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For a solution formed by mixing liquids $L$ and $M$, the vapour pressure of $L$ plotted against the mole fraction of $M$ in solution is shown in the following figure. Here $x_{L}$ and $x_M$ represent mole fractions of $L$ and $M$, respectively, in the solution. The correct statement(s) applicable to this system is(are)
(image)
$[A]$ Attractive intermolecular interactions between $L-L$ in pure liquid $L$ and $M-M$ in pure liquid $M$ are stronger than those between $L-M$ when mixed in solution
$[B]$ The point $Z$ represents vapour pressure of pure liquid $M$ and Raoult's law is obeyed when $x_{L} \rightarrow 0$
$[C]$ The point $Z$ represents vapour pressure of pure liquid $L$ and Raoult's law is obeyed when $x_{\mathrm{L}} \rightarrow 1$
$[D]$ The point $Z$ represents vapour pressure of pure liquid $M$ and Raoult's law is obeyed from $x_{L}=0$ to $x_{L}=1$
$A,C$
$A,B$
$A,D$
$A,C,D$
Solution
From graph it is clear that there is +ve deviation $w.r.t L$. Therefore option $\mathrm{A}$ is correct. When $\mathrm{x}_{\mathrm{L}} \rightarrow 1$, then $\mathrm{Z}$ will have value equal to $\mathrm{P}_{\mathrm{L}}^0$ (vapour pressure of pure $\mathrm{L}$ ). Therefore option $\mathrm{C}$ is also correct.
