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Iodine (I(2)) and bromine (Br(2)) are ad...

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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To solve the problem, we need to analyze the reactions involving iodine `(I2)` and bromine `(Br2)` in a solution containing iodine `(I^(-))` and bromide `(Br^(-))` ions. We will use the given standard electrode potentials to determine which species will be reduced and which will be oxidized. ### Step-by-Step Solution: 1. **Identify the Reactions**: - The reduction half-reaction for bromine is: \[ Br_2 + 2e^- \rightarrow 2Br^- ...
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