Q: Which equation represents the combined gas law?

$$\\frac{P_1$ V_1$}{T_1$} = \\frac{P_2$ V_2$}{T_2$}$$

Q: Which of the following is the correct value and units for the ideal gas constant $$R$$?

$$0.0821 \\ \text{L} \\cdot \\text{atm} / (\\text{mol} \\cdot \\text{K})$$

Question 1

A child is drinking soda through a straw. What is the primary reason the liquid rises up the straw when the child sucks on it?

Accepted Answer

Atmospheric pressure outside the straw pushes the liquid up due to the lower pressure inside the straw.

Question 2

Why is it impossible to drink from a straw longer than about 10.3 meters at sea level, even with a perfect vacuum inside the straw?

Accepted Answer

The weight of the liquid column would exceed atmospheric pressure, preventing further rise.

Question 3

According to the kinetic molecular theory, which of the following statements is FALSE?

Accepted Answer

Gas particles attract and repel each other strongly.

Question 4

Which property of gases allows them to be compressed much more than liquids?

Accepted Answer

There is a large amount of empty space between gas particles.

Question 5

A barometer measures atmospheric pressure by the height of a mercury column. If the atmospheric pressure is 1 atm, what is the height of the mercury column in mm Hg?

Accepted Answer

$$760 \ 	ext{ mm Hg}$$

Question 6

Convert a pressure of $$0.311$$ atm to mm Hg.

Accepted Answer

$$236 \ 	ext{ mm Hg}$$

Question 7

A scuba diver at a depth of 20 m breathes air at 3 atm. If the diver holds their breath and ascends to the surface (1 atm), 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 8

A gas occupies $$6.0 L at$$ $$4.0$$ atm. What will its volume be if the pressure is reduced to $$1.0$$ atm, assuming constant temperature?

Accepted Answer

$$24 \ 	ext{ L}$$

Question 9

A sample of gas has a volume of $$2.80 L at an $$unknown temperature. When cooled to $$0^{\circ}C$, its volume is 2.57$ L. What was the initial temperature in kelvins?

Accepted Answer

$$297 \ 	ext{ K}$$

Question 10

Which equation represents the combined gas law?

Accepted Answer

$$\frac{P_1$ V_1$}{T_1$} = \frac{P_2$ V_2$}{T_2$}$$

Question 11

A $$4.8-L $$sample of helium contains $$0.22$$ mol. How many additional moles are needed to expand the volume to $$6.4 L at $$constant temperature and pressure?

Accepted Answer

$$0.07 \ 	ext{mol}$$

Question 12

Which of the following is the correct value and units for the ideal gas constant $$R$$?

Accepted Answer

$$0.0821 \ 	ext{L} \cdot \text{atm} / (\text{mol} \cdot \text{K})$$

Question 13

Calculate the volume occupied by $$0.845$$ mol of nitrogen gas at $$1.37$$ atm and $$315 K.$$

Accepted Answer

$$16.0 \ 	ext{L}$$

Question 14

A mixture of helium, neon, and argon has a total pressure of $$558 mm Hg. If $$the partial pressures of helium and neon are $$341 mm Hg $$and $$112 mm Hg$$, respectively, what is the partial pressure of argon?

Accepted Answer

$$105 \ 	ext{mm Hg}$$

Question 15

At a depth of 90 m, a diver breathes a heliox mixture containing 2.0% oxygen at a total pressure of 10.0 atm. What is the partial pressure of oxygen?

Accepted Answer

$$0.20 \ 	ext{atm}$$

Question 16

Which of the following best explains why hot air balloons rise?

Accepted Answer

Hot air is less dense than cooler air, so the balloon floats.

Question 17

Which of the following is NOT a major gaseous air pollutant discussed in the study materials?

Accepted Answer

Methane (CH4)

Question 18

A sample of gas has a mass of $$0.136 g$$, a volume of $$0.112 L$$, a temperature of $$298 K$$, and a pressure of $$1.06$$ atm. What is the molar mass of the gas?

Accepted Answer

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

Chapter 11: Gases – Properties, Laws, and Applications

Study Guide - Practice Questions

Study Guide - Flashcards