For the reaction $A_{(g)} + 2B_{(g)} \rightleftharpoons 2C_{(g)}$,$1 \ mol$ of $A$ and $1.5 \ mol$ of $B$ are taken in a $2 \ L$ vessel. If the concentration of $C$ at equilibrium is $0.35 \ M$,then the equilibrium constant $K_c$ of the reaction will be ....... $M^{-1}$.

One mole of $PCl_5$ is heated in a closed container of $1 \ L$ capacity. At equilibrium,$20\%$ of $PCl_5$ is not dissociated. What should be the value of $K_C$?

For the reaction,$PCl_{3(g)} + Cl_{2(g)} \rightleftharpoons PCl_{5(g)}$,the value of $K_c$ at $250 \ ^oC$ is $26$. The value of $K_p$ at this temperature will be:

For the decomposition reaction $N_2O_4 \rightleftharpoons 2NO_2$ at constant temperature,the equilibrium constant is given by $K_p = \frac{4x^2P}{1 - x^2}$,where $P$ is the total pressure and $x$ is the degree of dissociation. Which of the following statements is correct?

At $-20^{\circ} C$ and $1 \ atm$ pressure,a cylinder is filled with equal number of $H_2$,$I_2$ and $HI$ molecules for the reaction $H_{2(g)} + I_{2(g)} \rightleftharpoons 2 HI_{(g)}$. The $K_p$ for the process is $x \times 10^{-1}$. Find the value of $x$. [Given: $R = 0.082 \ L \ atm \ K^{-1} \ mol^{-1}$]

The equilibrium constant for the reversible reaction,$N_2 + 3H_2 \rightleftharpoons 2NH_3$ is $K$ and for the reaction $\frac{1}{2}N_2 + \frac{3}{2}H_2 \rightleftharpoons NH_3$ the equilibrium constant is $K'$. $K$ and $K'$ will be related as