Thermal decomposition of gaseous $\mathrm{X}_2$ to gaseous X at 298 K takes place according to the following equation : $$ \mathrm{X}_2(\mathrm{~g}) \rightleftharpoons 2 \mathrm{X}(\mathrm{~g}) $$ The standard reaction Gibbs energy, $\Delta_{\mathrm{r}} \mathrm{G}^{\circ}$, of this reaction is positive. At the start of the reaction, there is one moe of $\mathrm{X}_2$ and no X . As the reaction proceeds, the number of moles of X formed is given by $\beta$. Thus, $\beta_{\text {equilibrium }}$ is the number of moles of $X$ formed at equilibrium. The reaction is carried out at a constant total pressure of 2 bar. Consider the gases to behave ideally. (Given : $\mathrm{R}=0.083 \mathrm{~L}$ bar $\mathrm{K}^{-1} \mathrm{~mol}^{-1}$ ) The Incorrect statement among the following, for this reaction is