In the reaction, H_2 + I_2 2HI. In a 2 litre flask 0.4 moles of e… - Vidyadip

MCQ

In the reaction, ${H_2} + {I_2}$ $\rightleftharpoons$ $2HI$. In a $2$ litre flask $0.4$ moles of each ${H_2}$ and ${I_2}$ are taken. At equilibrium $0.5$ moles of $HI$ are formed. What will be the value of equilibrium constant, ${K_c}$

A
$20.2$
B
$25.4$
C
$0.284$
✓
$11.1$

✓

Answer

Correct option: D.

$11.1$

(d) $\mathop {\mathop {{H_2}}\limits_{0.4} }\limits_{0.4 - 0.25\; = \;0.15} $$ + $ $\mathop {\mathop {{I_2}}\limits_{0.4} }\limits_{0.4 - 0.25\; = \;0.15/2} $ $ \rightleftharpoons $ $\mathop {\mathop {2HI\,\,\,\,}\limits_{0.50\,\,\,\,} }\limits_{0.50/2} $

${K_c} = \frac{{{{[HI]}^2}}}{{[{H_2}][{I_2}]}} = \frac{{{{\left[ {\frac{{0.5}}{2}} \right]}^2}}}{{\left[ {\frac{{0.15}}{2}} \right]\,\left[ {\frac{{0.15}}{2}} \right]}}$$ = \frac{{0.5 \times 0.5}}{{0.15 \times 0.15}} = 11.11$

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