Cambridge AS & A Level Chemistry
24.2Standard electrode potentials E⦵, standard cell potentials E⦵cell and the Nernst equation
Standard electrode potentials E⦵, standard cell potentials E⦵cell and the Nernst equation in Cambridge AS & A Level Chemistry: what the syllabus expects you to know, the learning objectives and how to practise.
Subtopic44 practice questions2 lessons
Learning objectives
What the syllabus expects you to be able to do.
- 24.2.1Define standard electrode (reduction) potential and standard cell potential.
- 24.2.2Describe the standard hydrogen electrode.
- 24.2.3Describe how to measure E⦵ for metals and non-metals with their ions and for ions of the same element.
- 24.2.4Calculate E⦵cell from two electrode potentials.
- 24.2.5Use E⦵cell to deduce electrode polarity and electron flow, and to predict feasibility.
- 24.2.6Deduce the relative strength of oxidising and reducing agents from E⦵ values.
- 24.2.7Construct redox equations from half-equations.
- 24.2.8Predict qualitatively how E changes with ion concentrations.
- 24.2.9Use the Nernst equation to predict E quantitatively.
- 24.2.10Use ΔG⦵ = −nE⦵cellF.
Lessons
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Standard electrode potentials and cell potentials
50 min
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The Nernst equation and ΔG = −nFE
40 min
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Sample question
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Turn Standard electrode potentials E⦵, standard cell potentials E⦵cell and the Nernst equation into a strength.
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