Standard electrode potential (°) (standard reduction potentialis) are defined by measuring the potential relative to a standard hydrogen electrode using 1 mol solution at 25 °C. The convention is to designate the cell so that the oxidized form is written first. For example, Pt(s)|H2(g)H+(aq)|Zn2+(aq)|Zn(s) The e.m.f. of this cell is -0.76 V and the standard electrode potential of the Zn2+|Zn half cell is -0.76 V.
The reversible or equilibrium potential of an electrode in an environment where reactants and products are at unit activity.
The potential of a half-cell when all reactants are present in their standard states relative to the standard hydrogen electrode Normally, standard electrode potentials are for reduction reactions
The reversible potential for an electrode process when all products and reactions are at unit activity on a scale in which the potential for the standard hydrogen half-cell is zero.
The standard potential E0 of an electrode is the reversible emf between the normal hydrogen electrode and the electrode with all components at unit activity.
By convention , potential, Eo, of a half-reaction as a reduction relative to the standard hydrogen electrode when all species are present at unit activity.
The standard electrode potentials are used to determine the electrochemical potential or the electrode potential of an electrochemical cell or Galvanic cell.
In electrochemistry, the standard electrode potential, abbreviated Eo, is the measure of individual potential of any electrode at standard ambient conditions, which is at a temperature of 298K, solutes at a concentration of 1 M, and gases at a pressure of 1 bar. The basis for an electrochemical cell such as the galvanic cell is always a redox reaction which can be broken down into two half-reactions: oxidation at anode (loss of electron) and reduction at cathode (gain of electron). Electricity is generated due to electric potential difference between two electrodes.