Using the data given below find out the strongest reducing agent.
$$\begin{gathered} \mathrm{E}{°}_{\raisebox{1ex}{${\mathrm{Cr}}_2{{\mathrm{O}}_7}^{2-}$}\!\left/ \!\raisebox{-1ex}{${\mathrm{Cr}}^{3+}$}\right. }=1.33 \mathrm{V}, \mathrm{E}{°}_{\raisebox{1ex}{${\mathrm{Cl}}_2$}\!\left/ \!\raisebox{-1ex}{${\mathrm{Cl}}^{-}$}\right.}=1.36 \mathrm{V} \\ \mathrm{E}{°}_{\raisebox{1ex}{${{\mathrm{MnO}}_4}^{-}$}\!\left/ \!\raisebox{-1ex}{${\mathrm{Mn}}^{2+}$}\right.}=1.51 \mathrm{V}, \mathrm{E}{°}_{\raisebox{1ex}{${\mathrm{Cr}}^{3+}$}\!\left/ \!\raisebox{-1ex}{$\mathrm{Cr}$}\right. }=-0.74 \mathrm{V} \end{gathered}$$

Standard reduction potentials of the half reactions are given below :

$$\begin{gathered} {\mathrm{F}}_2\left(\mathrm{g}\right)+2{\mathrm{e}}^{-}\to 2{\mathrm{F}}^{-}; \mathrm{E}°=+2.85 \mathrm{V} \\ {\mathrm{Cl}}_2\left(\mathrm{g}\right)+2{\mathrm{e}}^{-}\to 2{\mathrm{Cl}}^{-}; \mathrm{E}°=+1.36 \mathrm{V} \\ {\mathrm{Br}}_2\left(\mathrm{g}\right)+2{\mathrm{e}}^{-}\to 2{\mathrm{Br}}^{-}; \mathrm{E}°= +1.06 \mathrm{V} \\ {\mathrm{I}}_2\left(\mathrm{g}\right)+2{\mathrm{e}}^{-}\to 2{\mathrm{I}}^{-}; \mathrm{E}°= +0.53 \mathrm{V} \end{gathered}$$

The strongest oxidising and reducing agents respectively are

Consider the redox reaction, $2 {\mathrm{S}}_2{{\mathrm{O}}_3}^{2-}+{\mathrm{I}}_2\to {\mathrm{S}}_4{{\mathrm{O}}_6}^{2-}+2 {\mathrm{I}}^{-}$

Which of the following statements about the following reactions are wrong?

$2 {\mathrm{Cu}}_2\mathrm{O} \left(\mathrm{s}\right)+ {\mathrm{Cu}}_2\mathrm{S} \left(\mathrm{s}\right)\to 6 \mathrm{Cu} \left(\mathrm{s}\right) +{\mathrm{SO}}_2 \left(\mathrm{g}\right)$