On the basis of the following Eo values, the strongest oxidizing agent is
[Fe(CN)6]4$$-$$ $$ \to $$ [Fe(CN)6]3$$-$$ + e$$-$$; Eo = $$-$$0.35 V
Fe2+ $$ \to $$ Fe3+ + e$$-$$; Eo = $$-$$0.77 V
Explanation
Substances which have higher reduction
potential are stronger oxidizing agent.
[Fe(CN)6]4$$-$$ $$ \to $$ [Fe(CN)6]3$$-$$ + e$$-$$; Eo = $$-$$0.35 V
Fe2+ $$ \to $$ Fe3+ + e$$-$$; Eo = $$-$$0.77 V
Higher the +ve reduction potential, stronger will
be the oxidising agent. Oxidising agent oxidises
other compounds and gets itself reduced easily.