Two liquids A and B follow raoult law over entire range of concentration if a solution of A and B has mole Fraction of A as 0.3 then `Y_a` = `x/17` the value of x is
(given : `P_a`= 50 torr and `P_b` = 100 torr)

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. 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).

The vapour pressure of a liqid solution containing A and B is 99 torr. Colvulate mole % of in vapour phese. (Given : P_(A^(@)) = 100 torr , P_(B^(@)) =80 torr)

Two liquids A and B have P_(A)^(0):P_(B)^(0)=1:3 at a certain temperature. If the mole fraction ratio of x_(A) : x_(B) = 1:3 , the mole fraction of A in vapour in equilibrium with the solution at a given temperature is :

The vapour pressure of a pure liquid A is 60 torr at 300K. It forms an ideal solution with another liquid B. The mole fraction of B is 0.25 and the total pressure of the solution is 82.5 torr at 300K. The vapour pressure of pure liquid B at 300K is

Two liquid A & B form an ideal solution. What is the vapour pressure of solution containing 2 moles of A and 3 moles at B at 300K? [Given: At 300K, Vapour pr. Of pure liquid A ("P"_("A")^(@)) =100 torr, Vapour pr. Of pure liquid B ("P"_("B")^(@)) = 300 torr]

2 moles each of liquids A and B are dissolved to form an ideal solution. What will be the mole fraction of B in the vapour phases ? p_(A)^(@) = 120 " torr ", p_(B)^(@) = 80 torr

20 moles of liquid A are mixed with 20 moles of liquid B to form an ideal binary solution. Calculate moles of A in liquid state when half of the solution has vaporized : ( Given : P_(A)^(@)=100 " torr", P_(B)^(@)=121 " torr" )