Gas A is composed of nitrogen and oxygen. At 20 ºC, a 0.230 g sample of A exerts a pressure of 1.844 atm while in a 100 mL container. Determine the molar mass and a probable formula of gas A.

A gaseous hydrocarbon contains 79.85 % carbon and 20.15 % hydrogen by mass. At the pressure of 760 mmHg and temperature of 25 °C, a 256mL sample of the gas was measured to have a mass of 0.315 g. Identify the molecular formula of the compound.

Calculate the molar mass of the unknown liquid using the given information obtained via the Dumas method:

mass of vapor = 1.3214 g
volume of flask = 500 mL
pressure = 754.3 Torr
temperature = 99.43 ºC

Assuming you have two flasks at the same temperature, one has a volume of 4 L and the other one has a volume of 5 L. The 4-L flask contains 6.3 g of gas and the pressure is X atm. The 5-L flask contains 0.66 g of gas, and the pressure is 0.6X. Do the two gases have the same molar mass? If not, which flask would contain the gas with the higher molar mass?