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  2. Standard electrode potential (data page) - Wikipedia

    en.wikipedia.org/wiki/Standard_electrode...

    Electrode potentials of successive elementary half-reactions cannot be directly added. However, the corresponding Gibbs free energy changes (∆G°) must satisfy ∆G° = – z FE°, where z electrons are transferred, and the Faraday constant F is the conversion factor describing Coulombs transferred per mole electrons. Those Gibbs free energy ...

  3. Reactivity series - Wikipedia

    en.wikipedia.org/wiki/Reactivity_series

    The reactivity series is sometimes quoted in the strict reverse order of standard electrode potentials, when it is also known as the "electrochemical series". [8] The following list includes the metallic elements of the first six periods. It is mostly based on tables provided by NIST.

  4. Table of standard reduction potentials for half-reactions ...

    en.wikipedia.org/wiki/Table_of_standard...

    The values below are standard apparent reduction potentials (E°') for electro-biochemical half-reactions measured at 25 °C, 1 atmosphere and a pH of 7 in aqueous solution. [1] [2] The actual physiological potential depends on the ratio of the reduced (Red) and oxidized (Ox) forms according to the Nernst equation and the thermal voltage.

  5. Standard electrode potential - Wikipedia

    en.wikipedia.org/wiki/Standard_electrode_potential

    Bipolar electrochemistry scheme. In electrochemistry, standard electrode potential, or , is a measure of the reducing power of any element or compound.The IUPAC "Gold Book" defines it as; "the value of the standard emf (electromotive force) of a cell in which molecular hydrogen under standard pressure is oxidized to solvated protons at the left-hand electrode".

  6. Reduction potential - Wikipedia

    en.wikipedia.org/wiki/Reduction_potential

    In aqueous solutions, redox potential is a measure of the tendency of the solution to either gain or lose electrons in a reaction. A solution with a higher (more positive) reduction potential than some other molecule will have a tendency to gain electrons from this molecule (i.e. to be reduced by oxidizing this other molecule) and a solution with a lower (more negative) reduction potential ...

  7. Galvanic series - Wikipedia

    en.wikipedia.org/wiki/Galvanic_series

    The difference can be measured as a difference in voltage potential: the less noble metal is the one with a lower (that is, more negative) electrode potential than the nobler one, and will function as the anode (electron or anion attractor) within the electrolyte device functioning as described above (a galvanic cell).

  8. Category:Electrochemical potentials - Wikipedia

    en.wikipedia.org/wiki/Category:Electrochemical...

    Standard electrode potential (data page) ... Table of standard reduction potentials for half-reactions important in biochemistry; U.

  9. Electrode potential - Wikipedia

    en.wikipedia.org/wiki/Electrode_potential

    To avoid possible ambiguities, the electrode potential thus defined can also be referred to as Gibbs–Stockholm electrode potential. In both conventions, the standard hydrogen electrode is defined to have a potential of 0 V. Both conventions also agree on the sign of E for a half-cell reaction when it is written as a reduction.