Q. The formation of phosgene is represented as,
$CO+Cl_{2}\rightleftharpoonsCOCl_{2}$
The reaction is carried out in $500mL$ flask. At equilibrium $0.3$ mole of phosgene, $0.1$ mole of $CO$ and $0.1$ mole of $Cl_{2}$ are present. The equilibrium constant of the reaction is :

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$30$

$15$

$5$

$3$

Solution:

$CO+Cl_{2}\rightleftharpoonsCOCl_{2}$
$\left[CO\right]=\frac{0 . 1}{0 . 5}$
$\left[Cl_{2}\right]=\frac{0 . 1}{0 . 5}\left[COCl_{2}\right]=\frac{0 . 3}{0 . 5}$
$\therefore K_{C}=\frac{0 . 3 / 0 . 5}{\frac{0 . 1}{0 . 5} \times \frac{0 . 1}{0 . 5}}=15$

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