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Electrode potentials, electrochemical cells and feasibility

Redox and electrochemistry · Lesson 2 of 3

Lesson 2 of 3

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Lesson 2 of 3 · Redox and electrochemistry

Electrode potentials, electrochemical cells and feasibility

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By the end you’ll be able to

define a standard electrode potential $E^\circ$ as the emf of a half-cell compared with the standard hydrogen electrode under standard conditions
describe the standard hydrogen electrode and the standard conditions used for electrode potentials, including solutions at about $1.0\ \text{mol dm}^{-3}$, gases at about $100\ \text{kPa}$ and a stated temperature, typically $298\ \text{K}$

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construct conventional cell diagrams for electrochemical cells from given half-cells and identify the direction of electron flow

calculate standard cell potentials using $$E^\circ_{\text{cell}} = E^\circ_{\text{right}} - E^\circ_{\text{left}}$$ or equivalent reduction-potential conventions, and relate the sign and magnitude to feasibility

predict whether a redox reaction is feasible under standard conditions from $E^\circ$ data, and evaluate limits of such predictions when conditions are non-standard or when kinetics affects whether reaction is observed

apply electrode potential ideas to reactions involving metals, non-metals, ions and oxidising agents such as halogens or transition-metal ions, including interpretation of disproportionation feasibility where required

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