Copper Displaced by Iron

Fe + Cu2+ → Fe2+ + Cu

Overview

Iron reduces copper(II) ions to metallic copper while being oxidized to iron(II). This reaction proceeds because iron has a more negative standard reduction potential (-0.44 V) than copper (+0.34 V), making it a stronger reducing agent. The net cell potential is +0.78 V.

Participants

Role Substance Coefficient State
Reactant Iron Fe 1 (s)
Product Copper Cu 1 (s)

Everyday Example

Inserting an iron nail into blue copper sulfate solution shows copper plating on the nail as the solution loses its blue color.

Industrial Importance

Iron cementation of copper from mine waters is a cost-effective copper recovery method. Understanding electrode potentials is fundamental to electrochemistry.

Properties

Type
Redox
Reversible
No
Energy
Exothermic
ΔH
-152.3 kJ/mol

Related Reactions

Aqua Regia Dissolving Gold Bleaching with Sodium Hypochlorite Cerium(IV) Reduction by Iron(II) Chlorine Oxidation of Bromide Chromate-Dichromate Equilibrium Contact Process SO₂ Oxidation Copper Oxidation by Nitric Acid Copper Patina Formation (Verdigris) Copper Reduction of Silver Ion Dichromate Oxidation of Ethanol

Frequently Asked Questions

What is the equation for Copper Displaced by Iron?
The balanced equation is: Fe + Cu²⁺ → Fe²⁺ + Cu.
What type of reaction is Copper Displaced by Iron?
Copper Displaced by Iron is a redox reaction.
Is Copper Displaced by Iron exothermic or endothermic?
Copper Displaced by Iron is exothermic (releases energy). The enthalpy change (ΔH) is -152.3 kJ/mol.