Calculate E° cll from the tabulated standard reduction potentials for each of the following reactions in aqueous solution. Then calculate AG° and K at 25°C from E° cell' F = 9.65 x 1o J/V•mol e R = 8.314 J/mol•K Acidic solution Standard reduction potential, E (Volts) Cu2" (ag) + e → Cu'(aq) Cu'(aq) + e - Cu(s) Mno, (ag) + 8H"(aq) + 5e Mn?"(ag) + 4H,0 Fe"(aq) + e – Fe2"(aq) 0.153 0.521 1.507 0.771 Basic solution Zn(OH) (s) + 2e Zn(s) + 40H (aq) Mno, (aq) + 2H,0 + 3e MnO,(s) + 4OH(aq) -1.22 0,588 a Mn04 + 5FE2+= Mn2+ + 5FE3+ (acidic solution) E°cell = AG° = kJ/mol K =

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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.