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Using the standard reduction potentials given below, identify the species that acts as the strongest oxidizing agent: [Fe(CN)6]4- → [Fe(CN)6]3- + e- ; E° = -0.35 V Fe2+ → Fe3+ + e- ; E° = -0.77 V

1. [Fe(CN)6]4-
2. Fe2+
3. Fe3+
4. [Fe(CN)6]3-

Correct answer: Fe2+

Solution

Fe2+ is the strongest oxidizing agent among the options because it has the most negative standard reduction potential, indicating it is more likely to lose electrons and thus facilitate oxidation of other species.

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