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1 Table of standard electrode potentials. ... the table of contents. Standard electrode potential (data page) ... 2+ ion and two electrons is 2 × 0.44 eV = 0.88 eV ...
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".
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.
For example, for oxygen, the species would be in the order O 2 (0), H 2 O 2 (–1), H 2 O (-2): The arrow between O 2 and H 2 O 2 has a value +0.68 V over it, it indicates that the standard electrode potential for the reaction: O 2 (g) + 2 H + + 2 e − ⇄ H 2 O 2 (aq) is 0.68 volts.
The potential of zero charge is used for determination of the absolute electrode potential in a given electrolyte. IUPAC also defines the potential difference with respect to the potential of zero charge as: E pzc = E − E σ=0. where: E pzc is the electrode potential difference with respect to the point of zero charge, E σ=0; E is the ...
If the electrode has a positive potential with respect to the SHE, then that means it is a strongly reducing electrode which forces the SHE to be the anode (an example is Cu in aqueous CuSO 4 with a standard electrode potential of 0.337 V). Conversely, if the measured potential is negative, the electrode is more oxidizing than the SHE (such as ...
Absolute electrode potential, in electrochemistry, according to an IUPAC definition, [1] is the electrode potential of a metal measured with respect to a universal reference system (without any additional metal–solution interface).
A reference electrode is an electrode that has a stable and well-known electrode potential. The overall chemical reaction taking place in a cell is made up of two independent half-reactions , which describe chemical changes at the two electrodes.