text: A reduction–oxidation (redox) equilibrium can be handled in exactly the same way as any other chemical equilibrium. For example,
  :Fe + Ce  Fe + Ce;
  However, in the case of redox reactions it is convenient to split the overall reaction into two half-reactions. In this example
  :Fe + e  Fe
  :Ce + e  Ce
  The standard free energy change, which is related to the equilibrium constant by   
  can be split into two components,
  The concentration of free electrons is effectively zero as the electrons are transferred directly from the reductant to the oxidant. The standard electrode potential, E for the each half-reaction is related to the standard free energy change by
  where n is the number of electrons transferred and F is the Faraday constant. Now, the free energy for an actual reaction is given by
  where R is the gas constant and Q a reaction quotient. Strictly speaking Q is a quotient of activities, but it is common practice to use concentrations instead of activities. Therefore:
  For any half-reaction, the redox potential of an actual mixture is given by the generalized expression
  This is an example of the Nernst equation. The potential is known as a reduction potential. Standard electrode potentials are available in a table of values. Using these values, the actual electrode potential for a redox couple can be calculated as a function of the ratio of concentrations.
  The equilibrium potential for a general redox half-reaction (See #Equilibrium constant above for an explanation of the symbols)
  :α A + β B... + n e  σ S + τ T...
  is given by
  Use of this expression allows the effect of a species not involved in the redox reaction, such as the hydrogen ion in a half-reaction  such as
  : + 8 H + 5 e  Mn + 4 HO
  to be taken into account.
  The equilibrium constant for a full redox reaction can be obtained from the standard redox potentials of the constituent half-reactions. At equilibrium the potential for the two half-reactions must be equal to each other and, of course, the number of electrons exchanged must be the same in the two half reactions.
  Redox equilibrium play an important role in the electron transport chain. The various cytochromes in the chain have different standard redox potentials, each one adapted for a specific redox reaction. This allows, for example, atmospheric oxygen to be reduced in photosynthesis. A distinct family of cytochromes, the cytochrome P450 oxidases, are involved in steroidogenesis and detoxification.