1.

A solution contains Fe^(2+), Fe^(3+) and I^(-) ions. The solution was treated with iodine at 35^(@)C. E^(@) for Fe^(3+)//Fe^(2+) is +0.77" V " and E^(0) for I_(2)//2I^(-) is +0.536" V". The favourable redox reaction is :

Answer»

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

Solution :(c ) SINCE the reduction POTENTIAL of `Fe^(2+)//Fe^(3+)` is more than that of `l_(2)//L^(-)`, `l^(-)` in the redox reaction. `l^(-)` ions will be oxidised to `l_(2)` at the cost of `Fe^(3+)` ions which will be reduced :
`2Fe^(3+)+2L^(-) to 2Fe^(2+)+l_(2)`


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