Standard Electrochemical Series

Standard Reduction Potentials (E°) at 25°C

Legend:

Half-equations used in today's programme activities
Half-Equation (Reduction) E° (V) Relative Strength
LiMn₂O₄ + Li⁺ + e⁻ → Li₂Mn₂O₄ +4.00 Very strong oxidising agent
Au³⁺ + 3e⁻ → Au +1.50 Very strong oxidising agent
Cl₂ + 2e⁻ → 2Cl⁻ +1.36 Very strong oxidising agent
O₂ + 4H⁺ + 4e⁻ → 2H₂O +1.23 Very strong oxidising agent
Br₂ + 2e⁻ → 2Br⁻ +1.09 Very strong oxidising agent
VO₂⁺ + 2H⁺ + e⁻ → VO²⁺ + H₂O +1.00 Strong oxidising agent
Ag⁺ + e⁻ → Ag +0.80 Strong oxidising agent
Fe³⁺ + e⁻ → Fe²⁺ +0.77 Strong oxidising agent
I₂ + 2e⁻ → 2I⁻ +0.54 Strong oxidising agent
VO²⁺ + 2H⁺ + e⁻ → V³⁺ + H₂O +0.34 Moderate oxidising agent
Cu²⁺ + 2e⁻ → Cu +0.34 Moderate oxidising agent
Li⁺ + e⁻ + C₆ → LiC₆ +0.10 Moderate oxidising agent
2H⁺ + 2e⁻ → H₂ 0.00 Moderate reducing agent
Pb²⁺ + 2e⁻ → Pb -0.13 Moderate reducing agent
Sn²⁺ + 2e⁻ → Sn -0.14 Moderate reducing agent
Ni²⁺ + 2e⁻ → Ni -0.25 Moderate reducing agent
V³⁺ + e⁻ → V²⁺ -0.26 Moderate reducing agent
Fe²⁺ + 2e⁻ → Fe -0.44 Moderate reducing agent
Zn²⁺ + 2e⁻ → Zn -0.76 Strong reducing agent
V²⁺ + 2e⁻ → V -1.18 Very strong reducing agent
Al³⁺ + 3e⁻ → Al -1.66 Very strong reducing agent
Mg²⁺ + 2e⁻ → Mg -2.37 Very strong reducing agent
Na⁺ + e⁻ → Na -2.71 Very strong reducing agent
K⁺ + e⁻ → K -2.92 Very strong reducing agent
Li⁺ + e⁻ → Li -3.04 Very strong reducing agent

Design Your Galvanic Cell

Optimisation Challenge

Find the combination that generates the highest cell potential from the available half-cells.

Your Best Results

Design some cells to see your results!

Laboratory Challenge Mode

Scenario: You're in the lab with limited chemicals. Design the most efficient galvanic cell using only these available materials:

Al
E° = -1.66 V
I
E° = +0.54 V
Fe
E° = +0.77 V
Li
E° = -3.04 V

Challenge Goal:

Using only the chemicals above, design the galvanic cell with the highest possible E°cell value.

Target to beat: +3.810 V

Hint: Remember that E°cell = E°cathode - E°anode