Faraday's laws of electrolysis

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Faraday's laws of electrolysis are quantitative relationships based on the electrochemical researches published by Michael Faraday in 1834.[1]

Mathematical form[edit]

Faraday's laws can be summarized by

where:

  • m is the mass of the substance liberated at an electrode in gms
  • Q is the total electric charge passed through the substance in coulombs
  • F = 96500 C mol−1 is the Faraday constant
  • M is the molar mass of the substance in grams per mol
  • z is the valency number of ions of the substance (electrons transferred per ion).

Note that M/z is the same as the equivalent weight of the substance altered.

For Faraday's first law, M, F, and z are constants, so that the larger the value of Q the larger m will be.

For Faraday's second law, Q, F, and z are constants, so that the larger the value of M/z (equivalent weight) the larger m will be.

In the simple case of constant-current electrolysis, leading to

and then to

where:

  • n is the amount of substance ("number of moles") liberated: n = m/M
  • t is the total time the constant current was applied.

In the more complicated case of a variable electric current, the total charge Q is the electric current I() integrated over time :

Here t is the total electrolysis time.[2]

See also[edit]

References[edit]

  1. ^ Ehl, Rosemary Gene; Ihde, Aaron (1954). "Faraday's Electrochemical Laws and the Determination of Equivalent Weights". Journal of Chemical Education. 31 (May): 226–232. Bibcode:1954JChEd..31..226E. doi:10.1021/ed031p226. 
  2. ^ For a similar treatment, see Strong, F. C. (1961). "Faraday's Laws in One Equation". Journal of Chemical Education. 38 (2): 98. Bibcode:1961JChEd..38...98S. doi:10.1021/ed038p98. 

Further reading[edit]

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