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Characteristics of Equilibrium Constant

3.2 moles of...

Question

$3.2$ moles of $H I (g)$ were heated in a sealed bulb at $444$ till the equilibrium was reached. Its degree of dissociation was found to be $20$ . Calculate the number of moles of hydrogen iodide, hydrogen and iodine present at the equilibrium point and determine the value of equilibrium constant for the reaction $2 H I (g) ⇌ H_{2} (g) + I_{2} (g)$ . Considering the volume of the container $1 L$ .

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Solution

$2 H I ⇌ H_{2} + I_{2}$
At $3.2$ $0$ $0$
$t = 0$
At $3.2 - 2 x$ $2 x$ $2 x$
$t = e q$
$x = 20$ % of $3.2$
$\Rightarrow$ $\frac{1}{5} \times 3.2 = 0.64$
$1.92$ $1.28$ $1.28$
$K_{c} = \frac{1.28 \times 1.28}{{(1.92)}^{2}} = 0.444 = 44 \times 10^{- 2}$
Since volume $1$ lit concentration $=$ moles
$[H I] = 1.92$
$[H_{2}] = 1.28$
$[I_{2}] = 1.28$
$K = 0.444$

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