At 298 K the vapour pressure of pure benzene `C_(6) H_(6) ` is 0.256 bar and vapour pressure of pure toluene, `C_(6)H_(8) ` is 0.925 bar. If the mole fraction of benzene in solution is 0 . 40 , find the total vapour pressure of solution. Also find the mole fraction of toluene in vapour phase

At some temperature the vapour pressure of pure benzene, C_(6) H_(6) is 0 . 256 bar and vapour pressure of toluene, C_(6) H_(5) CH_(3) is 0 . 0 925 bar, if the mole fraction of toluene in a solution is 0 . 60 (i) What is the total vapour pressure of the solution ? (ii) Calculate the composition of the vapour phase in terms of mole fraction.

The vapour pressure of pure liquid A at 310^@C is 0.158bar. The vapour pressure of this liquid in solution with liquid B is 0.095 bar. Calculate the mole fraction of A in the solution if the mixture obeys Raoult's law.

The mole fraction of benzene in a solution with toluene 0.50 calculate the mass percent of benzene in the solution.

The vapour pressure of ethyl alcohol at 298K is 40 mm of Hg. Its mole fraction in a solution with methyl alcohol is 0.80. what is the vapour pressure in solution if the mixture obeys Raoult's law?

The vapour pressure of pure liquids A and B are 450 and 700 mm Hg at 350 K respectively. Find out the composition of the liquid mixture if total vapour pressure is 600 mm Hg. Also find the composition of the vapour phase.

The mole fraction of toluene in a solution with benzene is 0.50. calculate the weight percent of toluene in solution.