Chlor-Alkali Electrolysis

2NaCl + 2H2O → Cl2 + 2NaOH + H2

Descripción general

Electrolysis of concentrated brine (NaCl solution) produces three essential industrial chemicals simultaneously: chlorine gas at the anode, sodium hydroxide solution at the cathode, and hydrogen gas as a byproduct. Modern membrane cells use ion-exchange membranes to separate products and achieve 95%+ current efficiency.

Participantes

Rol Sustancia Coeficiente Estado
Reactivo Sodium Chloride NaCl 2 (aq)
Reactivo Water H₂O 2 (l)
Producto Sodium Hydroxide NaOH 2 (aq)

Ejemplo cotidiano

The chlorine in your tap water and the lye in drain cleaner both come from this single electrochemical process.

Importancia industrial

La industria cloro-álcali produce aproximadamente 75 millones de toneladas de NaOH y 65 millones de toneladas de Cl₂ al año, consumiendo alrededor del 1 % de la electricidad mundial.

Propiedades

Tipo
Electrochemical
Reversible
No
Energía
Endotérmico
ΔH
422,0 kJ/mol

Reacciones relacionadas

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

Frequently Asked Questions

What is the equation for Chlor-Alkali Electrolysis?
The balanced equation is: 2NaCl + 2H₂O → Cl₂ + 2NaOH + H₂.
What type of reaction is Chlor-Alkali Electrolysis?
Chlor-Alkali Electrolysis is a electrochemical reaction.
Is Chlor-Alkali Electrolysis exothermic or endothermic?
Chlor-Alkali Electrolysis is endothermic (absorbs energy). The enthalpy change (ΔH) is 422.0 kJ/mol.