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Electrochemical Series & The Nernst Equation

About This Model

This interactive tool allows you to build and explore electrochemical cells by combining different half-reactions. You can:

  • Select anode and cathode half-reactions from the electrochemical series
  • Adjust ion concentrations and observe how cell potential changes
  • Apply the Nernst equation to calculate actual cell potentials under non-standard conditions
  • Visualise electron flow and understand spontaneity (galvanic vs electrolytic cells)

Key equations:

Cell Potential: E°cell = E°cathode − E°anode

Nernst Equation: Ecell = E°cell − (RT/nF) ln Q

where R = 8.314 J/(mol·K), T = temperature (K), n = electrons transferred in the balanced cell reaction, F = 96485 C/mol, and Q = reaction quotient

Key concepts: Standard reduction potentials, electrochemical series, cell potential calculations, and the relationship between voltage and spontaneity. Useful for understanding batteries, fuel cells, and the fundamentals of electrochemistry.

Note: Q is computed assuming unit activity for solids/gases and a simplified ratio of the selected dissolved species. For multi-species reactions (e.g. lead-acid, water electrolysis) the calculated Q is therefore an approximation; the standard potential E° and qualitative trends remain correct.

Anode (Oxidation)

Select reduction half-reaction (the reaction is reversed at the anode)

E° = --- V
1.00 M

Cathode (Reduction)

Select reduction half-reaction

E° = --- V
1.00 M

Electrochemical Series

All reactions are written as reductions by convention

e⁻ flow: low E° → high E°

Quick Presets

Cell Potential

E°cell = E°cathode − E°anode

E°cell: --- V
Ecell: --- V
n (electrons): ---

Nernst Equation

E = E° − (RT/nF) ln Q

Select both half-cells to see calculation