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Encyclopedia > Faraday's law of electrolysis

Faraday studied the process of electrolysis in detail.On the basis of his research on electrolysis he published two laws of electrolysis that are commonly known as Faraday's law of electrolysis. Michael Faraday, FRS (September 22, 1791 – August 25, 1867) was an English chemist and physicist (or natural philosopher, in the terminology of that time) who contributed significantly to the fields of electromagnetism and electrochemistry. ... Process (lat. ... This article is about the chemical process. ... This article is about the chemical process. ... This article is about law in society. ... This article is about the chemical process. ...

Contents

Original form

Faraday's 1st Law of Electrolysis
The mass of a substance produced at an electrode during electrolysis is proportional to the number of moles of electrons (the quantity of electricity) transferred at that electrode.
Faraday's 2nd Law of Electrolysis
The number of Faradays of electric charge required to discharge one mole of substance at an electrode is equal to the number of "excess" elementary charges on that ion.

An electrode is an electrical conductor used to make contact with a metallic part of a circuit (e. ... This article is about the chemical process. ... The mole (symbol: mol) is the SI base unit that measures an amount of substance. ... e- redirects here. ... In physics the term quantity of electricity refers to the quantity of electric charge. ... I am the man. ...

Modern form

In modern form, Faraday's law states:

m = { Q over q n } cdot { M over N_A } = { 1 over q N_A } cdot { Q M over n } = { 1 over F } cdot { Q M over n } = { 1 over 96,485 mathrm{C} cdot mathrm{mol^{-1}} } cdot { Q M over n }

where

m is the mass of the substance produced at the electrode (in grams),
Q is the total electric charge that passed through the solution (in coulombs),
q is the electron charge = 1.602 x 10-19 coulombs per electron,
n is the valence number of the substance as an ion in solution (electrons per ion),
is Faraday's constant,
M is the molar mass of the substance (in grams per mole), and
NA is Avogadro's number = 6.022 x 1023 ions per mole.

In practice, the total charge Q is calculated by integrating the electric current I(t) over time t: For other meanings of gram, see gram (disambiguation). ... The coulomb (symbol: C) is the SI unit of electric charge. ... In physics and chemistry, the Faraday constant is the amount of electric charge in one mole of electrons. ... The mole (symbol: mol) is the SI base unit that measures an amount of substance. ... Avogadros number, also called Avogadros constant (NA), named after Amedeo Avogadro, is formally defined to be the number of carbon-12 atoms in 12 grams (0. ...

Q = int_0^T I(t) cdot dt

where T is the total amount of time of the electrolysis.


In the simple case of constant current electrolysis:

Q = I cdot t

Faraday's Electrolysis Limits Exceeded: lenr-canr.org/acrobat/MizunoTgeneration.pdf


References

  • Serway, Moses, and Moyer, Modern Physics, third edition (2005).

See also

v • d • e
Articles related to electrolysis

Principles of electrolysis • Electrochemical cell • Electrolytic process • Faraday's law of electrolysis • Half cell • High-temperature electrolysis • Standard electrode potential This article is about the chemical process. ... Michael Faraday, FRS (September 22, 1791 – August 25, 1867) was an English chemist and physicist (or natural philosopher, in the terminology of that time) who contributed significantly to the fields of electromagnetism and electrochemistry. ... I am the man. ... This article is about the chemical process. ... A demonstration electrochemical cell setup resembling the Daniell cell. ... It has been suggested that this article or section be merged into Electrolysis. ... A half cell is a structure that contains an electrode and a surrounding electrolyte. ... High-temperature electrolysis schema. ... It has been suggested that Electrode potential be merged into this article or section. ...


