A thermodynamic evaluation is conducted on four industrial chemical reactions. The standard enthalpy change, \(\Delta H^\circ\), and standard entropy change, \(\Delta S^\circ\), for each reaction at \(298 \text{ K}\) are shown in the table below.

Reaction	Chemical equation	\(\Delta H^\circ\ (\text{kJ/mol}_{\text{rxn}})\)	\(\Delta S^\circ\ (\text{J}/(\text{mol}_{\text{rxn}}\cdot\text{K}))\)
1	\(\text{N}_2\text{O}_4\text{(g)} \rightarrow 2\,\text{NO}_2\text{(g)}\)	\(+60\)	\(+200\)
2	\(\text{PCl}_5\text{(g)} \rightarrow \text{PCl}_3\text{(g)} + \text{Cl}_2\text{(g)}\)	\(+100\)	\(+200\)
3	\(\text{CaCO}_3\text{(s)} \rightarrow \text{CaO(s)} + \text{CO}_2\text{(g)}\)	\(+180\)	\(+225\)
4	\(\text{C(s)} + \text{H}_2\text{O(g)} \rightarrow \text{CO(g)} + \text{H}_2\text{(g)}\)	\(+120\)	\(+100\)

Assuming that \(\Delta H^\circ\) and \(\Delta S^\circ\) remain constant with changing temperature, which of the following correctly ranks the reactions in order of increasing minimum temperature at which each reaction becomes thermodynamically favorable under standard conditions (\(\Delta G^\circ < 0\))?