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

Stoichiometry

General Chemistry

3. Chemical Reactions

Stoichiometry

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Multiple Choice

How many grams of O₂ are required to produce 9.64 g of H₂O in the combustion of butane according to the balanced equation: 2C₄H₁₀(g) + 13O₂(g) → 8CO₂(g) + 10H₂O(g)?

18.2 g

12.5 g

15.6 g

10.3 g

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Verified step by step guidance

Identify the balanced chemical equation for the combustion of butane: 2C₄H₁₀(g) + 13O₂(g) → 8CO₂(g) + 10H₂O(g). This equation tells us that 13 moles of O₂ are required to produce 10 moles of H₂O.

Calculate the molar mass of H₂O. The molar mass of H₂O is the sum of the atomic masses of 2 hydrogen atoms and 1 oxygen atom. Use the periodic table to find these values.

Determine the number of moles of H₂O produced. Use the formula: \( \text{moles of H₂O} = \frac{\text{mass of H₂O}}{\text{molar mass of H₂O}} \). Substitute the given mass of H₂O (9.64 g) and the molar mass calculated in the previous step.

Use the stoichiometry of the balanced equation to find the moles of O₂ required. From the balanced equation, 10 moles of H₂O are produced from 13 moles of O₂. Set up a proportion to find the moles of O₂ needed for the moles of H₂O calculated.

Calculate the mass of O₂ required. Use the formula: \( \text{mass of O₂} = \text{moles of O₂} \times \text{molar mass of O₂} \). Find the molar mass of O₂ (32.00 g/mol) and multiply it by the moles of O₂ calculated in the previous step.