Two liquids A and B have vapour pressure in the ratio `P_A^(circ)` : `P_B^(circ)` = 1:3 at a certain temperature. Assume A and B form an ideal solution and the ratio of mole fractions of A to B in the vapour phase is 4:3. Then the mole fraction of B in the solution at the same temperature is :

Two liquid A and B have vapour pressure in the ratio P_A^(@) : P_B^(@) =1.3 at a certain temperature.Assume A and B from an ideal solution and the ratio of mole fractions of A to B in the vapour phase is 4 : 3, then the mole fraction of B in the solution at the same tempreature is : (a) 1/5 (b) 2/3 (c) 4/5 (d) 1/4

Two liquids A and B have vapour pressures in the ratio of p_(A)@,p_(B)@ = 1 : 2 at a certain temperature. Suppose we have an ideal solution of A and B in the mole fraction ratio A:B = 1:2 . What would be the mole fraction of A in the vapour in equilibrium with the solution at a given temperature? a. 0.25 , b. 0.2 , c. 0.5 d. 0.33

If Pa and Pb are 108 and 36 torr respectively. What will be the mole fraction of A is vapour phase if B has mole fraction in solution 0.5:

Draw a suitable diagram to express the relationship for ideal solutions of A and B between vapour pressure and mole fractions of components at constant temperature

At a certain temperature, the vapour pressure of pure ether is 640 mm and that of pure acetone is 280 mm . Calculate the mole fraction of each component in the vapour state if the mole fraction of ether in the solution is 0.50.

Two liquids A and B have vapour pressure of 0.600 bar and 0.2 bar, respectively. In an ideal solution of the two, calculate the mole fraction of A at which the two liquids have equal partial pressures.

The vapour pressure of pure liquid A is 0.80 atm. On mixing a non-volatile B to A, its vapour pressure becomes 0.6 atm. The mole fraction of B in the solution is:

A certain ideal solution of two liquids A and B has mole fraction of 0.3 and 0.5 for the vapour phase and liquid phase, respectively. What would be the mole fraction of B in the vapour phase, when the mole fraction of A in the liquid is 0.25 ?

Liquids A and B form ideal solution over the entire range of composition. At temperature T, equimolar binary solution of liquids A and B has vapour pressure 45 torr. At the same temperature, a new solution of A and B having mole fractions x_(A) and x_(B) , respectively, has vapours pressure of 22.5 torr. The value of x_(A)//x_(B) in the new solution is ______. (Given that the vapour pressure of pure liquid A is 20 torr at temperature T).

At 300 K two pure liquids A and B have vapour pressures respectively 150 mm Hg and 100 mm Hg. In a equimolar liquid mixture of A and B, the mole fraction of B in the vapour phase above the solution at this temperature is: