Q: Which of the following is the correct relationship for Dalton’s law of partial pressures?

$$P_{\text{total}} = P_1$ + P_2$ + P_3$ + \ldots$$

Question 1

According to the kinetic molecular theory, which of the following statements best explains why gases are compressible?

Accepted Answer

There is a lot of empty space between gas particles compared to their size.

Question 2

A scuba diver at a depth of 20 m breathes air at a pressure of 3 atm. If the diver ascends rapidly to the surface (1 atm) while holding their breath, 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 3

Which equation correctly represents Boyle’s law?

Accepted Answer

$$P_1V_1 = P_2V_2$$

Question 4

A sample of gas occupies 2.80 L at an unknown temperature. When cooled to 0 °C, its volume decreases to 2.57 L. What was the initial temperature in Kelvin? (Assume constant pressure.)

Accepted Answer

297 K

Question 5

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

Accepted Answer

Heating the air increases its volume, decreasing its density, so it floats in cooler, denser air.

Question 6

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

Accepted Answer

0.12 mol

Question 7

Which of the following is the correct form of the ideal gas law?

Accepted Answer

$$PV = nRT$$

Question 8

A mixture of gases contains 78% nitrogen, 21% oxygen, and 1% argon by mole. If the total pressure is 1.00 atm, what is the partial pressure of oxygen?

Accepted Answer

0.21 atm

Question 9

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? (Use $$R = 0.0821 L$$·atm/mol·K)

Accepted Answer

29.7 g/mol

Question 10

Which of the following scenarios would cause the greatest increase in the pressure of a gas inside a rigid container?

Accepted Answer

Adding more gas while keeping the temperature constant.

Question 11

A sample of gas has an initial volume of 158 mL at 735 mm Hg and 34 °C. If the gas is compressed to 108 mL and heated to 85 °C, what is the final pressure in mm Hg? (Use the combined gas law.)

Accepted Answer

1100 mm Hg

Question 12

Which of the following is NOT an assumption of the kinetic molecular theory for ideal gases?

Accepted Answer

Gas particles attract and repel each other strongly.

Question 13

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

Accepted Answer

0.20 atm

Question 14

Which of the following best explains why a person cannot breathe through a 10-m long snorkel while swimming underwater?

Accepted Answer

The air pressure at 10 m depth is too high for the lungs to inflate with air from the surface.

Question 15

Which of the following is the correct relationship for Dalton’s law of partial pressures?

Accepted Answer

$$P_{	ext{total}} = P_1$ + P_2$ + P_3$ + \ldots$$

Question 16

At standard temperature and pressure (STP), what is the volume occupied by 2.00 mol of an ideal gas?

Accepted Answer

44.8 L

Question 17

Which of the following pollutants is primarily produced by the incomplete combustion of fossil fuels and can cause sensory impairment at high levels?

Accepted Answer

Carbon monoxide

Question 18

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

Accepted Answer

734.2 mm Hg

Question 19

Which of the following changes would cause a decrease in the pressure of a gas, assuming the amount of gas and temperature remain constant?

Accepted Answer

Increasing the volume of the container.

Question 20

Which of the following best describes the relationship between the number of moles of a gas and its volume at constant temperature and pressure?

Accepted Answer

They are directly proportional.

Chapter 11: Gases – Properties, Laws, and Applications

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