MnO4– + Sn ---> MnO2 + Sn2+ a) What is the half reaction that takes place at the cathode? b) What is the standard cell potential? c) What will be the potential of a cell constructed using 57.0 g MnO2, 1.57 M MnO4–, 14.8 g Pt, 12.5 g Sn and 0.87 M Sn2+ at pH 2.5?

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Q: Cr3+(aq) → Cr(s) Zn2+(aq) → Zn(s) a. What will be the overall balanced reaction if you want to make…

A: The answer is discussed below, Oxidation occurs at the anode and reduction occurs at the cathode.

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Q: nO4– + Sn ----> MnO2 + Sn2+ A) Identify the half-reaction that occurs at the cathode. B) Identify…

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A: E°(cell) = E°(cathode) - E°(anode) Anode: oxidation occurs Cathode: Reduction occurs

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Electrolysis

Electrolysis is defined as the process of breaking down ionic compounds into their constituent elements by passing a direct electric current through the compound in a fluid state. The cathode reduces cations, while the anode oxidizes anions. An electrolyte, electrodes, and some form of external power source are the main components required for conducting electrolysis. A partition, such as an ion-exchange membrane or a salt bridge, may also be used, but this is optional. These are primarily used to prevent the products from diffusing near the opposing electrode.