When the reaction $A+2 B \rightleftharpoons 2 C+D$ was studied, it was observed that the initial…
When the reaction $A+2 B \rightleftharpoons 2 C+D$ was studied, it was observed that the initial concentration of $B$ was 1.5 times that of $A$, and the equilibrium concentrations of $A$ and $C$ were equal. Then $K_C$ for the given equilibrium is equal to
Given, $[A]=[C]$
$a-x=2 x$
$\therefore \quad x=a / 3$
Now, $K_C=\frac{[C]^2[D]}{[A][B]^2}=\frac{\left(\frac{2 a}{3}\right)^2 \times \frac{a}{3}}{\left(a-\frac{a}{3}\right)\left(\frac{3 a}{2}-\frac{2 a}{3}\right)^2}$
$\therefore \quad K_C=0.3$