At $450 \, K$,$K_{p} = 2.0 \times 10^{10} \, bar^{-1}$ for the given reaction at equilibrium.
$2 \, SO_{2(g)} + O_{2(g)} \longleftrightarrow 2 \, SO_{3(g)}$
What is $K_{c}$ at this temperature?

$K_p$ for the following reaction is $3.0$ at $1000 \ K$.
$CO_{2(g)} + C_{(s)} \rightleftharpoons 2CO_{(g)}$
What will be the value of $K_c$ for the reaction at the same temperature?
(Given: $R = 0.083 \ L \ bar \ K^{-1} \ mol^{-1}$)

$A$ mixture of $0.3 \ mol$ of $H_2$ and $0.3 \ mol$ of $I_2$ is allowed to react in a $10 \ L$ evacuated flask at $500 \ ^oC$. The reaction is $H_2 + I_2 \rightleftharpoons 2HI$,and the equilibrium constant $K_c$ is found to be $64$. The amount of unreacted $I_2$ at equilibrium is $...... \ mol$.

$A$ homogeneous ideal gaseous reaction $AB_{2(g)} \rightleftharpoons A_{(g)} + 2B_{(g)}$ is carried out in a $25 \ L$ flask at $27^{\circ}C$. The initial amount of $AB_{2}$ was $1 \ mole$ and the equilibrium pressure was $1.9 \ atm$. The value of $K_{P}$ is $x \times 10^{-2}$. The value of $x$ is $...$ (Integer answer)

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

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