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

General Chemistry

7. Gases

The Ideal Gas Law

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Multiple Choice

When 0.670 g argon is added to a 500 cm³ container with a sample of oxygen gas, the total pressure of the gases is found to be 1.52 atm at a temperature of 340 K. What is the mass of the oxygen gas in the bulb?

0.266 g

0.335 g

0.621 g

0.715 g

1.72 g

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Verified step by step guidance

First, use the ideal gas law to find the total number of moles of gas in the container. The ideal gas law is given by \( PV = nRT \), where \( P \) is the pressure, \( V \) is the volume, \( n \) is the number of moles, \( R \) is the ideal gas constant, and \( T \) is the temperature.

Convert the volume from cm³ to liters, since the ideal gas constant \( R \) is typically expressed in terms of liters. 500 cm³ is equivalent to 0.500 L.

Rearrange the ideal gas law to solve for \( n \): \( n = \frac{PV}{RT} \). Substitute the known values: \( P = 1.52 \text{ atm} \), \( V = 0.500 \text{ L} \), \( R = 0.0821 \text{ L atm K}^{-1} \text{ mol}^{-1} \), and \( T = 340 \text{ K} \).

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

Subtract the moles of argon from the total moles of gas to find the moles of oxygen. Then, convert the moles of oxygen to mass using the molar mass of oxygen (approximately 32.00 g/mol) with the formula \( m = n \times M \).