The vapour pressures of pure liquids A and B are 400 and 600 mm Hg respectively at 298 K . On mixing the two liquids, the sum of their volumes is equal to the volume of the final mixture. The mole fra

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The vapour pressures of pure liquids A and B are 400 and 600 mm Hg respectively at 298 K . On mixing the two liquids, the sum of their volumes is equal to the volume of the final mixture. The mole fraction of liquid B is 0.5 in the mixture. The vapour pressure of the final solution, the mole fractions of components A and B in the vapour phase, respectively are

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Raoult’s law for ideal solution, P T o t a l = P A + P B P T o t a l = x A × P A ∘ + x B × P B ∘ P T o t a l = 1 2 × 400 + 1 2 × 600 = 500 m m o f H g Dalton’s law, y A × P T o t a l = P A y A = x A × P A 0 P T o t a l = 1 2 × 400 500 = 0.4 y B = 1 - 0.4 = 0.6

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