Using standard electrode potentials, predict the reaction, if any, that ocurs between `Fe^(3+)(aq) and I^(-)(aq)`
`E_(Fe^(3+)(aq)//Fe^(2+)(aq))^(@)=0.77V,E_(I_(2)//2I^(-)(aq))^(@)=0.54V`

Explanation

To predict the reaction between \( \text{Fe}^{3+}(aq) \) and \( \text{I}^-(aq) \) using standard electrode potentials, we will follow these steps:

### Step 1: Identify the half-reactions and their standard electrode potentials
We have the following half-reactions and their standard electrode potentials:
1. Reduction of \( \text{Fe}^{3+} \) to \( \text{Fe}^{2+} \):
\[ \text{Fe}^{3+} + e^- \rightarrow \text{Fe}^{2+} \quad E^\circ = 0.77 \, \text{V} \]
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