Liquid $' M'$ and liquid 'N' form an ideal solution. The vapour pressures of pure liquids 'M' and $' N'$ are $450$ and $700 m m H g$ , respectively, at the same temperature. Then correct statement is
$X_{M}$ = Mole fraction of $' M'$ in solution ;
$X_{N}$ = Mole fraction of $' N'$ in solution ;
$Y_{M}$ = Mole fraction of $' M'$ in vapour phase ;
$Y_{N}$ = Mole fraction of $' N'$ in vapour phase)

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$(x_{M} - y_{M}) < (x_{N} - y_{N})$

$\frac{x_{M}}{x_{N}} < \frac{y_{M}}{y_{N}}$

$\frac{x_{M}}{x_{M}} > \frac{y_{M}}{y_{N}}$

$\frac{x_{M}}{x_{N}} = \frac{y_{M}}{y_{N}}$

answer is C.

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Detailed Solution

$\begin{aligned} ∵ P_{N}^{0} > P_{M}^{0} \\ ∴ y_{N} > X_{N} \end{aligned}$

and $X_{M} > y_{M}$

Multiply we get

$y_{N} X_{M} > X_{N} y_{M} .$

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