For the reaction ${N_2}_{(g)} + {O_2}_{(g)} \rightleftharpoons 2NO_{(g)}$,the equilibrium constant ${K_C}$ is $4 \times 10^{-4}$ at temperature $T$. Calculate ${K_P}$.

For the reaction $2NOCl_{(g)} \rightleftharpoons 2NO_{(g)} + Cl_{2_{(g)}}$ at $1060 \ K$,the equilibrium constant $K_p$ is $0.033 \ atm$. Find the value of $K_c$. (Given $R = 0.082 \ L \ atm \ K^{-1} \ mol^{-1}$)

For a reversible reaction $A \rightleftharpoons B$,the pre-exponential factor is the same for both the forward and backward reactions and has a value of $20 \ s^{-1}$. If the enthalpy change for the forward reaction is $-41.5 \ kJ \ mol^{-1}$,the value of the equilibrium constant at $500 \ K$ is:

For the reaction $N_{2(g)} + 3H_{2(g)} \rightleftharpoons 2NH_{3(g)}$,the equilibrium constant $K_p = 41$ at $400 \ K$. Calculate $K_c$ for the following reactions at $400 \ K$:
$(a)$ $2N_{2(g)} + 6H_{2(g)} \rightleftharpoons 4NH_{3(g)}$
$(b)$ $2NH_{3(g)} \rightleftharpoons N_{2(g)} + 3H_{2(g)}$
$(c)$ $\frac{1}{2}N_{2(g)} + \frac{3}{2}H_{2(g)} \rightleftharpoons NH_{3(g)}$

For a reversible reaction,the rate constants for the forward and backward reactions are $2.38 \times 10^{-4}$ and $8.15 \times 10^{-5}$ respectively. The equilibrium constant for the reaction is

$A$ mixture of $1 \ mol$ of $H_2O$ and $1 \ mol$ of $CO$ is taken in a $10 \ L$ container and heated to $725 \ K$. At equilibrium,$40\%$ of water reacts with carbon monoxide according to the equation:
$CO_{(g)} + H_2O_{(g)} \rightleftharpoons CO_{2(g)} + H_{2(g)}$
The equilibrium constant $K_C \times 10^2$ for the reaction is $.......$ (Nearest integer).