Operating Principle

Electrolysis process involves the use of water with a conductivity greater than 2 MΩ·cm introduced into the anode chamber of an electrolytic cell. Once electrical current is applied, water immediately undergoes decomposition at the anode according to the reaction: H2O = H⁺ + OH⁻. The hydroxide ions (OH⁻) generated at the anode release electrons, leading to the formation of oxygen gas (O2), which is then expelled from the anode chamber, carrying some water into the water tank for recirculation. Oxygen exits through a small hole at the upper part of the water tank.

Meanwhile, protons (H⁺) exist as hydrated ions (H⁺·XH2O) and, under the influence of the electric field, migrate through a solid polymer electrolyte (SPE) membrane to the cathode, where they absorb electrons to form hydrogen gas (H2). After leaving the cathode chamber, the water enters a gas-water separator, where the majority of the excess water is removed, allowing hydrogen gas with trace amounts of moisture to exit through the hydrogen outlet.