Home
Class 12
CHEMISTRY
At a certain temperature, the vapour pre...

At a certain temperature, the vapour pressure of pure ether is `640 mm` and that of pure acetone is `280 mm`. Calculate the mole fraction of each component in the vapour state if the mole fraction of ether in the solution is `0.50.`

Text Solution

Verified by Experts

In the given solution, both ether and acetone are volatile, so from Raoult’s Law, we can have vapour pressure of solution `(P_("Total"))`.
Let A : ether and B : acetone.
`P_("Total") =P_A+P_B =P_A^0chi_A+P_B^0chi_B`
`rArr P_("Total")= 646 xx0.5+283xx0.5 =464.5 mm`
Now mole fraction in vapour state is given as follows
`chi_A("vapour") =(P_A)/(P_("Total")) =(P_A^0chi_A)/(P_(" Total"))=(646xx0.5)/(464.5)=0.695`
`chi_B ("vapour")=(P_B)/(P_"Total")=(P_B^0chi_B)/(P_"Total")=(283xx0.5)/(464.5)=0.305`
Promotional Banner

Similar Questions

Explore conceptually related problems

The vapour pressure of a pure liquid at 25^(@)C is 100 mm Hg. Calculate the relative lowering of vapour pressure if the mole fraction of solvent in solution is 0.8.

Vapor pressure of a solution of Volatile components and composition of vapor: Consider a solution containing 738 g of water and 253 g of ethanol (C_(2)H_(5)OH) at 323 K . At this temperature, the vapour pressure of pure ethanol is 0.292 atm and the vapor pressure of pure water is 0.122 atm . Calculate the vapour pressure of the solution and mole fraction of every component in vapour phase. Strategy: First calculate the moles and the mole fraction of each component in the liquid solution. Then apply Raoult's law to each of the two volatile components to calculate their partial pressures. The total vapour pressure is the sum of the partial vapour pressures of the components and the mole fraction of a components in a gaseous mixture equals the ratio of its partial pressure to the total pressure.

The vapour pressure of pure benzene and toluene are 160 and 60 mm Hg respectively. The mole fraction of benzene in vapour phase in contact with equimolar solution of benzene and toluene is :

The vapour pressure of pure benzene at 25^@C is 640 mm Hg and that of the solute A in benzene is 630 mm of Hg. The molality of solution of

The vapour pressure of pure benzene and toluene at 40^(@)C are 184.0 torr and 59.0 torr, respectively. Calculate the partial presure of benzene and toluene, the total vapour pressure of the solution and the mole fraction of benzene in the vapour above the solution that has 0.40 mole fraction of benzene. Assume that the solution is ideal.

The vapour pressure of pure liquid solvent A is 0.80 atm . When a non-volatile substance B is added to the solvent, its vapour pressure drops to 0.60 atm , the mole fraction of component B in the solution is

The vapour pressure of a dilute aqueous solution of glucose is 740 mm of mercury at 373 K. The mole fraction of the solute is: