Question 1

A scuba diver descends to a depth where the pressure is 3 atm. If the diver's lungs have a volume of 6.0 L at the surface (1 atm), what will be the volume of the diver's lungs at this depth, assuming temperature is constant and the diver does not exhale?

Accepted Answer

$$2.0\ \mathrm{L}$$

Question 2

Which of the following best explains why gases are compressible, while solids and liquids are not?

Accepted Answer

Gas particles are far apart with a lot of empty space between them.

Question 3

A sample of gas occupies $$4.0\ \mathrm{L} at$$ $$2.0\ \mathrm{atm}$$ and $$300\ \mathrm{K}. If $$the pressure is decreased to $$1.0\ \mathrm{atm}$$ and the temperature is increased to $$600\ \mathrm{K}$$, what will be the new volume?

Accepted Answer

$$16.0\ \mathrm{L}$$

Question 4

Which of the following statements about the kinetic molecular theory is FALSE?

Accepted Answer

Gas particles lose energy when they collide with each other.

Question 5

A $$2.0\ \mathrm{g}$$ sample of helium gas is placed in a $$5.0\ \mathrm{L}$$ container at $$27\ ^\circ\mathrm{C}. $$What is the pressure in the container? ($$R = 0.08206\ \mathrm{L\ atm\ $$mol^{-1}$$\ K$$^{-1}$$})$$

Accepted Answer

$$2.4\ \mathrm{atm}$$

Question 6

Which of the following gases will effuse the fastest under identical conditions?

Accepted Answer

$$\mathrm{H_2$}$$

Question 7

A mixture of gases contains $$2.0\ \mathrm{mol} of$$ $$\mathrm{N_2$}$$, $$1.0\ \mathrm{mol} of$$ $$\mathrm{O_2$}$$, and $$1.0\ \mathrm{mol} of$$ $$\mathrm{Ar} in a$$ $$10.0\ \mathrm{L}$$ container at $$300\ \mathrm{K}. $$What is the partial pressure of $$\mathrm{O_2$}$$? ($$R = 0.08206\ \mathrm{L\ atm\ $$mol^{-1}$$\ K$$^{-1}$$})$$

Accepted Answer

$$2.46\ \mathrm{atm}$$

Question 8

Which of the following best describes the relationship between the density of a gas and its molar mass at STP?

Accepted Answer

Density is directly proportional to molar mass.

Question 9

A $$10.0\ \mathrm{L}$$ container holds a mixture of $$2.0\ \mathrm{mol}$$ $$\mathrm{N_2$}$$ and $$3.0\ \mathrm{mol}$$ $$\mathrm{O_2$} at$$ $$298\ \mathrm{K}. $$What is the total pressure in the container? ($$R = 0.08206\ \mathrm{L\ atm\ $$mol^{-1}$$\ K$$^{-1}$$})$$

Accepted Answer

$$12.2\ \mathrm{atm}$$

Question 10

A gas is collected over water at $$25\ ^\circ\mathrm{C}$$ and a total pressure of $$760\ \mathrm{mmHg}. If $$the vapor pressure of water at this temperature is $$23.8\ \mathrm{mmHg}$$, what is the partial pressure of the dry gas?

Accepted Answer

$$736.2\ \mathrm{mmHg}$$

Question 11

Which of the following is NOT a property of gases?

Accepted Answer

They have a fixed shape.

Question 12

A $$5.0\ \mathrm{L}$$ sample of gas at $$1.0\ \mathrm{atm}$$ and $$273\ \mathrm{K} is $$heated to $$546\ \mathrm{K} at $$constant pressure. What is the final volume?

Accepted Answer

$$10.0\ \mathrm{L}$$

Question 13

Which of the following equations correctly represents Boyle’s Law?

Accepted Answer

$$P_1$$ $$V_1$$ = $$P_2$$ $$V_2$$

Question 14

A $$1.0\ \mathrm{mol}$$ sample of an unknown gas occupies $$22.4\ \mathrm{L} at $$STP. What is the density of the gas if its molar mass is $$44.0\ \mathrm{g/mol}$$?

Accepted Answer

$$1.96\ \mathrm{g/L}$$

Question 15

Which of the following best describes Graham’s Law of Effusion?

Accepted Answer

The rate of effusion is inversely proportional to the square root of the molar mass.

Question 16

If the mole fraction of oxygen in air is $$0.21$$ and the total atmospheric pressure is $$1.00\ \mathrm{atm}$$, what is the partial pressure of oxygen?

Accepted Answer

$$0.21\ \mathrm{atm}$$

Question 17

A $$10.0\ \mathrm{g}$$ sample of an unknown gas occupies $$5.0\ \mathrm{L} at$$ $$2.0\ \mathrm{atm}$$ and $$300\ \mathrm{K}. $$What is the molar mass of the gas? ($$R = 0.08206\ \mathrm{L\ atm\ $$mol^{-1}$$\ K$$^{-1}$$})$$

Accepted Answer

$$24.6\ \mathrm{g/mol}$$

Chapter 6: Gases – Properties, Laws, and Applications

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