Ideal Gas Law and Partial Pressure

What is the pressure exerted by 5.00 moles of nitrogen gas contained in a 30.0 Liter container at 25.0 °C?

• 3670 atm
• 0.245 atm
• 4.08 atm
• 605 atm

At 17 °C, a 0.80 mole sample of a gas exerts a pressure of 1.2 atmospheres. What is the volume of the container?

• 22.9 Liters
• 2355 Liters
• 0.0630 Liters
• 15.9 Liters

An 18 liter container holds 16.00 grams of oxygen gas (O₂) at 45 °C. What is the pressure in the container?

• 0.725 atm
• 11.0 atm
• 23.2 atm
• 1.45 atm

At what temperature (in Kelvin) would 4.0 moles of hydrogen gas in a 100 liter container exert a pressure of 1.00 atmospheres?

• 0.0305 K
• 0.487 K
• 32.8 K
• 304.5 K

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.

A gaseous mixture contains 5.0 moles of nitrogen and 10.0 moles of helium. The total pressure in the container is 3.0 atmospheres. What is the partial pressure of the nitrogen?

• 1 atm

• 0.5 atm

• 3.0 atm

• 2.0 atm

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

The total pressure of a mixture of oxygen and nitrogen gas is 400.0 kPa. What is the partial pressure of nitrogen if the pressure of oxygen is 150.0 kPa?

• 400.0 kPa

• 550.0 kPa

• 250.0 kPa

• 101.3 kPa

What does the variable "n" represent in the ideal gas law?

• pressure

• volume

• moles

• the gas constant

• temperature

What does the variable "R" represent in the ideal gas law?

• pressure

• volume

• moles

• the gas constant

• temperature