question_answer

Standard reduction potentials of the half reactions are given below:

\[{{F}_{2}}(g)+2{{e}^{-}}\xrightarrow{{}}2{{F}^{-}}(aq);{{E}^{o}}=+2.85\,V\]

\[C{{l}_{2}}(g)+2{{e}^{-}}\xrightarrow{{}}2C{{l}^{-}}(aq);{{E}^{o}}=+1.36\,V\]

\[B{{r}_{2}}(i)+2{{e}^{-}}\xrightarrow{{}}2B{{r}^{-}}(aq);{{E}^{o}}=+1.06\,V\]

\[{{I}_{2}}(S)+2{{e}^{-}}\xrightarrow{{}}2{{I}^{-}}(aq);{{E}^{o}}=+0.53\,V\]

The strongest oxidizing and reducing agents respectively are

A)  \[{{F}_{2}}\]and\[{{I}^{-}}\]             

B)  \[B{{r}_{2}}\]and \[C{{l}^{-}}\]

C)  \[C{{l}_{2}}\]and\[B{{r}^{-}}\]                      

D)  \[C{{l}_{2}}\]and\[{{I}_{2}}\]