Gas Law quizz

An expandable container holds 15 liters of a gas at a pressure of 2.5 atm and a temperature of 320 K. The volume of the container is then increased to a new volume of 25 liters while the temperature is held constant at 320 K. What is the new pressure in the container?

• 1. 0.7 atm

• 1. 1.5 atm

• 1. 2.5 atm

• 1. 4.2 atm

Which statement is one of the assumptions of the Kinetic Molecular Theory of Gases?

• 1. Collisions between gas particles and container walls are inelastic.

• 1. The temperature of a gas depends on the average potential energy of the gas particles.

• 1. Gas particles are much larger than the distance between them

• 1. The volume of a gas is mostly empty space.

Oxygen gas in a 15.0 L container exerts a pressure of 0.48 atm at 21 ºC. How many moles of oxygen are in this container?

• 1. 4.2 moles

• 1. 3.4 moles

• 3.0×10−1 moles

• 8.7×10−3 moles

The total pressure of a mixture of three gases (helium, argon, and neon) inside a container is 810 mmHg. The partial pressure of the helium is 486 mmHg, and the partial pressure of the argon is 120 mmHg. What is the partial pressure of the neon in mmHg?

• 1. 204 mmHg

• 1. 303 mmHg

• 1. 465 mmHg

• 1. 810 mmHg

consider two atoms of a gas in a container. Atom #1 is large and dense, but Atom #2 is small and less dense. The atoms freely move around the container, but after a few seconds the two atoms collide. Describe what happens as the two atoms collide with one another.

• 1. The larger, denser atom is able to transfer its energy to the smaller atom, so the overall kinetic energy stays the same.

• 1. The smaller atom is forced to stop when it comes in contact with the larger atom, so the overall kinetic energy decreases slightly

• 1. The smaller, less dense atom is able to transfer its kinetic energy to the larger atom, so the overall kinetic energy increases slightly.

• 1. The two atoms collide and keep their own kinetic energy. This elastic collisions between the two atoms does not change the total kinetic energy

A sample of oxygen gas is in a closed container. The gas and the container are at room temperature. According to the kinetic molecular theory of gases, what happens when a molecule of the gas collides with the container wall?

• 1. Some, but not all, of the molecule’s kinetic energy is transferred to the container in the form of heat.

• 1. Some, but not all, of the container’s heat energy is transferred to the molecule in the form of kinetic energy.

• 1. All of the molecule’s energy is transferred to the container.

• 1. No energy is transferred between the molecule and the container.

Ten liters of an unknown gas are at an initial temperature, T_i = 293 K. With no change in pressure, the gas is heated to a final temperature, T_f = 352 K. What is the final volume of the gas, in liters?

• 8.3

• 10.0

• 12.0

• 39.5

At STP, 6.5 moles of nitrogen gas, N₂ , occupy a volume of 145 liters. How many moles of nitrogen gas, N₂ , occupy a volume of 179 liters at STP?

• 1. 27.5

• 1. 22.4

• 8.0

• 6.5

Gases are far more easily compressed that liquids and solids. Which postulate of the kinetic molecular theory explains this characteristic of gases?

• 1. The volume of a gas is mostly empty space.

• 1. Gas particles have inelastic collisions.

• 1. The energy of a gas particle depends on the average potential energy of the gas.

• 1. There are strong attractive forces between gas particles.

A balloon filled with carbon dioxide gas at room temperature is placed in a freezer at 5 °C. Which statement describes the resulting effect on the gas particles?

• 1. There is an increase in the kinetic energy of the gas particles.

• 1. There is a decrease in the kinetic energy of the gas particles.

• 1. There is no change in the kinetic energy of the gas particles.

• 1. There is a continuous change in the kinetic energy of the gas particles.