Question

In a mixture of $N_2$ and $H_2$ in the ratio of $1:3$ by mole at $64$ atmospheric equilibrium pressure and ${33}^{\circ }C$ the percentage of ammonia under equilibrium is $33.33$ by volume.

Calculate the equilibrium constant of the reaction using the equation.

$N_2\left(g\right)+3H_2\left(g\right)\rightleftharpoons 2N{H}_3\left(g\right).$

• A. $K_p=1.3\times {10}^{-3}at{m}^{-2}$
• B. $K_p=2.4\times {10}^{-3}at{m}^{-2}$
• C. $K_p=2.8\times {10}^{-3}at{m}^{-2}$
• D. $K_p=3.1\times {10}^{-3}at{m}^{-2}$

Answer 1

The correct option is A $K_p=1.3\times {10}^{-3}at{m}^{-2}$