Solve the following

Question:

Given that $\mathrm{E}_{\mathrm{O}_{2} / \mathrm{H}_{2} \mathrm{O}}^{\circ}=+1.23 \mathrm{~V}$;

$\mathrm{E}_{\mathrm{S}_{2} \mathrm{O}_{8}^{2-} / / \mathrm{SO}_{4}^{2-}}^{2-}=2.05 \mathrm{~V}$

$\mathrm{E}_{\mathrm{Br}_{2} / \mathrm{Br}}^{\circ}=+1.09 \mathrm{~V}$

$\mathrm{E}_{\mathrm{Au}^{3+} / \mathrm{Au}}^{\circ}=+1.4 \mathrm{~V}$

The strongest oxidising agent is :

1. $\mathrm{Au}^{3+}$

2. $\mathrm{O}_{2}$

3. $\mathrm{S}_{2} \mathrm{O}_{8}^{2-}$

4.  $\mathrm{Br}_{2}$

Correct Option: , 3

Solution:

More positive is the reduction potential stronger is the oxidising agent. Reduction potential is maximum for $\mathrm{S}_{2} \mathrm{O}_{8}^{2-}$, therefore, it is the strongest oxidising agent amongst the given species.

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