Faradaic current is the current produced at working and auxiliary electrodes due to the oxidation or reduction of an analyte.

The cathodic current produced by analyte reduction carries a positive charge, whereas the anodic current produced by analyte oxidation is negatively charged.

The faradaic current flow is governed by the applied potential at the working electrode, and its magnitude depends on the rate of the resulting oxidation or reduction reaction at the electrode surface.

Mass transport processes like diffusion, migration, and convection affect the faradaic current by facilitating the movement of ions or molecules from the electrode surface to the bulk solution and vice versa.

The rate of mass transport also influences the current. If the rate of electron transport kinetics is fast, the redox reaction is at equilibrium, and the system is electrochemically reversible.

In contrast, when the rate of electron transport kinetics is slow, the system is treated as electrochemically irreversible.

Finally, the Nonfaradaic current produced by changes in electrode potential must be accounted for before measuring the faradaic component.