`I_(2)` and ` F_(2)` are added to a solution containing 1M each of `I^(-) and F^(-)`. What reaction will take place? Given that the reduction potential of `I_(2) and F_(2)` are 0.54 volt and 2.87 volts respectively.

Explanation

To determine the reactions that will take place when \( I_2 \) and \( F_2 \) are added to a solution containing 1M each of \( I^- \) and \( F^- \), we need to analyze the reduction potentials of the species involved.

### Step 1: Identify the half-reactions and their reduction potentials
The half-reactions and their standard reduction potentials are as follows:
- For iodine:
\[ I_2 + 2e^- \rightarrow 2I^- \quad E^\circ = 0.54 \, \text{V} \]
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