SA 150 Lecture Notes - Lecture 85: Redox, Electrochemical Cell, Electroplating

• School: Simon Fraser University
• Department: Sociology and Anthropology
• Course: SA 150
• Professor: Amie Mc Lean

Document Summary

Electrochemical cell spontaneous redox reaction produces electricity. Electrolysis add electricity to non-spontaneous reactions to make them go: electrolysis of water. But if we add electricity (e-) we can start the reduction process: battery inert electrode (pt) E- (cathode) inert electrode (pt) o2 (anode) You require at least an input of 1. 23 v to electrolyze water. Half-cell overpotential in practice, these half-cells are not at standard state or there is resistance in the wire for example. Therefore, a half-cell might require more voltage (aka: over potential) to actually undergo oxidation/reduction. Electrolysis of water"s overpotential is shown on the table of standard reduction potentials: type 1 electrolysis cell. Inert electrodes in a molten salt: example: electrolysis of molten nacl makes cl2 and na! battery inert electrode (c) E- (cathode) inert electrode (c) cl2 na (s) (anode) Overall: 2na+ + 2cl- cl2 (g) + 2na (s) e cell = -4. 07 v.