Physical chemistry - 6. Electrochemistry


I Redox processes:

II Electrode potentials

III Electrolysis

Learning outcomes

Candidates should be able to:

(a) describe and explain redox processes in terms of electron transfer and/or of changes in oxidation number (oxidation state)

(b) explain, including the electrode reactions, the industrial processes of:

(c) define the terms:

(d) describe the standard hydrogen electrode

(e) describe methods used to measure the standard electrode potentials of:

(f) calculate a standard cell potential by combining two standard electrode potentials

(g) use standard cell potentials to:

(h) construct redox equations using the relevant half-equations (see also Section 9.5)

(i) predict qualitatively how the value of an electrode potential varies with the concentration of the aqueous ion

(j) state the possible advantages of developing other types of cell, e.g. the H2/O2 fuel cell and improved batteries (as in electric vehicles) in terms of smaller size, lower mass and higher voltage

(k) state the relationship, F = Le, between the Faraday constant, the Avogadro constant and the charge on the electron

(l) predict the identity of the substance liberated during electrolysis from the state of electrolyte (molten or aqueous), position in the redox series (electrode potential) and concentration

(m) calculate:

(n) describe the determination of a value of the Avogadro constant by an electrolytic method