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Faraday’s Laws of Electrolysis

Faraday's Laws of Electrolysis

The laws, which govern the deposition of substances (In the form of ions) on electrodes during the process of electrolysis, is called Faraday's laws of electrolysis. These laws given by Michael Faraday in 1833.

(1) Faraday's first law: It states that,

“The mass of any substance deposited or liberated at any electrode is directly proportional to the quantity of electricity passed.”i.e.,

Where,

W = Mass of ions liberated in gm,

Quantity of electricity passed in Coulombs

= Current in Amperes (I) × Time in second (t)

In case current efficiency is given, then

where, constant, known as electrochemical equivalent (ECE) of the ion deposited.

When a current of 1 Ampere is passed for 1 second (i.e.,), then,

Thus, electrochemical equivalent (ECE) may be defined as “the mass of the ion deposited by passing a current of one Ampere for one second (i.e., by passing Coulomb of electricity)”. It's unit is gram per coulomb.

Coulomb is the unit of electrical charge.

96500Coulombs electrons = 1 mole electrons.

1 Coulomb electrons,

or 1 electronic charge Coulomb.

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