Q: A 2.00 L container holds a gas at 3.00 atm and 300 K. If the temperature is increased to 600 K and the volume is doubled, what will be the new pressure of the gas (in atm)?

$$P_2$$ = \frac{3.00 \times 2.00 \times 600}{300 \times 4.00} = 3.00$$ atm

Q: A sample of nitrogen dioxide gas at 130°C and 315 torr occupies a volume of 1750 mL. What will the gas pressure be if the volume is reduced to 320 mL at 130°C?

$$P_2$$ = \frac{$$P_1$$ $$V_1$$}{$$V_2$$} = \frac{315 \times 1750}{320} = 1722$$ torr

Q: Which of the following is the correct formula for the partial pressure of a gas in a mixture, using the Ideal Gas Law?

$$P_{\text{gas}} = \frac{n_{\text{gas}}RT}{V}$$

Question 1

Which of the following best describes the relationship between pressure and volume for a fixed amount of gas at constant temperature, according to Boyle's Law?

Accepted Answer

Pressure and volume are inversely proportional.

Question 2

A 2.00 L container holds a gas at 3.00 atm and 300 K. If the temperature is increased to 600 K and the volume is doubled, what will be the new pressure of the gas (in atm)?

Accepted Answer

$$P_2$$ = \frac{3.00 	imes 2.00 	imes 600}{300 	imes 4.00} = 3.00$$ atm

Question 3

Which of the following is the correct SI unit for pressure, named after a French mathematician?

Accepted Answer

Pascal

Question 4

A 0.150 L flask contains carbon dioxide gas at 525 mmHg and 32°C. How many grams of CO$$_2$$ are present? (R = 0.08206 L·atm·mol$$^{-1}$$·K$$^{-1}$$, 1 atm = 760 mmHg, molar mass CO$$_2 = 44.01 g/$$mol)

Accepted Answer

0.187 g

Question 5

Which of the following statements about the Ideal Gas Law is correct?

Accepted Answer

It relates pressure, volume, temperature, and number of moles of a gas.

Question 6

A sample of nitrogen dioxide gas at 130°C and 315 torr occupies a volume of 1750 mL. What will the gas pressure be if the volume is reduced to 320 mL at 130°C?

Accepted Answer

$$P_2$$ = \frac{$$P_1$$ $$V_1$$}{$$V_2$$} = \frac{315 	imes 1750}{320} = 1722$$ torr

Question 7

Which of the following best represents the relationship between the partial pressure of a gas (P) and the number of moles of that gas (n) in a mixture, assuming constant volume and temperature?

Accepted Answer

A straight line with positive slope passing through the origin

Question 8

A sealed container with a movable piston contains a gas with a pressure of 1380 torr, a volume of 820 mL, and a temperature of 31°C. What would the volume be if the new pressure is now 2.83 atm, while the temperature decreased to 25°C? (1 atm = 760 torr)

Accepted Answer

0.472 L

Question 9

Which of the following is the correct formula for the partial pressure of a gas in a mixture, using the Ideal Gas Law?

Accepted Answer

$$P_{	ext{gas}} = \frac{n_{	ext{gas}}RT}{V}$$

Question 10

A sample of gas initially has a volume of 900 mL at 520 K and 1.85 atm. What is the pressure of the gas if the volume decreases to 330 mL, while the temperature increases to 770 K?

Accepted Answer

$$P_2$$ = \frac{$$P_1$$ $$V_1$$ $$T_2$$}{$$T_1$$ $$V_2$$} = \frac{1.85 	imes 900 	imes 770}{520 	imes 330} = 7.36$$ atm

Question 11

Which of the following best explains why it is dangerous to throw a nearly empty spray can into a fire?

Accepted Answer

The pressure inside the can will increase rapidly due to the temperature rise, possibly causing explosion.

Question 12

Which of the following is the correct value and units for the gas constant R when using the Ideal Gas Law with pressure in atm, volume in liters, and temperature in Kelvin?

Accepted Answer

$$R = 0.08206 L$$·atm·mol$$^{-1}$$·K$$^{-1}$$

Question 13

A 10.0 L cylinder with a movable piston contains 3.00 atm of pressure. What will happen to the pressure if the volume of the container increases to 20.0 L, assuming temperature and moles of gas remain constant?

Accepted Answer

It will decrease by half

Question 14

Which of the following gas laws states that the volume of a gas is directly proportional to the number of moles at constant temperature and pressure?

Accepted Answer

Avogadro's Law

Question 15

A sample of neon gas exerts a pressure of 1.85 atm inside a cylinder. Some nitrogen gas is also present, at a pressure of 500 torr. What is the total pressure inside the cylinder? (1 atm = 760 torr)

Accepted Answer

2.51 atm

Question 16

If the number of moles (n) inside a container were tripled while keeping the pressure (P) constant, what will happen to the volume (V)?

Accepted Answer

It will triple

Question 17

A 500 mL container at a pressure of 600 mmHg possesses 22.3 g nitrogen gas at 50°C. Which of the following is the correct set of units to use for the Ideal Gas Law calculation?

Accepted Answer

Pressure in atm, volume in L, temperature in K

Question 18

Which of the following is the correct formula for the mole fraction (X) of a component in a mixture?

Accepted Answer

$$X = \frac{	ext{moles of component}}{	ext{total moles}}$$

Gas Laws and Properties of Gases: Study Notes for General Chemistry

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