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Alicia Lin 2F
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Postby Alicia Lin 2F » Sat Feb 29, 2020 3:31 pm

For this question, if I choose the water reaction to occur at the cathode and the Mn2+ reaction to happen at the anode, wouldn't this yield a positive Ecell value? Since Ecell=-0.42V-(-1.18V)=+0.76V. But we are dealing with electrolytic cells which are supposed to be negative Ecell right? How does this make sense

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Re: 6O.3a

Postby Chem_Mod » Sat Feb 29, 2020 9:46 pm

You are electrolyzing an aqueous solution of metal cations; you are not “choosing” per se what reduction half reaction occurs but figuring out which one will occur. Even if you run a current through the cell to allow the non-spontaneous reaction to occur, the two reduction half reactions are still competing with each other and the more favorable one will occur

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