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For M2+/M and M3+/M2+ systems, the 
values for some metals are as follows:
Cr2+/Cr −0.9V
Cr3/Cr2+ −0.4 V
Mn2+/Mn −1.2V
Mn3+ /Mn2+ +1.5 V
Fe2+ /Fe −0.4V
Fe3+/Fe2+ +0.8 V
Use this data to comment upon:
(i) The stability of Fe3+ in acid solution as compared to that of Cr3+ or Mn3+ and
(ii) The ease with which iron can be oxidised as compared to a similar process for either chromium or manganese metal.
Asked by Pooja Last Modified
Answer (i) The value for Fe3+/Fe2+ is higher than that for Cr3+/Cr2+ and lower than that for Mn3+/Mn2+. So, the reduction of Fe3+ to Fe2+ is easier than the reduction of Mn3+ to Mn2+, but not as easy as the reduction of Cr3+ to Cr2+. Hence, Fe3+ is more stable than Mn3+, but less stable than Cr3+. These metal ions can be arranged in the increasing order of their stability as: Mn3+ < Fe3+ < Cr3+
(ii) The reduction potentials for the given pairs increase in the following order.
Mn2+ / Mn < Cr2+ / Cr < Fe2+ /Fe
So, the oxidation of Fe to Fe2+ is not as easy as the oxidation of Cr to Cr2+ and the oxidation of Mn to Mn2+. Thus, these metals can be arranged in the increasing order of their ability to get oxidised as: Fe < Cr < Mn
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