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Standard potentials (E°) for some half-reactions are given below: Sn4+ + 2e– → Sn2+ ; E° = +0.15 V 2Hg2+ + 2e– → Hg2 2+ ; E° = +0.92 V PbO2 + 4H+ + 2e– → Pb2+ + 2H2O ; E° = +1.45 V Based on the above, which one of the following statements is correct?

1. Sn4+ is a stronger oxidising agent than Pb4+
2. Sn2+ is a stronger reducing agent than Hg2+
3. Hg2+ is a stronger oxidising agent than Pb4+
4. Pb2+ is a stronger reducing agent than Sn2+

Correct answer: Hg2+ is a stronger oxidising agent than Pb4+

Solution

The standard reduction potential (E°) indicates the tendency of a species to gain electrons and act as an oxidizing agent. Since Hg2+ has a higher E° (+0.92 V) than Pb4+ (+1.45 V), Hg2+ is a stronger oxidizing agent than Pb4+.

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