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Given the following standard electrode potentials: Sn²⁺ transitioning to Sn⁴⁺ with 2 electrons released (E° = -0.15V) and Hg₂²⁺ splitting into 2Hg²⁺ with 2 electrons released (E° = -0.92V), which of the following statements is accurate?

1. The reaction Sn²⁺ → Sn⁴⁺ + 2e⁻ has E° = -0.15V.
2. The reaction Hg₂²⁺ → 2Hg²⁺ + 2e⁻ has E° = -0.92V.
3. Sn²⁺ undergoes oxidation more readily than Hg₂²⁺.
4. Sn²⁺ acts as a stronger reducing agent compared to Hg₂²⁺.

Correct answer: Sn²⁺ acts as a stronger reducing agent compared to Hg₂²⁺.

Solution

The standard electrode potential (E°) for Sn²⁺ → Sn⁴⁺ is higher (-0.15V) than that for Hg₂²⁺ → 2Hg²⁺ (-0.92V), indicating that Sn²⁺ is more easily oxidized and thus a stronger reducing agent.

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