Dalton's Law of Pressure Pressure

Dalton's law equation is used to find what?

• the density of a pure gas

• the total pressure of a pure gas

• the total pressure of a gas mixture

• the volume of a gas mixture

What does gas pressure depend on?

• size of the container and type of gas

• number of particles and average kinetic energy

• size of container and average mass

• the type of gas in the container

What variables must be kept constant in Dalton's law?

• the number of moles

• liters and volume

• temperature and volume

• temperature only

In a mixture of gases, each gas contributes to the total pressure. The individual contribution of each gas is known as the _________________.

• partial volume

• partial pressure

• molar mass

• mole ratio

A tank of gas contains 50 kPa of helium, 50 kPa of argon, and 100 kPa of neon. What is the total pressure of the gas mixture?

• 100 kPa

• 50 kPa

• 200 L

• 200 kPa

A container holds a mixture of two different gases. The oxygen in a container exerts 80 mmHg of pressure on the inside of the container. The total pressure inside the container is 120 mmHg. What is the pressure of the other gas in the container?

• 200 mmHg

• 80 mmHg

• 40 mmHg

• 120 mmHg

Which container will have a lower pressure?

• left

• right

• they both have the same pressure

• I don't know

A mixture of hydrogen, nitrogen, and water vapor has a total pressure of 864 mmHg. The partial pressure of hydrogen is 220 mmHg and that of nitrogen is 410 mmHg. What is the partial pressure of water vapor?

• 234 mmHg

• 1.37 mmHg

• 2.64 mmHg

• 1, 494 mmHg

Three gases, Ar, N2 and H2 are mixed in a 500L container. Ar has a pressure of 255 torr, N2 has a pressure of 228torr and H2 has pressure of 752torr. What is the total pressure in the container?

• 483torr

• 270torr

• 1235torr

Dalton's Law states...

• that at a constant temperature the volume of a confined ideal gas varies inversely with its pressure.

• that the total pressure exerted by the mixture of non-reactive gases is equal to the sum of the partial pressures of individual gases

• how gases tend to expand when heated

• that the density of an ideal gas at constant pressure varies inversely with the absolute temperature of the gas.