In some applications nickel–cadmium batteries have beenreplaced by nickel–zinc batteries. The overall cell reactionfor this relatively new battery is:2 H2O(l) + 2 NiO(OH)(s) + Zn(s)---->2 Ni(OH)2(s) + Zn(OH)2(s)(a)What is the cathode half-reaction? (b)What is the anodehalf-reaction? (c) A single nickel–cadmium cell has a voltageof 1.30 V. Based on the difference in the standard reductionpotentials of Cd2+ and Zn2+, what voltage would youestimate a nickel–zinc battery will produce? (d) Would youexpect the specific energy density of a nickel–zinc battery tobe higher or lower than that of a nickel–cadmium battery?

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Q: Question attached

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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.