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Standard reduction potentials of the half reactions are given below: F2(g) + 2e⁻ → 2F⁻(aq); E° = +2.85 V Cl2(g) + 2e⁻ → 2Cl⁻(aq); E° = +1.36 V Br2(l) + 2e⁻ → 2Br⁻(aq); E° = +1.06 V I2(s) + 2e⁻ → 2I⁻(aq); E° = +0.53 V The strongest oxidising and reducing agents respectively are:

1. F2 and I⁻
2. Br2 and Cl⁻
3. Cl2 and Br⁻
4. Cl2 and I2

Correct answer: F2 and I⁻

Solution

The strongest oxidizing agent corresponds to the species with the highest standard reduction potential, which is F2 (+2.85 V). The strongest reducing agent corresponds to the species with the lowest reduction potential, which is I⁻ (reverse of I2's reduction potential).

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