For a galvanic cell, the reaction happens in positive pole. Zn - 2e^- Zn^2+ E de

Question

For a galvanic cell, the reaction happens in positive pole. Zn - 2e^- Zn^2+ E degree = 0.76 V In negative pole. Cu^2+ + 2e^- = Cu E degree = 0.34 V (Assume all reactant is in Standard State) Since the E degree (Zn^2+/Zn) > 0, Delta G > 0, How the reaction happens spontaneously? Guess? The electrons produced in positive pole are transmitted to negative pole, so the potential of the electrons in ft electrode is more negative, they can reach a level high enough to transfer into vacant electronic states of Cu^2+ Could the ideal explain how Zn - 2e^- Zn^2+ + ??

Explanation / Answer

We have to consider the overall cell potential

Zn ----> Zn+2 + 2e-

Cu + 2e- ----> Cu+2

Overall reaction :

Zn + Cu+2 ------> Cu+2 + Zn

Ecell = 0.34+0.76 = 1.1 V

delta G = - nFEcell

Ecell is postive

So, delta G is negative

Since delta G is negative the reaction is spontanoeus ....

We already know as delta G is negative , reaction is spontaneous

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