The direct decomposition of solid titanium(IV) oxide into its elements is thermodynamically unfavorable at \(298\text{ K}\), as represented by the following equation:

\[\text{TiO}_2\text{(s)} \rightarrow \text{Ti(s)} + \text{O}_2\text{(g)} \quad \Delta G^\circ_{298} = +890\text{ kJ/mol}_{\text{rxn}}\]

To produce \(1.0\text{ mol}\) of \(\text{Ti(s)}\), the decomposition reaction is coupled with one of three auxiliary oxidation processes at \(298\text{ K}\), shown in the table below.

Auxiliary process	Balanced chemical equation	\(\Delta G^\circ_{298}\text{ (kJ/mol}_{\text{rxn}}\text{)}\)
Process X	\(2\,\text{Mg(s)} + \text{O}_2\text{(g)} \rightarrow 2\,\text{MgO(s)}\)	\(-1140\)
Process Y	\(\text{Ca(s)} + \frac{1}{2}\,\text{O}_2\text{(g)} \rightarrow \text{CaO(s)}\)	\(-600\)
Process Z	\(2\,\text{CO(g)} + \text{O}_2\text{(g)} \rightarrow 2\,\text{CO}_2\text{(g)}\)	\(-510\)

Which of the following correctly ranks the three coupled processes in order of thermodynamic favorability for the production of \(1.0\text{ mol}\) of \(\text{Ti(s)}\) at \(298\text{ K}\), from most favorable to least favorable?