Ideal gas law and density

What pressure, in atm, is exerted by 2.50 L of gas containing 1.35 mol at 47 ^oC?
PV=nRT

• 14.19 atm
• 16.53 atm
• 18.42 atm
• 22.54 atm

At 250 k and 1.75 atm, a gas has a mass of 15.3 g and occupies 5.60 L. What is the molar mass of the gas?
M=mRT/PV

• 32.04
• 42.15
• 48.91
• 54.28

Find the density of Neon gas at .725 atm and 25°C 
D=MP/RT

• .35
• .47
• .60
• .79

What volume does 13.6 g of O₂ gas at 37°C and 135 kPa occupy?
PV=nRT

• 6.22 L
• 8.11 L
• 10.54 L
• 12.73 L

Calculate the partial pressure of H₂ at 20 ^oC when the vapor pressure of water is 17.5 torr. The total pressure of the gases is 750 torr.

• 767.5torr
• 732torr
• 42.86torr

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?

• 483torr
• 270torr
• 1235torr

A 7.50 liter sealed jar at 18 °C contains 0.125 moles of oxygen and 0.125 moles of nitrogen gas. What is the pressure in the container?

• 7.38 atm
• 0.796 atm
• 0.684 atm
• 0.398 atm

A 15.50 gram sample of a gas exerts a pressure of 1.40 atmospheres when held in an 8.00 liter at 22 °C. What is the molar mass (grams/mol) of the gas?

• 33.5 g/mol
• 0.0298 g/mol
• 6.57 g/mol
• 62.2 g/mol

A 500 mL metal cylinder holding 0.100 moles of helium gas is known to rupture at a pressure of 10 atmospheres. At what temperature, in °C, will the container fail?

• 336 °C
• 608 740 °C
• - 272.4°C
• 609 °C

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

• 2222.08 moles
• 4.43 moles
• 22.4 moles 
• 76.8 moles