The relationship between $K_{p}$ and $K_{c}$ is $K_{p}=K_{c}(RT)^{\Delta n_{g}}$. What would be the value of $\Delta n_{g}$ for the reaction $NH_{4}Cl_{(s)} \rightleftharpoons NH_{3(g)} + HCl_{(g)}$?

Given below are certain reactions. Identify the reaction for which $K_p = K_c$.

For the reaction $N_2O_{4(g)} \rightleftharpoons 2NO_{2(g)}$,the value of $\frac{K_c}{K_p}$ is:

For the reaction $PCl_{5(g)} \rightleftharpoons PCl_{3(g)} + Cl_{2(g)}$ at equilibrium,the partial pressures of $PCl_5, PCl_3$ and $Cl_2$ are $2 \ atm, 4 \ atm$ and $4 \ atm$ respectively. The value of $K_C$ at $27^{\circ}C$ is (approx):-

The reaction between $N_2$ and $H_2$ to form ammonia has $K_c = 6 \times 10^{-2}$ at the temperature $500 \ ^oC$. The numerical value of $K_p$ for this reaction 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