Thermal decomposition of gaseous $X_2$ to gaseous X at 298 K takes place according to the following equation:$X_2\left(g\right)\stackrel{ }{\rightleftharpoons }2X\left(g\right)$

The standard reaction Gibbs energy,${\Delta }_r{G}^0$, of this reaction is positive. At the start of the reaction, there is one mole of $X_2$ and no X. As the reaction proceeds, the number of moles of  X formed is given by $\beta$ . Thus, ${\beta }_{equilibrium}$  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 : R=0.083 L bar $K^{-1}mo{l}^{-1}$) 

 

 

The INCORRECT statement among the following , for this reaction, is