Two liquids X and Y on mixing form an ideal solution. At `30^@C`, the vapour pressure of the solution containing 3 mol of X and 1 mol of Y is 550 mm Hg. But when 4 mol of X and 1 mol of Y are mixed, the vapour pressure of the solution thus formed is 560 mm Hg. What would be the vapour pressure of pure X and Y at this temperature?

Two liquids A and B form an ideal solution. At 300 k, the vapour pressure of a solution containing 1 mole of A and 3 moles of B is 550 mm of Hg. At the same temperature, if one mole of B is added to this solution, the vapour pressure of the solution increases by 10 mm of Hg. Determine the vapour pressure of A and B in their pure states.

What is the vapour pressure of pure water at 100^(@)C temperature ?

Calculate the vapour pressure of the solution. The molefraction of the solute is 0.25. The vapour pressure of the pure solvent is 0.8atm.

Two liquids A and B form an ideal solution. What is the vapour pressure of solution containing 2 moles of A and 3 moles of B at 300 K? [Given : At 300 K, vapour pressure of pure liquid A (p _A^0) = 100 torr and vapour pressure of pure liquid B (p _B^0) = 300 torr]

The vapour pressure of a given liquid will decrease if :

At 25^(@) C temperature, vapour pressure of water is 23.55mm. What will be the vapour pressure of the solution when 6g of urea is mixed with 100g of water?

At 25^(@) C temperature, vapour pressure of water is 23.55mm. What will be the vapour pressure of the solution when 6g of urea is mixed with 100g of water?

If relative decrease In vapour pressure is 0.4 for a solution containing 1 mol NaCl in 3 mol of H_2O , then % ionization of NaCl is

The vapour pressure of pure liquid Ais 70 torr at 27^@C It forms an ideal solution with another liquid B. The mole fraction of B 1s 0.2 and total vapour pressure of the solution is 84 torr at 27^@C . The vapour pressure of pure liquid B at 27^@C is