Standard reduction potentials of the half reactions are given below: F_2( g ) +2 e^- → 2 F^-_( aq ); E^°=+2.85 V; Cl_2( g ) +2 e^- → 2 Cl^-_( aq );…

Standard reduction potentials of the half reactions are given below : $$\begin{array}{ll} \mathrm{F}_{2(\mathrm{~g})}+2 \mathrm{e}^{-} \rightarrow 2 \mathrm{~F}^{-}{ }_{(\mathrm{aq})} ; & \mathrm{E}^{\circ}=+2.85 \mathrm{~V} \\ \mathrm{Cl}_{2(\mathrm{~g})}+2 \mathrm{e}^{-} \rightarrow 2 \mathrm{Cl}^{-}{ }_{(\mathrm{aq})} ; & \mathrm{E}^{\circ}=+1.36 \mathrm{~V} \\ \mathrm{Br}_{2(\mathrm{l})}+2 \mathrm{e}^{-} \rightarrow 2 \mathrm{Br}^{-}{ }_{(\mathrm{aq})} ; & \mathrm{E}^{\circ}=+1.06 \mathrm{~V} \\ \mathrm{I}_{2(\mathrm{~s})}+2 \mathrm{e}^{-} \rightarrow 2 \mathrm{I}^{-}{ }_{(\mathrm{aq})} ; & \mathrm{E}^{\circ}=+0.53 \mathrm{~V} \end{array} $$ The strongest oxidising and reducing agents respectively are :