Daniell Cell (Zinc-Copper Galvanic Cell)

Zn + Cu2+ → Zn2+ + Cu

Übersicht

The Daniell cell consists of a zinc anode in ZnSO₄ solution and a copper cathode in CuSO₄ solution, connected by a salt bridge. Zinc is oxidized (E° = -0.76 V) and copper ions are reduced (E° = +0.34 V), giving a cell potential of 1.10 V. Invented by John Frederic Daniell in 1836, it was the first reliable source of electricity.

Teilnehmer

Rolle Substanz Koeffizient Zustand
Reaktant Zinc Zn 1 (s)
Produkt Copper Cu 1 (s)

Alltägliches Beispiel

The Daniell cell powered early telegraph networks across America and Europe, enabling rapid long-distance communication.

Industrielle Bedeutung

While superseded by modern batteries, the Daniell cell remains the textbook example for teaching electrochemistry and electrode potentials.

Eigenschaften

Typ
Electrochemical
Reversibel
Ja
Energie
Exotherm
ΔH
-210,0 kJ/mol

Verwandte Reaktionen

Electrolysis of Water 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 Electrochemical CO₂ Reduction to CO

Frequently Asked Questions

What is the equation for Daniell Cell (Zinc-Copper Galvanic Cell)?
The balanced equation is: Zn + Cu²⁺ → Zn²⁺ + Cu.
What type of reaction is Daniell Cell (Zinc-Copper Galvanic Cell)?
Daniell Cell (Zinc-Copper Galvanic Cell) is a electrochemical reaction. It is reversible under certain conditions.
Is Daniell Cell (Zinc-Copper Galvanic Cell) exothermic or endothermic?
Daniell Cell (Zinc-Copper Galvanic Cell) is exothermic (releases energy). The enthalpy change (ΔH) is -210.0 kJ/mol.