Question 1

A weather balloon is released at sea level where the atmospheric pressure is 1.00 atm and the temperature is 27°C. As the balloon rises, the external pressure drops to 0.60 atm and the temperature drops to -13°C. If the initial volume of the balloon is 2.0 L, what is its final volume? (Assume the amount of gas remains constant.)

Accepted Answer

3.7 L

Question 2

Which of the following statements best explains why a sealed bag of chips appears inflated when taken to a high-altitude location?

Accepted Answer

The external atmospheric pressure decreases, so the pressure inside the bag is greater than outside, causing the bag to expand.

Question 3

A sample of gas occupies 4.0 L at 2.0 atm. If the pressure is increased to 8.0 atm at constant temperature, what is the new volume?

Accepted Answer

1.0 L

Question 4

Which of the following is NOT a correct conversion for standard atmospheric pressure?

Accepted Answer

1 atm = 100,000 Pa

Question 5

A scuba diver's tank contains 0.50 mol of oxygen gas at 25°C and 10.0 atm. What is the volume of the tank in liters? (R = 0.0821 L·atm/K·mol)

Accepted Answer

1.22 L

Question 6

Which scenario would most likely cause a real gas to deviate from ideal behavior?

Accepted Answer

High pressure and low temperature

Question 7

A hospital stores oxygen at 3000 psi. What is this pressure in atmospheres? (1 atm = 14.7 psi)

Accepted Answer

204 atm

Question 8

A 5.0 L container holds nitrogen gas at 27°C and 2.0 atm. If the temperature is increased to 127°C at constant volume, what is the new pressure?

Accepted Answer

2.7 atm

Question 9

Which of the following best describes Avogadro's Law?

Accepted Answer

At constant temperature and pressure, the volume of a gas is directly proportional to the number of moles.

Question 10

A gas sample at 1.0 atm and 273 K occupies 22.4 L. If the amount of gas is doubled at constant temperature and pressure, what will be the new volume?

Accepted Answer

44.8 L

Question 11

A patient receives a gas mixture through a mask at 760 mm Hg. What is the pressure in pascals (Pa)? (1 atm = 760 mm Hg = 101,325 Pa)

Accepted Answer

101,325 Pa

Question 12

A 2.0 L sample of gas at 300 K and 1.0 atm is compressed to 1.0 L and heated to 600 K. What is the final pressure?

Accepted Answer

4.0 atm

Question 13

Which of the following is a correct statement about the use of temperature in gas law calculations?

Accepted Answer

Temperature must always be converted to Kelvin.

Question 14

A tire is inflated to 32 psi at 20°C. On a hot day, the temperature rises to 40°C. Assuming the volume is constant, what is the new pressure in psi? (Use absolute temperature in Kelvin.)

Accepted Answer

34 psi

Question 15

Which of the following best explains why deep-sea divers must ascend slowly to the surface?

Accepted Answer

Rapid pressure decrease causes dissolved gases in the blood to form bubbles, which can be dangerous.

Question 16

A 10.0 L tank contains 2.0 mol of helium gas at 300 K. What is the pressure in atm? (R = 0.0821 L·atm/K·mol)

Accepted Answer

4.92 atm

Question 17

Which of the following is a real-world example of Boyle's Law?

Accepted Answer

A syringe plunger is pushed in, decreasing the volume and increasing the pressure inside.

Question 18

A gas occupies 3.0 L at 27°C and 1.0 atm. What will be its volume at 127°C and 1.0 atm?

Accepted Answer

4.0 L

Question 19

Which of the following best describes the combined gas law?

Accepted Answer

It relates pressure, volume, and temperature for a fixed amount of gas.

Question 20

A gas cylinder contains 5.0 L of gas at 3.0 atm and 300 K. If the gas is transferred to a 10.0 L container at 1.5 atm, what is the final temperature in Kelvin?

Accepted Answer

300 K

Key Concepts of Gases and Gas Laws

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