Copper Displaced by Iron

Fe + Cu2+ → Fe2+ + Cu

نظرة عامة

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.

المشاركون

الدور المادة المعامل الحالة
متفاعل Iron Fe 1 (s)
منتج Copper Cu 1 (s)

مثال من الحياة اليومية

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

الأهمية الصناعية

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

الخصائص

النوع
Redox
قابل للعكس
لا
الطاقة
طارد للحرارة
ΔH
-152,3 kJ/mol

التفاعلات ذات الصلة

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) Copper Oxidation by Nitric Acid Hypochlorite Oxidation of Hydrogen Peroxide Hydrogen Peroxide as Oxidizing Agent (Acidic) Hydrogen Peroxide Disproportionation 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.