question_answer 42)

  The more positive the value of\[{{E}^{O-}}\], the greater is the tendency of the species to get reduced. Using the standard electrode potential of redox couples given below find out which of the following is the strongest oxidising agent? \[{{E}^{O-}}Values\,:\,\,\,\,F{{e}^{3+}}/{{F}^{2+}}=+0.77;{{I}_{2}}(s)/{{I}^{-}}=+0.54;\]\[C{{u}^{2+}}/Cu=+0.34;A{{g}^{+}}/Ag=+0.80V\] (a)\[F{{e}^{3+}}\]                                            (b) \[{{I}_{2}}(s)\]                            (c) \[C{{u}^{2+}}\]                           (d)\[A{{g}^{+}}\]

Answer:

  (d)\[E_{A{{g}^{+}}/Ag}^{{}^\circ }=+0.80V\]will be the strongest oxidising species because standard reduction potential is maximum positive.