Question

A volatile compound with a mass of 0.8822 grams is placed in an evacuated 0.250 L flask. The flask is heated to evaporate the compound. At 99C, the pressure in the flask is 1.25 atm. What is the molar mass of the compound?

Answer 1

Using the gas equation,

$PV= nRT$

$1.25 \times 0.250 = \dfrac{0.8822}{x} \times 0.083 \times372$

$0.3125 = \dfrac{0.8822}{x} \times 30.876$

$x = \dfrac{27.23}{0.3125}$

$x = 87.16$