Electrolytic Production of Chlorate

NaCl + 3H2O → NaClO3 + 3H2

Übersicht

Electrolysis of hot NaCl solution without a membrane allows chlorine produced at the anode to react with hydroxide from the cathode, forming hypochlorite that disproportionates to chlorate at 70–80°C. Sodium chlorate (NaClO₃) is the precursor to chlorine dioxide (ClO₂), the dominant bleaching agent in modern paper mills.

Teilnehmer

Rolle Substanz Koeffizient Zustand
Reaktant Sodium Chloride NaCl 1 (aq)
Reaktant Water H₂O 3 (l)

Alltägliches Beispiel

The white paper in your books and notebooks was bleached using chlorine dioxide derived from electrolytically produced sodium chlorate.

Industrielle Bedeutung

About 3.6 million tonnes of sodium chlorate are produced annually, primarily for pulp bleaching, herbicides, and water treatment.

Eigenschaften

Typ
Electrochemical
Reversibel
Nein
Energie
Endotherm
ΔH
590,0 kJ/mol

Verwandte Reaktionen

Electrolysis of Water 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 Electrolytic Production of Chlorate?
The balanced equation is: NaCl + 3H₂O → NaClO₃ + 3H₂.
What type of reaction is Electrolytic Production of Chlorate?
Electrolytic Production of Chlorate is a electrochemical reaction.
Is Electrolytic Production of Chlorate exothermic or endothermic?
Electrolytic Production of Chlorate is endothermic (absorbs energy). The enthalpy change (ΔH) is 590.0 kJ/mol.