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Can Fe^(3+) oxidise Bromide to bromine under standard conditions ? Given : E_(Fe^(3+)|Fe^(2+))=0.771""E_(Br_(2)|Br^(-))^(@)=-1.09V

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Solution :Required half cell REACTION <BR> `2Br^(-)rarr Br^(2)+2e^(-)""(E_("ox")^(@))=-1.09V`
`2Fe^(3+)+2e^(-)rarr2Fe^(2+)""(E_("red")^(@))=+0.771V`
`2Fe^(3+)+2Br^(-)rarr 2Fe^(2+)+Br_(2)""(E_("cell")^(@))=?`
`E_("cell")^(@)=(E_("ox")^(@))+(E_("red")^(@))=-1.09+0.771=-0.319V`
We know that `DeltaG^(@)=-nFE_("cell")^(@)`
If `E_("cell")^(@)` is `-ve`, `DeltaG` is `+ve` and the cell reaction is non - spontaneous.
Hence, `Fe^(3+)` cannot oxidise Bromide to BROMINE.


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