AP Chemistry Gas Laws

Calculate the volume of a gas at STP if it contains 0.5 moles of gas and the pressure is 1 atm.

• 11.2 liters

• 5.6 liters

• 0.5 liters

• 112 liters

What are the factors that can cause a gas to deviate from ideal behavior?

• Low pressure, high temperature, and strong intermolecular forces.

• High pressure, low temperature, and intermolecular forces.

• High temperature, low pressure, and weak intermolecular forces.

• Low temperature, high pressure, and weak intermolecular forces.

State Dalton's Law of partial pressure.

• The total pressure exerted by a mixture of non-reacting gases is equal to the difference of the partial pressures of the individual gases.

• The total pressure exerted by a mixture of non-reacting gases is equal to the sum of the partial pressures of the individual gases.

• The total pressure exerted by a mixture of non-reacting gases is equal to the product of the partial pressures of the individual gases.

• The total pressure exerted by a mixture of non-reacting gases is equal to the average of the partial pressures of the individual gases.

Calculate the partial pressure of oxygen in a mixture of gases if the total pressure is 3 atm and the partial pressure of nitrogen is 2 atm.

• 2

• 3

• 4

• 1

What is the relationship between the average kinetic energy of gas particles and the temperature of the gas?

• Unrelated

• Depends on the pressure

• Directly proportional

• Inversely proportional

How does the size of gas particles affect the pressure of a gas?

• The pressure of a gas increases with the size of gas particles.

• The size of gas particles does not affect the pressure of a gas.

• The pressure of a gas decreases with the size of gas particles.

• The size of gas particles directly determines the pressure of a gas.

A gaseous mixture containing 7.0 moles of nitrogen, 2.5 moles of oxygen, and 0.5 moles of helium exerts a total pressure of 0.90 atmosphere. What is the partial pressure of the nitrogen?

• 0.13 atm

• 0.27 atm

• 0.63 atm

• 0.90 atm

A 2.00-liter sample of nitrogen gas at 27° C and 600. millimeters of mercury is heated until it occupies a volume of 5.00 liters. If the pressure remains unchanged, the final temperature of the gas is

• 68^o C

• 120^o C

• 477^o C

• 677^o C

The system shown above is at equilibrium at 28 °C. At this temperature, the vapor pressure of water is 28 millimeters of mercury. The partial pressure of O2(g) in the system is

• 28 mm Hg

• 56 mm Hg

• 133 mm Hg

• 161 mm Hg

A flask contains 0.25 mole of SO₂(g), 0.50 mole of CH₄(g), and 0.50 mole of O₂(g). The total pressure of the gases in the flask is 800 mm Hg. What is the partial pressure of the SO₂(g) in the flask?

• 600 mm Hg

• 250 mm Hg

• 200 mm Hg

• 160 mm Hg