We consider the electrochemical process shown by the formula

$$M\, \mathbin{\lower.3ex\hbox{$\buildrel\textstyle\rightarrow\over {\smash{\leftarrow}\vphantom{_{\vbox to.5ex{\vss}}}}$}} \,M^{n + } \, + \,ne$$
where \( \mathbin{\lower.3ex\hbox{$\buildrel\textstyle\rightarrow\over {\smash{\leftarrow}\vphantom{_{\vbox to.5ex{\vss}}}}$}} \) indicates reversibility. According to the theory of chemical processes, the reaction rate which can be measured from the outside is the difference between the forward reaction rate \(\vec \upsilon \) and the backward reaction rate \(\mathord{\buildrel{\lower3pt\hbox{$\scriptscriptstyle\leftarrow$}}\over \upsilon } \), i.e.,
$$\upsilon = \overrightarrow \upsilon - \overleftarrow \upsilon$$
The reaction will proceed in the forward direction when υ<0, and vice versa. It is clear that
$$\begin{array}{*{20}c} {\overrightarrow \upsilon = \overleftarrow \upsilon = \upsilon _0 ,} & {at} & {\upsilon = 0} \\ \end{array}$$

υ0 is the exchange reaction rate at equilibrium.


Polarization Curve Diffusion Layer Electrochemical Process Electrode Process Exchange Current Density 
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Copyright information

© Plenum Press, New York 1985

Authors and Affiliations

  • Fumio Hine
    • 1
  1. 1.Nagoya Institute of TechnologyNagoyaJapan

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