Liquid equilibrium -- real-life problem, not a homework?

Question

A mix of 2 (for simplicity) liquids at known concentrations is placed into a sealed vial. All physical parameters of liquids are known, e.g. MW, Density, Vapor pressure & any other that might be needed. The volumes of both vial and the mix in it are also know.
After gas-liquid equilibrium is achieved, what are concentrations of the compound in the liquid phase.

I'll appreciate any intermediate answers as well, i.e. #moles of either in either gas or liquid.

Edward,
I'm well aquinted with Dalton and Raoult's law, both of which are a part of the solution. I'm a chemist and the problem presented has real-life application related to my work.

I went as far as calculating total moles in both vapor and liquid phases after the equilibrium, but have difficulties obtaining moles of individual components.

Answer 1

1. This is not as straight forward as it seems since evaporation of denser liquid may be inhibited by lighter liquid as the lighter liquid would cover the surface of the denser one. A continuous and thorough mixing in a controlled environment is strongly recommended.
2. Each liquid based on environmental pressure and temperature will have a particular amount of vapor present
3. Dalton's Law of partial pressure would be of use to determine amount of vapor of each substance in each case.
4. If the amount of subsurface is known prior to mixing and it's amount of vapor computed then it is difference between these values that must tell you what is its amount in liquid state.
5. If by concentration you mean the ration of amount present to total volume of all liquids than we are done with the problem.

I wonder don't you have anything better to do but to ask these questions. Frankly I had nothing better to do answering yours. LOL
Have fun