List of top Chemistry Questions on Law Of Chemical Equilibrium And Equilibrium Constant asked in KEAM

Kc for the reaction A(g) + 2B(g) \(\rightleftharpoons\) C(g) + 2D(g) is 4.0 at 300 K. What is the value of K'c for the reaction, 2C(g) + 4D(g) \(\rightleftharpoons\) 2A(g) + 4B(g) at 300 K?
For the homogeneous equilibrium \(N_{2(g)} + 3H_{2(g)} \rightleftharpoons 2NH_{3(g)}\), the equilibrium constants \(K_P\) and \(K_C\) are related as:
Which one of the following conditions will favour maximum formation of the product in the reaction, \( A_{2}(g) + B_{2}(g) \rightleftharpoons X_{2}(g) \), \( \Delta_r H = -x \,\text{kJ} \):
For the equilibrium,
\( 2\text{A}_{(g)} \rightleftharpoons 2\text{B}_{(g)} + 2\text{C} \)
the value of \( K_p \) is 0.1662 atm at 1000 K. The value of \( K_c \) at the same temperature is ( \( R = 0.0831 \) )
The following concentrations were obtained in the formation of $NH_{3(g)}$ from $N_{2(g)}$ and $H_{2(g)}$ at equilibrium at $500\ \text{K}$: $[NH_{3}]=1.5\times10^{-2}\ \text{M}$, $[N_{2}]=5\times10^{-3}\ \text{M}$ and $[H_{2}]=0.10\ \text{M}$. Calculate the equilibrium constant $K_{c}$ for the reaction $N_{2(g)}+3H_{2(g)} \rightleftharpoons 2NH_{3(g)}$.
At a certain temperature, 2 moles of CO and 4 moles of Cl$_2$ gases were reacted to form COCl$_2$ in a 10 L vessel. At equilibrium if one mole of CO is present then equilibrium constant for the reaction is
The equilibrium constant for the reaction, N$_2$(g) + 3H$_2$ $\rightleftharpoons$ 2NH$_3$(g) and 2N$_2$(g) + 6H$_2$ $\rightleftharpoons$ 4NH$_3$(g) are $K_1$ and $K_2$, respectively. The relationship between $K_1$ and $K_2$ is
In the $\ln K$ vs $\frac{1}{T}$ plot of a chemical process having $\Delta S^\circ > 0$ and $\Delta H^\circ < 0$, the slope is proportional to (where $K$ is equilibrium constant)}
The equilibrium pressure for the reaction MSO\(_4\cdot 2\)H\(_2\)O(s) \( \rightleftharpoons \) MSO\(_4\)(s) + 2H\(_2\)O(g) is \( \frac{\pi}{4} \) atm at 400 K. The \( K_p \) for the given reaction (in atm\(^2\)) is
Equilibrium constants are given for the following two equilibria: \[ (i)\; A_2(g) + B_2(g) \rightleftharpoons 2AB(g); \quad K_1 = 2 \times 10^{-4} \] \[ (ii)\; 2AB(g) + C_2(g) \rightleftharpoons 2ABC(g); \quad K_2 = 2 \times 10^{-2}\, L\, mol^{-1} \] Calculate the equilibrium constant for: \[ ABC(g) \rightleftharpoons \frac{1}{2}A_2(g) + \frac{1}{2}B_2(g) + \frac{1}{2}C_2(g) \]