Question

5. At 20 °C the vapor pressure of pure benzene (C6H6) is 75.0 torr, and that of toluene (C7H8) is 22.0 torr. Assume that benzene and toluene form ideal solutions. What is the mole fraction of benzene in a solution that has a (total) vapor pressure of 55.0 torr at 20 °C? A) 1.764 B) 0.623 C) 0.106 D) −0.362 E) 4.451

Answer 1

B) 0.623

Step-by-step explanation:

In an ideal solution of benzene and toluene, vapor pressure is:

Total Pressure = Xbenzene× P°benzene + Xtoluene× P°toluene

Where X is mole fraction of each compound, and P° is vapor pressure of pure compound

Replacing with given values:

55.0 torr = Xbenzene× 75.0 torr + Xtoluene× 22.0 torr (1)

Also, the sum of moles fraction is = 1:

1 = Xbenzene + Xtoluene (2)

Replacing (2) in (1):

55.0 torr = Xbenzene× 75.0 torr + (1 - Xbenzene) × 22.0 torr

55.0 torr = Xbenzene×75.0 torr + 22.0 torr - Xbenzene×22.0 torr

33.0 torr = Xbenzene×53.0torr

0.623 = Xbenzene

Mole fraction of benzene is B) 0.623