Q: A sample of nitrogen gas is contained in a 10.0 L vessel at a pressure of 2.00 atm. If the volume is decreased to 5.00 L at constant temperature, what is the new pressure?

$$P_2$$ = \frac{$$P_1$$ $$V_1$$}{$$V_2$$} = \frac{2.00 \times 10.0}{5.00} = 4.00\ \text{atm}$$

Q: A gas sample has a pressure of 645 Torr at 128°C. If the pressure increases to 824 Torr and the volume and amount of gas remain constant, what is the new temperature in Kelvin?

$$T_2$$ = \frac{$$P_2$$ $$T_1$$}{$$P_1$$} = \frac{824 \times (128 + 273)}{645} = 513\ \text{K}$$

Q: A sample of oxygen gas has a volume of 420 mL at 18°C. At what temperature (in °C) will the volume be 640 mL, assuming pressure and amount are constant?

$$T_2$$ = \frac{$$V_2$$ $$T_1$$}{$$V_1$$} = \frac{640 \times (18 + 273)}{420} = 442\ \text{K} = 169\ ^\circ\text{C}$$

Q: A gas is collected in a rigid container at 1.00 atm and 300 K. If the temperature is increased to 600 K, what is the final pressure?

$$P_2$$ = \frac{$$P_1$$ $$T_2$$}{$$T_1$$} = \frac{1.00 \times 600}{300} = 2.00\ \text{atm}$$

Q: Which of the following is a correct pressure equality?

$$1\ \text{atm} = 760\ \text{mmHg}$$

Q: A gas sample is transferred from a 2.0 L container to a 6.0 L container at constant temperature and amount. If the initial pressure was 900 mmHg, what is the final pressure?

$$P_2$$ = \frac{$$P_1$$ $$V_1$$}{$$V_2$$} = \frac{900 \times 2.0}{6.0} = 300\ \text{mmHg}$$

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 sample of nitrogen gas is contained in a 10.0 L vessel at a pressure of 2.00 atm. If the volume is decreased to 5.00 L at constant temperature, what is the new pressure?

Accepted Answer

$$P_2$$ = \frac{$$P_1$$ $$V_1$$}{$$V_2$$} = \frac{2.00 	imes 10.0}{5.00} = 4.00\ 	ext{atm}$$

Question 3

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

Accepted Answer

$$\frac{V_1$}{T_1$} = \frac{V_2$}{T_2$}$$

Question 4

A gas sample has a pressure of 645 Torr at 128°C. If the pressure increases to 824 Torr and the volume and amount of gas remain constant, what is the new temperature in Kelvin?

Accepted Answer

$$T_2$$ = \frac{$$P_2$$ $$T_1$$}{$$P_1$$} = \frac{824 	imes (128 + 273)}{645} = 513\ 	ext{K}$$

Question 5

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 at higher altitudes, so water molecules require less energy to escape into the gas phase.

Question 6

If a gas is heated from 200 K to 400 K at constant volume and amount, what happens to the pressure?

Accepted Answer

The pressure doubles.

Question 7

Which of the following is NOT a correct unit of pressure?

Accepted Answer

L

Question 8

A sample of oxygen gas has a volume of 420 mL at 18°C. At what temperature (in °C) will the volume be 640 mL, assuming pressure and amount are constant?

Accepted Answer

$$T_2$$ = \frac{$$V_2$$ $$T_1$$}{$$V_1$$} = \frac{640 	imes (18 + 273)}{420} = 442\ 	ext{K} = 169\ ^\circ	ext{C}$$

Question 9

Which property of a gas is directly proportional to its Kelvin temperature, according to the Kinetic Molecular Theory?

Accepted Answer

Average kinetic energy

Question 10

A gas is collected in a rigid container at 1.00 atm and 300 K. If the temperature is increased to 600 K, what is the final pressure?

Accepted Answer

$$P_2$$ = \frac{$$P_1$$ $$T_2$$}{$$T_1$$} = \frac{1.00 	imes 600}{300} = 2.00\ 	ext{atm}$$

Question 11

Which of the following best describes the effect of decreasing the volume of a gas at constant temperature and amount?

Accepted Answer

The pressure increases because the gas particles collide with the walls more frequently.

Question 12

Which of the following is a correct pressure equality?

Accepted Answer

$$1\ 	ext{atm} = 760\ 	ext{mmHg}$$

Question 13

A gas sample is transferred from a 2.0 L container to a 6.0 L container at constant temperature and amount. If the initial pressure was 900 mmHg, what is the final pressure?

Accepted Answer

$$P_2$$ = \frac{$$P_1$$ $$V_1$$}{$$V_2$$} = \frac{900 	imes 2.0}{6.0} = 300\ 	ext{mmHg}$$

Question 14

Which of the following is the best example of a real-life application of Boyle’s Law?

Accepted Answer

A syringe draws in liquid when the plunger is pulled back, increasing the volume and decreasing the pressure inside.

Question 15

Which of the following statements about gas pressure is FALSE?

Accepted Answer

Gas pressure increases as the volume of the container increases (at constant temperature and amount).

Gas Laws and Properties: Study Notes for GOB Chemistry

Study Guide - Practice Questions

Study Guide - Flashcards