Determine the following in the standard galvanic cell?

The following standard redox couples are connected to make a galvanic cell.





Sn/Sn2+ E1o = -0.14


Hg/Hg2+ E2o = 0.85





Determine the following for the standard galvanic cell:


a) Eo =


b) delta G =


c) log K =

Determine the following in the standard galvanic cell?
Since you have written;


Sn/Sn2+ E1o = -0.14


Hg/Hg2+ E2o = 0.85


this implies that the values are the oxidation potentials, however I've checked and found that these are the reduction potentials.


Therefore, the reduction potential of Hg2+ is greater than that of Sn2+, Hg2+ will be reduced and Sn will be oxidized.





(a) Anode half-reaction: Sn ----%26gt; Sn2+ + 2e- ..... E° = 0.14 V


Cathode half-reaction: Hg2+ + 2e- ----%26gt; Hg ....... E° = 0.85 V





Cell reaction: Sn + Hg2+ ----%26gt; Sn2+ + Hg .. E°cell = 0.99 V





(b) ΔG° = - n F E°





n = 2 mol e-


F = 96,485 C/mol e- (charge of 1 mol e-)(C = coulomb)


E° = 0.99 V = 0.99 J/C





ΔG° = - n F E°





ΔG° = - (2 mol e-)(96,485 C/mol e-)(0.99 J/C)


ΔG° = - 191,040 J





Positive sign of E° and negative sign of ΔG° indicate that the the process is spontaneous.





(c) log K = n E° / 0.0591 = (2)(0.99) / 0.0591 = 33.5


K = 10^33.5 = 3.16x10^33