The vapour pressure of pure liquids A and B are 100mm and 200mm respectively. The total vapour pressure of the solution is 175mm. If A and B forms an ideal solution then the mole fraction of A in liquid and vapour phase respectively are

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0.25, 0.14

0.14, 0.25

0.52, 0.41

0.41, 0.52

answer is A.

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Detailed Solution

$P = P_{A}^{o} x_{A} + P_{B}^{o} x_{B}$

$175 = 100 \times x_{A} + 200 (1 - x_{A})$

$175 = 100 \times x_{A} + 200 - 200 x_{A}$

$- 25 = - 100 x_{A}$

$x_{A} = \frac{25}{100} = 0.25$

$y_{A} = \frac{P_{A}}{P} = \frac{P_{A}^{o} x_{A}}{P}$

$y_{A} = \frac{100 \times 0.25}{175} = \frac{25}{175} = 0.14$

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