The equilibrium constant for the reaction $N_{2(g)} + O_{2(g)} \rightleftharpoons 2NO_{(g)}$ at temperature $T$ is $4 \times 10^{-4}$. The value of $K_c$ for the reaction $NO_{(g)} \rightleftharpoons \frac{1}{2}N_{2(g)} + \frac{1}{2}O_{2(g)}$ at the same temperature is

The equilibrium constant for the reaction $SO_{3(g)} \rightleftharpoons SO_{2(g)} + \frac{1}{2} O_{2(g)}$ is $K_c = 4.9 \times 10^{-2}$. The value of $K_c$ for the reaction $2SO_{2(g)} + O_{2(g)} \rightleftharpoons 2SO_{3(g)}$ will be

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)
$(R=0.083 \ L \ \text{bar} \ K^{-1} \ mol^{-1})$

$(1) \ N_{2(g)} + 3H_{2(g)} \rightleftharpoons 2NH_{3(g)} \ ; \ K_1$
$(2) \ N_{2(g)} + O_{2(g)} \rightleftharpoons 2NO_{(g)} \ ; \ K_2$
$(3) \ H_{2(g)} + \frac{1}{2}O_{2(g)} \rightleftharpoons H_2O_{(g)} \ ; \ K_3$
The equation for the equilibrium constant of the reaction
$2NH_{3(g)} + \frac{5}{2}O_{2(g)} \rightleftharpoons 2NO_{(g)} + 3H_2O_{(g)}$
$(K_4)$ in terms of $K_1$,$K_2$,and $K_3$ is

For the reversible reaction $A + B \rightleftharpoons C + D$,the equilibrium concentrations of $C$ and $D$ are $0.8 \ mol/L$ each. If the initial concentrations of $A$ and $B$ were $1 \ mol/L$ each,calculate the equilibrium constant $K_c$.

$K_p$ for the following reaction is $3.0$ at $1000 \ K$.
$CO_{2(g)} + C_{(s)} \rightleftharpoons 2CO_{(g)}$
What will be the value of $K_c$ for the reaction at the same temperature?
(Given: $R = 0.083 \ L \ bar \ K^{-1} \ mol^{-1}$)