1.

Consider the change in oxidation state of Bromine corredponding to different emf values as shown in the diagram below : . The the species undergoing dispropprtionation is .A. `BrO_(3)^(-)`B. `BrO_(4)^(-)`C. `Br_(2)`D. `HBrO`

Answer» Correct Answer - D
disproprotionation involves oxidation as well as reaction of the same element
`{:("Species","O.N. of Br"),( B r O_(4)^(-),+7),(BrO_(3)^(-),+5),(HBrO,+1),(Br_(2),0),(Br^(-),-1):}`
`E_(cell)^(@)` corresopinding to compound undergoing disproporitonation reactioin should be positive so that the reaction is spontaneous `(DeltaG^(@)=-2FE^(@))`
`overset(+5)(BrO_(3))underset(1.5V)overset("oxidation")larroberset(+1)(HBrO)underset(1.59V)overset("reduction")tooverset(0)(Br_(2))`
`E_(cell)^(@)=E_(R)^(@)-E_(L)^(@)`
`=(1.595V)-(1.5V)`
`=0.095V`
Since `E_(cell)^(@)` is +ve, `DeltaG^(@)` will be negative i.e., HBrO will undergo disproportionation reaction.


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