Pressure of gasoline in a closed container

[barryj]

Homework Statement

A small amount of gasoline is placed in a 1 liter container along with the normal atmospheric pressure of 760 torr at 25C. Much but not all of the gasoline evaporates creating an increased pressure inside the container. At equilibrium, what will be the total pressure in the container?

Relevant Equations

pv = nrt P total = P atmosphere + P gasoline

If I knew how much of the gasoline evaporated, then I could use p = nRT/V to fine the partial pressure of the gasoline and add it to the pressure of the atmosphere. So my question is, How do I find how much of the gasoline will evaporate. I would think that the gasoline would evaporate until it reached some critical pressure at which time the evaporation rate would equal the disolving rate. but how do I find this? Is there some law I do not know about?

 

[Borek]

Gasoline is a mixture of hydrocarbons, and it doesn't have a definite composition - so it is not like there is an unambiguous answer to the question.

There is not much you can do without tables of saturated vapor pressure of gasoline (or it most typical components) at 25°C.