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 vapour pressure of two pure liquids A and B are 50 and 40 torr respectively. If 8 molrs of A is mixed with x moles of B , then vapour pressure of solution obtained is 48 torr. What is the value of x.

The vapour pressure of two pure liquids A and B are 5 and 10 torr respectively. Calculate the total pressure of the solution (in torr) obtained by mixing 2 mole of A and 3 mole of B.

At 20^@C the vapour pressure of pure liquid A is 22 mm Hg and that of pure liquid B is 75mm Hg. What is the composition of the solutions of these two components that has a vapour pressure of 48.5 mm Hg at this temperature?

Benzene and toluene form ideal solution over the entire range of composition. The vapour pressure of pure benzene and toluene at 300 K are 50.71 mm Hg and 32.06 mm Hg respectively. Calculate the mole fraction of benzene in vapour phase if 80 g of benzene is mixed with 100 g of toluene.

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

The vapour pressure of two liquids P and Q are 80 and 60 torr respectively. The total vapour pressure of solution obtained by mixing 3 mol of P and 2 mol of Q would be.

Heptane and octane form an ideal solution at 373 K, the vapour pressures of the pure liquids at this temperature are 105.2 kPa and 46.8 kPa respectively. If the solution contains 25 g of heptane and 28.5 g of octane, calculate. mole fraction of octane in the vapour phase.