Question

please solve this problem in detailed steps

Consider an electrochemical cell of iron and tin. The cell is tested at body temperature and the concentrations of the iron and tin solutions in each half-cell are 100 µg/dL and 108 µg/dL, respectively. Calculate the potential differences between the electrodes under these conditions.

Answer 1

standard Reduction potential of Fe : -0.41 and Sn is : -0.14

since Sn has higher reduction potential hence it will be cathode and Fe will be anode

Anode: Fe -------> Fe2+ + 2e-

Cathode : Sn2+ + 2e- ------> Sn

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Overall : Fe(s) + Sn2+ -------> Fe2+ + Sn (s)

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First calculate E⁰cell = E⁰(cathode) - E⁰(anode)

E⁰cell = -0.14 - (-0.41) = 0.27 V

Applying nernst equation

$E_{cell}=E^0_{cell}-\frac {0.059}{n} \times \frac {[Fe^{2+}]}{[Sn^{2+}]}$

Ecell = 0.27 - 0.059 / 2 * log [100] / [108]

Ecell = 0.27 - 0.03 * log (0.9259)

Ecell $\approx$0.27 V

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