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Electrochemical Cells

This program provides drill in identification of components of electrochemical cells and prediction of direction of movement of electrons and ions in cells, it also provides practice in determining if a reaction is spontaneous.  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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