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

Some solid $NH_4HS$ is placed in a flask containing $0.5 \ atm$ of $NH_3$. What would be the partial pressures of $NH_3$ and $H_2S$ when equilibrium is reached for the reaction $NH_4HS_{(s)} \rightleftharpoons NH_{3_{(g)}} + H_2S_{(g)}$,given $K_p = 0.11$?

$8 \ mol$ of $AB_3$ is taken in a $1.0 \ dm^3$ container. It dissociates according to the reaction $2AB_{3(g)} \rightleftharpoons A_{2(g)} + 3B_{2(g)}$. If $2 \ mol$ of $A_2$ are present at equilibrium,the equilibrium constant $K_c$ of the reaction is ....... $mol^2 \ L^{-2}$.

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

$A$ schematic plot of $\ln K_{eq}$ versus inverse of temperature $(1/T)$ for a reaction is shown below. The reaction must be

For the reaction $2NOBr_{(g)} \rightleftharpoons 2NO_{(g)} + Br_{2(g)}$,if $P_{Br_2} = \frac{P}{9}$ at equilibrium and $P$ is the total pressure,find the value of $\frac{K_P}{P}$.