Filter the Standard Reduction Potentials Table by element, minimum and maximum potential (V), and reaction type to narrow down exactly the half-reactions you need — the table instantly shows your matching reactions, plus flags the strongest oxidizer (highest E°) and strongest reducer (lowest E°) within your filtered range.
Reactions Shown
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Strongest Oxidizer (Highest E°)
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Strongest Reducer (Lowest E°)
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Standard reduction potential (E°) is the voltage associated with a reduction reaction at an electrode when all solutes are 1 M and all gases are at 1 atm pressure at 25°C, measured against a standard hydrogen electrode.
A reaction is spontaneous if the overall cell potential (E°cell) is positive. Calculate E°cell = E°cathode - E°anode using the values from this table.
A negative reduction potential indicates that the species is less likely to be reduced than hydrogen. These species are better reducing agents (electron donors) than hydrogen.
The standard hydrogen electrode is assigned a potential of 0.00 V by convention, providing a reference point for measuring all other electrode potentials.
These values are measured under standard conditions (1 M, 1 atm, 25°C) and are highly accurate for those conditions. Real-world conditions may require adjustments using the Nernst equation.
Higher reduction potentials indicate stronger oxidizing agents. Species with high E° values readily accept electrons and oxidize other substances.