The direct thermal decomposition of a solid metal oxide, \(\text{MO}_2\text{(s)}\), into its pure elements is thermodynamically unfavorable at \(298\text{ K}\):

\[ \text{MO}_2\text{(s)} \rightarrow \text{M(s)} + \text{O}_2\text{(g)} \quad \Delta G^\circ = +460\text{ kJ/mol}_{rxn} \]

To drive the extraction of pure \(\text{M(s)}\), this unfavorable decomposition can be coupled with an oxidation reaction through the shared intermediate \(\text{O}_2\text{(g)}\). Thermodynamic data for three candidate oxidation reactions at \(298\text{ K}\) are shown in the table below.

Reaction	Chemical equation	\(\Delta G^\circ_{298}\ (\text{kJ/mol}_{rxn})\)
1	\(2\,\text{C(s)} + \text{O}_2\text{(g)} \rightarrow 2\,\text{CO(g)}\)	\(-274\)
2	\(\text{C(s)} + \text{O}_2\text{(g)} \rightarrow \text{CO}_2\text{(g)}\)	\(-394\)
3	\(2\,\text{CO(g)} + \text{O}_2\text{(g)} \rightarrow 2\,\text{CO}_2\text{(g)}\)	\(-514\)

Which of the following balanced chemical equations represents an overall coupled process that is thermodynamically favorable at \(298\text{ K}\)?