Ch 11 - The Gas Laws

The force per unit area in which a gas particle collides with a container wall describes which physical property of a gas?

• Moles

• Temperature

• Volume

• Pressure

Which of the following is not atmospheric pressure at sea level?

• 1.0 atm

• 760 mmHg

• 101.1 kPa

• 273 torr

Dalton's Law of partial pressure explains why, when gases are collected over water,

• water vapor forms that mixes with the other gases.

• water vapor pressure must be subtracted to determine the final pressure of the other gases.

• the gas pressures add up to a total pressure.

• all of the above.

Gas A and gas B (both nonreactive) are allowed to mix. The total pressure is found to be 3.50 atm. If gas B was measured initially at 1.25 atm, what is the partial pressure of gas A?

• 4.38 atm

• -2.25 atm

• 2.25 atm

• 2.80 atm

Calculate the volume of 12.0g of helium gas at 100^oC and 1.2 atm.

• 0.013 L

• 76.5 L

• 7, 750 L

• 56.0 L

A flask contains 0.155 L of hydrogen that was collected under a pressure of 22.5 kPa. What pressure would have been required for the volume of the gas to be 0.090 L?

• 101.1 kPa

• 13.1 kPa

• 38.8 kPa

• 6.43 kPa

5.0 L of a gas goes from 1.0 atm to 1.3 atm. Calculate the final volume of this gas.

• 6.5 L

• 0.26 L

• 4.1 L

• 3.8 L

When the temperature of a gas is increased within a closed container, pressure increases due to which of the following?

• The frequency of collisions between molecules and the container walls decreases.

• The frequency of collisions between molecules and the container walls increases.

• The spaces between the molecules of gas decreases.

• The gas turns into a liquid.

Tags

NGSS.HS-PS1-5

A sample of hydrogen at 47^oC exerts a pressure of 250 mmHg. The gas is heated to 77^oC at constant volume. What will its new pressure be?

• 274 mmHg

• 410 mmHg

• 321 mmHg

• 650 mmHg

A sample of helium gas has a pressure of 1.20 atm at 22^oC. At what Celsius temperature will the helium reach a pressure of 2.00 atm, assuming constant volume?

• 219^oC

• 492^oC

• 36.7^oC

• 0.00^oC