When one mole of $A$ and one mole of $B$ were heated in a one-litre flask at $T \ K$,$0.5 \ mole$ of $C$ was formed at equilibrium for the reaction $A + B \rightleftharpoons C + D$. The equilibrium constant,$K_C$,is:

For the reaction $2AB_{(g)} \rightleftharpoons 2A_{(g)} + B_{2(g)}$; if the initial pressure of $AB$ is $100 \ atm$ and at equilibrium the total pressure becomes $125 \ atm$,the equilibrium constant $(K_p)$ will be:

Find out the value of $K_C$ for the following reaction from the value of $K_P$:
$2NOCl_{(g)} \rightleftharpoons 2NO_{(g)} + Cl_{2(g)}$
Given: $K_P = 8 \times 10^{12} \ atm$ at $500 \ K$,use $R = 0.08 \ L \ atm \ mol^{-1} \ K^{-1}$.

For the reaction $SO_{2(g)} + \frac{1}{2}O_{2(g)} \rightleftharpoons SO_{3(g)}$,the relationship is given by $K_P = K_C(RT)^x$. Find the value of $x$.

The reaction for which $K_{c} = 2.3 \times 10^3 \ mol \ L^{-1}$ is $-$

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 ....... $M^{-1}$.