Partial Pressure Monitoring Checklist 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 Done 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
4
Station Rotation (30-50m)
Station Key Mastery "Look-Fors" Intervention Question Check 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
Pressure Poster Workshop Handout 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
Pressure Parade Chunked Reading Passage 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 PArgon = 1.2 atm and PHelium = 0.8 atm. Total Pressure = 3.0 atm. Find PNeon.
Scenario 2
Why must you convert vapor pressure units to match the total pressure units?
Law Legend Card Sort Cards 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
Partial Pressure Monitoring Checklist 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 Done 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:
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:
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?"
Partial Pressure Station Cards Partial Pressure Station Pack
Based on POGIL Models 1-4
1
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 \(R = 0.0821 \frac{L \cdot atm}{mol \cdot K}\).
2
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.
3
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!
4
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?
Partial Pressure Parade Slides 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.
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
A
Partial Pressure
B
Mole Fraction
C
Vapor Pressure
Ratio of moles of one gas to the total moles.
Pressure of a single gas in a mixture.
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:
\[ P_{gas} = P_{atm} - P_{H_2O} \]
Bubble Bound Lab Handout 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
\(CO_2\)
\(H_2O\)
Pressure Power Unit • Partial Pressure Parade Lab Guide
Partial Pressure Parade Slides 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.
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
A
Partial Pressure
B
Mole Fraction
C
Vapor Pressure
Ratio of moles of one gas to the total moles.
Pressure of a single gas in a mixture.
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:
\[ P_{gas} = P_{atm} - P_{H_2O} \]
Partial Pressure Answer Key Reference Only 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 Addition05: "Dry Pressure" Oxygen08: SCUBA "Trimix" Blend11: 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."
Instructional Note
Ensure students convert mmHg to atm before subtracting from \(P_{total}\)!
v1.0 • PRESSURE-POWER-UNIT
Partial Pressure Station Cards 1
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 :
Total Pressure (atm)
2
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)
3
The Water Trap
Vapor Pressure Corrections
When collecting gas over water, some water evaporates and mixes with it. Subtract the water vapor pressure (PH₂O) to find the pressure of the pure gas.
Vapor Pressure Reference
<table class="w-full text-base font-mono"><tbody><tr class="border-b border-emerald-800"><td class="py-3">22.0 °C</td><td>19.8 mmHg</td></tr><tr class="border-b border-emerald-800 bg-emerald-800/40 font-black text-emerald-100"><td class="py-3">24.0 °C</td><td>22.4 mmHg</td></tr><tr class="border-b border-emerald-800"><td class="py-3">26.0 °C</td><td>25.2 mmHg</td></tr></tbody></table>
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)
4
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
Pgas = (\(\chi\)gas) × Ptotal
1. Find Mole Fraction (\(\chi\)) for 0.30 moles in 1.50 total moles:
Pressure Parade Chunked Reading Passage Pressure Parade
Chunked Reading Passage
Name: ____________________________________
Date: _____________________________________
CHUNK 1
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
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
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?"
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
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.
\[ P_{total} = P_{dry\ gas} + P_{water\ vapor} \]
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?
Station Parade Handout Station Parade Report
Partial Pressure Parade • Scaffolded Student Rotation Guide
Name:
Date:
1
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
2
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%
3
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
4
Fraction & Partiality
A. Mole Fraction Formula:
Xi =
moles of species
total moles
B. Verify Krypton Pressure:
Method: Ratio
PKr = (Xi) \(\times\) (Ptotal)
Method: Sum
PKr = 2.80 \(-\) (Sum of Others)
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
Station Parade Handout Station Parade Report
Partial Pressure Parade • Student Rotation Evidence
Name:
Date:
1
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!
2
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
3
The Water Trap
Conversion Sandbox
22.4 \(\div\) 760 = atm
Finding Pure Dry Gas Pressure
1.02 atm \(-\) =
atm
4
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
Partial Pressure Parade Lesson Plan 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.
Partial Pressure Station One Card 1
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.
Ptotal = 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?
Total Mixture Pressure (atm)
Pressure Parade • 2026
Laboratory Mastery Card
Gas Lab Explorer Worksheet Reference GAS LAB EXPLORER
Relationships Between Gas Variables
Name: ____________________________________
Date: _________________ Block: _________
Investigation Goal
How do pressure and temperature affect the volume of a trapped gas?
1
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 Measured Volume (mL) 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?
2
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) Temp (K) 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
Pressure Power Word Wall Handout Reference 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
Marshmallow Mission Handout 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.
Gas Law Slides Plus Vocab Expansion 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
01
How do changes in pressure, volume, and temperature affect gas behavior?
02
How can we use mathematical models to predict these changes accurately?
03
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
Boyle's Battle Practice Worksheet 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."
Marshmallow Mission Answer Key Reference Only 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.
Facilitation Tips
Ensure a tight seal! If using a thumb, press hard to prevent air leakage, or use tip caps.
