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 $K_c$.

At $T(K)$,$K_{c}$ value for $AO_{2(g)} + BO_{2(g)} \rightleftharpoons AO_{3(g)} + BO_{(g)}$ is $16$. In a closed $1 \ L$ flask,one mole each of $AO_2, BO_2, AO_3$ and $BO$ are taken and heated to $T(K)$. What is the concentration (in $mol \ L^{-1}$) of $AO_3$ at equilibrium?

For the reaction taking place at a certain temperature $NH_2COONH_{4(s)} \rightleftharpoons 2NH_{3(g)} + CO_{2(g)}$. If the equilibrium pressure is $3X \ bar$,then $\Delta _r G^o$ would be:

For the reaction $PCl_{5(g)} \rightleftharpoons PCl_{3(g)} + Cl_{2(g)}$ at equilibrium,the partial pressures of $PCl_5, PCl_3$ and $Cl_2$ are $2 \ atm, 4 \ atm$ and $4 \ atm$ respectively. The value of $K_C$ at $27^{\circ}C$ is (approx):-

For which one of the following reactions is $K_p = K_c$?

For the reactions $(1)$ and $(2)$ :
$A \rightleftharpoons B + C \dots (1)$
$D \rightleftharpoons 2E \dots (2)$
Given $K_{P_1} : K_{P_2} = 9 : 1$.
If the degree of dissociation of $A$ and $D$ is the same,then the total pressure at equilibria $(1)$ and $(2)$ are in the ratio (Assume reactions are started with equal number of moles of $A$ and $D$). (in $: 1$)