Free Practice Quiz Question List

11 Gases and Kinetic Molecular Theory Online Quiz Questions

Use this free practice quiz with 20 questions to review 11 Gases and Kinetic Molecular Theory, test your knowledge, and prepare for your next test or exam.

20 questions

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1 point

A fixed amount of gas is compressed isothermally from $4.00\ \mathrm{L}$ to $1.20\ \mathrm{L}$ . If its initial pressure is $1.50\ \mathrm{atm}$ , what is its final pressure?

A
$3.00\ \mathrm{atm}$
B
$5.00\ \mathrm{atm}$
C
$0.450\ \mathrm{atm}$
D
$6.00\ \mathrm{atm}$

Choose one

1 point

A flexible container holds $2.40\ \mathrm{L}$ of gas at $300\ \mathrm{K}$ . If the gas is heated to $450\ \mathrm{K}$ while pressure and amount remain constant, what is its new volume?

A
$1.60\ \mathrm{L}$
B
$2.40\ \mathrm{L}$
C
$3.60\ \mathrm{L}$
D
$4.80\ \mathrm{L}$

Choose one

1 point

Gas in a rigid container has a pressure of $96.0\ \mathrm{kPa}$ at $280\ \mathrm{K}$ . What pressure will it have at $350\ \mathrm{K}$ , assuming the amount of gas is unchanged?

A
$120\ \mathrm{kPa}$
B
$76.8\ \mathrm{kPa}$
C
$105\ \mathrm{kPa}$
D
$350\ \mathrm{kPa}$

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1 point

A flexible container holds $0.800\ \mathrm{mol}$ of gas in a volume of $4.80\ \mathrm{L}$ . If the amount is increased to $1.20\ \mathrm{mol}$ at constant pressure and temperature, what volume will the gas occupy?

A
$3.20\ \mathrm{L}$
B
$4.80\ \mathrm{L}$
C
$6.00\ \mathrm{L}$
D
$7.20\ \mathrm{L}$

Choose one

1 point

A fixed amount of gas changes from $P_1=0.950\ \mathrm{atm}$ , $V_1=3.20\ \mathrm{L}$ , and $T_1=280\ \mathrm{K}$ to $P_2=1.10\ \mathrm{atm}$ and $T_2=315\ \mathrm{K}$ . What is its final volume? Round to the nearest $0.01\ \mathrm{L}$ .

A
$2.48\ \mathrm{L}$
B
$3.11\ \mathrm{L}$
C
$3.20\ \mathrm{L}$
D
$4.10\ \mathrm{L}$

Choose one

1 point

What volume is occupied by $0.500\ \mathrm{mol}$ of an ideal gas at $300\ \mathrm{K}$ and $1.50\ \mathrm{atm}$ ? Use $R=0.08206\ \mathrm{L\,atm\,mol^{-1}\,K^{-1}}$ and round to the nearest $0.01\ \mathrm{L}$ .

A
$8.21\ \mathrm{L}$
B
$12.3\ \mathrm{L}$
C
$0.122\ \mathrm{L}$
D
$24.6\ \mathrm{L}$

Choose one

1 point

A nonreacting ideal-gas mixture has component partial pressures of $18.0\ \mathrm{kPa}$ , $27.0\ \mathrm{kPa}$ , and $45.0\ \mathrm{kPa}$ . What is the total pressure?

A
$45.0\ \mathrm{kPa}$
B
$72.0\ \mathrm{kPa}$
C
$90.0\ \mathrm{kPa}$
D
$121.5\ \mathrm{kPa}$

Choose one

1 point

Two gases are at the same temperature. Their particles have masses in the ratio $m_{\mathrm{light}}:m_{\mathrm{heavy}}=4:36$ . What is the ratio of their average speeds, $v_{\mathrm{light}}/v_{\mathrm{heavy}}$ , according to kinetic molecular theory?

A
$1/3$
B
$1$
C
$\sqrt{3}$
D
$3$

Choose one

1 point

A calculation uses pressure in kilopascals, volume in liters, amount in moles, and temperature in kelvins. Which ideal gas constant is consistent with all four units?

A
$8.314\ \mathrm{L\,kPa\,mol^{-1}\,K^{-1}}$
B
$8.314\ \mathrm{L\,atm\,mol^{-1}\,K^{-1}}$
C
$0.08206\ \mathrm{L\,kPa\,mol^{-1}\,K^{-1}}$
D
$0.08206\ \mathrm{L\,atm\,mol^{-1}\,^{\circ}C^{-1}}$

Choose one

1 point

A sealed rigid container of gas is heated without changing the amount of gas. Which explanation best accounts for the resulting pressure increase according to kinetic molecular theory?

