For the reaction,$CO_{(g)} + Cl_{2(g)} \rightleftharpoons COCl_{2(g)}$,the ratio $K_p/K_c$ is equal to:

For the reaction in equilibrium $N_2O_{4(g)} \rightleftharpoons 2NO_{2(g)}$,the equilibrium concentrations of $N_2O_4$ and $NO_2$ are $4.8 \times 10^{-2} \ mol/L$ and $1.2 \times 10^{-2} \ mol/L$,then $K_C$ is

The ratio $\frac{K_p}{K_C}$ for the reaction: $CO_{(g)} + \frac{1}{2} O_{2(g)} \rightleftharpoons CO_{2(g)}$ is:

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 $,M^2$)

For the reaction,$PCl_{3(g)} + Cl_{2(g)} \rightleftharpoons PCl_{5(g)}$,the value of $K_c$ at $250 \ ^oC$ is $26$. The value of $K_p$ at this temperature will be:

Find $\Delta n_g$ when $1 \text{ mol}$ of each $NH_{3(g)}$ and $HCl_{(g)}$ reacts to form solid $NH_4Cl_{(s)}$.