Electrochemistry

(a) describe and explain redox processes in terms of electron transfer and/or of changes in
oxidation number (oxidation state)
(b) define the terms:
     (i) standard electrode (redox) potential
     (ii) standard cell potential
(c) describe the standard hydrogen electrode
(d) describe methods used to measure the standard electrode potentials of:
     (i) metals or non-metals in contact with their ions in aqueous solution
     (ii) ions of the same element in different oxidation states
(e) calculate a standard cell potential by combining two standard electrode potentials
(f) use standard cell potentials to:
     (i) explain/deduce the direction of electron flow from a simple cell
     (ii) predict the feasibility of a reaction
(g) understand the limitations in the use of standard cell potentials to predict the feasibility of a reaction
(h) construct redox equations using the relevant half-equations (see also Section 9.4)
(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:
     (i) the quantity of charge passed during electrolysis
     (ii) the mass and/or volume of substance liberated during electrolysis, including those in the electrolysis of H2SO4(aq); Na2SO4(aq)
(n) explain, in terms of the electrode reactions, the industrial processes of:
     (i) the anodising of aluminium
     (ii) the electrolytic purification of copper

Tweet