Question

The equilibrium constants of the following are
$N_2+3H_2\rightleftharpoons 2N{H}_3;K_1$
$N_2+O_2\rightleftharpoons 2NO;K_2$

$H_2+\frac{1}{2}{O}_2\rightleftharpoons H_{2}O;K_3$
The equilibrium constant (K) of the reaction:
$2N{H}_3+\frac{5}{2}{O}_2\stackrel{K}{\rightleftharpoons }2NO+3H_{2}O$ will be

• A. $K_2{K}_3^3/K_1$
• B. $K_2{K}_3/K_1$
• C. $K_2^3{K}_3/K_1$
• D. $K_1{K}_3^3/K_2$

Answer 1

The correct option is A $K_2{K}_3^3/K_1$

From the given equation,
$2N{H}_3\rightleftharpoons N_2+3H_2;\frac{1}{K_1}$ ...(i)
$N_2+O_2\rightleftharpoons 2NO;K_2$ ...(ii)
$3H_2+\frac{3}{2}{O}_2\to 3H_{2}O;K_3^3$ ...(iii)
By adding equations (i), (ii) and (iii), we get
$2N{H}_3+\frac{5}{2}{O}_2\stackrel{K}{\rightleftharpoons }2NO+3H_{2}O,K=\frac{K_2{K}_3^3}{K_1}$