Here it is:
(BTW, it's harder than it looks)
You have a solution of two volatile liquids, A and B (assume ideal behavior). Pure liquid A has a vapor of 350.0 torr and pure liquid B has a vapor pressure of 100.0 torr at the temperature of the solution. The vapor at equilibrium above the solution has double the mole fraction of substance A that the solution does. What is the mole fraction of liquid A in the solution?
I used V sup as vapor state and L has solution (liquid state). The o sup means "pure solvent by itself"
Since both of the liquids are VOLATILE, I used the altered Raoult's Law equation.
Ptotal= XaL*Pao + XbL*Pbo
I cleaned up the messy work and reorganized it.
I didn't want to type it all above due to all the superscripts, so I took a picture.