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Effect of Concentrations on Cell Potentials; The Nernst Equation

This program provides drill in  calculations involving the Nernst equation.  The program will show the correct solution for incorrect answers.

Results Total Correct Score%

Click here for Electrode Potentials

Web Author: Dr. Walter S. Hamilton

Standard Electrode Potentials in Aqueous Solutions at 25°C and 1 atm

Cathode Half-Reaction Std Potential(V) Cathode Half-Reaction Std Potential(V)
Li+(aq) + e- = Li(s)         -3.04 IO-(aq) + H2O(l) + 2 e- = I-(aq) + 2 OH-(aq) 0.49
Na+(aq) + e- = Na(s)         -2.71 Cu+(aq) + e- = Cu(s) 0.52
Mg2+(aq) + 2 e- = Mg(s)         -2.38 I2(s) + e- = 2 I-(aq) 0.54
Al3+(aq) + 3 e- = Al(s)         -1.66 Fe3+(aq) + e- = Fe2+(aq)         0.77
2 H2O(l) + 2 e- = H2(g) + 2 OH-(aq) -0.83 Hg22+(aq) + 2 e- = 2 Hg(l) 0.80
Zn2+(aq) + 2 e- = Zn(s)         -0.76 Ag+(aq) + e- = Ag(s)  0.80
Cr3+(aq) + 3 e- = Cr(s)         -0.74 Hg2+(aq) + 2 e- = Hg(l) 0.85
Fe2+(aq) + 2 e- = Fe(s)         -0.41 ClO-(aq) + H2O(l) + 2 e- = Cl-(aq) + 2 OH-(aq) 0.90
Cd2+(aq) + 2 e- = Cd(s)         -0.40 2 Hg2+(aq) + 2 e- = Hg22+(aq) 0.90
Ni2+(aq) + 2 e- = Ni(s)         -0.23 NO3-(aq) + 4 H+(aq)  + 3 e- = NO(g) + 2  H2O(l) 0.96
Sn2+(aq) + 2 e- = Sn(s)         -0.14 Br2(l) + 2 e- = 2 Br-(aq) 1.07
Pb2+(aq) + 2 e- = Pb(s)         -0.13 O2(g) +  4 H+(aq)  + 4 e- =   2  H2O(l) 1.23
Fe3+(aq) + 3 e- = Fe(s)         -0.04 Cr2O72-(aq) + 14 H+(aq) + e- = 2 Cr3+(aq) + 7 H2O(l) 1.33
2 H+(aq) + 2 e- = H2(g)         0.00 Cl2(g) + e- = 2 Cl-(aq) 1.36
Sn4+(aq) + 2 e- = Sn2+(aq)         0.15 MnO4-(aq) + 8 H+(aq)  + 5 e- = Mn2+(aq) + 4  H2O(l) 1.49
Cu2+(aq) + e- = Cu+(aq)         0.16 H2O2(aq) +  2 H+(aq)  + 2 e- =   2  H2O(l)   1.78
Cu2+(aq) + 2 e- = Cu(s)         0.34 S2O82-(aq) + 2 e- = 2 SO42-(aq) 2.01
    F2(g) + 2 e- = 2 F-(aq) 2.87
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