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 oxidizing agent is:

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

Answer 1

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

The more positive the reduction potential, higher is the oxidising power. Thus, $S_2{O}_8^{2-}$ is the strongest oxidising agent.