Home
Class 12
CHEMISTRY
Two liquids Aand B have vapour pressures...

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`

Text Solution

AI Generated Solution

To solve the problem, we need to determine the mole fraction of liquid A in the vapor phase that is in equilibrium with an ideal solution of liquids A and B, given their vapor pressures and mole fractions. ### Step-by-Step Solution: 1. **Understand the Given Ratios**: - The vapor pressures of A and B are in the ratio \( P^0_A : P^0_B = 1 : 2 \). - The mole fraction ratio of A to B in the solution is \( X_A : X_B = 1 : 2 \). ...
Promotional Banner

Topper's Solved these Questions

  • SOLUTIONS

    CENGAGE CHEMISTRY ENGLISH|Exercise Solved Examples|40 Videos

  • SOLUTIONS

    CENGAGE CHEMISTRY ENGLISH|Exercise Exercises (Linked Comprehension)|58 Videos

  • SOLID STATE

    CENGAGE CHEMISTRY ENGLISH|Exercise Ex 1.2 (Objective)|9 Videos

  • SURFACE CHEMISTRY

    CENGAGE CHEMISTRY ENGLISH|Exercise Archives Subjective|2 Videos

Similar Questions

Explore conceptually related problems

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

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 ?

Two liquids A and B have P_A^(@)" and P_B^(@) in the ratio of 1 : 3 and the ratio of number of moles of A and B in liquid phese are 1 : 3 then mole fraction of 'A' in vapour phase in equilibrium with the solution is equal to :

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.

If two substances A and B have p_(A)^(@): p_(B)^(@) = 1:2 and have mole fraction in solution as 1:2 then mole fraction of A in vapour phase is

An ideal solution was found to have a vapour pressure of 80 torr when the mole fraction of a non-volatile solute was 0.2. What would be the vapour pressure of the pure solvent at the same temperature?

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:

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.

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:

The vapour pressure of a liquid decreases by 10 torr when a non-volatile solute is dissolved. The mole fraction of the solute in solution is 0.1. What would be the mole fraction of the liquid if the decrease in vapour pressure is 20 torr, the same solute being dissolved?