Vapour pressure of pure `A(p_(A)^(@))=100` mm Hg
Vapour pressure of pure `B(p_(B)^(@))= 150` mm Hg
2 mol of liquid A and 3 mol of liquid B are mixed to form an ideal solution. The vapour pressure of solution will be:

At a particular temperature, the vapour pressure of two liquids A and B are 120 and 180 mm Hg respectively. If 2 mole of A and 3 mole of B are mixed to form an ideal solution, the vapour pressure of the solution at the same temperature will be (in mm Hg)

A 300 K the vapour pressure of an ideal solution containing 1 mole of liquid A and 2 moles of liquid B is 500 mm of Hg. The vapour pressure of the solution increases by 25 mm of Hg if one more mole of B is added to the above ideal solution at 300 K. Then vapour pressure of A in its pure state is :

Liquids A (p_(A)^(@)=360" mm Hg") and B(p_(B)^(@)=320" mm Hg") are mixed. If solution has vapour pressure 340 mm Hg, then mole fraction of B will be

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 .

At 300 K the vapour pressure of an ideal solution containing 1 mole of liquid A and 2 moles of liquid B is 500 mm of Hg. The vapour pressure of the solution increases by 25 mm of Hg, if one more mole of B is added to the above ideal solution at 300K. Then the vapour pressure of A in its pure state is

4 mole of pure liquid A (P_(A)^(0)=80mm of Hg) and 6 mole of pure liquid B (P_(B)^(0)=100mm of Hg) are mixed . The vapour pressure of the resulting solution is found to be 90 mm of Hg then