Dissociation of a gas A_2 takes place according to the following chemical reaction. At equilibrium, the total pressure is 1 bar at 300 K. A_2( g ) ⇌…

Dissociation of a gas $\displaystyle \mathrm{A}_2$ takes place according to the following chemical reaction. At equilibrium, the total pressure is $\displaystyle 1$ bar at $\displaystyle 300$ K . $$\mathrm{A}_2(\mathrm{~g}) \rightleftharpoons 2 \mathrm{~A}(\mathrm{~g}) $$ The standard Gibbs energy of formation of the involved substances has been provided below:

Substance	$\displaystyle \Delta \mathrm{G}_{\mathrm{f}}^{\circ} / \mathrm{kJ} \mathrm{mol}^{-1}$
$\displaystyle \mathrm{A}_2$	-$\displaystyle 100.00$
A	-$\displaystyle 50.832$

The degree of dissociation of $\displaystyle \mathrm{A}_2(\mathrm{~g})$ is given by $\displaystyle \left(x \times 10^{-2}\right)^{1 / 2}$ where $\displaystyle x=$ $\displaystyle \_\_\_\_$. (Nearest integer). [Given: $\displaystyle \mathrm{R}=8 \mathrm{~J} \mathrm{~mol}^{-1} \mathrm{~K}^{-1}, \log 2=0.3010, \log 3=0.48$ ] Assume degree of dissociation is not negligible.