Culinary Chemistry Scaffolded Quiz Chemistry Assessment Suite
STOICHIOMETRY CRUCIBLE
Tier 1: Guided Pathways
STUDENT:
DATE:
PERIOD:
Scenario A: The Chemistry of Quick-Breads
When baking soda (sodium bicarbonate, \(\text{NaHCO}_3\)) is heated in an oven, it breaks down to produce sodium carbonate, water vapor, and carbon dioxide gas. The trapped \(\text{CO}_2\) gas forms tiny bubbles, causing the dough to rise and become light and fluffy.
Atomic Mass Reference Panel
Sodium (Na) 23.0 g/mol
Hydrogen (H) 1.0 g/mol
Carbon (C) 12.0 g/mol
Oxygen (O) 16.0 g/mol
1
Balancing the Culinary Reaction (4 pts)
Balance the chemical equation below by writing the correct coefficients in the boxes. If the coefficient is 1, write a "1".
___ \(\text{NaHCO}_3(s)\) → ___ \(\text{Na}_2\text{CO}_3(s)\) + ___ \(\text{H}_2\text{O}(g)\) + ___ \(\text{CO}_2(g)\)
2
Understanding Mole-to-Mole Ratios (6 pts)
Using the balanced chemical equation from Problem 1, complete the molar ratio conversion factors below.
Ratio A: Baking Soda to Carbon Dioxide
______ moles \(\text{NaHCO}_3\) ______ moles \(\text{CO}_2\)
or
______ moles \(\text{CO}_2\) ______ moles \(\text{NaHCO}_3\)
Ratio B: Water to Carbon Dioxide
______ moles \(\text{H}_2\text{O}\) ______ moles \(\text{CO}_2\)
or
______ moles \(\text{CO}_2\) ______ moles \(\text{H}_2\text{O}\)
Stoichiometry Crucible Assessment Suite Page 1 of 2
SECTION 2: QUANTITATIVE COOKING
Mass-to-Volume Scaffolding
3
Calculating Molar Mass (10 pts)
Before converting mass to moles, calculate the molar mass of Sodium Bicarbonate (\(\text{NaHCO}_3\)).
Element Quantity (Atoms) Atomic Mass Total Element Mass Sodium (Na) 1 23.0 g/mol 1 × 23.0 = _____ g/mol Hydrogen (H) 1 1.0 g/mol 1 × 1.0 = _____ g/mol Carbon (C) 1 12.0 g/mol 1 × 12.0 = _____ g/mol Oxygen (O) 3 16.0 g/mol 3 × 16.0 = _____ g/mol Molar Mass of \(\text{NaHCO}_3\): ________________ g/mol
4
The Bread Rising Calculation (15 pts)
A baker adds 16.8 grams of baking soda (\(\text{NaHCO}_3\)) to a cake batter. What mass of Carbon Dioxide (\(\text{CO}_2\)) gas will be produced? (Molar mass of \(\text{CO}_2 = 44.0\text{ g/mol}\)).
Pathway:
Mass \(\text{NaHCO}_3\) Moles \(\text{NaHCO}_3\) Moles \(\text{CO}_2\) Mass \(\text{CO}_2\)
Step 1: Given Mass 16.8 g \(\text{NaHCO}_3\)
To Moles
1 mol \(\text{NaHCO}_3\)
_______ g \(\text{NaHCO}_3\)
Mole Ratio
_____ mol \(\text{CO}_2\)
_____ mol \(\text{NaHCO}_3\)
To Mass
44.0 g \(\text{CO}_2\)
1 mol \(\text{CO}_2\)
Calculation scratch area:
Calculated Mass of \(\text{CO}_2\):
__________________ g
5
Conceptual Application (5 pts)
If a baker doubles the baking soda recipe but keeps all other ingredients the same, what will happen to the amount of gas produced? How might this affect the final cake?
Stoichiometry Crucible Assessment Suite Page 2 of 2
Aerospace Propulsion Standard Quiz Chemistry Assessment Suite
STOICHIOMETRY CRUCIBLE
Tier 2: Standard Assessment
STUDENT:
DATE:
PERIOD:
Scenario B: Rocket Engine Combustion Dynamics
Liquid hydrazine (\(\text{N}_2\text{H}_4\)) and dinitrogen tetroxide (\(\text{N}_2\text{O}_4\)) are hypergolic propellants—they ignite instantly on contact. This reaction is highly efficient and serves as primary thruster propulsion for deep-space spacecraft, emitting high-velocity nitrogen gas and superheated water vapor.
Molar Mass Lookup Values
Hydrogen (H) 1.01 g/mol
Nitrogen (N) 14.01 g/mol
Oxygen (O) 16.00 g/mol
1
Equation Verification and Balancing (5 pts)
Balance the chemical equation below. These coefficients represent the exact stoichiometric mole-to-mole ratios required for safe and controlled rocket combustion.
