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Standard Electrode Potential

In an electrochemical cell, an electric potential is created between two dissimilar metals. This potential isa measurementof the energy per unit charge which is available from the oxidation/reduction reactions to drive the reaction. It isusual to visualize the cell reaction in terms of two half-reactions, an oxidation half-reaction and a reduction half-reaction.




The cell potential (known aselectromotive force or emf) , is contributed from the anode, is a measure of its ability to lose electrons - known as its "oxidation potential". The cathodeis contributed to basedupon its ability to gain electrons, its "reduction potential".


“The standard potential is theelectromotive forceof anelectrochemical cellcomprised of the electrode in question and the standard hydrogen electrode.”-http://electrochem.cwru.edu/ed/dict.htm

-electrochemistry dictionary

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http://hyperphysics.phy-astr.gsu.edu/hbase/tables/electpot.html#c1

Standard Electrode Potentials in Aqueous Solution at 25C
Cathode (Reduction)
Half-Reaction Standard Potential
E (volts)
Li+(aq) + e- -> Li(s) -3.04
K+(aq) + e- -> K(s) -2.92
Ca2+(aq) + 2e- -> Ca(s) -2.76
Na+(aq) + e- -> Na(s) -2.71
Mg2+(aq) + 2e- -> Mg(s) -2.38
Al3+(aq) + 3e- -> Al(s) -1.66
2H2O(l) + 2e- -> H2(g) + 2OH-(aq) -0.83
Zn2+(aq) + 2e- -> Zn(s) -0.76
Cr3+(aq) + 3e- -> Cr(s) -0.74
Fe2+(aq) + 2e- -> Fe(s) -0.41
Cd2+(aq) + 2e- -> Cd(s) -0.40
Ni2+(aq) + 2e- -> Ni(s) -0.23
Sn2+(aq) + 2e- -> Sn(s) -0.14
Pb2+(aq) + 2e- -> Pb(s) -0.13
Fe3+(aq) + 3e- -> Fe(s) -0.04
2H+(aq) + 2e- -> H2(g) 0.00
Sn4+(aq) + 2e- -> Sn2+(aq) 0.15
Cu2+(aq) + e- -> Cu+(aq) 0.16
ClO4-(aq) + H2O(l) + 2e- -> ClO3-(aq) + 2OH-(aq) 0.17
AgCl(s) + e- -> Ag(s) + Cl-(aq) 0.22
Cu2+(aq) + 2e- -> Cu(s) 0.34
ClO3-(aq) + H2O(l) + 2e- -> ClO2-(aq) + 2OH-(aq) 0.35
IO-(aq) + H2O(l) + 2e- -> I-(aq) + 2OH-(aq) 0.49
Cu+(aq) + e- -> Cu(s) 0.52
I2(s) + 2e- -> 2I-(aq) 0.54
ClO2-(aq) + H2O(l) + 2e- -> ClO-(aq) + 2OH-(aq) 0.59
Fe3+(aq) + e- -> Fe2+(aq) 0.77
Hg22+(aq) + 2e- -> 2Hg(l) 0.80
Ag+(aq) + e- -> Ag(s) 0.80
Hg2+(aq) + 2e- -> Hg(l) 0.85
ClO-(aq) + H2O(l) + 2e- -> Cl-(aq) + 2OH-(aq) 0.90
2Hg2+(aq) + 2e- -> Hg22+(aq) 0.90
NO3-(aq) + 4H+(aq) + 3e- -> NO(g) + 2H2O(l) 0.96
Br2(l) + 2e- -> 2Br-(aq) 1.07
O2(g) + 4H+(aq) + 4e- -> 2H2O(l) 1.23
Cr2O72-(aq) + 14H+(aq) + 6e- -> 2Cr3+(aq) + 7H2O(l) 1.33
Cl2(g) + 2e- -> 2Cl-(aq) 1.36
Ce4+(aq) + e- -> Ce3+(aq) 1.44
MnO4-(aq) + 8H+(aq) + 5e- -> Mn2+(aq) + 4H2O(l) 1.49
H2O2(aq) + 2H+(aq) + 2e- -> 2H2O(l) 1.78
Co3+(aq) + e- -> Co2+(aq) 1.82
S2O82-(aq) + 2e- -> 2SO42-(aq) 2.01
O3(g) + 2H+(aq) + 2e- -> O2(g) + H2O(l) 2.07
F2(g) + 2e- -> 2F-(aq) 2.87

http://hyperphysics.phy-astr.gsu.edu/hbase/chemical/electrode.html