Question

An ideal liquid solution has two volatile components.

In the vapor in equilibrium with the solution, the mole fractions of the components are

(a) both 0.50; (b) equal, but not necessarily 0.50; (c) not very likely to be equal; (d) 1.00 for the solvent and 0.00 for the solute.

Is the answer A? The question is asking what will happen when the vapor is in equilibrium. or something like that. Its sort of vague.

No one has answered this question yet.

Answer 1

The answer most likely is c. The vapor in equilibrium with the solution is the sum of the vapor pressure of each liquid. Each liquid has a vapor pressure that depends upon two things; the mole fraction and the vapor pressure of the pure solvent.
P_solvent = X_solvent*P^o_{pure solvent}
So the solution is not likely to have the mole fraction the same AND not likely to make of two solvents that have the same vapor pressure for the pure solvent.

Answer 2

oh. that's the complete opposite of what i thought. thanks