Question 1

Calculate the number of moles in 75.0 g of O2, and the pressure that it would exert at 80.0°C in a 5.00 L steel tank.

Accepted Answer

A)  4.69 mol, 6.18 atm
B)  4.69 mol, 27.2 atm
C)  2.34 mol, 13.6 atm
D)  2.34 mol, 3.09 atm
E)  9.38 mol, 27.2 atm

Question 2

Given a fixed amount of gas held at constant pressure, calculate the temperature to which the gas would have to be changed if a 3.50 L sample at 23.0°C were to have a final volume of 1.50 L.

Accepted Answer

A)  2.0°C
B)  127°C
C)  −146°C
D)  9.8°C
E)  43.2°C

Question 3

Calculate the number of moles in 55 g of N2, and the volume that it would occupy at STP.

Accepted Answer

A)  2.0 mol, 45 L
B)  2.0 mol, 0.089 L
C)  1.5 x 103 mol, 67 L
D)  1.5 x 103 mol, 3.4 x 104 L
E)  3.9 mol, 88 L

Question 4

If the volume of a sample of gas is held constant, while the temperature is decreased, the pressure will

Accepted Answer

A)  become higher because of fewer collisions with the container.
B)  become lower because of fewer collisions with the container.
C)  become lower because of more collisions with the container.
D)  become higher because of more collisions with the container.
E)  stay the same because temperature has no effect on pressure.

Question 5

Convert 1.28 atm to mm Hg.

Accepted Answer

A)  1.28 x 103 mm Hg
B)  1.30 x 105 mm Hg
C)  1.68 x 10-3 mm Hg
D)  972.8 mm Hg
E)  1.03 x 10-3 mm Hg

Question 6

A sample of gas initially occupies 2.50 L at a pressure of 905 torr at 22.0°C. What will the temperature be if the pressure is changed to 2.00 atm, and the volume is changed to 1.50 L?

Accepted Answer

A)  22.2°C
B)  554°C
C)  1.09°C
D)  271°C
E)  24.5°C E

Question 7

Which characteristic does not describe an ideal gas?

Accepted Answer

A)  negligible volume occupied by ideal gas molecules
B)  no attractive forces between ideal gas molecules
C)  obeys the equation PV = nRT
D)  PV/RT = a constant
E)  strong repulsions between molecules

Question 8

A sample of gas initially occupies 2.50 L at a pressure of 0.900 atm at 22.0°C. What will the pressure be if the temperature is changed to 56.5°C, and the volume is changed to 1.50 L?

Accepted Answer

A)  0.584 atm
B)  3.85 atm
C)  1.68 atm
D)  1.34 atm
E)  3.77 atm

Question 9

A liter container of CO2 and a liter container of H2 are both at 25°C and 1 atm pressure. Which of the following statements about these gas samples is true?

Accepted Answer

A)  The CO2 and H2 molecules have the same average velocity.
B)  There are more H2 molecules than CO2 molecules.
C)  The average kinetic energy of the CO2 molecules is greater than that of the H2 molecules.
D)  The CO2 molecules on average are moving more slowly than the H2 molecules.
E)  The masses of the two gas samples are equal.

Question 10

Under which conditions would the density of helium be the smallest?

Accepted Answer

A)  high pressure and high temperature
B)  low pressure and high temperature
C)  high pressure and low temperature
D)  low pressure and low temperature
E)  The density of helium is independent of pressure and temperature.

Question 11

Given a fixed amount of gas held at constant pressure, calculate the temperature to which the gas would have to be changed if a 1.75 L sample at 23.0°C were to have a final volume of 3.50 L.

Accepted Answer

A)  46.0°C
B)  89.5°C
C)  169°C
D)  319°C
E)  592°C

Question 12

Calculate the density of NO2 in g/L at STP.

Accepted Answer

A)  22.41 g/L
B)  2.053 g/L
C)  1.031 x 103 g/L
D)  0.04462 g/L
E)  0.4871 g/L

Question 13

The "Before" image in the figure shows the initial condition of a gas at a certain temperature in a container with a movable piston. Which of the images represents the condition of the gas when the temperature of the gas is increased, and the external pressure is held constant?

Accepted Answer

A)  image I
B)  image II
C)  image III
D)  image IV
E)  None of the images

Question 14

A gas in a closed container with constant volume is heated from room temperature to 100°C. According to the kinetic molecular theory, the

Accepted Answer

A)  average velocity of the molecules will increase.
B)  gas will increase in weight.
C)  individual molecules of the gas will increase their size.
D)  average distance between molecules will increase.
E)  pressure on the sides of the container will decrease.

Question 15

A sample of gas initially occupies 5.50 L at a pressure of 0.750 atm at 13.0°C. What will the pressure be if the temperature is changed to 22.5°C, and the volume is changed to 1.50 L?

Accepted Answer

A)  6.39 atm
B)  11.4 atm
C)  0.211 atm
D)  2.84 atm
E)  1.59 atm

Question 16

Which of the following statements related to kinetic-molecular theory of gases is correct for an ideal gas?

Accepted Answer

A)  Gases are composed of small particles with a small amount of space between them.
B)  Gas particles move in a zigzag pattern until they collide with something.
C)  When gas particles collide, they lose some of their kinetic energy, and will slow down over time.
D)  In a mixture of gases, attractive forces between particles cause the measured pressure to be lower than that expected for a pure gas.
E)  The pressure of a gas arises from the sum of the collisions of the particles with the walls of the container.

