Electrochemistry & the Nernst Equation

Module 8 · 8 of 8

🔋Electrochemistry & the Nernst Equation

Turning ΔG into cell voltage

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Turning ΔG into cell voltage

Electrochemistry is thermodynamics you can read on a voltmeter. The cell potential is just −ΔG per electron, the Nernst equation shows how it responds to concentration, and standard potentials connect directly to equilibrium constants.

Difficulty

advanced

Time

~35 min

Equations

Practice Qs

Learning Objectives

✓Compute standard cell potential from half-cell reduction potentials
✓Relate ΔG° = −nFE° and predict spontaneity from E°
✓Apply the Nernst equation to non-standard concentrations
✓Connect E° to the equilibrium constant K
✓Identify anode/cathode and electron flow in a galvanic cell

Prerequisites

Gibbs energy & equilibriumBalancing redox half-reactions

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