At a certain temperature,only $50\%$ $HI$ is dissociated into $H_2$ and $I_2$ at equilibrium. The equilibrium constant is:

For the reversible reaction in equilibrium:
$N_{2(g)} + O_{2(g)} \underset{k_2}{\overset{k_1}{\longleftrightarrow}} 2NO_{(g)}$
Given $C_0 = C e^{-2.1 \times 10^{-3}t}$ for the forward reaction and $C'_0 = C' e^{-4.2 \times 10^{-4}t}$ for the backward reaction,calculate the equilibrium constant $K_c$ for the above reaction.

For the reaction in equilibrium
$2NOBr_{(g)} \rightleftharpoons 2NO_{(g)} + Br_{2(g)}$
if $P_{Br_2}$ is $\frac{P}{9}$ at equilibrium and $P$ is the total pressure,then calculate $\frac{P}{K_P}$.

For which of the following reactions is $K_p = K_c$?

For which of the following reactions is the relation $\frac{K_p}{K_c} + \log(RT) = 0$ correct?

The relationship between $K_{p}$ and $K_{c}$ is $K_{p}=K_{c}(RT)^{\Delta n_{g}}$. What would be the value of $\Delta n_{g}$ for the reaction $NH_{4}Cl_{(s)} \rightleftharpoons NH_{3(g)} + HCl_{(g)}$?