LESSON OBJECTIVE: Investigate the relationship between concentration and cell potential both qualitatively and, using the Nernst equation, quantitatively
Learning Outcomes:
(taken from the Cambridge International AS and A Level Chemistry curriculum)
24.2 Standard electrode potentials E⦵; standard cell potentials E⦵cell and the Nernst equation
6 deduce from E values the relative reactivity of elements, compounds and ions as oxidising agents or as
reducing agents
7 construct redox equations using the relevant half-equations
8 predict qualitatively how the value of an electrode potential, E, varies with the concentration of the aqueous ions
9 use the Nernst equation, e.g. E = E⦵ + (0.059/z) log [oxidised species]/[reduced species] to predict quantitatively how the value of an electrode potential varies with the concentrations of the aqueous ions; examples include Cu2+(aq) + 2e- ⇌ Cu(s), Fe3+(aq) + e- ⇌ Fe2+(aq)
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