Question 1

According to the Kinetic Molecular Theory, which of the following statements best explains why gases are easily compressed?

Accepted Answer

The actual volume occupied by gas molecules is extremely small compared to the volume the gas occupies.

Question 2

A weather balloon is released at sea level where the atmospheric pressure is 1 atm. As it rises to a higher altitude, what happens to the atmospheric pressure and why?

Accepted Answer

Atmospheric pressure decreases because there are fewer gas particles at higher altitudes.

Question 3

Which of the following is the correct relationship described by Boyle’s Law?

Accepted Answer

$$P_1V_1 = P_2V_2$$

Question 4

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

Accepted Answer

4.0 L

Question 5

Which of the following units is NOT commonly used to measure gas pressure?

Accepted Answer

mL

Question 6

A gas sample has a volume of 500 mL at 25°C. What will the volume be at 75°C, assuming pressure and amount of gas remain constant? (Use Charles’s Law.)

Accepted Answer

583 mL

Question 7

Why must temperatures be converted to Kelvin when using gas law equations?

Accepted Answer

Because the Kelvin scale starts at absolute zero, making all temperatures positive and proportional to kinetic energy.

Question 8

A gas has a pressure of 500 mmHg at 300 K. If the temperature increases to 600 K (with constant volume and amount), what is the new pressure?

Accepted Answer

1000 mmHg

Question 9

Which of the following best explains why water boils at a lower temperature in the mountains than at sea level?

Accepted Answer

The atmospheric pressure is lower in the mountains, so the vapor pressure of water equals atmospheric pressure at a lower temperature.

Question 10

A rigid container holds a gas at 2.0 atm and 300 K. If the temperature is increased to 450 K, what is the final pressure? (Assume the amount and volume of gas remain constant.)

Accepted Answer

3.0 atm

Question 11

Which property of a gas is directly proportional to its average kinetic energy?

Accepted Answer

Temperature (in Kelvin)

Question 12

A sample of gas is compressed from 10.0 L to 2.0 L at constant temperature. If the initial pressure was 1.0 atm, what is the final pressure?

Accepted Answer

5.0 atm

Question 13

Which of the following is the correct formula for Gay-Lussac’s Law?

Accepted Answer

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

Question 14

A gas sample at 300 K and 1.0 atm is heated to 600 K in a rigid container. What happens to the pressure?

Accepted Answer

It doubles to 2.0 atm.

Question 15

If a gas occupies 3.0 L at 27°C, what volume will it occupy at 127°C, assuming constant pressure and amount? (Use Charles’s Law.)

Accepted Answer

4.0 L

Question 16

Which of the following is NOT a postulate of the Kinetic Molecular Theory of Gases?

Accepted Answer

Gas particles are attracted to each other by strong forces.

Question 17

A scuba diver’s tank contains air at 200 atm in a 10 L tank. If the air is released into a balloon at 1 atm, what is the maximum volume the air could occupy? (Assume constant temperature.)

Accepted Answer

2000 L

Question 18

Which of the following best describes the effect of increasing the temperature of a gas in a flexible container?

Accepted Answer

The volume increases because the gas particles move faster and exert more pressure.

Question 19

A gas sample has a pressure of 750 mmHg at 20°C. What is the pressure at 60°C, assuming constant volume and amount? (Use Gay-Lussac’s Law.)

Accepted Answer

850 mmHg

Question 20

Which of the following is a correct pressure equality?

Accepted Answer

1 atm = 760 mmHg

Gas Laws and Properties: Kinetic Molecular Theory, Boyle’s, Charles’s, and Gay-Lussac’s Laws

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