Q: A diver holds her breath and dives to a depth where the pressure increases from 1.00 atm to 1.50 atm. If her lungs initially hold 4.2 L of air, what is the volume of her lungs at this new pressure? (Assume temperature is constant.)

$$V_f = \frac{P_i V_i}{P_f} = \frac{1.00 \times 4.2}{1.50} = 2.8\ \text{L}$$

Q: Convert 1.08 atm to mmHg. (1 atm = 760 mmHg)

$$1.08\ \text{atm} \times \frac{760\ \text{mmHg}}{1\ \text{atm}} = 821\ \text{mmHg}$$

Q: A pilot starts altitude training at 762 mmHg with 6.00 L of air in his lungs. After changing altitude, his lungs expand to 6.25 L. What is the new atmospheric pressure in mmHg? (Assume constant temperature.)

$$P_f = \frac{P_i V_i}{V_f} = \frac{762 \times 6.00}{6.25} = 731\ \text{mmHg}$$

Q: If you remove a balloon with a volume of 105 mL of air from a freezer at $$0^\circC $$and allow the balloon to warm to a room temperature of $$25^\circC$$, what would its final volume be? (Assume constant pressure.)

$$V_f = V_i \frac{T_f}{T_i} = 105 \times \frac{298}{273} = 114.6\ \text{mL}$$

Q: A 1.20-L sample of a gas at $$30^\circC $$and 1.00 atm is heated to $$225^\circC $$and 1.50 atm final pressure. What is the final volume of the gas?

$$V_f = \frac{P_i V_i T_f}{T_i P_f} = \frac{1.00 \times 1.20 \times 498}{303 \times 1.50} = 1.32\ \text{L}$$

Q: A child’s balloon containing 8.5 L of helium gas at sea level (1.00 atm) is released and floats away. What will the volume of the helium be when the balloon rises to the point where the atmospheric pressure is 380 mmHg? (1 atm = 760 mmHg)

$$V_f = \frac{P_i V_i}{P_f} = \frac{1.00 \times 8.5}{0.5} = 17\ \text{L}$$

Q: Convert 750 mmHg to psi. (1 atm = 760 mmHg = 14.7 psi)

$$750\ \text{mmHg} \times \frac{1\ \text{atm}}{760\ \text{mmHg}} \times \frac{14.7\ \text{psi}}{1\ \text{atm}} = 14.5\ \text{psi}$$

Question 1

Which of the following best describes the relationship between pressure and volume for a fixed amount of gas at constant temperature, according to Boyle’s Law?

Accepted Answer

Pressure and volume are inversely proportional.

Question 2

A diver holds her breath and dives to a depth where the pressure increases from 1.00 atm to 1.50 atm. If her lungs initially hold 4.2 L of air, what is the volume of her lungs at this new pressure? (Assume temperature is constant.)

Accepted Answer

$$V_f = \frac{P_i V_i}{P_f} = \frac{1.00 	imes 4.2}{1.50} = 2.8\ 	ext{L}$$

Question 3

Convert 1.08 atm to mmHg. (1 atm = 760 mmHg)

Accepted Answer

$$1.08\ 	ext{atm} 	imes \frac{760\ 	ext{mmHg}}{1\ 	ext{atm}} = 821\ 	ext{mmHg}$$

Question 4

A pilot starts altitude training at 762 mmHg with 6.00 L of air in his lungs. After changing altitude, his lungs expand to 6.25 L. What is the new atmospheric pressure in mmHg? (Assume constant temperature.)

Accepted Answer

$$P_f = \frac{P_i V_i}{V_f} = \frac{762 	imes 6.00}{6.25} = 731\ 	ext{mmHg}$$

Question 5

If you remove a balloon with a volume of 105 mL of air from a freezer at $$0^\circC $$and allow the balloon to warm to a room temperature of $$25^\circC$$, what would its final volume be? (Assume constant pressure.)

Accepted Answer

$$V_f = V_i \frac{T_f}{T_i} = 105 	imes \frac{298}{273} = 114.6\ 	ext{mL}$$

Question 6

A 1.20-L sample of a gas at $$30^\circC $$and 1.00 atm is heated to $$225^\circC $$and 1.50 atm final pressure. What is the final volume of the gas?

Accepted Answer

$$V_f = \frac{P_i V_i T_f}{T_i P_f} = \frac{1.00 	imes 1.20 	imes 498}{303 	imes 1.50} = 1.32\ 	ext{L}$$

Question 7

A child’s balloon containing 8.5 L of helium gas at sea level (1.00 atm) is released and floats away. What will the volume of the helium be when the balloon rises to the point where the atmospheric pressure is 380 mmHg? (1 atm = 760 mmHg)

Accepted Answer

$$V_f = \frac{P_i V_i}{P_f} = \frac{1.00 	imes 8.5}{0.5} = 17\ 	ext{L}$$

Question 8

Which of the following is NOT an assumption of the kinetic molecular theory of gases?

Accepted Answer

Gas particles have significant volume compared to the container.

Question 9

Convert 750 mmHg to psi. (1 atm = 760 mmHg = 14.7 psi)

Accepted Answer

$$750\ 	ext{mmHg} 	imes \frac{1\ 	ext{atm}}{760\ 	ext{mmHg}} 	imes \frac{14.7\ 	ext{psi}}{1\ 	ext{atm}} = 14.5\ 	ext{psi}$$

Question 10

Which of the following best explains why a balloon shrinks when placed in a freezer?

Accepted Answer

The volume of the gas decreases as the temperature decreases, according to Charles’s Law.

Question 11

Convert 0.94 atm to psi. (1 atm = 14.7 psi)

Accepted Answer

$$0.94\ 	ext{atm} 	imes \frac{14.7\ 	ext{psi}}{1\ 	ext{atm}} = 13.8\ 	ext{psi}$$

Question 12

Which of the following scenarios best illustrates Gay-Lussac’s Law?

Accepted Answer

A rigid aerosol can explodes when thrown into a fire because the pressure inside increases as the temperature rises.

Question 13

A gas sample is compressed from 2.0 L to 1.0 L at constant temperature. If the initial pressure was 0.50 atm, what is the final pressure?

Accepted Answer

$$P_f = \frac{P_i V_i}{V_f} = \frac{0.50 	imes 2.0}{1.0} = 1.0\ 	ext{atm}$$

Question 14

Which of the following is a correct application of the combined gas law?

Accepted Answer

Calculating the final volume of a gas when both temperature and pressure change.

Gas Laws and Pressure Conversion Practice – Step-by-Step Guidance

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