The oxidation of ferrocene (FeCp2) to ferrocenium cation (FeCp2+) (where Cp: cyclopentadienyl anion, C5H5-) was investigated by means of electrochemical impedance spectroscopy (EIS) and cyclic voltammetry (CV) on either platinum (Pt) or glassy carbon (G-C) electrodes in acetonitrile (ACN), acetone (ACE), and acetonitrile (ACN)/acetone (ACE) binary mixtures with n-tetrabutylammonium hexafluorophosphate (TBAPF(6)) as background electrolyte at T = 294.15 K. The half-wave potentials (E-1/2), the diffusion coefficients (D), and the heterogeneous electron-transfer rate constants (k(s)) were derived. The activation free energies for electron transfer (Delta G(exp)(not equal) =) were experimentally determined and compared with the theoretical values (Delta G(ca1)(not equal)). The electron-transfer process was reversible and diffusion-controlled in all investigated solvent mixtures. The changes on the metal-ligand bond lengths upon electron transfer were almost insignificant. The E-1/2 values were shifted to less positive potentials with the increase of the ACN content. The k(s) values obtained on Pt electrode were slightly larger compared to k(s) measured on G-C electrode, while in both cases the k(s) values were diminished with the enrichment of the mixtures in ACN. The EIS spectra confirmed that the rate-determining step in the whole process is the diffusion of the FeCp2 species and thus the process can be properly characterized as diffusion-controlled.