___ \(\text{N}_2\text{H}_4(l)\) + ___ \(\text{N}_2\text{O}_4(l)\) → ___ \(\text{N}_2(g)\) + ___ \(\text{H}_2\text{O}(g)\)
2
Reactant & Product Molar Masses (10 pts)
Calculate the individual molar masses for the primary reactant and the gaseous products. Show your chemical formula work in the spaces below.
A. Hydrazine (\(\text{N}_2\text{H}_4\)) Calculation scratch space:
Mass = ________________ g/mol
B. Nitrogen Gas (\(\text{N}_2\)) Calculation scratch space:
Mass = ________________ g/mol
Stoichiometry Crucible Assessment Suite Page 1 of 2
SECTION 2: ROCKET MASS PAYLOADS
Standard Mass-to-Mass Calculation
3
The Stoichiometric Yield Calculation (15 pts)
Suppose a spacecraft's thruster is loaded with exactly 96.0 grams of hydrazine reactant (\(\text{N}_2\text{H}_4\)), which reacts completely with excess dinitrogen tetroxide (\(\text{N}_2\text{O}_4\)). What mass of diatomic nitrogen gas (\(\text{N}_2\)) will be produced in this reaction?
Standard Conversion Pathway: Mass A → Moles A → Moles B → Mass B
Start Value 96.0 g \(\text{N}_2\text{H}_4\)
Convert to Mol Cancel Grams
Mole Ratio (Product) Mole Ratio (Reactant)
Convert to Mass Cancel Moles
Show all calculation arithmetic and canceling units below:
Calculated Theoretical Yield of \(\text{N}_2\):
__________________ g \(\text{N}_2\)
4
Calculating Percent Yield (10 pts)
In a physical rocket engine combustion test, the reaction of 96.0 g of hydrazine reactant actually produced an empirical yield of 112.5 grams of Nitrogen gas (\(\text{N}_2\)). Using your theoretical yield from Problem 3, calculate the rocket thruster's percent yield.
Automotive Catalysis Advanced Quiz Chemistry Assessment Suite
STOICHIOMETRY CRUCIBLE
Tier 3: Advanced Level
STUDENT:
DATE:
PERIOD:
Scenario C: Automotive Catalytic Conversions
Automotive catalytic converters utilize precious metal catalysts to convert hazardous emissions from combustion engines into safer exhaust gases. This process relies on a key redox reaction that converts toxic nitric oxide (\(\text{NO}\)) and carbon monoxide (\(\text{CO}\)) into harmless atmospheric nitrogen gas (\(\text{N}_2\)) and carbon dioxide (\(\text{CO}_2\)).
High-Precision Atomic Masses
Carbon (C) 12.011 g/mol
Nitrogen (N) 14.007 g/mol
Oxygen (O) 15.999 g/mol
Argon (Ar) 39.948 g/mol
1
Reaction Kinetics & Balancing (5 pts)
Balance the chemical reaction representing catalytic combustion. Show all coefficients (even "1" must be written explicitly).
___ \(\text{NO}(g)\) + ___ \(\text{CO}(g)\) → ___ \(\text{N}_2(g)\) + ___ \(\text{CO}_2(g)\)
2
Limiting Reactant Evaluation (15 pts)
A test chamber is injected with 30.0 grams of nitric oxide (\(\text{NO}\)) and 35.0 grams of carbon monoxide (\(\text{CO}\)). Calculate the theoretical yield of nitrogen gas (\(\text{N}_2\)) in moles from each starting reactant to identify the limiting reactant.
Calculation A: Starting with 30.0 g \(\text{NO}\)
Moles of \(\text{N}_2\) produced = _________________
Calculation B: Starting with 35.0 g \(\text{CO}\)
Moles of \(\text{N}_2\) produced = _________________
The Limiting Reactant is: The Excess Reactant is:
Stoichiometry Crucible Assessment Suite Page 1 of 2
SECTION 2: QUANTITATIVE RECONCILIATION
Advanced Yield & Green Metrics
3
Theoretical Yield of Greenhouse Product (15 pts)
Determine the theoretical yield of carbon dioxide (\(\text{CO}_2\)) produced in grams under the conditions of Problem 2. Use the identified limiting reactant to execute your final conversion stoichiometry.
Calculation scratch workspace:
Calculated Theoretical Yield of \(\text{CO}_2\):
__________________ g \(\text{CO}_2\)
4
Experimental Efficiency Analysis (10 pts)
During dynamic flow tests inside the exhaust manifold simulation, the catalyst reaction yielded an actual mass of 38.5 grams of carbon dioxide (\(\text{CO}_2\)). Calculate the actual percent efficiency of the conversion.
Show calculations:
Percent Yield = __________________ %
