Thermal decomposition of gaseous `X_(2)`to gaseous X at 298 K takes place accoeding to the following equation: `X_(2_(g)hArr2X(g)` 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.` The `beta_("equulibrium")` is the number of moles of X formed at equlibrium. The reaction is carried out at a constant total pressure of 2 bar. Consider the gases to behave ideally. (Given: The standard reaction Gibbs energy, `Delta_(r)G^(@),` of this reaction `R=0.08L barK^(-1)mol^(-1)`) The equlibrium constatn `K_(p)` for this reaction at 298 K, in terms of `beta_("equlibrium,")` isA. `(8beta_("equlibrium")^(2))/(2-beta_("equlibrium"))`B. `(8beta_("equlibrium")^(2))/(4-beta_("equlibrium")^(2))`C. `(4beta_("equlibrium")^(2))/(2-beta_("equlibrium"))`D. `(4beta_("equlibrium")^(2))/(4-beta_("equlibrium")^(2))`