Faradays law of electrolysis

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Faraday's law of electrolysis states that the amount of chemical change in an electrolytic cell is directly proportional to the amount of electricity that passes through it.

The law was discovered by Michael Faraday in 1834.
It is used to calculate the amount of substance produced or consumed during electrolysis.
The law is expressed as Q = It, where Q is the amount of substance produced or consumed, I is the current, and t is the time.
The law is applicable to both molten and aqueous electrolytes.
It is important in the production of metals such as aluminum and copper.
The law also helps in understanding the process of electroplating.
Faraday's constant is the amount of charge carried by one mole of electrons and is equal to 96,485.3329 coulombs per mole.

Faradays law of electrolysis

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