Copper Oxidation by Nitric Acid

3Cu + 8HNO3(dilute) → 3Cu(NO3)2 + 2NO + 4H2O

Descripción general

Dilute nitric acid oxidizes copper to Cu²⁺ while the nitrate ion is reduced to nitric oxide (NO) gas. Unlike HCl or H₂SO₄(dilute), nitric acid can dissolve copper because the nitrate ion acts as the oxidizing agent. The solution turns blue from Cu(NO₃)₂ and the NO gas oxidizes in air to brown NO₂.

Participantes

Rol Sustancia Coeficiente Estado
Reactivo Copper Cu 3 (s)
Reactivo Nitric Acid HNO₃ 8 (aq)
Producto Water H₂O 4 (l)

Ejemplo cotidiano

Chemistry students observe this reaction as a dramatic demonstration where copper dissolves in HNO₃ with brown fumes forming above the solution.

Importancia industrial

La disolución del cobre en ácido nítrico se utiliza en química analítica, en el grabado del cobre para la fabricación de placas de circuito impreso y en la refinación de metales.

Propiedades

Tipo
Redox
Reversible
No
Energía
Exotérmico
ΔH
-135,0 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 Hypochlorite Oxidation of Hydrogen Peroxide Hydrogen Peroxide as Oxidizing Agent (Acidic) Zinc Reduction of Silver Ion Displacement of Hydrogen from Acid by Magnesium

Frequently Asked Questions

What is the equation for Copper Oxidation by Nitric Acid?
The balanced equation is: 3Cu + 8HNO₃(dilute) → 3Cu(NO₃)₂ + 2NO + 4H₂O.
What type of reaction is Copper Oxidation by Nitric Acid?
Copper Oxidation by Nitric Acid is a redox reaction.
Is Copper Oxidation by Nitric Acid exothermic or endothermic?
Copper Oxidation by Nitric Acid is exothermic (releases energy). The enthalpy change (ΔH) is -135.0 kJ/mol.