$NH_4HS_{(s)} \rightleftharpoons NH_{3(g)} + H_2S_{(g)}$
The reaction was started with some amount of $NH_4HS$. The equilibrium pressure at $25^{\circ}C$ is $0.5 \ atm$. What is $K_p$ for the reaction (in $atm^2$)?

For the reaction $N_{2(g)} + O_{2(g)} \rightleftharpoons 2NO_{(g)}$,the value of $K_c$ at $800 \ ^oC$ is $0.1$. When the equilibrium concentrations of both the reactants are $0.5 \ M$,what is the value of $K_p$ at the same temperature?

For the reaction $N_{2(g)} + O_{2(g)} \rightleftharpoons 2NO_{(g)}$,the equilibrium constant at temperature $T$ is $4 \times 10^{-4}$. Find the value of $K_c$ for the reaction $NO_{(g)} \rightleftharpoons \frac{1}{2} N_{2(g)} + \frac{1}{2} O_{2(g)}$.

For the reaction $2AB_{(g)} \rightleftharpoons 2A_{(g)} + B_{2(g)}$; if the initial pressure of $AB$ is $100 \ atm$ and at equilibrium the total pressure becomes $125 \ atm$,the equilibrium constant $(K_p)$ will be:

At $298 \, K$,for which of the following reactions will the value of $\frac{K_p}{K_c}$ be maximum and minimum,respectively?
$(a) N_2O_4 \rightleftharpoons 2NO_2$
$(b) 2SO_2 + O_2 \rightleftharpoons 2SO_3$
$(c) X + Y \rightleftharpoons 4Z$
$(d) A + 3B \rightleftharpoons 7C$

For the reaction $C_{(s)} + CO_{2_{(g)}} \rightleftharpoons 2CO_{(g)}$,the partial pressure of $CO_2$ and $CO$ at equilibrium are $4 \ atm$ and $8 \ atm$ respectively. $K_p$ for the reaction is