$A + B \rightleftharpoons C + D$. If the final equilibrium concentrations of $A$ and $B$ are equal,and the equilibrium concentration of $D$ is twice that of $A$,what is the equilibrium constant $(K_c)$ of the reaction?

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

The equilibrium constant $(K_p)$ for the formation of ammonia from its constituent elements at $27^{\circ} C$ is $1.2 \times 10^{-4}$ and at $127^{\circ} C$ is $0.60 \times 10^{-4}$. Calculate the mean heat of formation of ammonia per mole in this temperature range. (in $cal$)

For the reversible reaction,$N_{2(g)} + 3H_{2(g)} \rightleftharpoons 2NH_{3(g)}$ at $500 \ ^oC$,the value of $K_P$ is $1.44 \times 10^{-5}$ when partial pressure is measured in atmospheres. The corresponding value of $K_c$ with concentration in $\text{mol L}^{-1}$ is:

$A$ mixture of $1 \ mol$ of $H_2O$ and $1 \ mol$ of $CO$ is taken in a $10 \ L$ container and heated to $725 \ K$. At equilibrium,$40\%$ of water reacts with carbon monoxide according to the equation:
$CO_{(g)} + H_2O_{(g)} \rightleftharpoons CO_{2(g)} + H_{2(g)}$
The equilibrium constant $K_C \times 10^2$ for the reaction is $.......$ (Nearest integer).

At a certain temperature in a $5\,L$ vessel,$2\,moles$ of carbon monoxide and $3\,moles$ of chlorine were allowed to reach equilibrium according to the reaction,$CO + Cl_2 \rightleftharpoons COCl_2$. At equilibrium,if $1\,mole$ of $CO$ is present,then the equilibrium constant $(K_c)$ for the reaction is: