Q: Which of the following is the correct value for the ideal gas constant $$R$$ when using atmospheres, liters, moles, and kelvin?

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

Question 1

Which of the following best explains why you cannot drink from a straw longer than about 10.3 meters, even if the straw is perfectly sealed and rigid?

Accepted Answer

Atmospheric pressure can only support a column of liquid up to a certain height, which is about 10.3 meters for water.

Question 2

According to the kinetic molecular theory, which of the following statements is NOT true for an ideal gas?

Accepted Answer

Gas particles attract and repel each other strongly.

Question 3

A scuba diver at a depth of 20 m breathes air at 3 atm. If the diver holds their breath and ascends rapidly to the surface (1 atm), what happens to the volume of air in their lungs?

Accepted Answer

The volume increases by a factor of 3.

Question 4

Which equation correctly expresses Boyle’s Law?

Accepted Answer

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

Question 5

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

Accepted Answer

$$297\ 	ext{K}$$

Question 6

Which of the following is the correct value for the ideal gas constant $$R$$ when using atmospheres, liters, moles, and kelvin?

Accepted Answer

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

Question 7

A 4.8-L sample of helium contains 0.22 mol. How many additional moles must be added to reach a volume of 6.4 L at constant temperature and pressure?

Accepted Answer

$$0.07\ 	ext{mol}$$

Question 8

Which of the following best describes why gases are compressible but liquids are not?

Accepted Answer

Gas particles are much farther apart than liquid particles, allowing them to be pushed closer together.

Question 9

A mixture of gases contains 78% nitrogen, 21% oxygen, and 1% argon by volume at a total pressure of 1.00 atm. What is the partial pressure of oxygen?

Accepted Answer

$$0.21\ 	ext{atm}$$

Question 10

Which of the following is the correct combined gas law equation?

Accepted Answer

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

Question 11

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

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

Question 12

Which of the following is a real-world consequence of Dalton’s law of partial pressures?

Accepted Answer

The total pressure in a scuba tank is the sum of the partial pressures of all gases present.

Question 13

A balloon filled with 1.00 mol of gas at STP has a volume of:

Accepted Answer

$$22.4\ 	ext{L}$$

Question 14

Which of the following is NOT a property predicted by the kinetic molecular theory for gases?

Accepted Answer

Gases have high densities compared to solids.

Question 15

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 16

Which of the following scenarios would most likely result in oxygen toxicity for a diver?

Accepted Answer

Breathing air at a depth where the partial pressure of oxygen exceeds 1.4 atm.

Question 17

A sample of hydrogen gas is collected over water at 25°C and a total pressure of 758 mm Hg. If the vapor pressure of water at 25°C is 23.8 mm Hg, what is the partial pressure of hydrogen gas?

Accepted Answer

$$734\ 	ext{mm Hg}$$

Question 18

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

Accepted Answer

Heating the air inside the balloon decreases its density, causing it to float in cooler, denser air.

Question 19

A heliox mixture contains 2.0% oxygen at a total pressure of 10.0 atm. What is the partial pressure of oxygen?

Accepted Answer

$$0.20\ 	ext{atm}$$

Chapter 11: Gases – Structured Study Notes for Introductory Chemistry

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