Mercuric oxide dry-cell batteries are often used where aflat discharge voltage and long life are required, such asin watches and cameras. The two half-cell reactions thatoccur in the battery areHgO(s) + H2O(l) + 2 e---->Hg(l) + 2 OH-(aq)Zn(s) + 2 OH-(aq)----->ZnO(s) + H2O(l) + 2 e-(a) Write the overall cell reaction. (b) The value of E°red forthe cathode reaction is +0.098 V. The overall cell potentialis +1.35 V. Assuming that both half-cells operate understandard conditions, what is the standard reduction potentialfor the anode reaction? (c) Why is the potential of theanode reaction different than would be expected if the reactionoccurred in an acidic medium?

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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.