Question 1

A diver descends to a depth where the pressure is 4 atm. If the diver inhales 2.0 L of air at this depth and then ascends to the surface (1 atm) without exhaling, what will be the volume of the air in the diver’s lungs at the surface? (Assume temperature is constant.)

Accepted Answer

$$8.0\ \mathrm{L}$$

Question 2

A sample of gas occupies $$3.00\ \mathrm{L} at$$ $$25^\circ\mathrm{C}$$ and $$1.00\ \mathrm{atm}. $$What will its volume be at $$75^\circ\mathrm{C}$$ and $$1.00\ \mathrm{atm}$$?

Accepted Answer

$$3.51\ \mathrm{L}$$

Question 3

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

Accepted Answer

The density of the air inside the balloon decreases as temperature increases, making it less dense than the surrounding air.

Question 4

A 5.00 L container holds $$0.250$$ mol of oxygen gas at $$300\ \mathrm{K}. $$What is the pressure inside the container? $$(R = 0.08206\ \mathrm{L\ atm\ $$mol^{-1}$$\ K$$^{-1}$$})$$

Accepted Answer

$$1.23\ \mathrm{atm}$$

Question 5

A high-performance bicycle tire is inflated to $$132\ \mathrm{psi}. $$What is this pressure in $$\mathrm{mmHg}$$? $$(1\ \mathrm{atm} = 14.7\ \mathrm{psi}, 1\ \mathrm{atm} = 760\ \mathrm{mmHg})$$

Accepted Answer

$$6,820\ \mathrm{mmHg}$$

Question 6

A mixture of gases contains $$2.0$$ mol $$\mathrm{N_2$}$$, $$1.0$$ mol $$\mathrm{O_2$}$$, and $$1.0$$ mol $$\mathrm{CO_2$} in a$$ $$10.0\ \mathrm{L}$$ 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

$$0.246\ \mathrm{atm}$$

Question 7

A $$0.133 g $$sample of helium gas is placed in a $$648 mL $$container at $$32^\circ\mathrm{C}. $$What is the pressure in $$\mathrm{mmHg}$$? $$(R = 0.08206\ \mathrm{L\ atm\ $$mol^{-1}$$\ K$$^{-1}$$},\ \mathrm{molar\ mass\ He} = 4.00\ \mathrm{g/mol})$$

Accepted Answer

$$98.6\ \mathrm{mmHg}$$

Question 8

Which of the following statements about real gases is TRUE?

Accepted Answer

Real gases deviate from ideal behavior at high pressures due to the finite volume of gas molecules.

Question 9

A $$1.00 L $$mixture of helium, neon, and argon has a total pressure of $$662\ \mathrm{mmHg} at$$ $$298\ \mathrm{K}. If $$the partial pressures of helium and neon are $$341\ \mathrm{mmHg}$$ and $$112\ \mathrm{mmHg}$$, respectively, what is the mass of argon present? $$(R = 0.08206\ \mathrm{L\ atm\ $$mol^{-1}$$\ K$$^{-1}$$},\ \mathrm{molar\ mass\ Ar} = 39.95\ \mathrm{g/mol})$$

Accepted Answer

$$0.89\ \mathrm{g}$$

Question 10

Which law explains why the volume of a gas increases when the number of moles increases at constant temperature and pressure?

Accepted Answer

Avogadro’s Law

Question 11

A gas is collected over water at $$25^\circ\mathrm{C}$$ and the total pressure is $$758.2\ \mathrm{mmHg}. If $$the vapor pressure of water at this temperature is $$23.78\ \mathrm{mmHg}$$, what is the pressure of the dry gas?

Accepted Answer

$$734.4\ \mathrm{mmHg}$$

Question 12

Which of the following best describes effusion?

Accepted Answer

The process by which gas molecules escape through a small hole into a vacuum.

Question 13

According to Graham’s law, how does the rate of effusion of hydrogen gas ($$\mathrm{H_2$}) $$compare to that of oxygen gas ($$\mathrm{O_2$}) at $$the same temperature?

Accepted Answer

Hydrogen effuses about four times faster than oxygen.

Question 14

A sample of gas has a volume of $$2.80\ \mathrm{L} at an $$unknown temperature. When the sample is submerged in ice water at $$0.00^\circ\mathrm{C}$$, its volume decreases to $$2.57\ \mathrm{L}. $$What was its initial temperature in $$^\circ\mathrm{C}$$?

Accepted Answer

$$24^\circ\mathrm{C}$$

Question 15

Which of the following is a correct statement of the kinetic molecular theory as it applies to ideal gases?

Accepted Answer

Gas particles are in constant, random motion and collisions are perfectly elastic.

Question 16

A $$3.24 L $$basketball is inflated to a total pressure of $$24.3$$ psi at $$25^\circ\mathrm{C}. $$How many moles of gas are in the basketball? $$(1\ \mathrm{atm} = 14.7\ \mathrm{psi},\ R = 0.08206\ \mathrm{L\ atm\ $$mol^{-1}$$\ K$$^{-1}$$})$$

Accepted Answer

$$0.219\ \mathrm{mol}$$

Question 17

Which of the following is the correct value for the molar volume of an ideal gas at STP?

Accepted Answer

$$22.4\ \mathrm{L}$$

Question 18

A reaction produces $$1.24\ \mathrm{L} of$$ $$\mathrm{H_2$}$$ gas at STP. How many grams of water are formed when this hydrogen reacts completely with oxygen? $$(\mathrm{molar\ mass\ H_2O} = 18.02\ \mathrm{g/mol})$$

Accepted Answer

$$0.998\ \mathrm{g}$$

Question 19

Which of the following best describes why the pressure inside a sealed container increases when the temperature is raised?

Accepted Answer

The average kinetic energy of the gas molecules increases, causing more frequent and forceful collisions with the container walls.

Chapter 5: Gases – Properties, Laws, and Applications

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