Part 1. Determine the molar mass of a 0.314-gram sample of gas having a volume of 1.6 L at 287 K and 0.92 atm. Show your work. Part 2. Describe the temperature and pressure conditions at which the gas behaves like an ideal gas.

See below

Explanation:

Part 1: We can use the equation PV=nRT where p is pressure of the gas in atm (0.92atm), V is the volume of gas in L (1.6L), n is the number of moles of the gas in mol (we don't know), R is the general gas constant (0.0821L.atm/mol.K), and T is the temperature of the gas in K (T=287K). n=(0.92atm)(1.6L)/(0.0821L.atm/mol.K)(287k)=0.1825mol. To find the molar mass, we can use the relation n= mass/molar mass which would be (0.314g)/(0.1825mol)= 1.721g/mol.

Part 2: A gas is considered to be ideal when the particles have zero volume and the intermolecular forces are also at zero. However, the gas has a significant volume and the intermolecular forces increase, thus deviating from ideal gas behavior. If the gas were to have a low pressure and high temperature, it will behave more like an ideal gas.