Faraday Constant

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Faraday constant

[′far·ə‚dā ‚kän·stənt]
(physics)

Faraday Constant

 

a fundamental physical constant equal to the product of Avogadro’s number NA and the charge of the electron e. The Faraday constant equals (9.648456 ± 0.000027) × 104 coulombs per mole. It is widely used in electrochemical calculations. The constant is named after M. Faraday, who discovered the fundamental laws of electrolysis.

References in periodicals archive ?
where N0 represents the number of cells in series, E0 is the voltage denoting the reaction free energy, R and F are the universal gas constant and Faraday's constant, respectively stands for temperature while the If0 denotes the current of the SOFC stack [P.
Table 1: SOFC Parameters Name Value Faraday's constant (F) 96484600 [C/kmol] Hydrosen valve constant 4.
where A is the equivalent gram of the substance affected by the electrochemical dissolution process, U--the voltage applied on the electrodes, [DELTA]U- the voltage necessary for the electrodes polarization, k--the electroyte electric conductivity, F--the Faraday's constant, and [[rho].
The value of Faraday's constant (96485 C/mol) is underestimated in the regression of [[summation of].
When the activities were considered instead of the concentrations (second column of Table 6), the regression coefficients became closer to the theoretical value of Faraday's constant (96485 C/mol), especially for the saturation soil extracts from Griffin and Jurinak (1973).
The overestimation of the Faraday's constant was consistent with the use of the Debye-Huckel equation and Davies' equation to predict the activity coefficients of the ions by the speciation program SOILSOLN.
Called the Faraday's constant, its numerical value, 96488 C (coulomb) is the product of Avogadro's number ([N.