)
1.5P = 110.53
P = 73.7 atm

11. Combined Law (Soda Bottle):

(1.50 × 40.0) / 280 = (1.75 × V2) / 276
V2 = 33.80 mL

12. Bag of nuts (Boyle's):

(101)(250) = (85)(V2)
V2 = 297 mL

Section 5: Stoichiometry

13. Propane combustion setup:

Answer: Setup A

14. Ammonia volume calculation:

128 g O2 / 32 = 4 mol O2
4 mol O2 × (4 mol NO / 5 mol O2) = 3.2 mol NO
3.2 mol × 22.4 L/mol = 71.7 L

15. Neon at STP:

2.0 moles × 22.4 L/mol = 44.8 L

cd:T3052,

Stoich Squad

Teacher Answer Key: Gas Reactions

Resource Type

TEACHER REFERENCE ONLY

The Volume Shortcut Solutions

1. Volume of fluorine for 50.0 mL chlorine?

50.0 mL Cl₂

1 mol F₂

1 mol Cl₂

50.0 mL F₂

2. Liters of water from 1.25 L ethylene?

1.25 L C₂H₄

2 mol H₂O

1 mol C₂H₄

2.50 L H₂O

3. Volume of NH₃ for 10.0 L N₂?

10.0 L N₂

2 mol NH₃

1 mol N₂

20.0 L NH₃

The STP Highway Solutions

4. Volume of Cl₂ from 3.50 g Ag at STP?

3.50 g Ag

1 mol Ag

107.87 g Ag

1 mol Cl₂

2 mol Ag

22.4 L Cl₂

1 mol Cl₂

Answer: 0.363 L Cl₂

5. Mass of iron for 0.500 L H₂ at STP?

0.500 L H₂

1 mol H₂

22.4 L H₂

3 mol Fe

4 mol H₂

55.85 g Fe

1 mol Fe

Answer: 0.935 g Fe

6. Mass of H₂O₂ for 0.460 L O₂ at STP?

0.460 L O₂

1 mol O₂

22.4 L O₂

2 mol H₂O₂

1 mol O₂

34.02 g H₂O₂

1 mol H₂O₂

Answer: 1.40 g H₂O₂

The Ideal Gauntlet Solutions

7. Volume of H₂ at 23.5°C, 779 torr from 0.2281 g Mg?

Phase 1 (n): 0.2281 / 24.31 × 1 = 0.00938 mol H₂

Phase 2 (P/T): P = 1.025 atm | T = 296.5 K

Calculation: $V = \frac{(0.00938)(0.0821)(296.5)}{1.025}$

Answer: 0.223 Liters H₂

8. Grams CaCO₃ for 3.45 L CO₂ at 740 mmHg, 121°C?

Phase A (n): $n = \frac{(0.974)(3.45)}{(0.0821)(394)}$ = 0.104 mol CO₂

Calculation: $0.104 \text{ mol CO}_2 \times \frac{1 \text{ mol CaCO}_3}{1 \text{ mol CO}_2} \times 100.09 \text{ g}$

Answer: 10.4 grams CaCO₃

9. Volume Cl₂ for 75.0 g C₂H₂Cl₄ at 1.90 atm, 30°C?

Phase 1: Stoich Moles

75.0 / 167.84 × 2 =
0.894 mol Cl₂

Phase 2: Ideal Solve

$V = \frac{(0.894)(0.0821)(303)}{1.90}$ =
11.7 Liters

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Includes 5 real-world word problems and a reflection section for identification strategies.","format":"document","id":"38d5db5c-40aa-4b7e-9fac-b9e6ee4907d1","name":"Law Lab Classifier Worksheet","selectedLocaleCode":null,"sourceLocaleCode":"en_US","sensitive":false},{"description":"A teacher answer key for the Law Lab Classifier Worksheet, including identification of constant variables, law classification, and step-by-step mathematical solutions for all 5 problems.","format":"document","id":"03806736-e6cc-4684-b12f-742289b5b43a","name":"Law Lab Classifier Answer Key Reference Only","selectedLocaleCode":null,"sourceLocaleCode":"en_US","sensitive":false}]},{"description":"Students develop, share, and evaluate visual models of the Combined Gas Law using a peer review rubric based on Kinetic Molecular Theory.","id":"29c2d1d8-c247-41f6-8723-4d2ca4ee3b1d","name":"Model Mastery","materials":[{"description":"A comprehensive peer review rubric for evaluating student models of the Combined Gas Law. 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Category	Boyle's Law	Charles's Law	Gay-Lussac's Law
Formula	\(P_1V_1 = P_2V_2\)	\(\frac{V_1}{T_1} = \frac{V_2}{T_2}\)	\(\frac{P_1}{T_1} = \frac{P_2}{T_2}\)
Constant	Temperature (T)	Pressure (P)	Volume (V)
Relationship	Inverse	Direct	Direct
Graph Type	Hyperbola (Curved down)	Linear (Upward slope)	Linear (Upward slope)
Scenario	Syringe / Bicycle Pump	Balloon in Freezer	Tire Pressure on Hot Road

Pressure Power

Partial Pressure Monitoring Checklist

Pressure Poster Workshop Handout

Pressure Parade Chunked Reading Passage

Law Legend Card Sort Cards

Partial Pressure Monitoring Checklist

Partial Pressure Station Cards

Partial Pressure Parade Slides

Bubble Bound Lab Handout

Partial Pressure Parade Slides

Partial Pressure Answer Key Reference Only

Partial Pressure Station Cards

Pressure Parade Chunked Reading Passage

Station Parade Handout

Station Parade Handout

Partial Pressure Parade Lesson Plan

Partial Pressure Station One Card

Gas Lab Explorer Worksheet Reference

Pressure Power Word Wall Handout Reference

Marshmallow Mission Handout

Gas Law Slides Plus Vocab Expansion

Boyle's Battle Practice Worksheet

Marshmallow Mission Answer Key Reference Only

Boyle's Battle Practice Worksheet

Boyles Battle Answer Key Reference Only

Partial Pressure Parade: Active Stations

Particle Artist

SCUBA Rescue

Fraction Duel

Vapor Hunter

Card Sort Race

Final Checklist

Partial Pressure Parade: Active Stations

Particle Artist

SCUBA Rescue

Fraction Duel

Vapor Hunter

Card Sort Race

Final Checklist

Wall Collisions

Kinetic Energy

Your Turn: Model It!

Checklist

VOCAB SPEED SHOWDOWN

VOCAB SPEED SHOWDOWN

Answer Bank

The "Ideal" Escape

The Golden Rule of Gas Math

Identity Verification Check

Critical Evidence Challenge

The "Which Law?" Quiz

The Grade Killers

Live-Fire Missions

4. Math Mastery (Quantitative)

5. Reaction Math (Stoichiometry)

The Identification Phase

Critical Failures

Phase 3: Solve for \(V\)

Mission Gamma: The Ideal Gauntlet

Expert Level Extraction

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