Question 1

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

Accepted Answer

$$2.0\ \mathrm{L}$$

Question 2

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

Accepted Answer

Helium has a lower density than air at the same temperature and pressure.

Question 3

A sample of gas occupies $$4.00\ \mathrm{L} at$$ $$300\ \mathrm{K}. $$What will its volume be at $$600\ \mathrm{K}$$, assuming constant pressure and amount of gas?

Accepted Answer

$$8.00\ \mathrm{L}$$

Question 4

Which of the following actions will increase the volume of a gas sample, assuming constant temperature and number of moles?

Accepted Answer

Decreasing the pressure.

Question 5

A $$2.00\ \mathrm{g}$$ sample of hydrogen gas ($$\mathrm{H}_2) $$and a $$2.00\ \mathrm{g}$$ sample of oxygen gas ($$\mathrm{O}_2) $$are placed in separate, identical containers at STP. Which gas has the greater volume?

Accepted Answer

Both have the same volume.

Question 6

A mixture contains $$2.0$$ moles of nitrogen and $$3.0$$ moles of oxygen at a total pressure of $$5.0\ \mathrm{atm}. $$What is the partial pressure of oxygen?

Accepted Answer

$$3.0\ \mathrm{atm}$$

Question 7

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

Accepted Answer

Gas particles lose energy during collisions.

Question 8

At the same temperature, which gas will have the highest root mean square velocity ($$u_{\mathrm{rms}}$$)?

Accepted Answer

Hydrogen ($$\mathrm{H}_2)$$

Question 9

A $$5.00\ \mathrm{L}$$ container holds $$0.200\ \mathrm{mol} of an $$ideal gas at $$300\ \mathrm{K}. $$What is the pressure inside the container? (Use $$R = 0.0821\ \mathrm{L\cdot atm\cdot $$mol^{-1}$$\cdot K$$^{-1}$$})$$

Accepted Answer

$$0.984\ \mathrm{atm}$$

Question 10

Which of the following best describes the behavior of real gases compared to ideal gases at high pressures?

Accepted Answer

The molar volume of a real gas is greater than that predicted by the ideal gas law.

Question 11

A gas sample has a density of $$1.25\ \mathrm{g/L} at $$STP. What is its molar mass?

Accepted Answer

$$28.0\ \mathrm{g/mol}$$

Question 12

Which of the following gases will diffuse the fastest at room temperature?

Accepted Answer

Hydrogen ($$\mathrm{H}_2)$$

Question 13

A $$10.0\ \mathrm{L}$$ container contains $$0.50\ \mathrm{mol} of$$ $$\mathrm{O}_2$$ and $$0.50\ \mathrm{mol} of$$ $$\mathrm{N}_2 at$$ $$300\ \mathrm{K}. $$What is the total pressure in the container?

Accepted Answer

$$2.46\ \mathrm{atm}$$

Question 14

Which of the following is a correct statement of Dalton’s Law of Partial Pressures?

Accepted Answer

The total pressure of a mixture of gases is the sum of the partial pressures of each individual gas.

Question 15

If the temperature of a gas is doubled at constant pressure, what happens to its volume?

Accepted Answer

The volume doubles.

Question 16

A $$1.00\ \mathrm{L}$$ flask contains $$0.040\ \mathrm{mol} of a $$gas at $$27.0^\circ\mathrm{C}. $$What is the pressure in the flask? ($$R = 0.0821\ \mathrm{L\cdot atm\cdot $$mol^{-1}$$\cdot K$$^{-1}$$})$$

Accepted Answer

$$0.98\ \mathrm{atm}$$

Question 17

Which of the following best explains why the pressure of a real gas is lower than that predicted by the ideal gas law at low temperatures?

Accepted Answer

Intermolecular attractions cause gas particles to collide with the walls less frequently.

Question 18

A mixture of $$2.0$$ moles of helium and $$2.0$$ moles of neon is in a $$10.0\ \mathrm{L}$$ container at $$273\ \mathrm{K}. $$What is the mole fraction of helium in the mixture?

Accepted Answer

$$0.50$$

Question 19

According to Graham’s law, what is the ratio of the rate of effusion of hydrogen ($$\mathrm{H}_2) to $$that of oxygen ($$\mathrm{O}_2$$)? ($$M_{\mathrm{H}_2$$} = 2.0\ \mathrm{g/mol}$$, M$$_{\mathrm{O}$$_2} = 32.0\ \mathrm{g/mol})$$

Accepted Answer

$$4:1$$

Chapter 6: Gases – Properties, Laws, and Real Gas Behavior

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