The @E01960@ rate constants are related to the partial currents by \[k_{\mathrm{ox}}=\frac{l_{\text{a}}}{n\ F\ A\ \Pi\: c_{i}^{\nu _{i}}}\] \[k_{\mathrm{red}}=\frac{l_{\text{c}}}{n\ F\ A\ \Pi\:c_{i}^{\nu _{i}}}\] where \(k_{\mathrm{ox}}\) and \(k_{\mathrm{red}}\) are the rate constants for the oxidizing (anodic) and reducing (cathodic) reactions respectively, \(n\) is the @C00993@ of the cell reaction, \(F\) is the @F02325@ and \(A\) is the geometric area of the electrode, the product \(\Pi\:c_{i}^{\nu _{i}}\) includes all the species \(i\) which take part in the partial reaction, \(c_{i}\) is the volume concentration of species \(i\) and \(\nu _{i}\) is the order of the reaction with respect to species \(i\). The conditional rate constant of an electrode reaction is the value of the @E01960@ @O04322@ at the @C01240@ of the @E01960@. When \(\alpha \) the transfer @C01124@ is independent of potential, \[k_{\text{c}} = \frac{k_{\text{ox}}}{\text{e}^{\frac{\alpha _{\text{a}}\ (E- E_{\text{c}}^{0'})\ n\ F}{\nu \ R\ T}}} = \frac{k_{\text{red}}}{\text{e}^{\frac{-\alpha _{\text{c}}\ (E- E_{\text{c}}^{0'})\ n\ F}{\nu \ R\ T}}}\] where \(\alpha _{\text{a}}\) and \(\alpha _{\text{c}}\) are the anodic and cathodic transfer coefficients respectively, \(E\) is the @E01935@ difference, \(E_{\text{c}}\) is the @C01240@, \(\nu \) is the @S06025@, \(R\) is the @G02579@ and \(T\) is the @T06321@. Similar rate constants can be defined using activities in place of concentrations in the first two equations, and the @S05912@ in place of the conditional potential in the latter two equations. This type of @O04322@ is called the standard @O04322@ of the @E01960@. The observable electrode @O04322@ is the constant of proportionality expressing the dependence of the rate of the @E01960@ on the @I03083@ of the chemical species involved in the reaction.