Question 17

According to kinetic-molecular theory, molecules of different gases at the same temperature always have the same

Accepted Answer

A)  molar mass.
B)  pressure.
C)  average kinetic energy.
D)  volume.
E)  number of moles. C

Question 18

A weather balloon filled with helium gas gets larger as it ascends to high altitudes. The expansion of the balloon is primarily due to

Accepted Answer

A)  a decrease in the average kinetic energy of the helium atoms inside the balloon.
B)  an increase in the average kinetic energy of the helium atoms inside the balloon.
C)  a decrease in the average kinetic energy of the air molecules outside the balloon.
D)  an increase in the rate of collision of the helium atoms against the inside walls of the balloon.
E)  a decrease in the rate of collision of the air molecules on the outside walls of the balloon.

Question 19

Propane burns in air according to the equation: C3H8(g) + 5O2(g) → 3CO2(g) + 4H2O(g) 
What volume of O2 would be required if 8.00 L of propane burns, assuming that all of the gases are under the same conditions?

Accepted Answer

A)  8.00 L
B)  40.0 L
C)  20.0 L
D)  15.0 L
E)  1.60 L B

Question 20

If a steel tank is filled with acetylene to a pressure of 7.50 atm in the morning, when the temperature is 18.0oC, what will the pressure (in atm)be in the afternoon, when the temperature rises to 33.5oC?

Accepted Answer

Exam 9: The Gaseous State

Calculate the number of moles in 75.0 g of O2, and the pressure that it would exert at 80.0°C in a 5.00 L steel tank.

Correct AnswerverifiedShow Answer

Given a fixed amount of gas held at constant pressure, calculate the temperature to which the gas would have to be changed if a 3.50 L sample at 23.0°C were to have a final volume of 1.50 L.

Correct AnswerverifiedShow Answer

Calculate the number of moles in 55 g of N2, and the volume that it would occupy at STP.

Correct AnswerverifiedShow Answer

If the volume of a sample of gas is held constant, while the temperature is decreased, the pressure will

Correct AnswerverifiedShow Answer

Convert 1.28 atm to mm Hg.

Correct AnswerverifiedShow Answer

A sample of gas initially occupies 2.50 L at a pressure of 905 torr at 22.0°C. What will the temperature be if the pressure is changed to 2.00 atm, and the volume is changed to 1.50 L?

Correct AnswerverifiedE

Which characteristic does not describe an ideal gas?

Correct AnswerverifiedShow Answer

A sample of gas initially occupies 2.50 L at a pressure of 0.900 atm at 22.0°C. What will the pressure be if the temperature is changed to 56.5°C, and the volume is changed to 1.50 L?

Correct AnswerverifiedShow Answer

A liter container of CO2 and a liter container of H2 are both at 25°C and 1 atm pressure. Which of the following statements about these gas samples is true?

Correct AnswerverifiedShow Answer

Under which conditions would the density of helium be the smallest?

Correct AnswerverifiedShow Answer

Given a fixed amount of gas held at constant pressure, calculate the temperature to which the gas would have to be changed if a 1.75 L sample at 23.0°C were to have a final volume of 3.50 L.

Correct AnswerverifiedShow Answer

Calculate the density of NO2 in g/L at STP.

Correct AnswerverifiedShow Answer

The "Before" image in the figure shows the initial condition of a gas at a certain temperature in a container with a movable piston. Which of the images represents the condition of the gas when the temperature of the gas is increased, and the external pressure is held constant?

Correct AnswerverifiedShow Answer

A gas in a closed container with constant volume is heated from room temperature to 100°C. According to the kinetic molecular theory, the

Correct AnswerverifiedShow Answer

A sample of gas initially occupies 5.50 L at a pressure of 0.750 atm at 13.0°C. What will the pressure be if the temperature is changed to 22.5°C, and the volume is changed to 1.50 L?

Correct AnswerverifiedShow Answer

Which of the following statements related to kinetic-molecular theory of gases is correct for an ideal gas?

Correct AnswerverifiedShow Answer

According to kinetic-molecular theory, molecules of different gases at the same temperature always have the same

Correct AnswerverifiedC

A weather balloon filled with helium gas gets larger as it ascends to high altitudes. The expansion of the balloon is primarily due to

Correct AnswerverifiedShow Answer

Propane burns in air according to the equation: C3H8(g) + 5O2(g) → 3CO2(g) + 4H2O(g) What volume of O2 would be required if 8.00 L of propane burns, assuming that all of the gases are under the same conditions?

Correct AnswerverifiedB

If a steel tank is filled with acetylene to a pressure of 7.50 atm in the morning, when the temperature is 18.0oC, what will the pressure (in atm)be in the afternoon, when the temperature rises to 33.5oC?

Correct AnswerverifiedShow Answer

Calculate the number of moles in 75.0 g of O₂, and the pressure that it would exert at 80.0°C in a 5.00 L steel tank.

Correct Answer
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Calculate the number of moles in 55 g of N₂, and the volume that it would occupy at STP.

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E

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A liter container of CO₂ and a liter container of H₂ are both at 25°C and 1 atm pressure. Which of the following statements about these gas samples is true?

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Calculate the density of NO₂ in g/L at STP.

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C

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Propane burns in air according to the equation: C₃H₈(g) + 5O₂(g) → 3CO₂(g) + 4H₂O(g) What volume of O₂would be required if 8.00 L of propane burns, assuming that all of the gases are under the same conditions?

Correct Answer
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B

If a steel tank is filled with acetylene to a pressure of 7.50 atm in the morning, when the temperature is 18.0^oC, what will the pressure (in atm)be in the afternoon, when the temperature rises to 33.5^oC?

Correct Answer
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