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  • Using the standard electrode potentials given in Table

3.17    Using the standard electrode potentials given in Table 3.1, predict if the reaction between the following is feasible:

         (ii) Ag^{+}_{aq}\ and\ Cu_{(s)}

              

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A reaction is feasible only if  E_{cell} ^{\circ}  is positive.

So, anode and cathode reactions will be as follows :- 

                                           (Ag^{+}\ +\ e^-\ =\ Ag)\times 2                                E^{\circ}\ = 0.80\ V

                                                              Cu\ =\ Cu^{+2}\ +\ 2e^-                     E^{\circ}\ = -0.34\ V

and                                  E_{cell} ^{\circ} = 0.80 - 0.34 = 0.46\ V

So this reaction is feasible.

Posted by

Devendra Khairwa

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