question_answer

Standard reduction potentials of the half reactions are given below : \[{{F}_{2}}(g)+2{{e}^{-}}\to 2{{F}^{-}}(aq);\] \[{{E}^{o}}=+2.85V\] \[C{{l}_{2}}(g)+2{{e}^{-}}\to 2C{{l}^{-}}(aq);\] \[{{E}^{o}}=+1.36V\] \[B{{r}_{2}}(l)+2{{e}^{-}}\to 2B{{r}^{-}}(aq);\] \[{{E}^{o}}=+1.06V\] \[{{I}_{2}}(s)+2{{e}^{-}}\to 2{{I}^{-}}(aq);\] \[{{E}^{o}}=+0.53V\] The strongest oxidising 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 \[{{I}_{2}}\]