Describe how a voltaic cell operates, with the concepts of electrodes, salt
bridges, half-cell reactions, net cell reaction, and cell diagram.
Describe the standard hydrogen electrode and explain how other standard
electrode potentials are related to it.
Use tabulated standard potentials, Eo to determine
Eocell for an oxidation-reduction reaction and predict
whether the reaction is spontaneous.
Quantitatively and qualitatively predict the effect of varying conditions
(concentrations and gas pressures) on values of Ecell.
Know and be able to use the equations that relate [Delta]Go,
Eocell, and K.
Describe some common voltaic cells: the flashlight or dry cell, the lead
storage battery, the silver-zinc cell, and the fuel cell.
Explain the corrosion of metals in electrochemical terms and describe
methods of corrosion protection.
Describe an electrolytic cell and how it differs from a voltaic cell.
Identify the possible half reactions that might occur in an electrolysis and
choose the pair that will occur, based on the highest (least negative) cell
potential.
Use Faraday's law to relate the quantity of chemical change produced by a
given amount of electric charge.