Answer:
[tex]$Cl_{2}$[/tex] is reduced in the reaction
Explanation:
The given reaction is
[tex]$2Fe^{2+}+Cl_{2} \to 2Fe^{3+}+2Cl^{-}$[/tex]
The oxidation number of [tex]$Fe$[/tex] is changed from [tex]$+2\, \to \, +3$[/tex]
[tex]$Fe^{2+} \to Fe^{3+}+e^{-}$[/tex]
And The oxidation number of [tex]$Cl$[/tex] is changed from [tex]$0\, \to \, -1$[/tex]
[tex]$Cl_{2}^{0} + 2e^{-} \to 2Cl^{-}$[/tex]
Hence, [tex]$Fe^{2+}$[/tex] is oxidized and [tex]$Cl_{2}$[/tex] is reduced
