`A` and `B` form ideal solution, at `50^(@)C,P_(A^(0)` is half `P_(B)^(0)`. `A` solution containing `0.2` mole of `A` and `0.8` mole of `B` has a normal boiling point of `50^(@)C`. Calculate `P_(A)^(0)` and `P_(A)^(0)` at `50^(@)C`.

A and B form ideal solution, at 50^(@)C,P_(A^(0) is half P_(B)^(0) . The solution containing 0.2 mole of A and 0.8 mole of B has a normal boiling point of 50^(@)C . Calculate P_(A)^(0) and P_(B)^(0) at 50^(@)C .

For an ideal solution with P_(A)^(0)gt P_(B)^(0) , which of the following is true?

The sum of mole fractions of A, B and C in an aqueous solution containing 0.2 moles of each A, B and C is

Two liquids A and B form an ideal solution. What is the vapour pressure of solution containing 2 moles of A and 3 moles of B at 300 K? [Given : At 300 K, vapour pressure of pure liquid A (p _A^0) = 100 torr and vapour pressure of pure liquid B (p _B^0) = 300 torr]

Liquid A and B form an ideal solution. The boiling point of solution is 72^(@) C, when the external pressure is 0.6 bar. If then solution contains 200 moles of liquid A, then moles of liquid B is : [Given : P_(A)^(@)=0.4 "bar" "and" P_(B)^(@)=1.0 "bar" "at" 72^(@)C]