Table of contents

1. Matter and Measurements4h 31m
2. Atoms and the Periodic Table5h 23m
3. Ionic Compounds2h 18m
4. Molecular Compounds2h 18m
5. Classification & Balancing of Chemical Reactions3h 17m
6. Chemical Reactions & Quantities2h 27m
7. Energy, Rate and Equilibrium3h 46m
8. Gases, Liquids and Solids3h 25m
9. Solutions4h 10m
10. Acids and Bases3h 29m
11. Nuclear Chemistry56m
BONUS: Lab Techniques and Procedures1h 38m
BONUS: Mathematical Operations and Functions47m
12. Introduction to Organic Chemistry1h 34m
13. Alkenes, Alkynes, and Aromatic Compounds2h 12m
14. Compounds with Oxygen or Sulfur1h 6m
15. Aldehydes and Ketones1h 1m
16. Carboxylic Acids and Their Derivatives1h 11m
17. Amines39m
18. Amino Acids and Proteins1h 51m
19. Enzymes1h 37m
20. Carbohydrates1h 41m
21. The Generation of Biochemical Energy2h 8m
22. Carbohydrate Metabolism2h 22m
23. Lipids2h 26m
24. Lipid Metabolism1h 45m
25. Protein and Amino Acid Metabolism1h 37m
26. Nucleic Acids and Protein Synthesis2h 54m

8. Gases, Liquids and Solids

The Ideal Gas Law

GOB Chemistry

8. Gases, Liquids and Solids

The Ideal Gas Law

Previous problemNext problem

Struggling with GOB Chemistry?

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

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

Previous problemNext problem

Verified step by step guidance

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

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

Substitute the values for argon into the ideal gas law to find its partial pressure. Rearrange the ideal gas law to solve for \( P \): \( P = \frac{nRT}{V} \). Use \( R = 0.0821 \text{ L atm/mol K} \) and convert the volume from cm³ to L.

Subtract the partial pressure of argon from the total pressure to find the partial pressure of oxygen. The total pressure is given as 1.52 atm, so \( P_{\text{oxygen}} = P_{\text{total}} - P_{\text{argon}} \).

Use the ideal gas law again to find the number of moles of oxygen using its partial pressure. Then, calculate the mass of oxygen using its molar mass (approximately 32.00 g/mol) with the formula \( \text{mass} = n \times \text{molar mass} \).