In the table of standard reduction potentials, locate the half-reactions for the reductions of the following metal ions to the metal: Sn^+2 (aq), Au^+ (aq), Zn^2+ (aq), Co^2+ (aq), Ag^+ (aq), and Cu^2+ (aq). Among the metal ions and metal that make up these half reactions: a. Which metal ion is the weakest oxidizing agent? b. Which metal ion is the strongest oxidizing agent? c. Which metal ion is the strongest reducing agent? d. Which metal ion is the weakest reducing agent? e. Will Sn(s) reduce Cu^2+(aq) to Cu(s)? f. Will Ag(s) reduce Co^2+ (aq) to Co(s)? g. Which metal ion on the list can be reduce by Sn(s)? h. What metals can be oxidized by Ag^+(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.