List of top Chemistry Questions on Chemical Equilibria and Dissociation asked in JEE Main

The reaction $A(g) \rightleftharpoons B(g) + C(g)$ was initiated with the amount 'a' of $A(g)$. At equilibrium it is found that the amount of $A(g)$ remaining is $(a - x)$ at a total pressure of p.
The equilibrium constant $K_p$ of the reaction can be calculated from the expression :

20 mL of a solution of acetic acid required 28.4 mL of 0.1 M NaOH for its neutralization. A solution (X) was prepared by mixing 20 mL of the above acetic acid and 14.2 mL of 0.1 M NaOH solution. What is the pH of the solution (X)? (\( pK_a \) value of acetic acid is 4.75).

The values of pressure equilibrium constant recorded at different temperatures for the following equilibrium reaction have been given below:
\(A(g) \rightleftharpoons B(g) + C(g)\)}

The magnitude of \(\frac{\Delta H^\circ}{R}\) calculated from the above data is ____. (Nearest integer)}

Decomposition of a hydrocarbon follows the equation} \[ k = (5.5 \times 10^{11}\, s^{-1})\, e^{\frac{-28000}{T}} \] The activation energy of reaction is _____ kJ mol\(^{-1}\). (Nearest Integer)} Given: \(R = 8.3\, J\,K^{-1}\,mol^{-1}\)}

Given is a concentrated solution of a weak electrolyte \(A_xB_y\) of concentration \(c\) and dissociation constant \(K\). The degree of dissociation is given by:

At T(K), the equilibrium constant of \(A_2(g) + B_2(g) \rightleftharpoons C(g)\) is \(2.7 \times 10^{-5}\). What is the equilibrium constant for \(\frac{1}{3} A_2(g) + \frac{1}{3} B_2(g) \rightleftharpoons \frac{1}{3} C(g)\) at the same temperature?

Solid carbon, CaO and CaCO$_3$ are mixed and allowed to attain equilibrium at T K. \[ \text{CaCO}_3(s) \rightleftharpoons \text{CaO}(s) + \text{CO}_2(g) \quad K_{P1} = 0.08 \, \text{atm} \] \[ \text{C}(s) + \text{CO}_2(g) \rightleftharpoons 2 \text{CO}(g) \quad K_{P2} = 2 \, \text{atm} \] The partial pressure of CO is _______ \(\times 10^{-1}\) atm.

Given at 298 K:
\(E^\circ_{\rm Fe^{2+}/Fe} = X\) Volt
\(E^\circ_{\rm Fe^{3+}/Fe} = Y\) Volt
The \(E^\circ_{\rm Fe^{3+}/Fe^{2+}}\) in Volt at 298 K is given by:

Consider the reaction: $$ X_2Y(g) \rightleftharpoons X_2(g) + \frac{1}{2} Y_2(g) $$ The equation representing the correct relationship between the degree of dissociation \( x \) of \( X_2Y(g) \) with its equilibrium constant \( K_p \) is: