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

Previous problemNext problem

Struggling with General Chemistry?

Join thousands of students who trust us to help them ace their exams!Watch the first video

Multiple Choice

A sample of oxygen is collected over water and has a volume of 7.18 mL. The pressure of the collected 'wet' gas is 68.68 kPa and the temperature is 20°C. What will the volume of the 'dry' oxygen be in mL if the pressure is changed to 93.57 kPa, assuming the temperature remains constant?

7.18 mL

9.45 mL

5.27 mL

6.12 mL

Previous problemNext problem

Verified step by step guidance

Identify the given values: the volume of the wet gas (V1) is 7.18 mL, the pressure of the wet gas (P1) is 68.68 kPa, and the pressure of the dry gas (P2) is 93.57 kPa. The temperature is constant, so it does not need to be converted.

Understand that the gas collected over water is 'wet' and contains water vapor. To find the volume of the 'dry' gas, we need to account for the vapor pressure of water at 20°C, which is approximately 2.34 kPa.

Calculate the pressure of the dry oxygen gas (P1') by subtracting the vapor pressure of water from the total pressure of the wet gas: P1' = P1 - vapor pressure of water.

Use Boyle's Law, which states that for a given mass of gas at constant temperature, the product of pressure and volume is constant: P1' * V1 = P2 * V2. Rearrange this equation to solve for the volume of the dry gas (V2): V2 = (P1' * V1) / P2.

Substitute the known values into the equation: V2 = ((68.68 kPa - 2.34 kPa) * 7.18 mL) / 93.57 kPa. Calculate V2 to find the volume of the dry oxygen gas.