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A solution of A and B with 30 mol % A...

A solution of A and B with 30 mol % A is in equilibrium with its vapour which contains 40 mol% % B. Assuming that the solution and the vapour behave ideally, calculate the ratio of vapour pressure of pure A and pure B.

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To solve the problem, we need to calculate the ratio of the vapor pressures of pure components A and B given the composition of the solution and the vapor phase. Here’s a step-by-step solution: ### Step 1: Determine the mole fractions in the solution Given that the solution contains 30 mol% A, we can find the mole fraction of A (χA) and B (χB) in the solution. \[ \chi_A = 0.30 \quad \text{(30 mol% A)} \] ...
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Knowledge Check

  • A solution of A and B with 30 mole percent of A is in equilibrium with its vapour which contains 60 mole percent of A. Assuming that the solution and the vapour behave ideally, the ratio of the vapour pressures of pure A and pure B is

    A
    1.5
    B
    2.5
    C
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    D
    4.5

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    A
    1.5
    B
    2.5
    C
    3.5
    D
    4.5

  • A mixture of two miscible liquids A and B is distilled under equilibrium conditions at 1 atm pressure. The mole fraction of A in solution and vapour phase are 0.30 and 0.60 respectively. Assuming ideal behaviour of the solution and the vapour, calculate the ratio of the vapour pressure of pure A to that of pure B.

    A
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