Step 1: Balance the unbalanced half oxidation reaction for Pb(s) → Pb2+ (aq) Step 2: Balance the unbalanced half reduction reaction for O2 (aq) + H2O(l)→ OH– (aq) Step 3: Add the two half reactions to give the full redox reaction: Step 4: Identify the oxidizing agent Step 5: Identify the reducing agent   For step 1 and step 2, along with balancing the equations, please show how many electrons are added. For example, for the first half reaction, 2 electrons are added. So how many electrons are added in the second half reaction?

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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.