| On the basis of the following \[E{}^\circ \] values, the strongest oxidising agent is [AIPMT (S) 2008] |
| \[{{[Fe{{(CN)}_{6}}]}^{4-}}\to {{[Fe{{(CN)}_{6}}]}^{3-}}]+{{e}^{-}};\]\[{{E}^{o}}=-0.35V\] |
| \[F{{e}^{2+}}\to F{{e}^{3+}}+{{e}^{-}};{{E}^{o}}=-0.77V\] |
A) \[{{[Fe{{(CN)}_{6}}]}^{4-}}\]
B) \[F{{e}^{2+}}\]
C) \[F{{e}^{3+}}\]
D) \[{{[Fe{{(CN)}_{6}}]}^{3-}}\]
Correct Answer: C
Solution :
| [c] Key Idea: |
| Oxidised form \[+n{{e}^{-}}\to \]Reduced form |
| The substances which have' lower reduction potential are stronger reducing agent while the substances which have higher reduction potential are stronger oxidising agent. |
| \[{{[Fe{{(CN)}_{6}}]}^{3-}}+{{e}^{-}}\to {{[Fe{{(CN)}_{6}}]}^{4-}};\]\[{{E}^{o}}=0.35V\] |
| \[F{{e}^{3+}}+{{e}^{-}}\to F{{e}^{2+}};\]\[{{E}^{o}}=0.77V\] |
| The reduction potential of \[F{{e}^{3+}}/F{{e}^{2+}}\] is higher, hence \[F{{e}^{3+}}\]is strongest oxidising agent. |
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