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Electrochemistry

Question

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The standard electrode potential for Daniell cell is 1.1 V. Calculate the standard Gibbs energy for the reaction:
$Zn (s) + {Cu}^{2 +} (aq) \to {Zn}^{2 +} (aq) + Cu (s)$

Solution

∆_{r} G ° = - nFE ° n = 2 and F = 96500 C E °_{cell} = + 1.10

∆_{r} G ° = - 2 \times 96500 \times 1.10

or

∆_{r} G ° = - 212300 J

W_{\max} = - ∆_{r} G ° = 212300 J

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