Vapour pressure of chloroform `(CHCl_3)` and dichloromethane `(CH_2Cl_2)` at 298 K are 200 mm Hg and 415 mm Hg respectively.
Calculate the vapour pressure of the solution prepared by mixing 25.5 g of `CHCl_3` and 40 g of `CH_2Cl_2` at 298 K and,

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

Vapour pressure of pure water at 298 K is 23.8 mm Hg. 50 g of urea (NH_2CONH_2) is dissolved in 850 g of water. Calculate the vapour pressure of water for the solution and its relative lowering.

At 40^@C , the vapour pressure of pure liquids, benzene and toluene, are 160 mm Hg and 60 mm Hg respectively. At the same temperature, the vapour pressure of an equimolar solution of the two liquids, assuming the ideal solution should be

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?

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.

Calculate the volume of 3.6g of water vapour at 273K temperature and 1 atm pressure.