The equilibrium $NH_4HS_{(s)} \rightleftharpoons NH_{3(g)} + H_2S_{(g)}$ is set up at $127 \,^oC$ in a closed vessel. The total pressure at equilibrium was $20 \,atm$. The $K_C$ for the reaction is: (in $,M^2$)

The value of $K_P / K_C$ for the reaction at $T(K)$ is:
$CO_{(g)} + \frac{1}{2} O_{2(g)} \rightleftharpoons CO_{2(g)}$

If equilibrium constants of the reaction,$N_2 + O_2 \rightleftharpoons 2NO$ is $K_1$ and $\frac{1}{2}N_2 + \frac{1}{2}O_2 \rightleftharpoons NO$ is $K_2$,then:

$K_{p} = 0.04 \ atm$ at $899 \ K$ for the equilibrium shown below. What is the equilibrium pressure of $C_{2}H_{6}$ when it is placed in a flask at $4.0 \ atm$ pressure and allowed to come to equilibrium?
$C_{2}H_{6(g)} \longleftrightarrow C_{2}H_{4(g)} + H_{2(g)}$

At $298 \ K$,the value of $K_p$ for $N_2O_{4(g)} \rightleftharpoons 2NO_{2(g)}$ is $0.113 \ atm$. The partial pressure of $N_2O_4$ at equilibrium is $0.2 \ atm$. What is the partial pressure (in $atm$) of $NO_2$ at equilibrium?

The degree of dissociation of $PCl_{5(g)}$ at $16.8 \ bar$ and $127 \ ^oC$ is $0.4$. The value of $K_p$ for the reaction $PCl_{5(g)} \rightleftharpoons PCl_{3(g)} + Cl_{2(g)}$ is