Chemistry - Liquid Solution Question with Solution | TestHub

ChemistryLiquid SolutionRaoult's LawMedium2 minQB

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Passage / Comprehension

The vapour pressure of two pure liquids, A and B that form an ideal solution are 300 and 800 torr respectively, at temperature T. A mixture of the vapour of A and B for which the mole fraction of A is 0.25 is slowly compressed at temperature T.

The pressure at which last traces of vapours remains, is :

Options:

Answer:

Solution:

Given vapor composition:

$y_{A} = 0.25$ , $y_{B} = 0.75$

For the last traces of vapor remaining, the liquid composition becomes equal to the initial vapor composition (bubble point condition).

Using Raoult's law:

$P = x_{A} P_{A}^{0} + x_{B} P_{B}^{0}$

Here:

$x_{A} = 0.25$ , $x_{B} = 0.75$

$P = 0.25 (300) + 0.75 (800)$

$P = 75 + 600 = 675 t orr$

Therefore, the pressure at which the last traces of vapor remain is $675 t orr$ .

Stream:JEESubject:ChemistryTopic:Liquid SolutionSubtopic:Raoult's Law

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