The vapor pressure of benzene is 750. Torr and the vapor pressure of toluene is
ID: 835609 • Letter: T
Question
The vapor pressure of benzene is 750. Torr and the vapor pressure of toluene is 300 torr at a certain temperature. You make a solution of benzene and toluene. You place this solution is a closed container and wait for the vapor to come into equilibrium with the solution. Next, you take some vapor and condensed the vapor all into liquid. You put this liquid (condensed vapor) into another closed container and wait for the vapor to come into equilibrium with the new liquid to come into equilibrium with the vapor phase. You then analyze this new vapor (using gas chromatograph) and find that the mole fraction of benzene in this vapor is 0.714. What is the mole fraction of benzene in the original solution, assuming the solution behalves ideally?
Please show work to show me how to approach this! Thanks!
Explanation / Answer
Assuming ideal mixtures and ideal gas phase, there is certain relation between liquid and vapor mole fractions in equilibrium.
Let x and y be the mole fraction of Benzene in liquid and vapor phase respectively. Since we consider a binary mixture the corresponding values for Toluene are (1-x) and (1-y).
Assuming ideal liquid mixture the partial pressure of each compound is given by Raoult's law, which states that partial pressure equals mole fraction times pure component vapor pressure
PB = x?PB
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