For a reaction $A_{(s)} \rightleftharpoons B_{(s)} + C_{(g)}$,the set of all correct statements are:
$(a) \ K$ is independent of $[A]$.
$(b) \ K$ is dependent on partial pressure of $C$ at a given temperature.
$(c) \ \Delta H$ will be independent of temperature.
$(d) \ \Delta H$ is independent of the catalyst addition.

For the reaction $A + 2B \rightleftharpoons 2C + D$,the initial concentration of $A$ is $a$ and the initial concentration of $B$ is $1.5$ times that of $A$. If the concentrations of $A$ and $D$ are equal at equilibrium,what will be the concentration of $B$ at equilibrium?

One mole each of $He$ and $A(g)$ are taken in a $10 \text{ L}$ closed flask and heated to $400 \text{ K}$ to establish the following equilibrium: $A(g) \rightleftharpoons B(g)$. $K_{c}$ for this reaction at $400 \text{ K}$ is $4.0$. The partial pressures (in $\text{atm}$) of $He$ and $B(g)$ are respectively (at equilibrium) (Assume $He$,$A(g)$ and $B(g)$ behave as ideal gases) (Given: $R = 0.082 \text{ L atm K}^{-1} \text{ mol}^{-1}$)

$A$ mixture of $SO_2$ and $O_2$ at $5 \, atm$ pressure reacts $30\%$ until equilibrium is reached. Determine the total pressure of the equilibrium mixture in $atm$.
$2SO_{2(g)} + O_{2(g)} \rightleftharpoons 2SO_{3(g)}$

Eight moles of a gas $AB_3$ attained equilibrium in a closed container of volume $1 \, dm^3$. The reaction is $2AB_{3(g)} \rightleftharpoons A_{2(g)} + 3B_{2(g)}$. If at equilibrium $2 \, moles$ of $A_2$ are present,then the equilibrium constant is ...... $mol^2 \, L^{-2}$.

For the reactions $X \rightleftharpoons 2Y$ and $Z \rightleftharpoons P + Q$,the equilibrium constants $K_p$ and $K_q$ are in the ratio $1:9$. If the degree of dissociation of $X$ and $Z$ is the same,then the ratio of their total pressures is: