Difference between revisions of "Standard electrode potential"
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==General== | ==General== | ||
| − | 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. This potential difference is created as a result of the difference between individual potentials of the two metal electrodes with respect to the electrolyte. (Reversible electrode is an electrode that owes its potential to changes of a reversible nature, in contrast to electrodes used in electroplating which are destroyed during their use.) It is the measure of reducing power of any element or compound. | + | 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. This potential difference is created as a result of the difference between individual potentials of the two metal electrodes with respect to the electrolyte. (Reversible electrode is an electrode that owes its potential to changes of a reversible nature, in contrast to electrodes used in electroplating which are destroyed during their use.) It is the measure of reducing power of any element or compound. |
==Standard reduction potential table== | ==Standard reduction potential table== | ||
Latest revision as of 20:44, 23 August 2019
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In electrochemistry, standard electrode potential is defined as the measure of the individual potential of reversible electrode at standard state with ions at an effective concentration of 1 mol/l at the pressure of 1 atm.
Contents
General
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. This potential difference is created as a result of the difference between individual potentials of the two metal electrodes with respect to the electrolyte. (Reversible electrode is an electrode that owes its potential to changes of a reversible nature, in contrast to electrodes used in electroplating which are destroyed during their use.) It is the measure of reducing power of any element or compound.
Standard reduction potential table
| Reaction | E°/V |
|---|---|
