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

If the degree of dissociation is $\sqrt{0.5}$,what will be the value of $K_p$ for the reaction $N_2O_3 \rightleftharpoons NO + NO_2$ in terms of the total pressure $P$?

For which of the following reactions will ${K_p} > {K_c}$?

For a reaction $2A_{(g)} \rightleftharpoons 2B_{(g)} + C_{(g)}$,$K_c = 3.75 \times 10^{-6}$ at $1069 \ K$. The approximate value of $K_p$ for this reaction at the same temperature is $(R = 0.082 \ L \ bar \ mol^{-1} \ K^{-1})$.

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 equilibrium concentrations of $N_2, H_2$ and $NH_3$ in the formation of $NH_3$ at $500 \ K$ are $1.25 \times 10^{-2} \ M, 4.0 \times 10^{-2} \ M$ and $1.6 \times 10^{-2} \ M$ respectively. The equilibrium constant $K_{p}$ at the same temperature is