Process of Electrolysis

What is Chemical Equation?

A chemical equation is the symbolic representation of a chemical reaction in the form of symbols and formulae.

For example, the redox reaction involved in the electrolysis of CuSO4 involves the oxidation of Cu at the anode and the reduction of Cu2+ at the cathode.

• Anode Half Reaction: Cu(s)  ? Cu²⁺ (aq) + 2e^–
• Cathode Half Reaction: Cu²⁺(aq) + 2e^–  ? Cu(s) 

Let us study the electrolysis of CuSO₄ through a simulation. 

This experiment aims to study the process of electrolysis. 

The apparatus and chemicals required for this experiment are: 

Apparatus Required

• Glass rod
• Battery of 3V 
• Key
• Beaker
• Wooden block with two holes
• Connecting wires
• Piece of sandpaper

Chemicals Required

• Impure thick copper metal rod, 
• Thin pure copper metal rod
• 3 g of copper sulphate crystals
• Distilled water
• Dil. sulphuric acid

Procedure

The procedure to be followed is as follows: 

1. Add around 150mL of water to the 250mL beaker.
2. Add pure copper sulphate crystals and a few drops of dil. sulphuric acid to the water.
3. Stir the reaction mixture using a glass rod.
4. Now cover this beaker with a cardboard or wooden block with two holes well separated from each other so that it is possible to dip the copper metal strips through them.
5. Now make sure the ends of the wires are cleaned with sandpaper and connect the impure thick copper metal strip and pure thin copper metal strip with the wire through a battery and a plug. (Do not plug the key yet).
6. Now dip the copper metal strips in the beaker containing copper sulphate solution through the cardboard or wooden block holes.
7. Insert the key into the plug and allow the current to flow until you can see the change in the thickness of the electrodes. 

Hence, we can conclude that: 

In the electrolysis process, copper ions are released from the impure copper strip (positive electrode) and move through the solution in the electrolytic cell towards the pure copper strip (negative electrode), where they get discharged and deposited. Due to this movement of copper ions, the thickness of the impure copper strip keeps decreasing, and the thickness of the pure copper strip keeps increasing on passing the current through the electrolyte.

FAQs on Electrolysis Process