$K_{c}$ for the reaction,$A_{2(g)} \rightleftarrows B_{2(g)}$ is $99.0$. In a $1 \ L$ closed flask,two moles of $B_{2(g)}$ are heated to $T(K)$. What is the concentration of $B_{2(g)}$ (in $mol \ L^{-1}$) at equilibrium?

At $T(K)$,$K_{c}$ value for $AO_{2(g)} + BO_{2(g)} \rightleftharpoons AO_{3(g)} + BO_{(g)}$ is $16$. In a closed $1 \ L$ flask,one mole each of $AO_2, BO_2, AO_3$ and $BO$ are taken and heated to $T(K)$. What is the concentration (in $mol \ L^{-1}$) of $AO_3$ at equilibrium?

For which of the following reactions is the relation $\log \frac{K_P}{K_C} + \log RT = 0$ correct?

Find the value of $\frac{P}{K_p}$ for the reaction at a certain temperature: $2NOBr_{(g)} \rightleftharpoons 2NO_{(g)} + Br_{2(g)}$,where $P$ is the total pressure of gases at equilibrium and $P_{Br_2} = \frac{P}{9}$.

For the reaction $N_{2(g)} + O_{2(g)} \rightleftharpoons 2NO_{(g)}$,the value of $K_c$ at $800 \ ^oC$ is $0.1$. When the equilibrium concentrations of both the reactants are $0.5 \ M$,what is the value of $K_p$ at the same temperature?

For the dissociation reaction $N_2O_{4(g)} \rightleftharpoons 2NO_{2(g)}$,the degree of dissociation $(\alpha)$ in terms of $K_p$ and total equilibrium pressure $P$ is