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Electrode potentials and electrochemical cells (A-level only)
This A-level-only topic links redox chemistry to electrochemical cells.
9
Objectives
10
Flashcards
10
Questions
90 min
Study time
AqaA LevelChemistryPhysical chemistry
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Start revising Electrode potentials and electrochemical cells (A-level only)
Syllabus checklist
What you need to know
9 objective pages available
Standard electrode potentials (A-level only)5 objectives
- Describe the standard hydrogen electrode.
- Define standard electrode potential.
- Calculate cell potentials from standard electrode potentials.
- Set up and interpret electrochemical cell diagrams.
- Required practical: measure the EMF of an electrochemical cell.
Feasibility and applications of cells (A-level only)4 objectives
- Predict the feasibility of redox reactions using electrode potentials.
- Explain limitations of predictions based on standard conditions.
- Compare fuel cells with rechargeable and non-rechargeable cells.
- Explain how concentration and conditions affect cell potentials.
Key terms
Standard Electrode PotentialStandard Hydrogen Electrode (SHE)Standard Electrode Potential (E°)Galvanic CellAnodeCathodeOxidationReductionOxidizing AgentReducing AgentElectrochemical CellVoltage
Exam tips
- Memorize key values: Ensure you remember that the standard electrode potential of the SHE is 0.00 V.
- Always state the conditions for standard electrode potentials: When defining or using standard electrode potentials, always mention the standard conditions (1 M, 1 atm, 25°C).
Common mistakes
- Confusing electrode potentials: Remember that the SHE is defined as 0.00 V and serves as a reference point for all other measurements.
- Confusing oxidation and reduction: Remember that oxidation is the loss of electrons and reduction is the gain of electrons. Use the standard electrode potentials to identify the anode and cathode.
Practice preview
- What is the standard electrode potential of the standard hydrogen electrode (SHE)?
- Describe the setup of a standard hydrogen electrode.
- Calculate the standard electrode potential of a half-cell if the reaction is: Cu²⁺(aq) + 2e⁻ ⇌ Cu(s) and the standard electrode potential of the SHE is 0.00 V. Given that the standard electrode potential of the copper half-cell is +0.34 V, what is the overall cell potential when combined with the SHE?
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