Table of contents

1. The Chemical World9m
- The Scientific Method
  9m
2. Measurement and Problem Solving2h 19m
3. Matter and Energy2h 15m
4. Atoms and Elements2h 33m
5. Molecules and Compounds1h 50m
6. Chemical Composition1h 23m
7. Chemical Reactions1h 43m
8. Quantities in Chemical Reactions1h 8m
9. Electrons in Atoms and the Periodic Table2h 32m
10. Chemical Bonding2h 10m
11 Gases2h 7m
12. Liquids, Solids, and Intermolecular Forces1h 11m
13. Solutions3h 1m
14. Acids and Bases2h 14m
15. Chemical Equilibrium1h 27m
16. Oxidation and Reduction1h 33m
17. Radioactivity and Nuclear Chemistry53m

11 Gases

The Ideal Gas Law

Introduction to Chemistry

11 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

Start by using the ideal gas law, which is expressed as \( PV = nRT \), 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.

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

Determine the partial pressure of argon using the ideal gas law rearranged to \( P_{\text{Ar}} = \frac{n_{\text{Ar}}RT}{V} \). Substitute the values for \( n_{\text{Ar}} \), \( R \) (0.0821 L·atm/mol·K), \( T \) (340 K), and \( V \) (0.500 L) to find \( P_{\text{Ar}} \).

Subtract the partial pressure of argon from the total pressure to find the partial pressure of oxygen: \( P_{\text{O}_2} = P_{\text{total}} - P_{\text{Ar}} \).

Use the ideal gas law again to find the number of moles of oxygen gas: \( n_{\text{O}_2} = \frac{P_{\text{O}_2}V}{RT} \). Then, calculate the mass of oxygen using its molar mass (approximately 32.00 g/mol) with the formula \( \text{mass} = n_{\text{O}_2} \times \text{molar mass} \).