Overpotential

In electrochemistry, overpotential is the potential difference (voltage) between a half-reaction's thermodynamically determined reduction potential and the potential at which the redox event is experimentally observed.^[1] The term is directly related to a cell's voltage efficiency. In an electrolytic cell the overpotential requires more energy than thermodynamically expected to drive a reaction. In a galvanic cell overpotential means less energy is recovered than thermodynamics would predict. In each case the extra or missing energy is lost as heat. Overpotential is specific to each cell design and will vary between cells and operational conditions even for the same reaction. Practically, it is also useful to define the current density (typically small) at which the overpotential is measured.

Thermodynamics

The four possible polarities of overpotentials are listed below.

• An electrolytic cell's anode is more positive using more energy than thermodynamics require.
• An electrolytic cell's cathode is more negative using more energy than thermodynamics require.
• A galvanic cell's anode is less negative supplying less energy than thermodynamically possible.
• A galvanic cell's cathode is less positive supplying less energy than thermodynamically possible.

The overpotential increases with increasing current density (or rate), as described by the Tafel equation. An electrochemical reaction is a combination of two half-cells and multiple elementary steps. Each of these electrochemical steps is associated with multiple forms of overpotential. The overall overpotential is the summation of many individual losses. Voltage efficiency describes the energy lost through overpotential. For an electrolytic cell this is the ratio of a cell's thermodynamic potential divided by the cell's experimental potential converted to a percentile. For a galvanic cell it is the ratio of a cell's experimental potential divided by the cell's thermodynamic potential converted to a percentile. Voltage efficiency should not be confused with Faraday efficiency. Each term refers to a mode through which electrochemical systems can lose energy. Energy can be expressed as the product of potential, current and time (joules = volts × amps × seconds). Losses in the potential term through overpotentials are described by voltage efficiency. Losses in the current term through misdirected electrons are described by Faradaic efficiency.

Varieties of overpotential

Overpotential can be divided into many different subcategories that are not always well defined. For example "polarization overpotential" can refer to the electrode polarization and the hysteresis found in forward and reverse peaks of cyclic voltammetry. A likely reason for the lack of strict definitions is that it's difficult to determine how much of a measured overpotential is derived from a specific source. There is precedent for grouping overpotentials into three categories: activation, concentration, and resistance.^[2]

Activation overpotential

The activation potential is the potential difference above the equilibrium value required to produce a current which depends on the activation energy of the redox event. While ambiguous, "activation overpotential" often refers exclusively to the activation energy necessary to transfer an electron from an electrode to an analyte. This sort of overpotential can also be called "electron transfer overpotential" and is a component of "polarization overpotential", a phenomenon observed in cyclic voltammetry and partially described by the Cottrell equation.

Reaction overpotential

Reaction overpotential is an activation overpotential that specifically relates to chemical reactions that precede electron transfer. Reaction overpotential can be reduced or eliminated with the use of homogeneous or heterogeneous electrocatalysts. The electrochemical reaction rate and related current density is dictated by the kinetics of the electrocatalyst and substrate concentration.

The platinum electrode common to much of electrochemistry is electrocatalytically involved in many reactions. For example, hydrogen is oxidized and protons are reduced readily at the platinum surface of a standard hydrogen electrode in aqueous solution. Substituting an electrocatalytically inert glassy carbon electrode for the platinum electrode produces irreversible reduction and oxidation peaks with large overpotentials.

Concentration overpotential

Concentration overpotential span a variety of phenomenon but all involve the depletion of charge-carriers at the electrode surface. Bubble overpotential is a specific form of concentration overpotential in which the concentration of charge-carriers is depleted by the physical formation of a bubble. The confusing "diffusion overpotential" can refer to a concentration overpotential created by slow diffusion rates as well as "polarization overpotential" whose overpotential is derived mostly from activation overpotential but peak current is limited by diffusion of analyte.

The potential difference is caused by differences in concentration of the charge-carriers between bulk solution and on the electrode surface. It occurs when electrochemical reaction is sufficiently rapid to lower the surface concentration of the charge-carriers below that of bulk solution. The rate of reaction is then dependent on the ability of the charge-carriers to reach the electrode surface.

Bubble overpotential

Bubble overpotential is a specific form of concentration overpotential and is due to the evolution of gas at either the anode or cathode. This reduces the effective area for current and increases the local current density. An example would be the electrolysis of an aqueous sodium chloride solution—although oxygen should be produced at the anode based on its potential, bubble overpotential causes chlorine to be produced instead, which allows the easy industrial production of chlorine and sodium hydroxide by electrolysis.

Resistance overpotential

Resistance overpotentials are all the overpotentials tied to a cell design. These include "junction overpotentials" which occur at electrode surfaces and interfaces like electrolyte membranes. They can also include aspects of electrolyte diffusion, surface polarization (capacitance), and other sources of counter electromotive forces.

See also

• Electrolysis
• Electrosynthesis

References