In which one of the following gaseous equilibria is $K_p$ less than $K_c$?

For the reaction $N_{2(g)} + 3H_{2(g)} \rightleftharpoons 2NH_{3(g)}$,the value of $K_p = 41$ at $400 \ K$. Find out the value of $K_p$ for the following reaction at the same temperature: $2N_{2(g)} + 6H_{2(g)} \rightleftharpoons 4NH_{3(g)}$

If the degree of dissociation is $\sqrt{0.5}$,what will be the value of $K_p$ for the reaction $N_2O_3 \rightleftharpoons NO + NO_2$ in terms of the total pressure $P$?

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

Find $\Delta n_g$ when $1 \text{ mol}$ of each $NH_{3(g)}$ and $HCl_{(g)}$ reacts to form solid $NH_4Cl_{(s)}$.

For the reaction $A_{(g)} \rightleftharpoons B_{(g)}$ at $495 \ K$,$\Delta_{r}G^{\circ} = -9.478 \ kJ \ mol^{-1}$. If we start the reaction in a closed container at $495 \ K$ with $22 \ mmol$ of $A$,the amount of $B$ in the equilibrium mixture is $x \ mmol$. Find $x$ (Round off to the nearest integer). $[R = 8.314 \ J \ mol^{-1} \ K^{-1}; \ln 10 = 2.303]$