Question 1

A weather balloon is released at sea level where the atmospheric pressure is 1.00 atm and the temperature is 20°C. As the balloon rises, the external pressure drops to 0.60 atm and the temperature drops to -10°C. Assuming the amount of gas in the balloon remains constant, which of the following best describes what happens to the volume of the balloon as it ascends?
Correct answer: The volume increases because the decrease in pressure has a greater effect than the decrease in temperature.

Accepted Answer

The volume increases because the decrease in pressure has a greater effect than the decrease in temperature.

Question 2

Which of the following statements best explains why a sealed bag of chips appears inflated when taken from sea level to a high mountain?
Correct answer: The external atmospheric pressure decreases at higher altitudes, so the pressure inside the bag is greater than outside, causing the bag to expand.

Accepted Answer

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

Question 3

A sample of gas occupies 2.50 L at 1.00 atm and 300 K. If the pressure is increased to 2.00 atm and the temperature is increased to 400 K, what is the new volume of the gas? (Use the combined gas law.)
Correct answer: 1.67 L

Accepted Answer

1.67 L

Question 4

Which of the following is NOT a correct conversion for standard atmospheric pressure?
Correct answer: 1 atm = 1000 psi

Accepted Answer

1 atm = 1000 psi

Question 5

A scuba diver's tank contains 12.0 L of air at a pressure of 200 atm. If the air is released at the surface where the pressure is 1.00 atm, what volume will the air occupy? (Assume constant temperature.)
Correct answer: 2400 L

Accepted Answer

2400 L

Question 6

Which of the following best describes why real gases deviate from ideal behavior at high pressures and low temperatures?
Correct answer: Intermolecular forces and the finite volume of gas molecules become significant.

Accepted Answer

Intermolecular forces and the finite volume of gas molecules become significant.

Question 7

A 5.00 g sample of O2 gas is placed in a 10.0 L container at 27°C. What is the pressure in the container? (R = 0.0821 L·atm/(mol·K); molar mass O2 = 32.0 g/mol)
Correct answer: 0.512 atm

Accepted Answer

0.512 atm

Question 8

Which of the following scenarios best illustrates Avogadro's Law?
Correct answer: Increasing the number of moles of gas in a balloon at constant temperature and pressure causes the balloon to expand.

Accepted Answer

Increasing the number of moles of gas in a balloon at constant temperature and pressure causes the balloon to expand.

Question 9

A hospital stores oxygen at 3000 psi in a 50.0 L tank. If the oxygen is released to fill 1.00 L cylinders at 1.00 atm, how many full cylinders can be filled? (1 atm = 14.7 psi; assume constant temperature)
Correct answer: 1020 cylinders

Accepted Answer

1020 cylinders

Question 10

Which of the following best explains why a mercury barometer is used to measure atmospheric pressure?
Correct answer: Mercury's high density allows for a manageable column height to measure atmospheric pressure.

Accepted Answer

Mercury's high density allows for a manageable column height to measure atmospheric pressure.

Question 11

A gas sample at 25°C and 1.00 atm occupies 10.0 L. If the temperature is increased to 100°C at constant pressure, what is the new volume?
Correct answer: 13.2 L

Accepted Answer

13.2 L

Question 12

Which of the following is a correct statement about the relationship between gas pressure and molecular collisions?
Correct answer: Gas pressure results from the collisions of gas molecules with the walls of their container.

Accepted Answer

Gas pressure results from the collisions of gas molecules with the walls of their container.

Question 13

A 2.00 L container holds 0.100 mol of an ideal gas at 300 K. What is the pressure inside the container? (R = 0.0821 L·atm/(mol·K))
Correct answer: 1.23 atm

Accepted Answer

1.23 atm

Question 14

Which of the following best describes the effect of increasing the temperature of a fixed amount of gas at constant volume?
Correct answer: The pressure increases because the gas molecules move faster and collide with the walls more frequently.

Accepted Answer

The pressure increases because the gas molecules move faster and collide with the walls more frequently.

Question 15

A tire is inflated to a pressure of 32.0 psi at 20°C. On a hot day, the temperature inside the tire rises to 50°C. What is the new pressure in psi, assuming the volume is constant? (1 atm = 14.7 psi)
Correct answer: 36.3 psi

Accepted Answer

36.3 psi

Question 16

Which of the following is a correct application of Boyle's Law?
Correct answer: A syringe plunger is pulled back, increasing the volume and decreasing the pressure inside.

Accepted Answer

A syringe plunger is pulled back, increasing the volume and decreasing the pressure inside.

Question 17

A 1.00 L flask contains 0.0400 mol of nitrogen gas at 27°C. What is the pressure in the flask? (R = 0.0821 L·atm/(mol·K))
Correct answer: 0.984 atm

Accepted Answer

0.984 atm

Question 18

Which of the following best explains why temperature must be converted to Kelvin when using the gas laws?
Correct answer: Kelvin is the only temperature scale that starts at absolute zero, ensuring proportionality in the gas laws.

Accepted Answer

Kelvin is the only temperature scale that starts at absolute zero, ensuring proportionality in the gas laws.

Question 19

A 3.00 L container holds a gas at 2.00 atm and 273 K. If the gas is transferred to a 6.00 L container at 546 K, what is the new pressure?
Correct answer: 1.00 atm

Accepted Answer

1.00 atm

Key Concepts of Gases and Gas Laws

Study Guide - Practice Questions

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