For the reaction $NH_4COONH_2(s) \rightleftharpoons 2NH_3(g) + CO_2(g)$,the equilibrium pressure is $3 \ atm$. Calculate $K_p$.

In a chemical equilibrium,the rate constant of the backward reaction is $7.5 \times 10^{-4}$ and the equilibrium constant is $1.5$. The rate constant of the forward reaction is:

At $298 \ K$,the value of $K_c$ for the following reaction is $x \ mol \ L^{-1}$. What is the approximate $K_p$ value for this reaction? $(R=0.082 \ L \ atm \ mol^{-1} \ K^{-1})$ $A_2O_{4(g)} \rightleftharpoons 2AO_{2(g)}$

For the equilibrium $SO_2Cl_{2(g)} \rightleftharpoons SO_{2(g)} + Cl_{2(g)}$,what is the temperature at which $\frac{K_p}{K_c} = \frac{1}{3}$? (Given $R = 0.0821 \ L \ atm \ K^{-1} \ mol^{-1}$)

For the reaction ${N_{2(g)}} + {O_{2(g)}} \rightleftharpoons 2NO_{(g)}$,the value of $K_c$ at $400 \ K$ is $4.0 \times 10^{-6}$. The value of $K_p$ for this reaction is .....

The equilibrium constant $K_p$ for the following reaction at $191\,^{\circ}C$ is $1.24$. What is the value of $K_c$? $B_{(s)} + \frac{3}{2}F_{2(g)} \rightleftharpoons BF_{3(g)}$