At 50.0 ºC and a pressure of 703 torr, a gas was found to have a density of 1.34 g L-1.?
At 50.0 ºC and a pressure of 703 torr, a gas was found to have a density of 1.34 g L-1. Calculate its molar mass.
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PV = nRT
let weight of gas be w and molecular mass be M
PV = w/M RT
PM = w/V RT
PM = dRT
where P = 703 torr = 703/760 = 0.925 atm
M = ? g/mole
d = 1.34 g/L
R = 0.0821 L atm/k/mole
T = 50 + 273 = 323 K
putting the values....
0.925 X M = 1.34 X 0.0821 X 323
M = 35.535/0.925 = 38.416 g/mole