Why do Cathodes carry a positive charge and Anodes carry a negative charge in galvanic cells, but in electrolytic cells, Cathodes have a negative charge and Anodes have a positive charge? I’m a grade 12 chemistry student and I’m having trouble understanding this concept. Could someone please explain the rationale behind this apparent reversal of charges in the two types of cells?
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Think of it as what work is being done and who’s doing it. Both are electrochemical cells but what’s happening underneath – chemical energy to electrical versus the other way around ( electrical work to perform a chemical reaction) matters defines them better.
Anode and cathode definitions are not who holds what charge but where the oxidation and reduction reactions are taking place.
In the galvanic case chemical reaction occurs spontaneously while in the electrolytic case it is work done against a potential.
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