If `P_(A)` is the vapour pressure of a pure liquid A and the mole fraction of A in the mixture of two liquids A and B is x, the parial vapour pressure of A is:

P_(A)=(235y -125xy)mm of HgP_(A) is partial pressure of A,x is mole fraction of B in liquid phase in the mixture of two liquids A and B and y is the mole fraction of A in vapour phase, then P_(B)^(@) in mm of Hg is:

P_(A)=(235y -125xy)mm of HgP_(A) is partial pressure of A,x is mole fraction of B in liquid phase in the mixture of two liquids A and B and y is the mole fraction of A in vapour phase, then P_(B)^(@) in mm of Hg is:

P_(A)=(235y -125xy)mm of HgP_(A) is partial pressure of A,x is mole fraction of B in liquid phase in the mixture of two liquids A and B and y is the mole fraction of A in vapour phase, then P_(B)^(@) in mm of Hg is:

Two liquids A and B form an ideal solution. The ratio of vapour pressures of pure liquids A and B are 3: 5. If the mole fraction of A in the liquid solution at equilibrium with vapours is 0.4, then the mole-fraction of B in the liquid is

Two liquids A and B are mixed to form an ideal solution. The totol vapour pressure of the solution is 800 mm Hg. Now the mole fractions of liquid A and B are interchanged and the total vapour pressure becomes 600 mm of Hg. Calculate the vapour pressure of A and B in pure form. (Given : p_(A)^(@)-p_(B)^(@)=100 )

Two liquids A and B are mixed to form an ideal solution. The totol vapour pressure of the solution is 800 mm Hg. Now the mole fractions of liquid A and B are interchanged and the total vapour pressure becomes 600 mm of Hg. Calculate the vapour pressure of A and B in pure form. (Given : p_(A)^(@)-p_(B)^(@)=100 )

At 300 K the vapour pressure of two pure liquids, A and B are 100 and 500 mm Hg, respectively. If in a mixture of a and B, the vapoure is 300 mm Hg, the mole fractions of a in the vapour phase, respectively, are -

The vapour pressure of a mixure of 1 mole of liquid 'A' and 3 mole of liquid 'B' is 550 mm of Hg. When one mole of liquid 'B' is further added, the vapour pressure of the solution increases by 10 mm of Hg. The vapour pressure of pure liquid A and B are respectively in mm of Hg .

In a mixture of A and B having vapour pressure of pure A and B are 400 m Hg and 600 mm Hg respectively. Mole fraction of B in liquid phase is 0.5. Calculate total vapour pressure and mole fraction of A and B in vapour phase .