For which of the following reactions is $K_p = K_c$?

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 $atm^2$)

At $800 \ K$ in a closed vessel,the molar concentrations of $N_2, O_2$ and $NO$ at equilibrium are $3.2 \times 10^{-3} \ M, 4.2 \times 10^{-3} \ M$ and $2.8 \times 10^{-3} \ M$ respectively. The approximate values of $K_{c}$ and $\frac{1}{K_{c}}$ for the following reaction are respectively: $N_{2(g)} + O_{2(g)} \rightleftharpoons 2 NO_{(g)}$

What is the value of the equilibrium constant $K_p$ for the reaction ${H_2O_{(l)}} \rightleftharpoons {H_2O_{(g)}}$ at $60^{\circ}C$? (The vapor pressure of water at $60^{\circ}C$ is $0.185 \ bar$.)

Calculate $K_{C}$ for the reversible process given below if $K_{P}=167$ and $T=800^{\circ}C$.
$CaCO_{3(s)} \rightleftharpoons CaO_{(s)} + CO_{2(g)}$

For the formation of ammonia gas from its constituent elements,the $K_{P} / K_{C}$ is