Copper Displaced by Iron

Fe + Cu2+ → Fe2+ + Cu

Aperçu

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

Rôle Substance Coefficient État
Réactif Iron Fe 1 (s)
Produit Copper Cu 1 (s)

Exemple du quotidien

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

Importance industrielle

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

Propriétés

Type
Redox
Réversible
Non
Énergie
Exothermique
ΔH
-152,3 kJ/mol

Réactions associées

Iron(II) to Iron(III) Oxidation by Oxygen Bleaching with Sodium Hypochlorite Copper Reduction of Silver Ion Aqua Regia Dissolving Gold Cerium(IV) Reduction by Iron(II) Chlorine Oxidation of Bromide Copper Oxidation by Nitric Acid Hypochlorite Oxidation of Hydrogen Peroxide Hydrogen Peroxide as Oxidizing Agent (Acidic) Displacement of Hydrogen from Acid by Magnesium

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.