Applications of Ideal Gas Law

Determine the Celsius temperature of 2.49 moles of gas contained in a 1.00-L vessel at a pressure of 143 kPa. 

• -266 degrees C

• -622 degrees C

• 622 degrees C 

• 266 degrees C

Determine the Kelvin temperature required for 0.0470 mol of gas to fill a balloon to 1.20 L under .998 atm pressure. 

• 10 K 

• 110 K 

• 210 K 

• 310 K 

Calculate the volume that a 0.323-mol sample of a gas will occupy at 265 K and a pressure of 0.900 atm.

• 7.18 L 

• 7.81 L

• 4.63 L

• 4.36 L

If the pressure exerted by a gas at 25 degrees C in a volume of 0.044 L is 3.81 atm, how many moles of gas are present?

• .00277 mole

• .00685 mol

• 2.77 mol

• 9.89 mol

Determine the number of moles in a container of gas at STP with a volume of 99.2 L. 

• 2220 moles

• 4.43 moles

• 22.4 moles 

• 76.8 moles

At 250K and 1.75atm, a gas has a mass of 15.3g and occupies 5.60L. What is the molar mass of the gas?

• 32.0g/mol

• 42.2g/mol

• 48.9g/mol

• 54.3g/mol

Find the density of neon gas at .725 atm and 25°C?

• .350g/L

• .473g/L

• .598g/L

• .791g/L

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

• 483 Torr

• 270 Torr

• 1235 Torr

A container holds three gases: oxygen, carbon dioxide, and helium. The partial pressures of the three gases are 2.00 atm, 3.00 atm, and 4.00 atm, respectively. What is the total pressure inside the container?

• 2 atm

• 4 atm

• 3 atm

• 9 atm

The density of an unknown gas is 2.00 g/L at 3.00 atm of pressure and 127^oC. What is the molar mass of this gas?

• 6.94 g/mol

• 15.4 g/mol

• 21.9 g/mol

• 49.2 g/mol