An electrolytic cell is used to decompose individual samples of three pure molten chloride salts: \(\text{NaCl(l)}\), \(\text{MgCl}_2\text{(l)}\), and \(\text{ZnCl}_2\text{(l)}\). The standard reduction potentials for the relevant half-reactions are shown in the table below.

Half-reaction	\(E^\circ\text{ (V)}\)
\(\text{Zn}^{2+} + 2\,\text{e}^- \rightarrow \text{Zn(s)}\)	\(-0.76\)
\(\text{Mg}^{2+} + 2\,\text{e}^- \rightarrow \text{Mg(s)}\)	\(-2.37\)
\(\text{Na}^+ + \text{e}^- \rightarrow \text{Na(s)}\)	\(-2.71\)
\(\text{Cl}_2\text{(g)} + 2\,\text{e}^- \rightarrow 2\,\text{Cl}^-\)	\(+1.36\)

Which of the following lists the three molten salts in order of the minimum theoretical external voltage required to induce decomposition, from greatest to least?