Vapour pressure of chloroform $({CHCl}_{3})$ and dichloromethane $({CH}_{2} {Cl}_{2})$
at 25°C are 200mm Hg and 41.5mm Hg respectively. Vapour pressure of
the solution obtained by mixing 25.5g of ${CHCl}_{3}$ and 40g of at the ${CH}_{2} {Cl}_{2}$
same temperature will be (Molecular mass of ${CHCl}_{3} = 119.5 u$ and molecular
mass of ${CH}_{2} {Cl}_{2} = 85 u)$

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90.92 mm Hg

615.0 mm Hg

347.9 mm Hg

285.5 mm Hg

answer is A.

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Detailed Solution

$\begin{array}{l} n_{{CHCl}_{3}} = \frac{25.5}{119.5} = 0.213 \\ n_{{CH}_{2} {Cl}_{2}} = \frac{40}{85} = 0.47 \\ P_{T} = P_{A}^{\circ} X_{A} + P_{B}^{\circ} X_{B} \\ = 200 \times \frac{0.213}{0.683} + 41.5 \times \frac{0.47}{0.683} \\ = 62.37 + 28.55 = 90.92 \end{array}$