Question 1

Which of the following statements best describes the kinetic-molecular theory of gases?

Accepted Answer

Gas particles move randomly at high velocities and have negligible volume compared to the container.

Question 2

A car tire has a pressure of 2.00 atm. What is this pressure in Pascals (Pa)? Use $1 	ext{ atm} = 101325 	ext{ Pa}$.

Accepted Answer

$202650 	ext{ Pa}$

Question 3

Which property of gases explains why a balloon expands when filled with air?

Accepted Answer

Gas particles move very fast in random directions and exert pressure on the container walls.

Question 4

A 1.0 L metal cylinder contains a gas at $100^\circ 	ext{C}$ and $775 	ext{ mmHg}$. How many moles of gas are present? ($R = 0.0821 	ext{ L} \cdot 	ext{atm} \cdot 	ext{mol}^{-1} \cdot 	ext{K}^{-1}$, $1 	ext{ atm} = 760 	ext{ mmHg}$)

Accepted Answer

$0.033 	ext{ mol}$

Question 5

Which gas law describes the relationship between pressure and volume at constant temperature and moles?

Accepted Answer

Boyle's Law

Question 6

A sample of oxygen gas at $273 	ext{ K}$ has a volume of $12.0 	ext{ L}$ at $600 	ext{ mmHg}$. What is the new pressure if the volume is changed to $36.0 	ext{ L}$? (Assume temperature and moles are constant.)

Accepted Answer

$200 	ext{ mmHg}$

Question 7

Which of the following gases exists as a diatomic molecule at room temperature and pressure?

Accepted Answer

Oxygen ($	ext{O}_2$)

Question 8

A 1.0 L flexible container of gas at $300 	ext{ K}$ and $1.0 	ext{ atm}$ contains $0.10 	ext{ mol}$ of gas. If the temperature is raised to $600 	ext{ K}$ and the pressure to $4.0 	ext{ atm}$, what is the new volume?

Accepted Answer

$0.50 	ext{ L}$

Question 9

Which of the following best explains why water boils at a lower temperature in the mountains than at sea level?

Accepted Answer

Atmospheric pressure is lower at higher altitudes, so the vapor pressure required for boiling is reached at a lower temperature.

Question 10

Which equation represents the combined gas law?

Accepted Answer

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

Question 11

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

Accepted Answer

$24^\circ 	ext{C}$

Question 12

Which of the following is the correct value for the molar volume of an ideal gas at STP?

Accepted Answer

$22.4 	ext{ L}$

Question 13

A scuba tank contains a mixture of $	ext{O}_2$ and He gases with a total pressure of $1200 	ext{ mmHg}$. If the partial pressure of He is $855 	ext{ mmHg}$, what is the partial pressure of $	ext{O}_2$?

Accepted Answer

$345 	ext{ mmHg}$

Question 14

Which variable must be in Kelvin for gas law calculations?

Accepted Answer

Temperature

Question 15

Which of the following is NOT a property of gases?

Accepted Answer

Gases have strong intermolecular attractions.

Question 16

Which law describes the relationship between volume and temperature at constant pressure and moles?

Accepted Answer

Charles's Law

Question 17

A gas has a pressure of $2.0 	ext{ atm}$ at $18^\circ 	ext{C}$. What is the new pressure when the temperature changes to $62^\circ 	ext{C}$? (Assume volume and moles are constant.)

Accepted Answer

$2.3 	ext{ atm}$

Question 18

Which of the following best describes the effect of increasing altitude on atmospheric pressure?

Accepted Answer

Atmospheric pressure decreases as altitude increases.

Question 19

Which equation is used to calculate the number of moles of a gas in a container using the ideal gas law?

Accepted Answer

$n = \dfrac{P V}{R T}$

Gases: Properties, Laws, and Applications (Chapter 8 Study Notes)

Study Guide - Practice Questions

Study Guide - Flashcards