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.

P_{total}= X_{a}^{L}*P_{a}^{o} + X_{b}^{L}*P_{b}^{o}

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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.