Q: A 56 kg person stands on a floor wearing a pointed heel with an area of $0.45 \ \mathrm{cm}^2$. What is the pressure exerted on the floor in pascals? (Assume $g = 9.81 \ \mathrm{m/s}^2$)

$1.22 \times 10^6 \ \mathrm{Pa}$

Q: A climber carries a $10.0 \ \mathrm{L}$ oxygen tank with an internal pressure of $3.04 \times 10^4 \ \mathrm{mmHg}$. If the atmospheric pressure at the summit is $0.200 \ \mathrm{bar}$, what will be the volume of the gas when released at the summit? (Assume constant temperature and amount of gas)

$2.03 \times 10^3 \ \mathrm{L}$

Q: Which of the following best describes the relationship between temperature and average kinetic energy of gas molecules according to the Kinetic Molecular Theory?

Average kinetic energy is directly proportional to the absolute temperature.

Question 1

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

Accepted Answer

Gases have particles that are far apart compared to their size, allowing them to be compressed.

Question 2

A 56 kg person stands on a floor wearing a pointed heel with an area of $0.45 \ \mathrm{cm}^2$. What is the pressure exerted on the floor in pascals? (Assume $g = 9.81 \ \mathrm{m/s}^2$)

Accepted Answer

$1.22 	imes 10^6 \ \mathrm{Pa}$

Question 3

Which sample in the diagram (A, B, C, D) has the highest pressure, given that all samples have the same temperature but different volumes and number of particles?

Accepted Answer

Sample B

Question 4

Convert a pressure of $760 \ \mathrm{mmHg}$ to bar.

Accepted Answer

$1.000 \ \mathrm{bar}$

Question 5

A manometer is used to measure the pressure of a gas sample. If the mercury column is 65 mm higher on the side open to the atmosphere and the barometric pressure is $101.6 \ \mathrm{kPa}$, what is the pressure of the gas in the container (in kPa)? (Assume $1 \ \mathrm{mmHg} = 0.1333 \ \mathrm{kPa}$)

Accepted Answer

$110.3 \ \mathrm{kPa}$

Question 6

Which of the following is the correct mathematical expression for Boyle's Law?

Accepted Answer

$P_1 V_1 = P_2 V_2$

Question 7

A balloon filled with helium gas is sealed and floats to a higher altitude with no change in temperature or amount of gas. Which balloon (A, B, or C) shows the final volume?

Accepted Answer

C

Question 8

A climber carries a $10.0 \ \mathrm{L}$ oxygen tank with an internal pressure of $3.04 	imes 10^4 \ \mathrm{mmHg}$. If the atmospheric pressure at the summit is $0.200 \ \mathrm{bar}$, what will be the volume of the gas when released at the summit? (Assume constant temperature and amount of gas)

Accepted Answer

$2.03 	imes 10^3 \ \mathrm{L}$

Question 9

Given a sealed container of oxygen gas with an initial volume of $269 \ \mathrm{L}$ at $27.3^{\circ}\mathrm{C}$ ($300.5 \ \mathrm{K}$), calculate the volume if the temperature is changed to $-2.4^{\circ}\mathrm{C}$ ($270.8 \ \mathrm{K}$). Assume pressure remains constant.

Accepted Answer

$243 \ \mathrm{L}$

Question 10

A gas has a volume of $4.00 \ \mathrm{L}$ at $0.00^{\circ}\mathrm{C}$ ($273.15 \ \mathrm{K}$). What final temperature, in degrees Celsius, is needed to change the volume of the gas to $0.0500 \ \mathrm{L}$? (Assume constant amount of gas and pressure)

Accepted Answer

$-270^{\circ}\mathrm{C}$

Question 11

A $4.8 \ \mathrm{L}$ sample of helium gas contains $0.22 \ \mathrm{mol}$ of helium. How many additional moles of helium gas must be added to the sample to obtain a volume of $6.4 \ \mathrm{L}$? (Assume constant temperature and pressure)

Accepted Answer

$0.07 \ \mathrm{mol}$

Question 12

If $5.00 \ \mathrm{g}$ of $O_2$ gas has a volume of $7.20 \ \mathrm{L}$ at a certain temperature and pressure, what volume does $15.0 \ \mathrm{g}$ of $O_2$ have under the same conditions?

Accepted Answer

$21.6 \ \mathrm{L}$

Question 13

What is the value of the gas constant $R$ in $\mathrm{L \cdot bar \cdot mol^{-1} \cdot K^{-1}}$?

Accepted Answer

$0.08314 \ \mathrm{L \cdot bar \cdot mol^{-1} \cdot K^{-1}}$

Question 14

Using the ideal gas law, determine the final temperature (in K) of $1.85 \ \mathrm{mol}$ of He in a $72.8 \ \mathrm{L}$ constant-volume cylinder at a pressure of $1.50 \ \mathrm{atm}$ ($1.52 \ \mathrm{bar}$).

Accepted Answer

$719 \ \mathrm{K}$

Question 15

What is the mass of Argon gas (in grams) in a $75.0 \ \mathrm{mL}$ volume at STP?

Accepted Answer

$0.132 \ \mathrm{g}$

Question 16

Rank the following gases in order of increasing density under identical conditions of temperature and pressure: Ar, He, SF$_6$, Xe.

Accepted Answer

He < Ar < Xe < SF$_6$

Question 17

The density of phosphorus vapor at $310^{\circ}\mathrm{C}$ ($583.15 \ \mathrm{K}$) and $775 \ \mathrm{mmHg}$ ($1.03 \ \mathrm{bar}$) is $2.64 \ \mathrm{g/L}$. What is the molecular formula of the phosphorus under these conditions?

Accepted Answer

$P_4$

Question 18

Which of the following best describes the relationship between temperature and average kinetic energy of gas molecules according to the Kinetic Molecular Theory?

Accepted Answer

Average kinetic energy is directly proportional to the absolute temperature.

Chapter 5: Gases – Properties, Laws, and Applications

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