For a gaseous reaction $pA + qB \rightleftharpoons qC + pD$,which of the following relationships is true?

One mole of $N_2O_4$ in a $1 \ L$ flask decomposes to attain the equilibrium $N_2O_{4(g)} \rightleftharpoons 2NO_{2(g)}$. At the equilibrium the mole fraction of $NO_2$ is $1/2$. Hence $K_C$ will be:

For the reaction $2NO_{2(g)} \rightleftharpoons 2NO_{(g)} + O_{2(g)}$,$K_c = 1.8 \times 10^{-6}$ at $184 \, ^\circ C$. Given $R = 0.0831 \, kJ/(mol \cdot K)$,when $K_p$ and $K_c$ are compared at $184 \, ^\circ C$,it is found that:

For the reaction $2NOCl_{(g)} \rightleftharpoons 2NO_{(g)} + Cl_{2(g)}$,the value of equilibrium constant $K_p$ is $0.033 \ bar$ at $1060 \ K$. Calculate the value of $K_c$.

In a $500 \ mL$ capacity vessel,$CO$ and $Cl_2$ are mixed to form $COCl_2$. At equilibrium,it contains $0.2 \ mol$ of $COCl_2$ and $0.1 \ mol$ of each of $CO$ and $Cl_2$. The equilibrium constant $K_c$ for the reaction $CO + Cl_2 \rightleftharpoons COCl_2$ is:

If $K_C$ for the equilibrium reaction $2 ABC_{(g)} \rightleftharpoons 2 AB_{(g)} + C_{2(g)}$ is $X$ at $T \ K$,its $K_P$ at the same temperature is: