Ideal Gas Law

A sample of 1.00 moles of oxygen at 50^oC and 98.6 kPa occupies a volume of (a)   L.

A sample of 4.25 moles of hydrogen at 20.0^oC occupies a volume of 25.0 L. The pressure of the sample is (a)   kPa.

An unknown gas has a mass of 153 g and occupies 15.0 L at a temperature of 300.0 K and a pressure of 2.00 atm. The molar mass of the gas is (a)   g/mol? (R = 0.082 L atm K^-1 mol^-1)

At 22.0^oC and a pressure of 100.6 kPa, a gas was found to have a density of 1.14 g/L. The molar mass of the gas is (a)   g/mol.

What is the formula for the ideal gas law?

• pv = nrt

• pt = nvr

• pv = ntr

• pt = nrv

What are the units for pressure in the ideal gas law equation?

• Atmospheres

• Torr

• Pascals

• All of the above

What are the units for volume in the ideal gas law equation?

• Milliliters

• Liters

• Cubic meters

• Cubic centimeters

A sample of 2.00 moles of nitrogen gas at 25^oC and 101.3 kPa occupies a volume of ______ L.

• A) 48.9

• B) 24.5

• C) 22.4

• D) 44.8

If the pressure of a gas is doubled while the temperature remains constant, what happens to the volume of the gas according to the ideal gas law?

• A) It doubles

• B) It halves

• C) It remains the same

• D) It quadruples

A gas occupies a volume of 10.0 L at a pressure of 2.00 atm. If the volume is increased to 20.0 L at constant temperature, what is the new pressure?

• A) 1.00 atm

• B) 0.50 atm

• C) 2.00 atm

• D) 4.00 atm