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My question: the higher the reduction potential value, the more it's likely to be reduced and is more inclined to be the cathode reaction? Sometimes this isn't the case, why?
Thanks
Thanks
Sometimes this isn't the case, why?
Thanks
Electrolysis reverses the potential.
My question: the higher the reduction potential value, the more it's likely to be reduced and is more inclined to be the cathode reaction? Sometimes this isn't the case, why?
Thanks
yes, the higher (more positive) the reduction potential, the greater the tendency for that atom to be reduced. Compounds that want to be reduced will gain electrons at the cathode. Electrons will flow from the atom being oxidized at the anode (something with a large, negative reduction potential, which means it favors oxidation) and the electrons will flow to the cathode, which is where what's in solution grabs those electrons and becomes reduced.
When in a galvanic cell do you see that it is not the case?
When in a galvanic cell do you see that it is not the case?