A
The particles become larger, so they occupy more of the fixed container.
B
The particles attract each other more strongly, pulling on the walls.
C
The particles’ average kinetic energy increases, making their wall collisions more forceful and raising pressure.
D
The amount of gas must increase as temperature rises.

Choose one

1 point

Under which conditions would a real gas generally be expected to deviate most from ideal-gas behavior?

A
Low pressure and high temperature
B
High pressure and low temperature
C
Low pressure and low temperature
D
High pressure and high temperature

Choose one

1 point

An ideal gas changes from $P_1=100\ \mathrm{kPa}$ , $V_1=10.0\ \mathrm{L}$ , $n_1=1.00\ \mathrm{mol}$ , and $T_1=300\ \mathrm{K}$ to $V_2=12.0\ \mathrm{L}$ , $n_2=1.50\ \mathrm{mol}$ , and $T_2=400\ \mathrm{K}$ . What is its final pressure? Round to the nearest $1\ \mathrm{kPa}$ .

A
$100\ \mathrm{kPa}$
B
$167\ \mathrm{kPa}$
C
$225\ \mathrm{kPa}$
D
$300\ \mathrm{kPa}$

Choose one

1 point

A fixed amount of gas is held at constant temperature and compressed until its volume is half its original value. Which statement correctly describes the pressure change and the relationship that explains it?

A
The pressure becomes half as large because the gas occupies less space.
B
The pressure doubles because pressure and volume are inversely related.
C
The pressure stays constant because the temperature does not change.
D
The pressure quadruples because the volume is reduced twice.

Choose one

1 point

Why must temperature be expressed in kelvins when using gas-law relationships?

A
Gas-law relationships require an absolute temperature scale, and kelvins measure temperature from absolute zero.
B
Celsius temperatures cannot be used because the Celsius scale has smaller degree intervals than the kelvin scale.
C
Kelvins are required because gas particles stop moving at $0\ ^{\circ}\mathrm{C}$ .
D
Kelvins are required only when the gas is in a rigid container.

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1 point

Which conditions are most likely to produce a noticeable departure from ideal-gas behavior, and why?

A
High pressure and low temperature, because particle volume and attractions become more significant.
B
Low pressure and high temperature, because particles are far apart and attractions dominate.
C
Low pressure and low temperature, because particle volume becomes zero.
D
High pressure and high temperature, because collisions cease to be elastic.

Choose one

1 point

According to the kinetic molecular theory for an ideal gas, what does it mean for particle collisions to be elastic?

A
Particles lose kinetic energy during every collision, but the lost energy is restored between collisions.
B
The total kinetic energy of the particles is conserved during collisions.
C
Particles exert no forces on one another, including during collisions.
D
Particles stop moving briefly whenever they collide with a container wall.

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1 point

A helium sample and a xenon sample are at the same temperature. Which comparison of their average translational kinetic energies and average particle speeds is consistent with KMT?

A
Xenon has greater average kinetic energy because its particles are heavier, but helium moves faster.
B
They have the same average translational kinetic energy, and helium particles move faster on average.
C
They have the same average speed because their temperatures are equal, but xenon has greater average kinetic energy.
D
Helium has greater average kinetic energy, while xenon particles move faster on average.

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1 point

A flexible container holds a gas at constant pressure. The amount of gas increases by a factor of $1.5$ , and its absolute temperature doubles. By what factor does the volume change?

A
The final volume is $1.5$ times the initial volume.
B
The final volume is $2$ times the initial volume.
C
The final volume is $3$ times the initial volume.
D
The final volume is $3.5$ times the initial volume.

Choose one

1 point

An inert ideal gas is added to a mixture of nonreacting ideal gases in a rigid container, while temperature stays constant. What happens to the original gases’ partial pressures and to the mixture’s total pressure?

A
The existing gases’ partial pressures stay the same, while the total pressure increases.
B
The existing gases’ partial pressures decrease, while the total pressure stays the same.
C
The existing gases’ partial pressures and the total pressure both increase.
D
The existing gases’ partial pressures stay the same, and the total pressure also stays the same.

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1 point

A fixed amount of gas changes from $120\ \mathrm{kPa}$ , $2.0\ \mathrm{L}$ , and $27^{\circ}\mathrm{C}$ to $100\ \mathrm{kPa}$ and $127^{\circ}\mathrm{C}$ . What is its final volume?

A
$1.6\ \mathrm{L}$
B
$2.4\ \mathrm{L}$
C
$2.7\ \mathrm{L}$
D
$3.2\ \mathrm{L}$