Select electrochemistry module (galvanic cells, electrolysis, or corrosion) from cat-filter dropdown
Enter material pairs (e.g., zinc anode, copper cathode), electrolyte concentration (mol/L), temperature (°C), and applied voltage or current density (A/m²)
Run simulation to compute standard cell potential (V), Faraday efficiency (%), mass deposition rate (mg/h), and corrosion penetration depth (μm/year)

Worked Example

Copper electroplating on steel substrate: anode Cu (pure), cathode steel, 0.5 M CuSO₄ electrolyte at 25°C, applied voltage 2.5 V, current density 500 A/m². Theoretical standard potential E° = +0.34 V. With 85% Faraday efficiency, deposit rate = 0.18 mg/cm²/h. Over 4 hours, copper thickness = 72 μm. Overpotential loss ≈ 0.6 V due to activation and concentration gradients.

Practical Notes

For galvanic couples, worst-case galvanic corrosion occurs when zinc (anode) connects to stainless steel (cathode) in seawater; penetration rates exceed 150 μm/year without isolation sleeves
Faraday efficiency drops 10–20% in dilute electrolytes (<0.1 M) due to hydrogen evolution competing with metal deposition
Temperature increase by 30°C typically reduces cell overpotential by 0.15–0.25 V, improving efficiency but accelerating corrosion kinetics
Always verify ionic strength and conductivity assumptions; high-chloride environments (>5000 ppm Cl⁻) invalidate neutral pH models