Electrolytic cell
Electrolytic Cell
An Electrolytic Cell (pronounced: e-lek-tro-lit-ik sel) is a type of cell that uses electricity to drive a non-spontaneous chemical reaction. This term originates from the Greek words "ηλεκτρον" (electron) meaning amber, from which electricity was first known, and "λυτικός" (lytikos) meaning able to loosen or dissolve.
Structure
An Electrolytic Cell consists of two electrodes: an anode and a cathode, and an electrolyte. The anode is the electrode where oxidation occurs, and the cathode is the electrode where reduction occurs. The electrolyte is often a solution of water and salt, which allows the flow of ions.
Function
In an Electrolytic Cell, an external source of voltage is used to create an electric current which passes through the electrolyte. This current causes the ions in the electrolyte to move towards the electrodes, where they either gain or lose electrons, resulting in a chemical reaction.
Applications
Electrolytic Cells are used in various applications such as electroplating, electrorefining, and the production of certain chemicals like chlorine and sodium hydroxide.
Related Terms
- Galvanic cell: A type of cell that generates an electric current from a spontaneous chemical reaction.
- Electrolysis: The process of causing a chemical reaction to occur in an electrolytic cell.
- Faraday's laws of electrolysis: Two scientific laws that quantify electrolysis.
See Also
External links
- Medical encyclopedia article on Electrolytic cell
- Wikipedia's article - Electrolytic cell
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