Electrolytic processes • Betts electrolytic process • Castner Process • Castner-Kellner process • Chloralkali process • Downs Cell • Electrolysis of water • Electrowinning • Hall-Héroult process • Hofmann voltameter • Kolbe electrolysis The Betts electrolytic process is an industrial process for separating lead and bismuth. ... The Castner process is a process for manufacturing sodium metal. ... The Castner-Kellner process is a method of electrolysis on an aqueous alkali chloride solution (usually sodium chloride solution) to produce the corresponding alkali hydroxide,[1] invented by Hamilton Castner and Karl Kellner in the 1890s. ... The chloralkali process is a redox reaction, an electrolysis of an aqueous solution of sodium chloride: 2 NaCl(aq) + 2 H2O(l) —→ 2 NaOH(aq) + Cl2(g) + 2 H+ + 2 e- 2 H+ + 2 e- —→ H2(g) The process is primarily used to produce chlorine, but one of its byproducts... The Downs process is a method for the commercial preparation of metallic sodium, in which molten NaCl is electrolyzed in a special apparatus called the Downs cell. ... Hoffman voltameter used to electrolyze water. ... This article needs to be cleaned up to conform to a higher standard of quality. ... The Hall-Héroult process is the major industrial process for the production of aluminium. ... Hofmann voltameter schema Figure of the apparatus from Hofmanns 1866 book. ... Kolbe electolysis or Kolbe reaction is a organic reaction named after Adolph Wilhelm Hermann Kolbe. ...


Materials produced by electrolysis • Aluminum • Calcium metal • Chlorine • Copper • Electrolyzed water • Fluorine • Hydrogen • Lithium metal • Magnesium • Potassium metal • Sodium metal • Sodium hydroxide • Zinc Aluminum is a soft and lightweight metal with a dull silvery appearance, due to a thin layer of oxidation that forms quickly when it is exposed to air. ... General Name, Symbol, Number calcium, Ca, 20 Chemical series alkaline earth metals Group, Period, Block 2, 4, s Appearance silvery white Standard atomic weight 40. ... General Name, Symbol, Number chlorine, Cl, 17 Chemical series halogens Group, Period, Block 17, 3, p Appearance yellowish green Standard atomic weight 35. ... Currently, the most common source of copper ore is the mineral chalcopyrite (CuFeS2), which accounts for about 50% of copper production. ... Alkaline Electrolyzed Water and Acidic Electrolyzed Water are produced by the electrolysis of ordinary tap water in the presence of a specific amount of salt, generally sodium chloride. ... General Name, Symbol, Number fluorine, F, 9 Chemical series halogens Group, Period, Block 17, 2, p Appearance Yellowish brown gas Atomic mass 18. ... General Name, Symbol, Number hydrogen, H, 1 Chemical series nonmetals Group, Period, Block 1, 1, s Appearance colorless Atomic mass 1. ... General Name, Symbol, Number lithium, Li, 3 Chemical series alkali metals Group, Period, Block 1, 2, s Appearance silvery white/grey Standard atomic weight 6. ... General Name, Symbol, Number magnesium, Mg, 12 Chemical series alkaline earth metals Group, Period, Block 2, 3, s Appearance silvery white solid at room temp Standard atomic weight 24. ... General Name, Symbol, Number potassium, K, 19 Chemical series alkali metals Group, Period, Block 1, 4, s Appearance silvery white Standard atomic weight 39. ... General Name, Symbol, Number sodium, Na, 11 Chemical series alkali metals Group, Period, Block 1, 3, s Appearance silvery white Standard atomic weight 22. ... Sodium hydroxide (NaOH), also known as lye or caustic soda or sodium hydrate, is a caustic metallic base. ... General Name, Symbol, Number zinc, Zn, 30 Chemical series transition metals Group, Period, Block 12, 4, d Appearance bluish pale gray Standard atomic weight 65. ...


See also • Electrochemistry • Standard electrode potential (data page) English chemists John Daniell (left) and Michael Faraday (right), both credited to be founders of electrochemistry as known today. ... The standard electrode potentials are used to determine the electrochemical potential or the electrode potential of an electrochemical cell or Galvanic cell. ...


  Results from FactBites:
 
Faradays Law: Free Encyclopedia Articles at Questia.com Online Library (1279 words)
physical law stating that the number of moles of substance produced at an electrode during electrolysis is directly proportional to the number of moles of electrons transferred at that electrode; the law is named for Michael Faraday, who formulated it in 1834.
It is the second law of thermodynamics that holds dominion over...organization of the universe, and what the law has to say we find verified by ordinary...
FARADAYS LAW physical law stating that the number...electrons transferred at that electrode; the law is named for Michael Faraday, who formulated...equal to 96,500 coulombs.
  More results at FactBites »


 

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