For the reaction: $Fe_{2}N_{(s)} + \frac{3}{2}H_{2(g)} \rightleftharpoons 2Fe_{(s)} + NH_{3(g)}$,which of the following relations is correct?

For the reactions $N_{2(g)} + O_{2(g)} \rightleftharpoons 2NO_{(g)}$ and $NO_{(g)} \rightleftharpoons 1/2N_{2(g)} + 1/2O_{2(g)}$,the equilibrium constants are $K_1$ and $K_2$ respectively. What is the relationship between $K_1$ and $K_2$?

For $NH_4HS_{(s)} \rightleftharpoons NH_{3_{(g)}} + H_2S_{(g)}$; the observed pressure for the reaction mixture at equilibrium is $1.12 \ atm$ at $106 \ ^oC$. The value of $K_p$ for the reaction is: (in $atm^2$)

For the dissociation reaction $N_2O_{4(g)} \rightleftharpoons 2NO_{2(g)}$,the degree of dissociation $(\alpha)$ in terms of $K_p$ and total equilibrium pressure $P$ is

For the reaction ${H_2}_{(g)} + {I_2}_{(g)} \rightleftharpoons 2HI_{(g)}$ at $721 \ K$,the value of the equilibrium constant $({K_c})$ is $50$. When the equilibrium concentration of both is $0.5 \ M$,the value of ${K_p}$ under the same conditions will be:

For the equilibrium $N_2O_{4(g)} \rightleftharpoons 2NO_{2(g)}$,$K_p$ is equal to $K_c$ when $T = ....... \ K$.