Question

a) Whatis the composition in mole fractions of a solution of benzene and toluene that has a vapor pressure of 35 torr at 20 °C? Assume the mixture formsan ideal solution. The vapor pressure of benzene (C6H6) is 75 torr and the vapor pressure of toluene (C7H8)is 22 torr at 20 °C.b) What is the composition in mole fractions of the vapor above the solution in part a? How does this problem relate to the process of fractional distillation?

Answer 1

molar composition for liquid

xb= 0.24

xt=0.76

molar composition for vapor

yb=0.51

yt=0.49

Step-by-step explanation:

For an ideal solution we can use the Raoult law.

Raoult law: in an ideal liquid solution, the vapor pressure for every component in the solution (partial pressure) is equal to the vapor pressure of every pure component multiple by its molar fraction.

For toluene and benzene would be:

`P_(B)=x_(B)*P_(B)^(o)`

`P_(T)=x_(T)*P_(T)^(o)`

Where:

`P_(B)` is partial pressure for benzene in the liquid

`x_(B)` is benzene molar fraction in the liquid

`P_(B)^(o)` vapor pressure for pure benzene.

The total pressure in the solution is:

`P= P_(T)+ P_(B)`

And

`1=x_(B)+x_(T)`

Working on the equation for total pressure we have:

`P=x_(B)*P_(B)^(o) + x_(T)*P_(T)^(o)`

Since
`x_(T)=1-x_(B)`

`P=x_(B)*P_(B)^(o) + (1-x_(B))*P_(T)^(o)`

We know P and both vapor pressures so we can clear
`x_(B)` from the equation.

`x_(B)=(P- P_(T)^(o))/( P_(B)^(o) - P_(T)^(o))`

`x_(B)=(35- 22)/(75-22) = 0.24`

So

`x_(T)=1-0.24 = 0.76`

To get the mole fraction for the vapor we know that in the equilibrium:

`P_(B)=y_(B)*P`

`y_(T)=1-y_(B)`

So

`y_(B) =(P_(B))/(P)=( x_(B)*P_(B)^(o))/(P)`

`y_(B)=(0.24*75)/(35)=0.51`

`y_(T)=1-0.51=0.49`

Something that we can see in these compositions is that the liquid is richer in the less volatile compound (toluene) and the vapor in the more volatile compound (benzene). If we take away this vapor from the solution, the solution is going to reach a new state of equilibrium, where more vapor will be produced. This vapor will have a higher molar fraction of the more volatile compound. If we do this a lot of times, we can get a vapor that is almost pure in the more volatile compound. This is principle used in the fractional distillation.