Question 1

A scuba diver at a depth of 20 m breathes air at a pressure of 3 atm. If the diver ascends rapidly to the surface (1 atm) while holding their breath, what happens to the volume of air in their lungs according to Boyle’s Law?

Accepted Answer

The volume increases by a factor of 3.

Question 2

Which of the following best explains why gases are compressible but liquids are not, according to the kinetic molecular theory?

Accepted Answer

There is a lot of empty space between gas particles.

Question 3

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

Accepted Answer

$$1.0\ \mathrm{L}$$

Question 4

Which of the following is the correct mathematical expression for Charles’s Law?

Accepted Answer

$$V_1$$/$$T_1$$ = $$V_2$$/$$T_2$$

Question 5

A 2.0 L sample of gas at 300 K is heated to 600 K at constant pressure. What is the final volume?

Accepted Answer

$$4.0\ \mathrm{L}$$

Question 6

Which of the following statements about atmospheric pressure and drinking through a straw is correct?

Accepted Answer

Atmospheric pressure pushes the liquid up the straw when the pressure inside is reduced.

Question 7

Convert a pressure of $$0.500\ \mathrm{atm} to mm Hg.$$

Accepted Answer

$$380\ \mathrm{mm\ Hg}$$

Question 8

A mixture of gases contains 70% nitrogen and 30% oxygen by volume at a total pressure of 1.0 atm. What is the partial pressure of oxygen?

Accepted Answer

$$0.30\ \mathrm{atm}$$

Question 9

Which of the following is NOT an assumption of the kinetic molecular theory for ideal gases?

Accepted Answer

Gas particles attract and repel each other strongly.

Question 10

A 0.50 mol sample of gas occupies 12.0 L at 300 K. What is the pressure in atm? (Use $$R = 0.0821\ \mathrm{L\ atm\ $$mol^{-1}$$\ K$$^{-1}$$})$$

Accepted Answer

$$0.51\ \mathrm{atm}$$

Question 11

A sample of hydrogen gas is collected over water at 25°C and a total pressure of 755 mm Hg. If the vapor pressure of water at 25°C is 24 mm Hg, what is the partial pressure of hydrogen gas?

Accepted Answer

$$731\ \mathrm{mm\ Hg}$$

Question 12

Which of the following best describes why a hot air balloon rises?

Accepted Answer

Heating the air decreases its density, causing it to float in cooler, denser air.

Question 13

A 5.0 L sample of gas at 1.0 atm and 273 K is compressed to 2.5 L and heated to 546 K. What is the final pressure?

Accepted Answer

$$2.0\ \mathrm{atm}$$

Question 14

Which of the following is the correct expression for the ideal gas law?

Accepted Answer

$$PV = nRT$$

Question 15

A sample of gas has a mass of 0.200 g, a volume of 0.100 L, a temperature of 300 K, and a pressure of 1.00 atm. What is the molar mass of the gas? (Use $$R = 0.0821\ \mathrm{L\ atm\ $$mol^{-1}$$\ K$$^{-1}$$})$$

Accepted Answer

$$49.2\ \mathrm{g/mol}$$

Question 16

Which of the following is a real-world consequence of Dalton’s law of partial pressures?

Accepted Answer

The total pressure in a scuba tank is the sum of the partial pressures of all gases present.

Question 17

A mixture of helium, neon, and argon has a total pressure of 600 mm Hg. If the partial pressures of helium and neon are 300 mm Hg and 200 mm Hg, respectively, what is the partial pressure of argon?

Accepted Answer

$$100\ \mathrm{mm\ Hg}$$

Question 18

Which of the following pollutants is primarily responsible for the formation of acid rain?

Accepted Answer

Sulfur dioxide

Question 19

At STP, what volume is occupied by 2.00 mol of an ideal gas?

Accepted Answer

$$44.8\ \mathrm{L}$$

Question 20

A balloon contains 0.50 mol of gas and occupies 12.0 L. If you add enough gas to double the number of moles at constant temperature and pressure, what will be the new volume?

Accepted Answer

$$24.0\ \mathrm{L}$$

Study Guide: Gases and Their Properties (Chapter 11, Introductory Chemistry)

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