Question

For the reaction,
$I _{2}(g) \rightleftharpoons 2 I (g) ; K_{C}=37.6 \times 10^{-6}$
at $1000 \,K$. If $1.0$ mole of $I _{2}$ is introduced into a $1.0 \,L$ flask at $1000 \, K$, at equilibrium

• A. $\left[ I _{2}\right]>[ I ]$
• B. $\left[ I _{2}\right]=[ I ]$
• C. $\left[ I _{2}\right]<[ I ]$
• D. Unpredictable

Answer 1

Answer: (A)

As $K_{C}$ is very low and $K_{C}=\frac{[ I ]^{2}}{\left[ I _{2}\right]}$
For the reaction, $I _{2}(g) \rightleftharpoons 2 I (g)$
$\therefore \left[ I _{2}\right]>[ I ]$