Can nitrate and sulfate ions be oxidised during electrolysis of their molten compounds?

\begin{align} \ce{O2 + 4H+ + 4e- \;&<=> 2H2O}\quad\quad &&E^\circ = +1.229\ \mathrm{V}\\ \ce{S2O8^2- + 2e- \;&<=> 2SO4^2-}\quad\quad &&E^\circ = +2.01\ \mathrm{V} \end{align}

From the above, I know that an aqueous solution of a sulfate salt undergoing electrolysis will not oxidise to peroxydisulfate ions over water being oxidised to oxygen at the anode unless it is at extremely high concentrations.

However, what if the solution is molten? Will the product at the anode be peroxydisulfate?

Also, can nitrate ions be oxidised? Perhaps to peroxynitrate or peroxynitrite?

• Peroxysulfates are industrially created in aqueous electrolysis. Nothing extreme is needed, just concentrated solution and high density current. You didn't think about overpotential here, it seems. – Mithoron Oct 19 '17 at 14:08

Whether or not the products will be some peroxyanions is another question. At high temperatures typical of molten salts, I don't think they will survive. Hence I would expect $\ce{O2}$ + disulfate in the first case and $\ce{O2 + NO2}$ in the second.
• Nitrogen would get reduced because it has nowhere else to go. There are no binitrates (unlike bisulfates), and $\ce{N2O5}$ is not particularly stable. This has little to do with electrolysis. – Ivan Neretin Oct 19 '17 at 13:30
• Note the autoionization of dinitrogen tetroxide given by en.wikipedia.org/wiki/Molecular_autoionization. Oxygen seems to transfer with one negative charge. Might the effective oxidation state of oxygen in nitrogen oxide/nitrate solvent systems be $-1$ instead of $-2$? It would give a more parsimonious description of the anodic reaction of nitrate ion in nitrate solvents. – Oscar Lanzi Oct 19 '17 at 14:33