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$2 \mathrm{HI}(\mathrm{g}) \rightleftharpoons \mathrm{H}_{2}(\mathrm{~g})+\mathrm{I}_{2}(\mathrm{~g})$
The equilibrium constant of the above reaction is $6.4$ at $300 \mathrm{~K}$. If $0.25$ mole each of $\mathrm{H}_{2}$ and $\mathrm{I}_{2}$ are added to the system, the equilibrium constant will be
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The equilibrium constant of the above reaction is $6.4$ at $300 \mathrm{~K}$. If $0.25$ mole each of $\mathrm{H}_{2}$ and $\mathrm{I}_{2}$ are added to the system, the equilibrium constant will be
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Verified Answer
The correct answer is:
$6.4$
The value of equilibrium constant remains constant for a given reaction at constant temperature.
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