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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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.
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.
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 × 104 Nm-2
Mole fraction of A = xA = 0.85
Mole fraction of B = xB = 1 – xA
= 1 – 0.85
= 0.15
The vapour solution is given by,
Psoln = XA\(P_A^0\) + XB\(P_B^0\)
= 0.85 × 3.4 × 10 + 0.15 × 5.2 × 104
= 2.89 × 10 + 0.78 × 104
= (2.89 + 0.78) × 104
Psoln = 3.67 × 104 Nm-2
Vapour pressure of a solution = 3.67 × 104 Nm-2