8.26 Using the standard electrode potentials given in the Table 8.1, predict if the reaction between the following is feasible

(a) Fe^{3+}(aq) and I^{-}(aq)
(b) Ag^{+}(aq) and Cu(s)
(c) Fe^{3+}(aq) and Cu(s)
(d) Ag(s) and Fe^{3+} (aq)
(e) Br_{2}(aq) and  Fe^{2+}(aq).

Answers (1)

Answer- 

If E^{0} for the overall reaction is positive \rightarrow feasible

                                                 negative\rightarrownot feasible

(a)                        [Fe^{3+}+ e^{-}\rightarrow Fe^{2+} ]*2: E^{0} = 0.77V

                                               2I^{-}\rightarrow I_{2}+2e^{-}: E^{0} = -0.54V

                      ---------------------------------------------------------------------------------------

                             2Fe^{3+}+2I^{-}\rightarrow Fe^{2+}+I_{2}: E^{0} = +0.23V

 

(b)                           Ag^{+}+e^{-}\rightarrow Ag(s)]*2: E^{0} = +0.80V

                               Cu\rightarrow Cu^{2+}+2e^{-}:E^{0} =-0.34V

                    ---------------------------------------------------------------------------------------

                   2Ag^{+}+Cu\rightarrow 2Ag+Cu^{2+}: E^{0}=+0.46V

 

(c)     Fe^{3+}+e^{-}\rightarrow Fe^{2+}]*2 :E^{0}=+0.77V

        2Br^{-}\rightarrow Br+2e^{- }:E^{0}=-1.09V

-------------------------------------------------------------------------

2Fe^{3+}+2Br^{-}\rightarrow 2Fe^{3+}+Br_{2}:E^{0}=-0.32

 

(d)     Ag\rightarrow Ag^{+}+e^{-}:E^{0}=-0.80V

         Fe^{3+}+e^{-}\rightarrow Fe^{2+}:E^{0}==0.77V

------------------------------------------------------------------------------

   Ag+Fe^{3+}\rightarrow Ag^{+}+Fe^{2+}:E^{0}=-0.03V

 

(e)   Br_{2}+2e^{-}\rightarrow 2Br^{-}:E^{0}=+1.09V

       Fe^{2+}\rightarrow Fe^{3+}+e^{-}]*2:E^{0}=-0.77V

-------------------------------------------------------------------------------

Br_{2}+2Fe^{2+}\rightarrow 2Br^{-}+2Fe^{3+}:E^{0}=+0.32V

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