Chemistry Question from JEE Main 2026 · 22 January, Shift 1

Dissociation of a gas $A_2$ takes place according to the following chemical reaction. At equilibrium, the total pressure is $1 \, \text{bar}$ at $300 \, \text{K}$.

The standard Gibbs energy of formation of the involved substances is given below:

Substance $\Delta G_f^\circ$ ($\text{kJ mol}^{-1}$) $A_2$ $-100.00$ $A$ $-50.832$

The degree of dissociation of $A_2(\text{g})$ is given by $\left(x \times 10^{-2}\right)^{1/2}$ where $x =$ _____ (Nearest integer).

[Given: $R = 8 \, \text{J mol}^{-1}\text{K}^{-1}$, $\log 2 = 0.3010$, $\log 3 = 0.48$. Assume degree of dissociation is not negligible.]