Mole fraction of vapour of `A` above solution in mixture of `A` and `B(X_(A) = 0.4)` will be `(P_(A)^(@) = 100mm, P_(B)^(@) = 200 mm)`:

Molal fraction of A vapours above te solution in mixture of A and B ["MA"_(5)]"A"_(3) will be ["Given ":"P"_("A")^(@)=100"mm Hg and"" P"_("B")^(@)=200"mm Hg"]

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 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 )

The total vapour pressure of a mixture of 1 mole of A ( P_A = 200 mm Hg ) and 3 mole of B ( P_B= 360 mm Hg) is 350 mm Hg. Then