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 ${K_P}$.

Assertion : For reaction $N_{2(g)} + 3H_{2(g)} \rightleftharpoons 2NH_{3(g)}$,the unit of $K_C$ is $L^2 \, mol^{-2}$.
Reason : For the reaction $N_{2(g)} + 3H_{2(g)} \rightleftharpoons 2NH_{3(g)}$,the equilibrium constant $K_C = \frac{[NH_3]^2}{[N_2][H_2]^3}$.

$x A_{(s)} \rightleftharpoons y B_{(g)} + z C_{(g)}$. If $\frac{K_c}{K_p} = (RT)^{-2}$,then which is correct?

For the reaction $2NOCl_{(g)} \rightleftharpoons 2NO_{(g)} + Cl_{2(g)}$,the value of equilibrium constant $K_p$ is $0.033 \ bar$ at $1060 \ K$. Calculate the value of $K_c$.

Value of $K_{p}$ for the equilibrium reaction $N_{2}O_{4(g)} \rightleftharpoons 2NO_{2(g)}$ at $288 \ K$ is $47.9$. The $K_{C}$ for this reaction at same temperature is $......$ (Nearest integer)
$(R=0.083 \ L \ \text{bar} \ K^{-1} \ mol^{-1})$

At $3000 \ K$ the equilibrium pressures of $CO_2$,$CO$ and $O_2$ are $0.6 \ atm$,$0.4 \ atm$ and $0.2 \ atm$ respectively. $K_p$ for the reaction,$2CO_2 \rightleftharpoons 2CO + O_2$ is