An aqueous SnCl2 solution is electrolyzed under 1 bar pressure using platinum electrodes. (a) Write the half-reactions predicted to occur at the anode and cathode, based on the standard cell potentials given below. Standard Reduction Potentials (Volts) at 25 °C Cl2(g) + 2 e- 2 Cl-(aq) 1.360 O2(g) + 4 H3O+(aq) + 4 e- 6 H2O(l) 1.229 2 H2O(l) + 2 e- H2(g) + 2 OH-(aq) -0.828 Sn2+(aq) + 2 e- Sn(s) -0.140     Half-reaction at anode:   Half-reaction at cathode:

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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.