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

7. Gases

The Ideal Gas Law Applications

General Chemistry

7. Gases

The Ideal Gas Law Applications

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Multiple Choice

A sample of oxygen is collected over water and has a volume of 2.23 mL. The pressure of the collected 'wet' gas is 61.78 kPa and the temperature is 20°C. What will the volume of the 'dry' oxygen be in mL if the pressure is changed to 94.91 kPa, assuming the temperature remains constant?

2.23 mL

3.56 mL

4.12 mL

1.45 mL

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Verified step by step guidance

Understand that the problem involves a gas collected over water, which means the gas is 'wet' and contains water vapor. To find the volume of 'dry' oxygen, we need to account for the water vapor pressure.

Use Dalton's Law of Partial Pressures to find the pressure of the 'dry' oxygen. Dalton's Law states that the total pressure of a gas mixture is the sum of the partial pressures of each component. Therefore, subtract the water vapor pressure at 20°C from the total pressure of the 'wet' gas to find the pressure of the 'dry' oxygen.

Look up the water vapor pressure at 20°C, which is approximately 2.34 kPa. Subtract this value from the total pressure of the 'wet' gas (61.78 kPa) to find the pressure of the 'dry' oxygen.

Apply Boyle's Law, which states that for a given amount of gas at constant temperature, the pressure and volume are inversely proportional: \( P_1V_1 = P_2V_2 \). Use the initial pressure and volume of the 'dry' oxygen and the final pressure to solve for the final volume.

Substitute the known values into Boyle's Law equation: \( V_2 = \frac{P_1V_1}{P_2} \), where \( P_1 \) is the pressure of the 'dry' oxygen, \( V_1 \) is the initial volume, and \( P_2 \) is the final pressure. Calculate \( V_2 \) to find the volume of the 'dry' oxygen at the new pressure.