5 moles each of hydrogen and iodine were heated in a sealed 10 li… - Vidyadip

MCQ

$5\ moles$ each of hydrogen and iodine were heated in a sealed $10\ litre$ vessel. At equilibrium, $2\ moles$ of $HI$ were found. The equilibrium constant for the reaction

${H_2}(g)\, + \,{I_2}(g)\, \rightleftharpoons \,2HI(g)$ is

A
$1$
B
$10$
C
$5$
✓
$0.25$

✓

Answer

Correct option: D.

$0.25$

d
$\mathrm{H}_{2}+\mathrm{I}_{2} \rightleftharpoons 2 \mathrm{HI}$

$\begin{array}{*{20}{l}}
{t = 0}&{ \Rightarrow 5{\text{ mol }}}&{5{\text{ mol }}}&0 \\
{Eq}&{ \Rightarrow (5 - x)}&{(5 - x)}&{2x}
\end{array}$

$\therefore \quad 2 x=2$

$x=1$

$\mathrm{K}_{\mathrm{c}}=\frac{[\mathrm{HI}]^{2}}{\left[\mathrm{H}_{2}\right] \times\left[\mathrm{I}_{2}\right]}$

$=\frac{\left(\frac{2}{10}\right)^{2}}{\left(\frac{4}{10}\right) \times\left(\frac{4}{10}\right)}=0.25$

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