Given the following species: MnO4^-, Cl2, Fe^3+, and H2O2, which is the strongest oxidizing agent?

• A. Cl2
• B. Fe^3+
• C. MnO4^-
• D. H2O2

Answer: (C)

Verified step by step guidance

1. Understand that an oxidizing agent is a species that gains electrons (is reduced) in a redox reaction, so the strongest oxidizing agent is the one with the highest tendency to be reduced.
2. Look up or recall the standard reduction potentials (E°) for the half-reactions involving each species: MnO4⁻, Cl2, Fe³⁺, and H2O2. The species with the highest positive standard reduction potential is the strongest oxidizing agent.
3. Write the relevant half-reactions for each species in acidic or neutral solution, for example, for permanganate ion (MnO4⁻): \(\mathrm{MnO_4^- + 8H^+ + 5e^- \rightarrow Mn^{2+} + 4H_2O}\), and note its standard reduction potential.
4. Compare the standard reduction potentials of all species: Cl2/Cl⁻, Fe³⁺/Fe²⁺, H2O2/H2O or OH⁻, and MnO4⁻/Mn²⁺. The species with the highest E° value is the strongest oxidizing agent.
5. Conclude that since MnO4⁻ has the highest standard reduction potential among the given species, it is the strongest oxidizing agent.