Electrolysis — Faraday's Laws & Electrode Reactions

Visualise DC-driven decomposition of water and electrolyte solutions. Adjust voltage, concentration, and electrode material to explore bubble formation, current, and Faraday yield.

Electrolytic cell cross-section — cathode (left) and anode (right)

Controls

Water electrolysis: Cathode: 2H₂O + 2e⁻ → H₂↑ + 2OH⁻ | Anode: 2H₂O → O₂↑ + 4H⁺ + 4e⁻

Applied voltage V (V) 6.0

Concentration c (mol/L) 1.00

Electrode area A (cm²) 20

Time elapsed t (s) 300

Faraday Analysis

Current I (A)— Charge Q (C)— H₂ produced (mg)— O₂ produced (mg)— H₂ volume (mL)— O₂ volume (mL)— Cathode reaction2H₂O→H₂ Anode reaction2H₂O→O₂ Faradaic eff. η— Cell overpotential—

Faraday's Laws

First Law: m = MIt/nF — mass deposited proportional to charge passed.

Second Law: Equivalent masses are deposited by the same charge. F = 96485 C/mol.

Minimum voltage: Water: E° = 1.23 V. In practice 1.5–2.0 V due to overpotential (η_a + η_c + iR).