Electrolysis of Water

2H2O → 2H2 + O2

Übersicht

An electric current passed through water splits it into hydrogen gas at the cathode and oxygen gas at the anode. The minimum voltage required is 1.23 V (thermodynamic), but practical electrolyzers operate at 1.8–2.0 V due to overpotential. A small amount of electrolyte (acid, base, or salt) is needed to make water conductive.

Teilnehmer

Rolle Substanz Koeffizient Zustand
Reaktant Water H₂O 2 (l)

Alltägliches Beispiel

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

Industrielle Bedeutung

Water electrolysis produces about 4% of the world's hydrogen. Green hydrogen from electrolysis is projected to reach $1.5/kg by 2030.

Eigenschaften

Typ
Electrochemical
Reversibel
Ja
Energie
Endotherm
ΔH
572,0 kJ/mol

Verwandte Reaktionen

Electrolytic Production of Chlorate Electrorefining of Copper Alkaline Battery Discharge Anodizing of Aluminum Cathodic Protection (Zinc Sacrificial Anode) Chlor-Alkali Electrolysis Chrome Electroplating Nickel-Metal Hydride Battery Sodium-Sulfur Battery Electrochemical CO₂ Reduction to CO

Frequently Asked Questions

What is the equation for Electrolysis of Water?
The balanced equation is: 2H₂O → 2H₂ + O₂.
What type of reaction is Electrolysis of Water?
Electrolysis of Water is a electrochemical reaction. It is reversible under certain conditions.
Is Electrolysis of Water exothermic or endothermic?
Electrolysis of Water is endothermic (absorbs energy). The enthalpy change (ΔH) is 572.0 kJ/mol.