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

What volume, in liters, of hydrogen gas at 32.5 °C and 722 torr is needed to produce 0.224 g of methanol, CH₃OH, according to the reaction: CO(g) + 2 H₂(g) → CH₃OH(g)?

0.112 L

0.336 L

0.448 L

0.224 L

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Verified step by step guidance

First, determine the number of moles of methanol (CH₃OH) produced using its molar mass. The molar mass of CH₃OH is approximately 32.04 g/mol. Use the formula: \( \text{moles of CH}_3\text{OH} = \frac{0.224 \text{ g}}{32.04 \text{ g/mol}} \).

According to the balanced chemical equation, 1 mole of CH₃OH is produced from 2 moles of H₂. Use stoichiometry to find the moles of H₂ needed: \( \text{moles of H}_2 = 2 \times \text{moles of CH}_3\text{OH} \).

Use the ideal gas law to find the volume of hydrogen gas. The ideal gas law is \( PV = nRT \), where \( P \) is pressure, \( V \) is volume, \( n \) is moles, \( R \) is the ideal gas constant (0.0821 L·atm/mol·K), and \( T \) is temperature in Kelvin.

Convert the given temperature from Celsius to Kelvin: \( T = 32.5 + 273.15 \). Also, convert the pressure from torr to atm: \( P = \frac{722}{760} \text{ atm} \).

Rearrange the ideal gas law to solve for volume \( V \): \( V = \frac{nRT}{P} \). Substitute the values for \( n \), \( R \), \( T \), and \( P \) to find the volume of hydrogen gas needed.