Use "Mini" marshmallows. Standard sized ones are too large for 60mL syringes and may get stuck.
After multiple compressions, the marshmallow will stay shriveled due to air escaping the bubbles.
Boyle's Battle Practice Worksheet 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
P1
1.0 atm
V1
500 L
P2
0.25 atm
V2
?
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?
P1
V1
P2
V2
?
Show Work (P1V1 = P2V2):
Boyles Battle Answer Key Reference Only 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
P1
1.0 atm
V1
500 L
P2
0.25 atm
V2
2000 L
(1.0 atm) * (500 L) = (0.25 atm) * V2
2. The Submarine Window Key
P1
100 kPa
V1
10 mL
P2
500 kPa
V2
2 mL
(100 kPa) * (10 mL) = (500 kPa) * V2
Charles's Chill Practice Worksheet 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 =
V1
3.0 L
T1 (in K)
298.15 K
V2
?
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:
Charles's Chill Practice Worksheet 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
V1
2.0 L
T1 (K)
298 K
T2 (K)
_______
V2
?
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:
Charles Chill Answer Key Reference Only 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
V1
2.0 L
T1
298 K
T2
268 K
V2
~1.80 L
2.0 L / 298 K = V2 / 268 K
2. The Hot Air Balloon Key
T1 = 20 + 273 = 293 K
Gay-Lussacs Punch Practice Worksheet Reference 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:
Gas Master Chart Anchor Chart 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
Mixed Law Medley Worksheet 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!
1
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
2
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: ________________________
3
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
Pressure Cooker CER Worksheet 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.
Gay-Lussacs Punch Practice Worksheet 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
P1
1.0 atm
T1 (K)
293 K
T2 (K)
_______
P2
?
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:
Mixed Law Medley Answer Key Reference Only Answer Key
Mixed Law Medley • Teacher Reference Only
Official Key
1
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
\(P_1V_1 = P_2V_2\)
2
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
\(\frac{V_1}{T_1} = \frac{V_2}{T_2} \rightarrow V_2 = \frac{V_1T_2}{T_1}\)
3
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
\(\frac{P_1}{T_1} = \frac{P_2}{T_2} \rightarrow P_2 = \frac{P_1T_2}{T_1}\)
Answer Key (Page 2)
4
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
\(\frac{P_1V_1}{T_1} = \frac{P_2V_2}{T_2} \rightarrow V_2 = \frac{P_1V_1T_2}{P_2T_1}\)
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.
Note: Students may have minor rounding differences depending on when they perform calculations. Answers in the bank are rounded to three significant figures to match the precision of the input data.
Gay Lussacs Punch Answer Key Reference Only 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
P1
1.0 atm
T1
293 K
T2
393 K
P2
~1.34 atm
1.0 atm / 293 K = P2 / 393 K
2. The Aerosol Can Key
T1 = 25 + 273 = 298 K
Law Lab Classifier Worksheet 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)
1
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):
2
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
3
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
4
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
5
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
Law Lab Classifier Answer Key Reference Only 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 = P2V2P2 = 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 KV2 ≈ 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 KP2 ≈ 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 KP2 ≈ 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)P2 = 5.0 atm
Peer Review Pro Rubric 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
Ideal Identity Chunked Reading Passage 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
Gases consist of large numbers of tiny particles.
Collisions are elastic (no energy lost).
Particles move in continuous, rapid, random motion.
There are no forces of attraction between particles.
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..."
Ideal Identity Monitoring Checklist 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 Check 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:
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:
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?"
Syringe Models Activity Handout 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.
1
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):
2
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):
3
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):
Ideal Identity Answer Key Reference Only 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).
Ideal Equation Engine Worksheet Ideal Equation Engine
Mathematical Modeling: \(PV = nRT\)
Name: ____________________________________
Date: _____________________________________
The Formula
PV = nRT
Variable Calibration
P
Pressure
atm
V
Volume
Liters (L)
n
Amount
moles (mol)
T
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
2
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
3
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
4
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
Ideal Equation Engine Answer Key Reference Only 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)
Gas Glossary Cards Handout 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
Formula Finder Worksheet 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 Investigator Handout 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 Variable Held Constant Pressure Prediction Volume Prediction Heating an aerosol can over a fire.
Word Wall Workshop Handout Reference Only 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
Gas Law Shuffle Activity Handout 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).
Gas Law Gear Reference Project Gas Law Gear
Unit Assessment Strategy & Reference
Name: __________________________
Date: ___________
KMT & Particle Logic
Temp (\(T\)) = Average Kinetic Energy . Higher temp = faster particles = more collisions.
Pressure (\(P\)) is caused by collisions with walls. No collisions = No pressure.
Rigid Containers : Volume (\(V\)) is constant . Cans/Tanks can explode if heated!
