CHEM 1214 Lecture Notes - Lecture 2: Equilibrium Constant, Nernst Equation, Standard Tuning
Document Summary
The zn anode is wrapped with a metallic shell. The mno2 cathode is capped with a metallic plate. The cathode and anode are separated from each other by an insulating material: oxidation occurs at the anode of voltaic cells, including batteries. Oxidation involves the loss of electrons from the reducing agent (or reductant) At the alkaline battery anode, zinc metal acts as the reductant, and becomes oxidized. This oxidation half-reaction occurs in a basic aqueous environment and involves the loss of two electrons from zn to form zn2+: Zn (s) + 2oh- (aq) zno (s) + h2o (aq) + 2e- An oxidation half-reaction is not a complete reaction and does not occur unless it is coupled with a reduction half-reaction. The electrons lost in the oxidation of zn metal to form zn2+ in the alkaline cell will flow from the anode through an external circuit. At the alkaline battery cathode, the mno2 compound acts as the oxidant, and becomes reduced.