Working of Electrolytic Cell
In an electrolytic cell, two electrodes are dipped into an electrolyte. When electric current is supplied to the electrolytic cell, the electrolyte breaks down into its constituent cations and anions. Now cations being positive in nature get attracted to negative diode which is cathode. The anion of the electrolyte being negative in nature get attracted to the anode which is a positive diode.
In this process, the anion at anode get lose its electron and get deposited as element. This process is called oxidation. Hence, in electrolytic cell oxidation occurs at anode.
The cation at cathode gains the electron and get deposited as metal. This process is called reduction. Hence, in electrolytic cell reduction occur at cathode.
This complete process is called electrolysis which is discussed below:
Reaction at Cathode: [Na+ + e– → Na] × 2
Reaction at Anode: 2Cl– → Cl2 + 2e–
Cell Reaction: 2NaCl → 2Na + Cl2
Thus, molten sodium chloride when subjected to electric current in an electrolytic cell to generate metallic sodium and chlorine gas as the products.
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