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

Chemistry Gas Laws

GOB Chemistry

8. Gases, Liquids and Solids

Chemistry Gas Laws

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2:16 minutes

Problem 67c

Textbook Question

A balloon is filled with helium gas with a partial pressure of 1.00 atm and neon gas with a partial pressure of 0.50 atm. For each of the following changes (a to e) of the initial balloon, select the diagram (A, B, or C) that shows the final volume of the balloon:
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c. All of the neon gas is removed (T and P do not change).

Verified step by step guidance

Step 1: Begin by understanding the concept of partial pressure. The total pressure of a gas mixture is the sum of the partial pressures of each individual gas. In this case, the initial total pressure is the sum of helium's partial pressure (1.00 atm) and neon's partial pressure (0.50 atm), which equals 1.50 atm.

Step 2: Recognize that removing all the neon gas will reduce the total pressure of the gas mixture. Since the partial pressure of neon is 0.50 atm, removing it leaves only the helium gas with a partial pressure of 1.00 atm.

Step 3: Recall Boyle's Law, which states that for a given amount of gas at constant temperature, the pressure and volume are inversely proportional: \( P_1 V_1 = P_2 V_2 \). Here, the temperature and pressure are constant, so the volume of the balloon will adjust to reflect the change in pressure.

Step 4: Analyze the diagrams provided (A, B, or C). The final volume of the balloon will correspond to the new pressure of 1.00 atm, which is lower than the initial total pressure of 1.50 atm. This means the balloon's volume will decrease.

Step 5: Select the diagram that visually represents the reduced volume of the balloon after the neon gas is removed. Compare the diagrams to identify the one that matches the expected decrease in volume.

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Key Concepts

Here are the essential concepts you must grasp in order to answer the question correctly.

Partial Pressure

Partial pressure refers to the pressure exerted by a single type of gas in a mixture of gases. In this scenario, the balloon contains helium and neon gases, each contributing to the total pressure. The partial pressures of 1.00 atm for helium and 0.50 atm for neon indicate how much each gas contributes to the overall pressure within the balloon.

Gas Laws

Gas laws describe the behavior of gases under various conditions of temperature and pressure. In this case, the relevant gas law is Boyle's Law, which states that the volume of a gas is inversely proportional to its pressure when temperature is constant. Removing neon gas will decrease the total pressure, leading to an increase in the balloon's volume.

Volume Change in Gases

The volume of a gas can change in response to alterations in pressure and the amount of gas present. When neon gas is removed from the balloon while keeping temperature and pressure constant, the remaining helium gas will occupy a larger volume due to the decrease in total gas pressure, demonstrating the principle of gas expansion.

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Multiple Choice

A 10.0 L cylinder with a movable piston exerts 3.00 atm of pressure. What will happen to the pressure if the volume of the container increases to 20.0 L?

A sealed container with a movable piston contains a gas with a pressure of 1380 torr, a volume of 820 mL and a temperature of 31°C. What would the volume be if the new pressure is now 2.83 atm, while the temperature decreased to 25°C?

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