Q: A 1.00 mol sample of oxygen occupies a volume of 24.47 L at 1.000 atm. What volume will the same amount of oxygen occupy at 22.00 psi? (1 atm = 14.70 psi)

$$V_2$$ = \frac{24.47 \times 14.70}{22.00} = 16.35\,L$$

Q: A balloon contains 500 mL of helium at 300 K. What will be its new volume at standard temperature (273 K), assuming constant pressure?

$$V_2$$ = \frac{500 \times 273}{300} = 455\,mL$$

Q: At STP, 1.00 mol of $$O_2$$ occupies 22.4 L. What volume will 0.100 mol of $$O_2$$ occupy at STP?

$$V = 0.100 \times 22.4 = 2.24\,L$$

Question 1

Which of the following statements best explains why increasing the temperature of a gas in a sealed container increases its pressure?

Accepted Answer

The gas molecules move faster, causing more frequent and forceful collisions with the container walls.

Question 2

A scuba diver inhales air at 3 bar pressure deep underwater and swims quickly to the surface while holding her breath. According to Boyle's Law, what happens to the volume of air in her lungs?

Accepted Answer

The volume of air in her lungs would increase by a factor of 3.

Question 3

Which equation correctly represents Boyle's Law for a fixed amount of gas at constant temperature?

Accepted Answer

$$V_1P_1 = V_2P_2$$

Question 4

A 1.00 mol sample of oxygen occupies a volume of 24.47 L at 1.000 atm. What volume will the same amount of oxygen occupy at 22.00 psi? (1 atm = 14.70 psi)

Accepted Answer

$$V_2$$ = \frac{24.47 	imes 14.70}{22.00} = 16.35\,L$$

Question 5

Which of the following best describes Charles' Law?

Accepted Answer

At constant pressure, the volume of a gas is directly proportional to its absolute temperature.

Question 6

A balloon contains 500 mL of helium at 300 K. What will be its new volume at standard temperature (273 K), assuming constant pressure?

Accepted Answer

$$V_2$$ = \frac{500 	imes 273}{300} = 455\,mL$$

Question 7

Which equation represents Charles' Law?

Accepted Answer

$$\frac{V_1$}{T_1$} = \frac{V_2$}{T_2$}$$

Question 8

Gay-Lussac’s Law relates which two properties of a gas, assuming the amount and volume are constant?

Accepted Answer

Pressure and temperature

Question 9

If the temperature of a gas in a rigid container doubles from 250 K to 500 K, what happens to the pressure according to Gay-Lussac’s Law?

Accepted Answer

The pressure doubles.

Question 10

Which equation correctly represents Gay-Lussac’s Law?

Accepted Answer

$$\frac{P_1$}{T_1$} = \frac{P_2$}{T_2$}$$

Question 11

Avogadro’s Law states that, at constant temperature and pressure, which of the following is true?

Accepted Answer

The volume of a gas is directly proportional to the number of moles of gas.

Question 12

Which equation represents Avogadro’s Law?

Accepted Answer

$$\frac{V_1$}{n_1$} = \frac{V_2$}{n_2$}$$

Question 13

At STP, 1.00 mol of $$O_2$$ occupies 22.4 L. What volume will 0.100 mol of $$O_2$$ occupy at STP?

Accepted Answer

$$V = 0.100 	imes 22.4 = 2.24\,L$$

Question 14

A student blows up a balloon to 1.2 L, and each breath supplies the balloon with 0.060 mol of exhaled air. How many moles of air are in 3 balloons of this size?

Accepted Answer

$$n = 3 	imes 0.060 = 0.180\,mol$$

Question 15

Which of the following would NOT increase the pressure of a gas in a sealed container?

Accepted Answer

Increasing the volume of the container

Question 16

A hot air balloon rises because the air inside the balloon is heated. Which gas law best explains why the balloon expands as it rises?

Accepted Answer

Charles' Law

Question 17

A sample of gas at 1.00 atm and 300 K occupies 2.00 L. If the temperature is increased to 600 K at constant pressure, what is the new volume?

Accepted Answer

$$V_2$$ = \frac{2.00 	imes 600}{300} = 4.00\,L$$

Question 18

Which of the following is a real-world consequence of Boyle’s Law that scuba divers must consider?

Accepted Answer

Rapid ascent can cause the air in the lungs to expand and potentially damage lung tissue.

Chapter 5.2 : Gases and Gas Laws – General Chemistry Study Notes

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