A 1.49 g sample of a pure gas occupies a volume of 981 mL at 42 degrees celcius and 878 mm Hg. Determine the molar mass of the compound.
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Using the ideal gas equation;
`PV = nRT`
`n = (PV)/(RT)`
`P = 878mmHg = 878/760 atm = 1.155atm`
`V = 981mL = 0.981L`
`R = 0.08206(atmL/)(molK)`
`T = 273+42 = 315K`
`n = (1.155xx0.981)/(0.8206xx315)`
`n = 0.0044 mol`
`n = m/M`
`0.004 = 1.49/M`
`M = 1.49/0.004 = 338.64g/(mol)`
So the molar mass of the compound is 338.64g/mol
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