Daniell Cell (Zinc-Copper Galvanic Cell)

Zn + Cu2+ → Zn2+ + Cu

Overview

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.

Participants

Role Substance Coefficient State
Reactant Zinc Zn 1 (s)
Product Copper Cu 1 (s)

Everyday Example

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

Industrial Importance

While superseded by modern batteries, the Daniell cell remains the textbook example for teaching electrochemistry and electrode potentials.

Properties

Type
Electrochemical
Reversible
Yes
Energy
Exothermic
ΔH
-210.0 kJ/mol

Related Reactions

Alkaline Battery Discharge Anodizing of Aluminum Cathodic Protection (Zinc Sacrificial Anode) Chlor-Alkali Electrolysis Chrome Electroplating Copper Electroplating Electrochemical CO₂ Reduction to CO Electrochemical Machining (ECM) Electrolysis of Molten NaCl (Downs Process) Electrolysis of Water

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.