Copper Displaced by Iron

Fe + Cu2+ → Fe2+ + Cu

Descripción general

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.

Participantes

Rol Sustancia Coeficiente Estado
Reactivo Iron Fe 1 (s)
Producto Copper Cu 1 (s)

Ejemplo cotidiano

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

Importancia industrial

La cementación con hierro del cobre a partir de aguas de minas es un método rentable de recuperación de cobre. Comprender los potenciales de electrodo es fundamental para la electroquímica.

Propiedades

Tipo
Redox
Reversible
No
Energía
Exotérmico
ΔH
-152,3 kJ/mol

Reacciones relacionadas

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.