For each of the following redox reactons, (i) Write the half-reactions; (ii) write the balanced equation for the whole reaction; (iii) determine in which direction the reaction will proceed spontaneously under standard-state conditions: (a) H₂(g) + Ni²+ (aq) - H+ [+ (aq) + Ni(s) (b) MnO4 (aq) + Cl¯(aq) - Mn²+ (aq) + Cl₂(g) (in acid solution) Cr³+ (aq) + Zn(s) (c) Cr(s) + Zn²+ (aq) -

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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.