CHEM 1A03 Lecture Notes - Lecture 36: Standard Hydrogen Electrode, Redox, Electrochemical Cell

• School: McMaster University
• Department: Chemistry
• Course: CHEM 1A03
• Professor: Linda Davis, Sharonna Greenberg

Document Summary

Standard electrode potentials: absolute half-cells potentials cannot be measured: all potentials are measured relative to the standard hydrogen electrode (she); assigned a potential of 0v, standard conditions: conc. Under standard conditions: oxidation of metallic zn by cu2+ (eo cell = 1. 100 v) has a greater tendency to go to completion than does the oxidation of metallic cu by ag+ ions (eo cell= 0. 4600 v) Spontonaeity: eo cell and deltago: electromotive force or cell potential, joule=volt x coulomb (or volt= energy/unit charge, welec=zfecell, where work= -deltag, z= # electrons transferred (moles, f= 96485 c/mol e- (faraday constant) Negative deltag = spontaneous: any positive value of eo cell will result in a negative deltago (the reaction is spontaneous in forward direction) If you know eo positive eo cell, you can calculate k for a given redox reaction (for even a modestly cell value, k can be very large)