What is the vapor pressure at 30°C of a solution of 9.26 g of benzene (C6H6, pure liquid vapor pressure...?
What is the vapor pressure at 30°C of a solution of 9.26 g of benzene (C6H6, pure liquid vapor pressure is 155 torr) and 4.26 g of chloroform (CHCl3, pure liquid vapor pressure is 333 torr)?
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Molar mass benzene = 78 g/mol
Moles benzene = 9.26 / 78 = 0.119
Molar mass chloroform = 119.3 g/mol
Moles chloroform = 4.26 / 119.3 = 0.0357
mole fraction benzene = 0.119 / 0.119 + 0.0357 = 0.769
mole fraction chloroform = 0.0357 / 0.119 + 0.0357 = 0.231
Pa = P°a Xa
This is Raoult's law
Let b = benzene and c = chloroform
Pb = P°b Xb = 155 x 0.769 = 119.2 torr
Pc = P°c Xc = 333 x 0.231 =76.9 torr
Vapor pressure = 119.2 + 76.9 = 196.1 torr