Faraday's Laws of Electrolysis

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Faraday's laws of electrolysis

[′far·ə‚dāz ¦lȯz əv i‚lek′träl·ə·səs]
(physical chemistry)
The amount of any substance dissolved or deposited in electrolysis is proportional to the total electric charge passed.
The amounts of different substances dissolved or desposited by the passage of the same electric charge are proportional to their equivalent weights.
McGraw-Hill Dictionary of Scientific & Technical Terms, 6E, Copyright © 2003 by The McGraw-Hill Companies, Inc.
The following article is from The Great Soviet Encyclopedia (1979). It might be outdated or ideologically biased.

Faraday’s Laws of Electrolysis


the quantitative laws of electrolysis that were discovered by M. Faraday in 1833–34. Faraday’s laws express the relationship between the quantity of electricity passed through an electrolyte and the mass and chemical nature, in terms of chemical equivalents, of substances deposited or dissolved at the electrodes.

Faraday’s first law of electrolysis states that the masses m of deposited or dissolved substances are proportional to the quantity of electricity q passed through the electrolyte. The second law states that the masses of different substances deposited or dissolved as a result of the passage of the same quantity of electricity through the electrolyte are proportional to the chemical equivalents A of the substances. It follows from the second law that the same quantity of electricity, called the Faraday constant F, is required for the deposition of the same gram-equivalent weight of different substances. Mathematically, Faraday’s laws may be written as one equation m = (A/F)q = kq, where the coefficient k = A/F is called the electrochemical equivalent.

Both of Faraday’s laws are exact if the ions of the electrolyte carry all the electricity passed through the electrolyte. Deviations from the laws are observed in certain cases; such deviations may be associated with electrochemical side reactions that are not taken into account—for example, the liberation of gaseous hydrogen during the electrodeposition of some metals—or with partial electron conduction—for example, during the electrolysis of certain alloys.


Faraday, M. Eksperimental’nye issledovaniia po eleklricheslvu, vol. 1. [Moscow] 1947. Pages 176–226 and 265–346. (Translated from English.)


The Great Soviet Encyclopedia, 3rd Edition (1970-1979). © 2010 The Gale Group, Inc. All rights reserved.
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[21] has applied the Nernst equation, mass balance equation of redox reaction and Faraday's law of electrolysis to establish the relationship between the half-cell redox concentration of Ce(IV)/Ce(III) and the ORP during electrolysis.
The concentration parameters of the species, [C.sub.red] and [C.sub.oxd], can be determined using Faraday's law of electrolysis. The law describes the amount of substance undergoing an electrochemical change in a constant volume reaction [21].
This is in agreement with Faraday's law of electrolysis. The longer the deposition time, the higher the quantity of electricity passed, and the thicker the polymer film deposited.