CHEM 1E03 Lecture Notes - Lecture 32: Voltmeter, Electroplating, Electrochemistry

• School: McMaster University
• Department: Chemistry
• Course: CHEM 1E03
• Professor: Randall Dumont; Linda Davis

Document Summary

Electrochemistry: electron transfer reactions of redox reactions, electrons move from reducing agent to oxidizing agent, the net reaction is composed of two half reactions, one reduced, one oxidized. Electrochemical cells: galvanic or voltaic cells cause the release of electrons by the oxidation of the half reaction. Because electrons travel from the anode to the cathode, the anode decreases in size, and the cathode will increase in size as electrons move towards it. Contents: solution of anode in one beaker, solution of cathode in another beaker, salt bridge an inert ionic solution that continues to allow electricity to flow (closed circuit). Without the salt bridge the reaction would stop and reach equilibrium: flowing ions flow in opposite direction to electrons. If there are no metals among the reactants and products, use an inert metal (platinum) to serve as the anode/cathode: this is an inactive electrode. Solution: fe(s) | fe2+(aq) || sn2+(aq) | sn(s)