The Chemistry of HHO: Electrolysis, Faraday Laws, and Brown's Gas

Water Electrolysis Chemistry

When direct current passes through water containing an electrolyte, oxidation occurs at the anode (positive) and reduction at the cathode (negative). At the anode: 2H₂O → O₂ + 4H⁺ + 4e⁻. At the cathode: 4H⁺ + 4e⁻ → 2H₂. Net: 2H₂O → 2H₂ + O₂.

Faraday's Laws Applied

First Law: mass of substance produced is proportional to the total electric charge. Second Law: mass produced by the same charge is proportional to the substance's equivalent weight. For hydrogen: 96,485 coulombs (1 Faraday) produces 1.008 grams of H₂. At 10A continuous, you produce approximately 0.37 liters/minute of H₂ and 0.18 liters/minute of O₂ — 0.55 LPM total HHO under ideal conditions.

Overpotential Reality

The theoretical minimum voltage for water electrolysis is 1.23V per cell. In practice, overpotential at the electrode surfaces requires 1.8–2.2V for practical rates. This overpotential manifests as heat — the primary efficiency loss in any electrolyzer.

Brown's Gas Claims

Yull Brown claimed his gas had anomalous properties including imploding rather than exploding and achieving temperatures beyond conventional oxyhydrogen. Mainstream chemistry explains these observations as artifacts of the 2:1 H₂:O₂ ratio creating complete combustion with no excess reactant. The "implosion" is simply rapid recombination back to water with net volume reduction.