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 decreases to -10°C. Assuming the amount of gas in the balloon remains constant and the balloon is flexible, which of the following best describes what happens to the volume of the balloon as it rises?
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 atmospheric pressure decreases with increasing altitude?
Correct answer: There are fewer gas molecules per unit volume at higher altitudes, resulting in fewer molecular collisions and lower pressure.

Accepted Answer

There are fewer gas molecules per unit volume at higher altitudes, resulting in fewer molecular collisions and lower pressure.

Question 3

A scuba diver uses a tank containing 12.0 L of compressed air at 200 atm. If the air is released at the surface where the pressure is 1.0 atm and the temperature remains constant, what volume will the air occupy? (Assume ideal gas behavior.)
Correct answer: 2,400 L

Accepted Answer

2,400 L

Question 4

Which of the following is the correct conversion for a pressure of 500 mm Hg to atmospheres (atm)?
Correct answer: 0.658 atm

Accepted Answer

0.658 atm

Question 5

A sealed syringe contains 0.050 mol of oxygen gas at 1.0 atm and 300 K. If the plunger is pulled out to double the volume while keeping the temperature constant, what is the new pressure inside the syringe?
Correct answer: 0.50 atm

Accepted Answer

0.50 atm

Question 6

A patient is administered oxygen at a pressure of 2.0 atm in a hyperbaric chamber. If the chamber has a volume of 5.0 L and the temperature is 27°C, how many moles of oxygen are present? (R = 0.0821 L·atm/(mol·K))
Correct answer: 0.41 mol

Accepted Answer

0.41 mol

Question 7

Which of the following best describes the relationship between the number of moles of gas and the volume it occupies at constant temperature and pressure?
Correct answer: The volume is directly proportional to the number of moles.

Accepted Answer

The volume is directly proportional to the number of moles.

Question 8

A tire is inflated to a pressure of 32 psi. What is this pressure in atmospheres? (1 atm = 14.7 psi)
Correct answer: 2.18 atm

Accepted Answer

2.18 atm

Question 9

A 2.0 L container holds a gas at 3.0 atm and 400 K. If the gas is compressed to 1.0 L and heated to 600 K, what is the new pressure? (Assume the amount of gas is constant.)
Correct answer: 9.0 atm

Accepted Answer

9.0 atm

Question 10

Which of the following real-life scenarios best illustrates Boyle’s Law?
Correct answer: A syringe plunger is pulled back, increasing the volume and causing the pressure inside to decrease.

Accepted Answer

A syringe plunger is pulled back, increasing the volume and causing the pressure inside to decrease.

Question 11

A sample of gas occupies 10.0 L at 27°C and 1.0 atm. What will be its volume at 127°C and 1.0 atm?
Correct answer: 13.3 L

Accepted Answer

13.3 L

Question 12

Which of the following is NOT a correct statement about atmospheric pressure?
Correct answer: Atmospheric pressure is higher at the top of Mount Everest than at sea level.

Accepted Answer

Atmospheric pressure is higher at the top of Mount Everest than at sea level.

Question 13

A gas sample at 25°C and 1.00 atm has a volume of 2.50 L. How many moles of gas are present? (R = 0.0821 L·atm/(mol·K))
Correct answer: 0.10 mol

Accepted Answer

0.10 mol

Question 14

Which of the following best explains why it is important to use Kelvin rather than Celsius in gas law calculations?
Correct answer: Kelvin is an absolute temperature scale, so zero Kelvin corresponds to zero kinetic energy, preventing negative values in calculations.

Accepted Answer

Kelvin is an absolute temperature scale, so zero Kelvin corresponds to zero kinetic energy, preventing negative values in calculations.

Question 15

A 5.0 L tank contains nitrogen gas at 2.0 atm and 300 K. If 0.50 mol of nitrogen is added to the tank without changing the volume or temperature, what is the new pressure? (Assume initial moles = 0.41 mol; R = 0.0821 L·atm/(mol·K))
Correct answer: 4.44 atm

Accepted Answer

4.44 atm

Question 16

Which of the following is a correct application of Avogadro’s Law?
Correct answer: Doubling the number of moles of gas in a container at constant temperature and pressure will double the volume.

Accepted Answer

Doubling the number of moles of gas in a container at constant temperature and pressure will double the volume.

Question 17

A hospital stores oxygen in a 50.0 L tank at 150 atm and 298 K. How many grams of O2 are in the tank? (R = 0.0821 L·atm/(mol·K); molar mass O2 = 32.0 g/mol)
Correct answer: 3,060 g

Accepted Answer

3,060 g

Question 18

Which of the following best describes the cause of gas pressure in a container?
Correct answer: Gas pressure results from collisions of gas molecules with the walls of the container.

Accepted Answer

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

Question 19

A gas occupies 4.0 L at 300 K and 2.0 atm. If the temperature is increased to 600 K and the pressure is decreased to 1.0 atm, what is the final volume?
Correct answer: 16.0 L

Accepted Answer

16.0 L

Key Concepts of Gas Laws and Atmospheric Pressure

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