What Forms at the Anode During Electrolysis of Molten Chromium Sulphate?

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SUMMARY

During the electrolysis of molten chromium sulfate, chromium forms at the cathode, while the anode produces sulfur dioxide (SO2) and oxygen (O2). The reaction can be represented as 2SO4^2- -> 2SO3 + O2 + 4e-. The discussion highlights the complexity of oxidation states, specifically the reduction of sulfur from VI to IV, and questions the plausibility of producing peroxodisulfate in a molten state. Overall, the electrolysis process involves significant chemical transformations that may differ from theoretical predictions.

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During the electrolysis of a molten sulphate, for example Chromium sulphate. At the cathode, chromium forms but what forms at the anode? Is it sulphur dioxide and oxygen?
 
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Peroxodisulfate? Why dioxide and not trioxide?

But honestly I am just thinking aloud.
 
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Wow, that comment confused me more :D
 
Electrolytic oxidation of sulfate to peroxodisulfate in water solution is part of the old method of a hydrogen peroxide production, no idea if it will happen in molten state as well - but perhaps it can.

To get sulfur dioxide you need to reduce sulfur from VI to IV, and reduction at anode doesn't sound plausible to me. On the other hand oxidation of oxygen and production of SO3

2SO42- -> 2SO3 + O2 + 4e-

seems to be reasonable idea.

But this is just shifting of the atoms on paper, reality can be completely different.
 
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Thanks :)
 

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