A mixture of two liquids A and B have vapour pressures 3.4 × 104 Nm-2

1.	A mixture of two liquids A and B have vapour pressures 3.4 × 104 Nm-2 and 5.2 × 10 Nm-2. If the mole fractions of A is 0.85, find the vapour pressure of the solution.
Answer» Given : Vapour pressure of pure liquid A = \(P_A^0\) = 3.4 × 10⁴ Nm^-2 Vapour pressure of pure liquid B = \(P_B^0\) = 5.2 × 10⁴Nm^-2 Mole fraction of A = x_A = 0.85 Mole fraction of B = x_B = 1 – x_A = 1 – 0.85 = 0.15 The vapour solution is given by, P_soln= X_A\(P_A^0\) + X_B\(P_B^0\) = 0.85 × 3.4 × 10 + 0.15 × 5.2 × 10⁴ = 2.89 × 10 + 0.78 × 10⁴ = (2.89 + 0.78) × 10⁴ P_soln = 3.67 × 10⁴ Nm^-2 Vapour pressure of a solution = 3.67 × 10⁴ Nm^-2

A mixture of two liquids A and B have vapour pressures 3.4 × 104 Nm-2 and 5.2 × 10 Nm-2. If the mole fractions of A is 0.85, find the vapour pressure of the solution.

Answer»

Given :

Vapour pressure of pure liquid A

= \(P_A^0\) = 3.4 × 10⁴ Nm^-2

Vapour pressure of pure liquid B
= \(P_B^0\) = 5.2 × 10⁴Nm^-2

Mole fraction of A = x_A = 0.85

Mole fraction of B = x_B = 1 – x_A

= 1 – 0.85

= 0.15

The vapour solution is given by,

P_soln= X_A\(P_A^0\) + X_B\(P_B^0\)

= 0.85 × 3.4 × 10 + 0.15 × 5.2 × 10⁴

= 2.89 × 10 + 0.78 × 10⁴

= (2.89 + 0.78) × 10⁴

P_soln = 3.67 × 10⁴ Nm^-2

Vapour pressure of a solution = 3.67 × 10⁴ Nm^-2

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A mixture of two liquids A and B have vapour pressures 3.4 × 104 Nm-2 and 5.2 × 10 Nm-2. If the mole fractions of A is 0.85, find the vapour pressure of the solution.

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