For the reaction $SO_2 + \frac{1}{2} O_2 \rightleftharpoons SO_3$, if we write $K_p = K_c(RT)^x$, then $x$ becomes

$K_{c}$ 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?

$18.4 \ g$ of $N_2O_4$ was placed in a $1 \ L$ vessel at $400 \ K$ and allowed to attain the following equilibrium: $N_2O_{4(g)} \rightleftharpoons 2NO_{2(g)}$. If the total pressure at equilibrium was $10.64 \ bar$,the approximate $K_p$ is (Given: $R = 0.083 \ L \ bar \ K^{-1} \ mol^{-1}$,assume $N_2O_4$ and $NO_2$ behave as ideal gases).

For the equilibrium system $A_{(s)} \rightleftharpoons 2B_{(g)} + 3C_{(g)}$,if the concentration of $C$ is doubled at equilibrium,then the concentration of $B$ at equilibrium will become ...

When $2 \, mol$ of $PCl_5$ is heated in a closed vessel of $2 \, L$ capacity,$40\%$ of $PCl_5$ dissociates into $PCl_3$ and $Cl_2$ at equilibrium. The value of the equilibrium constant $K_c$ will be:

For the formation of ammonia gas from its constituent elements,the $K_{P} / K_{C}$ is