Question 1

A scuba diver descends to a depth where the pressure is 3.00 atm. If the diver inhales 2.00 L of air at the surface (1.00 atm), what will be the volume of this air in the diver's lungs at depth, assuming temperature remains constant?

Accepted Answer

$$0.667\ \mathrm{L}$$

Question 2

Which of the following statements is NOT an assumption of the kinetic molecular theory (KMT) of gases?

Accepted Answer

Gas molecules are attracted to each other by strong forces.

Question 3

A sample of gas occupies $$500.0\ \mathrm{mL} at$$ $$25^\circ\mathrm{C}$$ and $$1.00\ \mathrm{atm}. $$What will its volume be at $$100^\circ\mathrm{C}$$ and $$1.00\ \mathrm{atm}$$?

Accepted Answer

$$635\ \mathrm{mL}$$

Question 4

Which gas will effuse the fastest under identical conditions, according to Graham's law?

Accepted Answer

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

Question 5

A 0.250 mol sample of gas is contained in a 5.00 L vessel at $$27^\circ\mathrm{C}. $$What is the pressure of the gas in atm? ($$R = 0.0821\ \mathrm{L\cdot atm\cdot $$mol^{-1}$$\cdot K$$^{-1}$$})$$

Accepted Answer

$$1.23\ \mathrm{atm}$$

Question 6

A gas sample has a mass of $$2.80\ \mathrm{g}$$ and occupies $$1.50\ \mathrm{L} at$$ $$25^\circ\mathrm{C}$$ and $$1.00\ \mathrm{atm}. $$What is the molar mass of the gas?

Accepted Answer

$$45.7\ \mathrm{g/mol}$$

Question 7

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

Accepted Answer

Gas molecules are far apart compared to their size, so the volume can decrease significantly under pressure.

Question 8

A weather report states that the atmospheric pressure is $$30.44\ \mathrm{in\ Hg}. $$What is this pressure in $$\mathrm{atm}$$? ($$1\ \mathrm{atm} = 29.92\ \mathrm{in\ Hg})$$

Accepted Answer

$$1.02\ \mathrm{atm}$$

Question 9

If the temperature of a fixed amount of gas is doubled (in Kelvin) at constant pressure, what happens to the volume?

Accepted Answer

The volume doubles.

Question 10

A 1.00 L sample of gas at STP has a mass of $$1.25\ \mathrm{g}. $$What is the molar mass of the gas?

Accepted Answer

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

Question 11

Which of the following changes will increase the pressure of a gas in a rigid container?

Accepted Answer

Increasing the temperature.

Question 12

A gas sample is collected in a rigid 2.00 L container at $$300\ \mathrm{K}$$ and $$2.00\ \mathrm{atm}. If $$the temperature is increased to $$600\ \mathrm{K}$$, what is the new pressure?

Accepted Answer

$$4.00\ \mathrm{atm}$$

Question 13

A hot spring emits a gas that effuses at 0.342 times the rate of helium ($$M_{\mathrm{He}} = 4.00\ \mathrm{g/mol}). $$What is the molar mass of the unknown gas?

Accepted Answer

$$34.2\ \mathrm{g/mol}$$

Question 14

Which of the following best describes diffusion of a gas?

Accepted Answer

The spread of one gas through another.

Question 15

A 5.00 L container holds 0.200 mol of oxygen gas at $$27^\circ\mathrm{C}. $$What is the density of the gas in $$\mathrm{g/L}$$? ($$M_{\mathrm{O}_2$$} = 32.0\ \mathrm{g/mol}$$)

Accepted Answer

$$1.28\ \mathrm{g/L}$$

Question 16

Which of the following is a correct statement about the relationship between molar mass and the rate of effusion?

Accepted Answer

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

Question 17

A 10.0 L tank contains nitrogen gas at $$2.00\ \mathrm{atm}$$ and $$300\ \mathrm{K}. $$How many moles of nitrogen are present? ($$R = 0.0821\ \mathrm{L\cdot atm\cdot $$mol^{-1}$$\cdot K$$^{-1}$$})$$

Accepted Answer

$$0.813\ \mathrm{mol}$$

Question 18

Which of the following best explains why helium balloons deflate faster than air-filled balloons?

Accepted Answer

Helium atoms are lighter and effuse more rapidly through small holes in the balloon.

Question 19

A 2.00 L sample of gas at $$1.00\ \mathrm{atm}$$ and $$273\ \mathrm{K}$$ contains how many molecules?

Accepted Answer

$$5.38 	imes 10$$^{22}$$

Question 20

Which of the following is the correct value for the molar volume of an ideal gas at STP (0°C, 1 atm)?

Accepted Answer

$$22.4\ \mathrm{L}$$

Properties of Gases and the Kinetic Molecular Theory

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