1.

A solution contains Fe^(2+),Fe^(3+) and I^(-) ions. This solution was treated with iodine at 35^(@)C. E^(@) for Fe^(3+)//Fe^(2+) is +0.77V and E^(@) for I_(2)//2I^(-)=0.536V. The favourable redox reaction is

Answer»

`I^(-)` will oxidised to `I_(2)`
`Fe^(2+)` will be oxidised to `Fe^(3+)`
`I_(2)` will be reduced to `I^(-)`
There will be no redox reaction

Solution :`2(e^(-)+Fe^(+3)toFe^(+2)""E^(@)=0.77V`
`underline(2I^(-)toI_(2)+2E^(-)""E^(@)=0.536V"")`
`2FE^(+3)+2e^(-)to2Fe^(+2)+I_(2)""E^(o)=E_(o x)^(o)+E_(RED)^(o)`
`=0.77=0.536=0.164V`
So, Reaction will TAKEN place.


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