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 carbon monoxide gas at 78.5 °C and 848 torr is needed to produce 4.54 g of methanol, CH₃OH, according to the reaction: CO(g) + 2 H₂(g) → CH₃OH(g)?

5.00 L

2.50 L

3.75 L

1.25 L

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Verified step by step guidance

First, convert the mass of methanol (CH₃OH) to moles using its molar mass. The molar mass of CH₃OH is approximately 32.04 g/mol. Use the formula: \( \text{moles of CH₃OH} = \frac{\text{mass of CH₃OH}}{\text{molar mass of CH₃OH}} \).

Next, use the stoichiometry of the balanced chemical equation \( \text{CO(g) + 2 H₂(g) → CH₃OH(g)} \) to determine the moles of CO needed. According to the equation, 1 mole of CH₃OH is produced from 1 mole of CO.

Convert the pressure from torr to atm, as the ideal gas law requires pressure in atm. Use the conversion: \( 1 \text{ atm} = 760 \text{ torr} \). Therefore, \( \text{pressure in atm} = \frac{848 \text{ torr}}{760 \text{ torr/atm}} \).

Convert the temperature from Celsius to Kelvin, as the ideal gas law requires temperature in Kelvin. Use the formula: \( \text{temperature in K} = \text{temperature in °C} + 273.15 \).

Finally, use the ideal gas law \( PV = nRT \) to solve for the volume \( V \) of CO gas. Rearrange the equation to \( V = \frac{nRT}{P} \), where \( n \) is the moles of CO, \( R \) is the ideal gas constant (0.0821 L·atm/mol·K), \( T \) is the temperature in Kelvin, and \( P \) is the pressure in atm.