List of top Chemistry Questions on Equilibrium Constant asked in AP EAPCET

At \(450\,K\), for the reaction \[ 2SO_2(g)+O_2(g)\rightleftharpoons 2SO_3(g), \] the value of \[ K_p=2.0\times10^{10}. \] What is the value of \(K_c\) for the decomposition of sulphur trioxide at the same temperature? \[ R=0.083\ \text{L bar mol}^{-1}\text{K}^{-1} \]
At T(K) the $K_c$ for the reactions (I) and (II) are $2.4 \times 10^{30}$ and 1.4 respectively. What is the $K_c$ value for: $\frac{1}{2}N_2(g) + \frac{1}{2}O_2(g) + \frac{1}{2}Br_2(g) \rightleftharpoons NOBr(g)$?
At a given temperature T in a 10.0 L flask, 2.0 moles of N$_2$O$_4$(g) is heated. At equilibrium, 20% of N$_2$O$_4$(g) dissociates into NO$_2$(g). The value of K$_C$ for the reaction N$_2$O$_4$(g) $\rightleftharpoons$ 2NO$_2$(g) is:
For the reaction X(g) $\rightarrow$ Y(g) at equilibrium, the partial pressure of Y is one-third that of X. What is the standard Gibbs energy change ($\Delta G^\circ$) for this reaction?
For ammonia formation from constituent elements, the expression for \(K_c\) is
At \(500\,\text{K}\), for the reaction, \[ N_2(g)+3H_2(g)\rightleftharpoons 2NH_3(g), \] the \(K_p\) is \(0.036\,\text{atm}^{-2}\). What is its \(K_c\) in \(L^2\text{mol}^{-2}\)? \((R=0.082\,L\,\text{atm mol}^{-1}\text{K}^{-1})\)
At $1000\, K$, the equilibrium constant. $K_{C}$ for the reaction $2 NOCl (g) \rightleftharpoons 2 NO (g)+ Cl _{2}(g)$ is $4.0 \times 10^{-6} mol\, L ^{-1}$. The $K_{P}$ (in bar) at the same temperature is $\left(R=0.083 \,L\right.$ bar $\left. K ^{-1}\, mol ^{-1}\right)$