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An electrochemical cell is based on the following two half-reactions: Ox: Sn(s)?Sn2+(aq, 1.60 M )+2e? Red:...

An electrochemical cell is based on the following two half-reactions:

Ox: Sn(s)?Sn2+(aq, 1.60 M )+2e?

Red: ClO2(g, 0.195 atm )+e??ClO?2(aq, 1.70 M ).

Compute the cell potential at 25 degrees C.

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Answer #1

The two half cell reactions are

Oxidation reaction

Sn(s) = Sn2+(aq) + 2e-

Eox = 0.14 V

Reduction reaction

ClO2(g) + e- = ClO2-(aq)

Multiply by 2

2ClO2(g) + 2e- = 2ClO2-(aq)

Ered = 0.95 V

Overall cell reaction

Sn(s) + 2ClO2(g) = 2ClO2-(aq) + Sn2+(aq)

Standard reduction potential

E°cell = Eox + Ered

= 0.14 + 0.95

= 1.09 V

From the Nernst equation

E = E°cell - (0.0592/2) log [Sn2+] [ClO2-]2/ [PClO2]2

= 1.09 - (0.0592/2) log [1.60] [1.70]2/ [0.195]2

= 1.09 - 0.0617

= 1.028 V

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