The standard reduction potential for the half-reaction Sn^4+ + 2e^- rightarrow S

Question

The standard reduction potential for the half-reaction Sn^4+ + 2e^- rightarrow Sn^2+ is +0.15 V. Consider data from the table of standard reduction potentials for common half-reactions, in your text. For a galvanic cell under standard conditions, which of the following anodic half reactions would produce at the anode, a spontaneous oxidation of Sn to Sn^2+ but not Sn^2+ to Sn^4+. Sn^4+ + 2e^- rightarrow Sn^2+ Pb^2+ + 2e^- rightarrow Pb 2H^+ + 2e^- rightarrow H_2 Fe^2+ + 2e^- rightarrow Fe PbSO_4 + 2e^- rightarrow Pb + SO^2-_4 2H_2O + 2e^- rightarrow H_2 + 2OH^-

Explanation / Answer

The standerd potential for the half reaction Sn4+ + 2e- ---> Sn2+ is 0.15 v E= + 0.15 V

anodic half reaction would produce spontaneous reduction of Sn4+ to Sn 2+ but not Sn2+ to Sn

The equations

Pb-----> Pb2+ +2e-                    E= -0.13 V

2H------> H2 + 2e-                      E=+0.00 V

H2 +2 OH- ----> 2H2O +2e-        E =-0.83V

Sn----> Sn2+ +2e-                     E =-0.14V

Pb + So42- ----> PbSO4 +2e-      E=

Fe----> Fe2++ 2e-                       E= -0.44V

Answer 2H------> H2 + 2e-           E=+0.00 V

Ecell = Ecathode - E anode = +0.15 -(+0.00) = 0.15V

Sn4+ + 2e- ---> Sn2+

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