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Chemistry Question on Redox reactions

On the basis of the following E0E^0 values, the strongest oxidising agent is [Fe(CN)6]4−→[Fe(CN)6]3−+e−;[Fe(CN)_6]^{4-} \rightarrow [Fe(CN)_6]^{3-}+e^-; \hspace15mm E^0=-0.35 V Fe2+→Fe3++e−;E0=−0.77VFe^{2+} \rightarrow Fe^{3+} + e^-;E^0=-0.77 V

A

[Fe(CN)6]4−[Fe(CN)_6]^{4-}

B

Fe2+Fe^{2+}

C

Fe3+Fe^{3+}

D

[Fe(CN)6]3−[Fe(CN)_6]^{3-}

Answer

Fe3+Fe^{3+}

Explanation

Solution

Substance which have higher reduction potential are stronger oxidising agent. [Fe(CN)6]4−→[Fe(CN)6]3−+e−,[Fe(CN)_6]^{4-}\rightarrow[Fe(CN)_6]^{3-}+e^-, \hspace20mm E^0=-0.35 \, V     Fe2+→Fe3++e−,E0=−0.77 V\, \, \, \, Fe^{2+}\rightarrow Fe^{3+}+e^-, E^0=-0.77 \, V \because \hspace5mm E^0_{oxi}=-E^0_{red} ∴    [Fe(CN)6]3−+e−→[Fe(CN)6]4−,E0=0.35 V\therefore \, \, \, \, [Fe(CN)_6]^{3-}+e^- \rightarrow[Fe(CN)_6]^{4-}, E^0=0.35 \, V Fe3++e−→Fe2+,      E0=0.77 VFe^{3+}+e^- \rightarrow Fe^{2+}, \, \, \, \, \, \, E^0=0.77 \, V Hence, Fe3+Fe^{3+} has maximum tendency to reduced, so it is the strongest oxidising agent.