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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: Fe3+

Solution

Strongest oxidizing agent = the oxidized form with the highest standard reduction potential. Reduction potentials: Fe3+ + e- -> Fe2+ is +0.77 V; [Fe(CN)6]3- + e- -> [Fe(CN)6]4- is +0.35 V. Fe3+ has the higher value, so Fe3+ is the strongest oxidizing agent.

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