If ${K_c}$ is the equilibrium constant for the formation of $NH_3$,the dissociation constant of ammonia under the same temperature will be

Value of $K_p$ in the reaction $MgCO_{3(s)} \rightleftharpoons MgO_{(s)} + CO_{2(g)}$ is

At $1000 \ K$,the value of $K_c$ for the reaction $A_{(g)} \rightleftharpoons B_{(g)} + C_{(g)}$ is $10 \ mol \ L^{-1}$. The value of $K_p$ (in $atm$) is: (Given $R = 0.082 \ L \ atm \ K^{-1} \ mol^{-1}$)

Two gaseous equilibria $SO_{2(g)} + \frac{1}{2}O_{2(g)} \rightleftharpoons SO_{3(g)}$ and $2SO_{3(g)} \rightleftharpoons 2SO_{2(g)} + O_{2(g)}$ have equilibrium constants $K_1$ and $K_2$ respectively at $298 \ K$. Which of the following relationships between $K_1$ and $K_2$ is correct?

For the following gaseous reaction $H_2(g) + I_2(g) \rightleftharpoons 2HI(g)$,the equilibrium constant relationship is:

The value of equilibrium constant of the reaction $HI_{(g)} \rightleftharpoons \frac{1}{2} H_{2_{(g)}} + \frac{1}{2} I_{2_{(g)}}$ is $8.0$. The equilibrium constant of the reaction $H_{2_{(g)}} + I_{2_{(g)}} \rightleftharpoons 2HI_{(g)}$ will be