PARAGRAPH 1

Thermal decomposition of gaseous $$X_2$$ to gaseous X at 298 K takes place according to the following equation :
$$ X_2(g) \rightleftharpoons 2X(g)$$
The standard reaction Gibbs energy, $$\triangle_rG^\circ$$, 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 2bar. Consider the gases to behave ideally. (Given: $$R = 0.083 L bar K^{-1} mol^{-1})