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2 moles of a volatile liquid (A) and 3 moles of another volatile liquid (B) are present in a solution at 25°C temperature in a closed container if vapor pressure of pure A and pure B at 25°C are $P_{A}^{0} = 300 t orr$ and $P_{B}^{0} = 200 t orr$ , respectively (the above solution follows Raoult's law of partial vapor pressure).

Which of the following is incorrect?

Options:

Answer:

A

Solution:

Question Explanation: Select the incorrect statement.

Concept: This question is based on non-ideal solutions.

Solution: The above solution is ideal and cannot form an azeotropic mixture. Therefore, it can be separated by fractional distillation.

$P_{T} = P_{A}^{0} X_{A} + P_{B}^{0} X_{B} = 300 \times \frac{2}{5} + 200 \times \frac{3}{5} = \frac{1200}{5} = 240 t orr$

$\frac{Y _{A}}{Y _{B}} = \frac{P _{A}^{0} X _{A}}{P _{B}^{0} X _{B}} = \frac{300 \times 2}{200 \times 3} = \frac{1}{1}$

$Y_{A} = 0.5 an d Y_{B} = 0.5$

Final Answer: The correct option is (A).

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

⏱ 2mℹ️ Source: QB

Chemistry - Liquid Solution Question with Solution | TestHub

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