Table of contents

1. Intro to General Chemistry3h 48m
2. Atoms & Elements4h 16m
3. Chemical Reactions4h 10m
4. BONUS: Lab Techniques and Procedures1h 38m
5. BONUS: Mathematical Operations and Functions48m
6. Chemical Quantities & Aqueous Reactions3h 53m
7. Gases3h 49m
8. Thermochemistry2h 37m
9. Quantum Mechanics2h 58m
10. Periodic Properties of the Elements3h 9m
11. Bonding & Molecular Structure3h 29m
12. Molecular Shapes & Valence Bond Theory1h 57m
13. Liquids, Solids & Intermolecular Forces2h 23m
14. Solutions3h 1m
15. Chemical Kinetics2h 53m
16. Chemical Equilibrium2h 29m
17. Acid and Base Equilibrium5h 1m
18. Aqueous Equilibrium4h 47m
19. Chemical Thermodynamics1h 50m
20. Electrochemistry2h 42m
21. Nuclear Chemistry2h 36m
22. Organic Chemistry5h 7m
23. Chemistry of the Nonmetals2h 39m
24. Transition Metals and Coordination Compounds3h 16m

3. Chemical Reactions

Percent Yield

General Chemistry

3. Chemical Reactions

Percent Yield

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Multiple Choice

Propane (C₃H₈) reacts with oxygen in the air to produce carbon dioxide and water. In a particular experiment, 38.0 grams of carbon dioxide are produced from the reaction of 22.05 grams of propane with excess oxygen. What is the percentage yield in this reaction?

85.0%

90.0%

75.0%

95.0%

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Verified step by step guidance

Identify the balanced chemical equation for the combustion of propane: \( \text{C}_3\text{H}_8 + 5\text{O}_2 \rightarrow 3\text{CO}_2 + 4\text{H}_2\text{O} \).

Calculate the molar mass of propane (C₃H₈) by adding the atomic masses of its constituent atoms: \( 3 \times 12.01 \text{ g/mol (C)} + 8 \times 1.01 \text{ g/mol (H)} \).

Determine the moles of propane used in the reaction by dividing the given mass of propane (22.05 grams) by its molar mass.

Using the stoichiometry of the balanced equation, calculate the theoretical moles of carbon dioxide produced from the moles of propane. Since 1 mole of propane produces 3 moles of carbon dioxide, multiply the moles of propane by 3.

Convert the theoretical moles of carbon dioxide to grams using its molar mass (44.01 g/mol) and compare it to the actual mass of carbon dioxide produced (38.0 grams) to calculate the percentage yield using the formula: \( \text{Percentage Yield} = \left( \frac{\text{Actual Yield}}{\text{Theoretical Yield}} \right) \times 100 \% \).