An iron rod is immersed in a solution containing `1.0 M NiSO_(4)` and `1.0 M ZnSO_(4)` Predict giving reasons which of the following reactions is likely to proceed ?
(i) Fe reduces `Zn^(2+)` ions,
(ii) Iron reduces `Ni^(2+)` ions.
Given : `E_(Zn^(2+)| Zn )^(0)` = -0.76 volt and ,`E_(Fe^(2+)|Fe)^(0)` = -0.44 volt and `E_(Ni^(2+)|Ni)^(0)`= -0.25 V

Explanation

(i) since `E^(@)` of Zn is more negative than that of fe therefore zn will be oxidised to `Zn^(+)` ions while `Fe^(2+)` ions will be reduced to fe in other words fe wil not reduce `Zn^(2+)` ions
(ii) since `E^(@)` of Fe is more negative than that of ni therefore fe will be oxidized to `Fe^(2+)` ions while `Ni^(2+)` ions will be reduced to Ni thus fe reduces `Ni^(2+)` ions