Question

the mass of a gaseous compound of phosphorus is 3.9 g at 457.4 K in a 1.16 L container and at a pressure of 732.3 mm Hg. What is the molar mass of the compound

Answer 1

Its a gas so : PV=nRT
We need to convert the pressure from mmHg to atm so we dived it by 760

n=PV/RT =(732.3/760 x 1.16 )/(0.08205x 457.4)= 0.029

And we know that n=m/M
M= m/n= 3.9/0.029 = 130,95 g/mol