Given the following standard oxidation potentials (): ; . Based on these thermodynamic values, the s — Electrochemistry Chemistry Question

💡 Solution & Explanation

The provided values are oxidation potentials. Converting them to standard reduction potentials ($E^\circ_{red}$) by reversing the sign gives $+0.35\text{ V}$ for $[Fe(CN)_6]^{3-} \rightarrow [Fe(CN)_6]^{4-}$ and $+0.77\text{ V}$ for $Fe^{3+} \rightarrow Fe^{2+}$. The species with the highest positive standard reduction potential is the strongest oxidizing agent. Thus, $Fe^{3+}$ is the strongest oxidizing agent.