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

Partial Pressure

General Chemistry

7. Gases

Partial Pressure

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Multiple Choice

A sample of 3.51 g argon and an unknown amount of oxygen are mixed in a container at room temperature. The partial pressure of argon was calculated as 71.0 torr and the partial pressure of oxygen as 188 torr. What is the mass of the oxygen within the container?

4.27 g

6.18 g

7.44 g

9.16 g

15.2 g

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Verified step by step guidance

First, understand that the problem involves a mixture of gases, and we need to use the concept of partial pressures and the ideal gas law to find the mass of oxygen.

Use the ideal gas law in the form \( PV = nRT \) to find the number of moles of argon. Here, \( P \) is the partial pressure of argon, \( V \) is the volume of the container, \( n \) is the number of moles, \( R \) is the ideal gas constant, and \( T \) is the temperature in Kelvin.

Calculate the number of moles of argon using its given mass and molar mass. The molar mass of argon is approximately 39.95 g/mol. Use the formula \( n = \frac{\text{mass}}{\text{molar mass}} \).

Since the volume \( V \) and temperature \( T \) are constant for both gases, use the ratio of partial pressures to find the moles of oxygen. The ratio of moles of oxygen to moles of argon is the same as the ratio of their partial pressures: \( \frac{n_{\text{O}_2}}{n_{\text{Ar}}} = \frac{P_{\text{O}_2}}{P_{\text{Ar}}} \).

Finally, calculate the mass of oxygen using the number of moles of oxygen and its molar mass (approximately 32.00 g/mol). Use the formula \( \text{mass} = n \times \text{molar mass} \).