Chemical Quest Study Packet
Unit 4: Chemical Reactions & Stoichiometry
Chemical Quest Study Packet
Comprehensive Core Concept & Vocabulary Review
Name __________________
Date ______ / ______
The Reaction Roadmap
Chemical reactions tell a story of transformation. To master this topic, you must trace how atoms rearrange, speak the vocabulary of balancing, and master the conversion pathways between the microscopic and macroscopic worlds.
1. Reaction Lineup Matrix
S
Synthesis vs. Decomposition
Combining elements vs. breaking down a compound.
\[ A + B \rightarrow AB \quad \text{vs.} \quad AB \rightarrow A + B \]
R
Single vs. Double Replacement
One active element swaps vs. partner exchange.
\[ A + BC \rightarrow AC + B \quad \text{vs.} \quad AB + CD \rightarrow AD + CB \]
2. The Chemist's Lexicon
Match the term with its corresponding operational definition on the right.
1. Stoichiometry
A. The reactant that is completely consumed first, stopping the reaction.
2. Molar Mass
B. The study of quantitative relationships between reactants and products.
3. Limiting Reactant
C. The mass (in grams) of one mole of a substance, found using Periodic Table.
4. Percent Yield
D. The ratio of actual yield to theoretical yield, as a percentage.
3. Balancing Warmup Challenge
Balance the following chemical equation and identify its reaction type. Show your ratio below.
___ \( \text{Al(s)} \) + ___ \( \text{O}_2\text{(g)} \) → ___ \( \text{Al}_2\text{O}_3\text{(s)} \)
Reaction Type:
Coefficient Ratio:
: :
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Unit 4: Chemical Reactions & Stoichiometry
Stoichiometry Master Guide
Scaffolded Calculations & Practice Problems
Exam Prep
The 3-Step Stoichiometry Pathway
1 Grams to Moles
Divide given grams by molar mass of the starting reactant.
\( \text{g} \div \text{Molar Mass} = \text{mol} \)
2 Mole Ratio Swap
Multiply by coefficients ratio from balanced equation.
\( \text{mol A} \times \frac{\text{coeff B}}{\text{coeff A}} \)
3 Moles to Grams
Multiply newly found moles by product's molar mass.
\( \text{mol} \times \text{Molar Mass} = \text{g} \)
Practice Problem 1 (Scaffolded Walkthrough)
Scenario: Using \( 2\text{H}_2 + \text{O}_2 \rightarrow 2\text{H}_2\text{O} \), find how many grams of \( \text{H}_2\text{O} \) will be produced from 8.0 grams of Hydrogen gas (\( \text{H}_2 \)) with excess oxygen. (Molar Masses: \( \text{H}_2 = 2.0\text{g/mol} \), \( \text{H}_2\text{O} = 18.0\text{g/mol} \)).
A
Convert Starting Grams of \( \text{H}_2 \) to Moles:
\( 8.0\,\text{g H}_2 \div 2.0\,\text{g/mol} = \)
moles of \( \text{H}_2 \)
B
Apply the Mole Ratio:
moles \( \text{H}_2 \times \frac{2\,\text{mol H}_2\text{O}}{2\,\text{mol H}_2} = \)
moles of \( \text{H}_2\text{O} \)
C
Convert Moles of \( \text{H}_2\text{O} \) back to Grams:
moles \( \text{H}_2\text{O} \times 18.0\,\text{g/mol} = \)
g of \( \text{H}_2\text{O} \)
Practice Problem 2 (On Your Own)
Challenge: For the synthesis of ammonia: \( \text{N}_2\text{(g)} + 3\text{H}_2\text{(g)} \rightarrow 2\text{NH}_3\text{(g)} \). If you completely react 28.0 grams of Nitrogen gas (\( \text{N}_2 \)), how many grams of Ammonia (\( \text{NH}_3 \)) will you produce?
(Molar Masses: \( \text{N}_2 = 28.0\text{g/mol} \), \( \text{NH}_3 = 17.0\text{g/mol} \))
Chemist's Tip: Ensure you use the correct mole ratio: \( \frac{2\,\text{mol NH}_3}{1\,\text{mol N}_2} \) in your middle step!
Show your step-by-step math here:
Final Calculated Mass of \( \text{NH}_3 \):
________ g
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