Faraday's Law of Electrolysis is a basic law of electromagnetism that explains the relationship between the amount of electricity passed through an electrolytic cell and the amount of chemical reaction that takes place.
Michael Faraday, a British scientist, discovered Faraday's Law of Electrolysis in the early 19th century through his experiments with electrical currents and electrolytic cells.
An electrolytic cell is a device that uses electricity to cause a chemical reaction. It consists of two electrodes (an anode and a cathode) and an electrolyte solution. When an electric current is passed through the cell, the electrolyte solution is decomposed, and a chemical reaction occurs at the electrodes.
Faraday's Law of Electrolysis is expressed as Q = I x t, where Q is the amount of electric charge passed through the electrolytic cell, I is the current in amperes, and t is the time in seconds. This equation shows that the amount of chemical reaction that takes place is directly proportional to the amount of electricity passed through the cell.
Faraday's Law of Electrolysis has many practical applications, including electroplating, metal refining, and the production of various chemicals. It is also used in batteries, fuel cells, and other electrochemical devices.