$1.1 \ mol$ of $A$ and $2.2 \ mol$ of $B$ are mixed in a $1 \ L$ flask until equilibrium is reached. At equilibrium,$0.2 \ mol$ of $C$ is formed. If the equilibrium reaction is $A + 2B \rightleftharpoons 2C + D$,the value of the equilibrium constant $K_C$ is:

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

For the reaction $2NOCl_{(g)} \rightleftharpoons 2NO_{(g)} + Cl_{2_{(g)}}$ at $1060 \ K$,the equilibrium constant $K_p$ is $0.033 \ atm$. Find the value of $K_c$. (Given $R = 0.082 \ L \ atm \ K^{-1} \ mol^{-1}$)

If equilibrium constants of the reaction,$N_2 + O_2 \rightleftharpoons 2NO$ is $K_1$ and $\frac{1}{2}N_2 + \frac{1}{2}O_2 \rightleftharpoons NO$ is $K_2$,then:

Which among the following denotes the correct relationship between $K_{p}$ and $K_{c}$ for the reaction $2A_{(g)} \rightleftharpoons B_{(g)} + C_{(g)}$?

$4.0 \, mol$ of argon and $5.0 \, mol$ of $PCl_5$ are introduced into an evacuated flask of $100 \, L$ capacity at $610 \, K$. The system is allowed to equilibrate. At equilibrium,the total pressure of the mixture was found to be $6.0 \, atm$. The $K_p$ for the reaction is ...... [Given: $R = 0.082 \, L \, atm \, K^{-1} \, mol^{-1}$]