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The vapour pressure of a pure liquid A is 70 torr at 300 K. It forms an ideal solution with another liquid B. The mole fraction of B is 0.2 and total vapour pressure of the solution is 84 torr at the same temperature. The vapour pressure of pure liquid B (in torr) is

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Detailed Solution

$x_{A} + x_{B} = 1 x_{A} = 1 - x_{B} x_{A} = 1 - 0.2 = 0.8 p_{A}^{0} = 70 torr, p_{total} = 84 torr$

Using Raoult's Law:

$p_{A} = p_{A}^{0} x_{A} p_{A} = 70 \times 0.2 = 56 torr p_{B} = p_{B}^{0} x_{B} p_{B} = p_{B}^{0} \times 0.2$

Using Dalton's law of partial pressure and substitute the values:

$p_{total} = p_{A} + p_{B} 84 = 56 + 0.2 \times p_{B}^{0} p_{B}^{0} = 140 torr$

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