Question

For the reaction $I_2\left(g\right)\rightleftharpoons 2I\left(g\right)$, $K_c=37.6\times {10}^4$ at $1000K$. If $1$ mole of $I_2$ is introduced into a $1$ litre flask at $1000K$. at equilibrium

• A. $\left[I_2\right]>\left[I\right]$
• B. $\left[I_2\right]=\left[I\right]$
• C. $\left[I_2\right]<\left[I\right]$
• D. unpredictable

Answer 1

The correct option is C $\left[I_2\right]<\left[I\right]$

given

$K_c=37.6\times {10}^4$

$K_c=\frac{{\mu }_f}{{\mu }_b}=37.6\times {10}^4$

${\mu }_f$ - rate of forward reaction

${\mu }_b$ - rate of backward reaction

${\mu }_b=\frac{{\mu }_f}{37.6\times {10}^4}$

so, here the rate of forwarding reaction is greater than the rate of backward reaction that means the concentration product is greater than the concentration of the reactant.

$I_2\left(g\right)\rightleftharpoons 2I\left(g\right)$

Hence, option(c) is the correct answer.