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

(i) EMF of cell$=$(Oxidation potential of anode)$-$(Reduction potential of cathode)
(ii) EMF of cell$=$(Oxidation potential of anode)$+$(Reduction potential of cathode)
(iii) EMF of cell$=$(Reduction potential of anode)$+$(Reduction potential of anode)
(iv) EMF of cell$=$(Oxidation potential of anode)$-$(Oxidation potential of cathode)

Which of the above relations are correct?

Given: $$\begin{gathered} {\mathrm{Zn}}^{2+}| \mathrm{Zn}=-0.76 \mathrm{V}, \\ {\mathrm{Cu}}^{2+}| \mathrm{Cu} =+0.34 \mathrm{V}, {\mathrm{Fe}}^{2+}| \mathrm{Fe}=-0.41 \mathrm{V} \end{gathered}$$

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