Which of the following is the strongest oxidizing agent?

E°(S₂O₈²⁻/SO₄²⁻)= 2.05 V

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E° (Br₂/Br⁻) = 1.40 V

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E° (Au³⁺/Au) = 1.10V

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E° (O₂/H₂O) =1.20V

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Solution

The correct option is A
E°(S₂O₈²⁻/SO₄²⁻)= 2.05 V

Explanation for the correct option
The correct option is (A)
The compound that has more positive reduction potential will reduce easy, So that will we the strong oxidising agent.
From above option A [E°(S₂O₈²⁻/SO₄²⁻)= 2.05 V] has the highest reduction potential.
So, the correct option is A.
hus, remaining other options are incorrect because of the lower reduction potential as compared to option A.

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