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:
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
\(g \to mol\)
Moles B
MOLE RATIO
Liters
\(mol \to L\)
The Tactical Set-up (Tracks)
Multiply Top | Divide Bottom
Given \(g\) (A)
1
1 mol (A)
Stoich Mission Manual Reading Passage Stoich Mission Manual
Tactical Briefing: Gas Stoichiometry Operations
Codename:
Date:
Mission: Solve Gas Reactions
T: STP vs Non-STP
Tools: PV=nRT & 22.4L
01
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.
02
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:
03
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 _________________________."
Stoich Squad Worksheet Project 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
01
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
02
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!
03
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)
Gas Gauntlet Study Guide Project 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.
Formula Finder Answer Key Reference Only 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)
\( 5.0 \times 10 = 1.0 \times V_2 \implies V_2 = \mathbf{50\text{ mL}} \)
Station Scramble Activity Handout STATION SCRAMBLE
Final Review Rotation
1
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
2
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
3
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
4
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
Gas Law Investigator Answer Key Reference Only 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%.
Word Wall Workshop Answer Key Reference Only 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.
Stoich Mission Manual Answer Key Reference Only 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. Gas Gauntlet Answer Key Reference Only 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 kPa92.04 kPa
6. Balloon partial pressure:
P_total = 103 kPa | P_CO2 = 40 kPa63 kPa
Section 4: Master Equation Answers
7. Bag of nuts (Boyle's Law):
P1 = 101 kPa, V1 = 250 mL, P2 = 85 kPa297.06 mL
8. Soda bottle sinking (Combined Law):
P1 = 1.50 atm, V1 = 40.0 mL, T1 = 280 K (7 + 273)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): 4.0 moles O2
Gas Law Shuffle Answer Key Reference Only 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.
Tip: Encourage students to visualize the "collision" frequency when explaining the relationship. Boyle's is the only inverse relationship because it's the only one where one variable "crowds" the other.
Gas Law Gear Reference Project Gas Law Gear
Unit Assessment Strategy & Reference
Name: __________________________
Date: ___________
KMT & Particle Logic
Temp (\(T\)) = Average Kinetic Energy . Higher temp = faster particles = more collisions.
Pressure (\(P\)) is caused by collisions with walls. No collisions = No pressure.
Rigid Containers : Volume (\(V\)) is constant . Cans/Tanks can explode if heated!
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:
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)
Stoich Squad Scaffolded Worksheet Project 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
L1
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?
C2H4(g) + 3O2(g) → 2CO2(g) + 2H2O(g)
1.25 L C2H4
×
____ L H2O
____ L C2H4
=
_________ L H2O
L2
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) + 1Cl2(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
L3
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
Pressure Power Quiz Handout 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.
Gas Gauntlet Answer Key Reference Only 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)2.46 atm
10. Combined Law (Soda Bottle):
(1.50 × 40.0) / 280 = (1.75 × V2) / 27633.80 mL
11. Boyle's Law (Constant T):
P1V1 = P2V20.5 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 mol14.0 g
14. Volume of 4.0 moles CO2 at STP:
4.0 mol × 22.4 L/mol = 89.6 L
Verification Code: GAS-GAUNTLET-V2-ANSWERS
Stoich Squad Ultimate Scaffold Worksheet Project 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
01
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 NH3(g) → 1 N2(g) + 3 H2(g)
10.0 L N2
____ mol NH3
____ mol N2
_________ L NH3
02
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
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 H2O2(aq) → 2 H2O(l) + 1 O2(g)
Build your own Railroad Tracks here!
03
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
Stoich Mission Coloring Page Stoich Mission Map
The Visual Protocol for Gas Stoichiometry
1
The Intel
Scan the environment: Is it STP or Non-STP?
STP = 22.4L NON = PV=nRT
2
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.
A
B
4
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.
Pressure Power Quiz Answer Key Reference Only 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
6. Gay-Lussac's Law Problem
Variables
T1 = 300 K
P1 = 5.0 atm
P2 = 12.0 atm
T2 = ?
P1 / T1 = P2 / T2
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
Stoich Squad Ultimate Scaffold Worksheet Project 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
01
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
02
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
1
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
Gas Gauntlet Answer Key Reference Only 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 K73.7 atm
11. Combined Law (Soda Bottle):
(1.50 × 40.0) / 280 = (1.75 × V2) / 27633.80 mL
12. Bag of nuts (Boyle's):
(101)(250) = (85)(V2)297 mL
Section 5: Stoichiometry
13. Propane combustion setup:
Answer: Setup A
14. Ammonia volume calculation:
128 g O2 / 32 = 4 mol O271.7 L
15. Neon at STP:
2.0 moles × 22.4 L/mol = 44.8 L
Study Guide Key | Behavior of Gases Unit
Stoich Squad Answer Key Reference Only Stoich Squad
Teacher Answer Key: Gas Reactions
Resource Type
TEACHER REFERENCE ONLY
01
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
02
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
03
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 =
Phase 2: Ideal Solve
\(V = \frac{(0.894)(0.0821)(303)}{1.90}\) =
