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The \( E_{R P}^{\circ} \) and their respective half reactions of some changes are given below:
(I) \( \mathrm{MnO}_{4}^{-}(a q)+8 \mathrm{H}^{+}(a q)+5 e \longrightarrow \mathrm{Mn}^{2+}(a q)+4 \mathrm{H}_{2} 0 ; E^{0}=+1.52 \mathrm{~V} \)
(II) \( \frac{1}{2} \mathrm{I}_{2}(s)+e \longrightarrow \mathrm{I}^{-}(a q) ; E^{0}=+0.54 \mathrm{~V} \)
(III) \( \frac{1}{2} \mathrm{Br}_{2}(l)+e \longrightarrow \mathrm{Br}^{-}(a q) ; E^{0}=+1.07 \mathrm{~V} \)
(IV) \( \frac{1}{2} \mathrm{Cl}_{2}(g)+e \longrightarrow \mathrm{Cl}^{-}(a q) ; E^{0}=+1.36 \mathrm{~V} \)
At \( \mathrm{pH}=0 \) and rest all reductant and oxidant in change (I) being in standard state, \( \mathrm{MnO}_{4}^{-} \)can oxidise :
(A) \( I^{-} \)or \( I_{2} \)
(B) \( \mathrm{Br}^{-} \)to \( \mathrm{Bi}_{2} \)
(C) \( \mathrm{Cl}^{-} \)to \( \mathrm{Cl}_{2} \)
(D) all of these
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