229, $\mathrm{At} T(\mathrm{~K}), K_C$ value for the reaction, $\frac{1}{3} \mathrm{~N}_2(g)+\mathrm{H}_2(g) \rightleftharpoons \frac{2}{3} \mathrm{NH}_3(g)$ is 50 . The $K_C$ value for the reaction, $2 \mathrm{NH}_3(g) \rightleftharpoons \mathrm{N}_2(g)+3 \mathrm{H}_2(g)$ at the same temperature is

At $T(\mathrm{~K})$ when one mol of $X$ and one mol of $Y$ are heated in a 1 L flask, 0.5 moles of $Z$ is formed at the equilibrium. The $K_C$ value of the reaction is

$$ X(g)+Y(g) \rightleftharpoons Z(g)+A(g) $$

At 780 K and 10 atmosphere pressure the equilibrium constant for the reaction $2 A(g) \rightleftharpoons B(g)+C(g)$ is 3.52 . At the same temperature and 7.04 atmosphere pressure, the equilibrium constant for the same reaction is

Calculate the value of the equilibrium constant $\left(K_p\right)$ for the reaction of oxygen gas oxidising ammonia gas to nitric oxide and water vapour. The pressure of each gas at equilibrium is 0.5 atm .