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  • Using the standard electrode potentials given in Table 3 .1

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

               Ag_{s}\ and\ Fe^{3+}_{aq}

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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\ =\ Ag^{+}\ +\ e^-                        E^{\circ}\ = -0.80\ V

                                       Fe^{+3}\ +\ e^-\ =\ Fe^{+2}                     E^{\circ}\ = 0.77\ V

and                                  E_{cell} ^{\circ} = -0.80 + 0.77 = -0.03\ V

So this reaction is not feasible.

Posted by

Devendra Khairwa

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