Galvanoplastie au Cuivre

Dépôt d'une fine couche de cuivre sur un objet métallique

Electrochemistry Intermediate (High School) 60 min ~$15,00

Objectif

Galvaniser une clé ou une pièce métallique avec du cuivre, démontrant le procédé industriel d'électrodéposition et les lois de Faraday.

Contexte

Electroplating uses electrolysis to deposit a thin layer of metal onto a conductive surface. The object to be plated is made the cathode, and the plating metal (copper) is the anode. Copper ions from the solution are reduced and deposited on the cathode surface.

Avertissements de sécurité

  • Copper sulfate solution is toxic
  • Dilute sulfuric acid is corrosive
  • Wear gloves and goggles
  • Handle electrical connections with care

EPI requis

goggles gloves lab_coat

Matériaux

  • Copper(II) sulfate (CuSO₄) (200 mL)
    1M solution
  • Sulfuric acid (H₂SO₄) (10 mL)
    Dilute, to improve conductivity
  • Copper strip or sheet (1 piece)
    Anode
  • Metal key or coin (1)
    Object to plate (cathode)
  • Acetone or alcohol (20 mL)
    For cleaning the object

Équipement

DC power supply (3-6V) Beaker (400 mL) Wires with alligator clips Sandpaper Analytical balance

Procédure

1

Clean the object (key/coin) by sanding lightly and degreasing with acetone. A clean surface is critical for good plating.

5 min Acetone is flammable
2

Weigh the clean object on the analytical balance and record the mass.

2 min
3

Prepare the plating solution: 200 mL of 1M CuSO₄ with 5 mL of dilute H₂SO₄.

3 min Wear gloves
4

Suspend the copper strip (anode) and the object (cathode) in the solution, connected to the power supply.

5 min
5

Set the power supply to 3V and turn it on. Observe the copper being deposited on the cathode.

2 min
6

Allow plating to continue for 30 minutes. Periodically check that gas bubbles are minimal (indicates correct voltage).

30 min
7

Turn off the power supply. Remove the plated object, rinse with water, and dry gently.

3 min
8

Weigh the plated object. Calculate the mass of copper deposited and compare with Faraday's law prediction.

5 min

Résultats attendus

A smooth, shiny copper coating should cover the object. The mass increase should correlate with Faraday's law: m = (M x I x t) / (n x F), where M is molar mass of Cu, I is current, t is time, n=2, and F is Faraday's constant.

Nettoyage

Dispose of copper sulfate solution in heavy metal waste. Rinse all equipment. Clean the copper anode for reuse.

Détails

Catégorie
Electrochemistry
Difficulté
Intermediate (High School)
Durée
60 min
Coût estimé
$15,00
Étapes
8
Matériaux
5

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Frequently Asked Questions

What is the objective of Galvanoplastie au Cuivre?
Galvaniser une clé ou une pièce métallique avec du cuivre, démontrant le procédé industriel d'électrodéposition et les lois de Faraday.
How difficult is Galvanoplastie au Cuivre?
This experiment is rated as Intermediate (High School). It takes approximately 60 minutes to complete.
What safety precautions are needed for Galvanoplastie au Cuivre?
Key safety precautions include: Copper sulfate solution is toxic; Dilute sulfuric acid is corrosive; Wear gloves and goggles.
What materials are needed for Galvanoplastie au Cuivre?
The main materials required are: Copper(II) sulfate (CuSO₄), Sulfuric acid (H₂SO₄), Copper strip or sheet, Metal key or coin, Acetone or alcohol.
What results should I expect from Galvanoplastie au Cuivre?
A smooth, shiny copper coating should cover the object. The mass increase should correlate with Faraday's law: m = (M x I x t) / (n x F), where M is molar mass of Cu, I is current, t is time, n=2, and F is Faraday's constant.