Question

Given that $E_{O_2/H_{2}O}^o=+1.23V;$

$E_{S_2{O}_8^{2-}/S{O}_4^{2-}}^o=2.05V$

$E_{B{r}_2/B{r}^{-}}^o=+1.09V$

$E_{A{u}^{3+}/Au}^o=+1.4V$

The strongest oxidising agent is:

• A. $A{u}^{3+}$
• B. $O_2$
• C. $S_2{O}_8^{2-}$
• D. $B{r}_2$

Answer 1

The correct option is C $S_2{O}_8^{2-}$

$S_2{O}_8^{2-}$ is correct
Higher the reduction potential of the species, stronger oxidising power is of the species.
The standard reduction potential is the highest for $S_2{O}_8^{2-}toS{O}_4^{2-}$.