Learning outcomes - after studying this topic, you should be able to:

• relate the sign of the electrode potential to the direction of spontaneous change
• combine half cells to produce balanced redox reactions and to calculate cell potentials
• identify the species which are being oxidzied and those being reduced in a redox reaction
• write down the cell notation for a Galvanic cell including ones involving inert electrodes
• use the Nernst equation to calculate the effect of concentration on the cell potential
• relate the electrode potential and the reaction quotient
• relate the standard electrode potential, the equilibrium constant and the change in Gibbs free energy

• Sections 12.1 - 12.5 (in Blackman, Bottle, Schmid, Mocerino and Wille, Chemistry, 3^rd Edition, 2015 (John Wiley) )

• Electrochemistry (in ChemWiki)

Balancing redox equations Tags: Redox equations Contributed by Adam Bridgeman

Electrochemistry Tags: electrochemistry Contributed by Adam Bridgeman

Complexes and redox equations Tags: redox reactions Contributed by Adam Bridgeman

Electrochemistry Tags: electrochemistry Contributed by Adam Bridgeman

Redox Reactions and Cell Potentials Tags: redox | cell potentials | half cells Contributed by Adam Bridgeman

Electrochemical Cells (short video tutorial) Tags: Galvanic | voltaic | electrolytic Contributed by Adam Bridgeman

Cell potentials Tags: Galvanic cells | voltaic cells Contributed by Adam Bridgeman

Galvanic Cells Tags: Galvanic cells | voltaic cells Contributed by Adam Bridgeman