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 $K_c$.

For which of the following reactions is $K_c \leq K_p$ at $298 \ K$?

For the reaction $A_{(g)} \rightleftharpoons B_{(g)}$ at $495 \ K$,$\Delta_{r}G^{\circ} = -9.478 \ kJ \ mol^{-1}$. If we start the reaction in a closed container at $495 \ K$ with $22 \ mmol$ of $A$,the amount of $B$ in the equilibrium mixture is $x \ mmol$. Find $x$ (Round off to the nearest integer). $[R = 8.314 \ J \ mol^{-1} \ K^{-1}; \ln 10 = 2.303]$

For the reaction $SO_{3(g)} \rightleftharpoons SO_{2(g)} + \frac{1}{2}O_{2(g)}$,the equilibrium constant $K_C = 4.9 \times 10^{-2}$. Calculate the $K_C$ for the reaction $2SO_{2(g)} + O_{2(g)} \rightleftharpoons 2SO_{3(g)}$.

At $717 \ K$,$1.50 \ mol$ each of hydrogen and iodine are placed in a $10 \ L$ closed vessel. At equilibrium,$1.25 \ mol$ of each hydrogen and iodine remain. The value of the equilibrium constant $K_c$ for the reaction $H_2(g) + I_2(g) \rightleftharpoons 2HI(g)$ at $717 \ K$ is .......

For the reaction $A + B \rightleftharpoons C + D$ at $298 \ K$,the equilibrium constant is $10.0$. If the initial concentration of all four species is $1 \ M$,what will be the equilibrium concentration of $D$ (in $mol \ L^{-1}$)?