Diffusion layer: Difference between revisions
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In [[electrochemistry]], the '''diffusion layer''', according to [[IUPAC]], is defined as the "region in the vicinity of an electrode where the concentrations are different from their value in the bulk solution. The definition of the thickness of the diffusion layer is arbitrary because the concentration approaches asymptotically the value in the bulk solution".<ref>{{GoldBookRef | file = D01725 | title = diffusion layer (concentration boundary layer)}}</ref> The diffusion layer thus depends on the [[diffusion coefficient]] (D) of the analyte and for voltammetric measurements on the scan rate (V/s). It is usually considered to be some multiple of (Dt)<sup>1/2</sup> (where 1/t = scan rate). At slow scan rates, the diffusion layer is large, on the order of [[micrometre|micrometers]], whereas at fast scan rates the diffusion layer is nanometers in thickness. The relationship is described in part by the [[Cottrell equation]].<ref>Bard, A. J.; Faulkner, L. R. “Electrochemical Methods. Fundamentals and Applications” 2nd Ed. Wiley, New York. 2001. ISBN 0-471-04372-9</ref> |
In [[electrochemistry]], the '''diffusion layer''', according to [[IUPAC]], is defined as the "region in the vicinity of an electrode where the concentrations are different from their value in the bulk solution. The definition of the thickness of the diffusion layer is arbitrary because the concentration approaches [[asymptotically]] the value in the bulk solution".<ref>{{GoldBookRef | file = D01725 | title = diffusion layer (concentration boundary layer)}}</ref> The diffusion layer thus depends on the [[diffusion coefficient]] (D) of the analyte and for voltammetric measurements on the scan rate (V/s). It is usually considered to be some multiple of (Dt)<sup>1/2</sup> (where 1/t = scan rate). At slow scan rates, the diffusion layer is large, on the order of [[micrometre|micrometers]], whereas at fast scan rates the diffusion layer is nanometers in thickness. The relationship is described in part by the [[Cottrell equation]].<ref>Bard, A. J.; Faulkner, L. R. “Electrochemical Methods. Fundamentals and Applications” 2nd Ed. Wiley, New York. 2001. ISBN 0-471-04372-9</ref> |
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Relevant to [[cyclic voltammetry]], the diffusion layer has negligible volume compared the volume of the bulk solution. For this reason, cyclic voltammetry experiments have an inexhaustible supply of fresh analyte. |
Relevant to [[cyclic voltammetry]], the diffusion layer has negligible volume compared the volume of the bulk solution. For this reason, cyclic voltammetry experiments have an inexhaustible supply of fresh analyte. |
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Revision as of 11:04, 1 November 2016
In electrochemistry, the diffusion layer, according to IUPAC, is defined as the "region in the vicinity of an electrode where the concentrations are different from their value in the bulk solution. The definition of the thickness of the diffusion layer is arbitrary because the concentration approaches asymptotically the value in the bulk solution".[1] The diffusion layer thus depends on the diffusion coefficient (D) of the analyte and for voltammetric measurements on the scan rate (V/s). It is usually considered to be some multiple of (Dt)1/2 (where 1/t = scan rate). At slow scan rates, the diffusion layer is large, on the order of micrometers, whereas at fast scan rates the diffusion layer is nanometers in thickness. The relationship is described in part by the Cottrell equation.[2]
Relevant to cyclic voltammetry, the diffusion layer has negligible volume compared the volume of the bulk solution. For this reason, cyclic voltammetry experiments have an inexhaustible supply of fresh analyte.
References
- ^ IUPAC, Compendium of Chemical Terminology, 2nd ed. (the "Gold Book") (1997). Online corrected version: (2006–) "diffusion layer (concentration boundary layer)". doi:10.1351/goldbook.D01725
- ^ Bard, A. J.; Faulkner, L. R. “Electrochemical Methods. Fundamentals and Applications” 2nd Ed. Wiley, New York. 2001. ISBN 0-471-04372-9