I_2 + 2e^{-} to 2I^{-}; E^{o} = 0.54 VCl_2 + | vedclass

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(B) substance with a higher reduction potential acts as a stronger oxidizing agent and can oxidize a substance with a lower reduction potential.Compar

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Iodide ion is oxidised by chlorine

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(B) substance with a higher reduction potential acts as a stronger oxidizing agent and can oxidize a substance with a lower reduction potential.Comparing the reduction potentials:$E^{o}(Cl_2/Cl^-) = 1.36 \ V > E^{o}(I_2/I^-) = 0.54 \ V$. Therefore,$Cl_2$ can oxidize $I^-$ to $I_2$.$E^{o}(Mn^{3+}/Mn^{2+}) = 1.50 \ V > E^{o}(Fe^{3+}/Fe^{2+}) = 0.77 \ V$. Therefore,$Mn^{3+}$ can oxidize $Fe^{2+}$.Option $B$ states that the iodide ion $(I^-)$ is oxidised by chlorine $(Cl_2)$,which is correct because $E^{o}_{cell} = E^{o}_{cathode} - E^{o}_{anode} = 1.36 \ V - 0.54 \ V = 0.82 \ V > 0$.

$I_2 + 2e^{-} \to 2I^{-}$; $E^{o} = 0.54 \ V$
$Cl_2 + 2e^{-} \to 2Cl^{-}$; $E^{o} = 1.36 \ V$
$Mn^{3+} + e^{-} \to Mn^{2+}$; $E^{o} = 1.50 \ V$
$Fe^{3+} + e^{-} \to Fe^{2+}$; $E^{o} = 0.77 \ V$
Which of the following is a correct statement?

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$I_2 + 2e^{-} \to 2I^{-}$; $E^{o} = 0.54 \ V$$Cl_2 + 2e^{-} \to 2Cl^{-}$; $E^{o} = 1.36 \ V$$Mn^{3+} + e^{-} \to Mn^{2+}$; $E^{o} = 1.50 \ V$$Fe^{3+} + e^{-} \to Fe^{2+}$; $E^{o} = 0.77 \ V$Which of the following is a correct statement?