Iodine `(I_(2))` and bromine `(Br_(2))` are added to a solution containing iodine and bromide `(Br^(-))` ions. What reaction would occur if the concentration of each species is 1M? The electrode potentials for the reaction are: `E_(I_(2)//I^(-))^(@)=0.54V,E_(Br_(2)//Br^(-))^(@)=1.08V`

Iodine `(I_(2))` and bromine `(Br_(2))` are added to a solution contai

1.	Iodine `(I_(2))` and bromine `(Br_(2))` are added to a solution containing iodine and bromide `(Br^(-))` ions. What reaction would occur if the concentration of each species is 1M? The electrode potentials for the reaction are: `E_(I_(2)//I^(-))^(@)=0.54V,E_(Br_(2)//Br^(-))^(@)=1.08V`
Answer» The reaction can be either `Br_(2)+2I^(-)to2Br^(-)+I_(2)` or `I_(2)+2Br^(-)to2I^(-)+Br_(2)` For 1st reaction, E.M.F.`=E_(Br_(2)//Br^(-))^(@)-E_(I_(2)//I^(-))^(@)=1.08-0.54=0.54V` For 2nd reaction, E.M.F.`=E_(I_(2)//I^(-))^(@)-E_(Br_(2)//Br^(-))^(@)=0.54-1.08=-0.54V` As E.M.F. is positive for the 1st reaction, hence the cell reaction is `Br_(2)+2I^(-)to2Br^(-)+I_(2)`.

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Iodine `(I_(2))` and bromine `(Br_(2))` are added to a solution containing iodine and bromide `(Br^(-))` ions. What reaction would occur if the concentration of each species is 1M? The electrode potentials for the reaction are: `E_(I_(2)//I^(-))^(@)=0.54V,E_(Br_(2)//Br^(-))^(@)=1.08V`

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