Electrolytic Cell and Electrolysis
Electrolysis is a technique that uses an electric current to drive a chemical reaction that would otherwise not occur. Electrolytic cells are electrochemical cells that use an external source of electrical energy to force a chemical reaction.
The voltage needed for electrolysis to occur is called the decomposition potential. The solutions in electrolytic cells are usually either molten salt or aqueous.
Let’s consider an example of electrolysis of brine solution. In brine solution, the electrolyte is NaCl solution. When electric current is passed, NaCl breaks down into Na+ and Cl– ion. The sodium ion moves to cathode and get deposited as metal ion while Cl– get moves to anode and get deposited as element. The reaction for the process is given below:
Reaction at Cathode: [Na+ + e– → Na] × 2 where, E° = –2.71 V
Reaction at Anode: 2Cl– → Cl2 + 2e– where, E° = –1.36 V
Cell Reaction: 2NaCl → 2Na + Cl2 where, E° = –4.1 V
Electrolysis is used in many industrial processes, including:
- Refining metals.
- Producing inorganic and organic products.
- Producing chlorine and caustic soda.
- Refining aluminum.
Electrolytic Cell – Definition, Diagram, Working, Applications
An electrolytic cell is a electrochemical cell in which electrical energy is used to carry out chemical reaction in the cell. The chemical reaction happening inside an electrolytic cell is a redox reaction, which is spontaneous in nature. This whole process of carrying out chemical reactions with the help of electric current is called electrolysis.
In this article, we will learn in detail about electrolytic cell, its component, diagram and working. We will also learn difference between electrolytic cell and galvanic cell.
Table of Content
- What is an Electrolytic Cell?
- Working of Electrolytic Cell
- Electrolytic Cell and Electrolysis
- Difference Between Galvanic Cells and Electrolytic Cells
- Applications of Electrolytic Cells
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