`I_(2)` and `Br_(2)` are added to a solution containing `I^(-)` and `Br^(-)` ions. As solution `I^(-) and Br^(-)` ions, each with a concentration of 1M. What reactions would occur if `I_(2) and Br_(2)` are added to this solution ?
`["Given : "I_(2)+2e rarr 2I^(-)," "E^(@)=0.54V and Br_(2)+2e rarr 2Br^(-), E^(@)=+1.08V]`

Explanation

Two possible reduction half - reactions are :
`Br_(2)(l)+2e rarr Br^(-)(aq), E^(@)=1.08V`
`I_(2)(s)+2e rarr 2I^(-)(aq), E^(@)=0.54V`
The oxidising agent of half - reaction with a high standard reduction potential is strong. Therefore in the above half - reactions, `Br_(2)` is the stronger oxidising agent and `I^(-)` is the stronger reducing agent. In a spontaneous redox reaction, a stronger oxidising reacts with stronger reducing agents agent to form a weaker oxidising and a weaker reducing agent. Hence, `Br_(2)` will react with `I^(-)` spontaneously to from `Br^(-) and I_(2)`.
`Br_(2)(l)+2I^(-)(aq)rarr 2Br^(-)(aq)+I_(2)(s)`