Question

On the basis of standard electrode potential of redox couples given below, find out which of the following is the strongest oxidising agent.
(E${}^{\circ }$ values : $F{e}^{3+}\left|F{e}^{2+}=+0.77V;<br/>I_{2\left(s\right)}\right|I^{-}=$ $+0.54V;C{u}^{2+}\left|Cu=+.34V;A{g}^{+}\right|Ag=+0.80V$)

• A. $F{e}^{3+}$
• B. $I_{2(s)}$
• C. $C{u}^{2+}$
• D. $A{g}^{+}$

Answer 1

Answer: (D)

Higher the electrode potential, better is the oxidising agent. Since, the electrode potential decreases in the order :
$A{g}^{+}\left|Ag\left(+0.80V\right)>F{e}^{3+}\right|F{e}^{2+}\left(+0.77V\right)>$
$I_{2\left(2\right)}\left|I^{-}\left(+0.54V\right)>C{u}^{2+}\right|Cu\left(+0.34V\right)$
Hence, Ag⁺ is the strongest oxidising agent.