I2 and Br2 are added to a solution containing Br– and I– ions. What reaction will occur if,
`I_(2) + 2e^(-) rarr 2I^(-)`, `E^(0) = + 0.54V` and `Br_(2) + 2e^(-) rarr 2Br^(-)`, `E^(0) = +1.09 V?`

Explanation

To solve the problem, we need to analyze the given half-reactions and their standard reduction potentials (E° values) to determine which species will be oxidized and which will be reduced.

### Step 1: Identify the half-reactions and their standard reduction potentials
We have two half-reactions:
1. \( I_2 + 2e^- \rightarrow 2I^- \) with \( E^\circ = +0.54 \, V \)
2. \( Br_2 + 2e^- \rightarrow 2Br^- \) with \( E^\circ = +1.09 \, V \)

### Step 2: Compare the standard reduction potentials
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