Decomposition of Water (Electrolysis)

2H2O → 2H2 + O2

Übersicht

Water decomposes into hydrogen and oxygen gases when an electric current is passed through it. This electrolysis reaction is the reverse of the synthesis of water. It requires a minimum voltage of 1.23 V at standard conditions, though practical electrolyzers use higher voltages.

Teilnehmer

Rolle Substanz Koeffizient Zustand
Reaktant Water H₂O 2 (l)
Produkt Oxygen O 1 (g)
Produkt Hydrogen H 2 (g)

Alltägliches Beispiel

Green hydrogen production uses renewable electricity to split water, producing clean hydrogen fuel for vehicles and industry.

Industrielle Bedeutung

Water electrolysis is central to the green hydrogen economy, producing hydrogen for fuel cells, ammonia synthesis, and steel production without carbon emissions.

Eigenschaften

Typ
Decomposition
Reversibel
Ja
Energie
Endotherm
ΔH
571,6 kJ/mol

Verwandte Reaktionen

Decomposition of Ammonium Nitrate Decomposition of Calcium Hypochlorite Decomposition of Carbonic Acid Decomposition of Iron(II,III) Oxide (Direct Reduction) Decomposition of Nitrous Oxide (Laughing Gas) Decomposition of Barium Peroxide Decomposition of Sodium Bicarbonate Thermal Decomposition of Copper(II) Carbonate Thermal Decomposition of Mercury(II) Oxide Cracking of Octane (Thermal Cracking)

Frequently Asked Questions

What is the equation for Decomposition of Water (Electrolysis)?
The balanced equation is: 2H₂O → 2H₂ + O₂.
What type of reaction is Decomposition of Water (Electrolysis)?
Decomposition of Water (Electrolysis) is a decomposition reaction. It is reversible under certain conditions.
Is Decomposition of Water (Electrolysis) exothermic or endothermic?
Decomposition of Water (Electrolysis) is endothermic (absorbs energy). The enthalpy change (ΔH) is 571.6 kJ/mol.