Using the standard electrode potentials given in Table, predict if the reaction between the following is feasible`:`
` Fe^(3+)(aq)` and `I^(c-)(aq)`

Explanation

To determine if the reaction between \( \text{Fe}^{3+}(aq) \) and \( \text{I}^-(aq) \) is feasible, we can follow these steps:

### Step 1: Identify the half-reactions
The reaction involves the reduction of \( \text{Fe}^{3+} \) to \( \text{Fe}^{2+} \) and the oxidation of iodide ions \( \text{I}^- \) to iodine \( \text{I}_2 \).

1. **Reduction half-reaction**:
\[ \text{Fe}^{3+}(aq) + e^- \rightarrow \text{Fe}^{2+}(aq) \]

2. **Oxidation half-reaction**:
\[ 2 \text{I}^-(aq) \rightarrow \text{I}_2(s) + 2 e^- \]

### Step 2: Find the standard electrode potentials
From standard electrode potential tables, we can find the values for these half-reactions:

- For the reduction of \( \text{Fe}^{3+} \):
\[ E^\circ(\text{Fe}^{3+}/\text{Fe}^{2+}) = +0.77 \, \text{V} \]

- For the oxidation of iodide:
\[ E^\circ(\text{I}_2/\text{I}^-) = -0.54 \, \text{V} \]
(Note: The standard potential for the oxidation half-reaction is the negative of the reduction potential.)

### Step 3: Calculate the standard cell potential
The standard cell potential \( E^\circ_{\text{cell}} \) can be calculated using the formula:
\[ E^\circ_{\text{cell}} = E^\circ_{\text{cathode}} - E^\circ_{\text{anode}} \]
Here, \( \text{Fe}^{3+}/\text{Fe}^{2+} \) is the cathode (reduction) and \( \text{I}_2/\text{I}^- \) is the anode (oxidation).

Substituting the values:
\[ E^\circ_{\text{cell}} = E^\circ(\text{Fe}^{3+}/\text{Fe}^{2+}) - E^\circ(\text{I}_2/\text{I}^-) \]
\[ E^\circ_{\text{cell}} = 0.77 \, \text{V} - (-0.54 \, \text{V}) = 0.77 \, \text{V} + 0.54 \, \text{V} = 1.31 \, \text{V} \]

### Step 4: Determine feasibility
A positive \( E^\circ_{\text{cell}} \) indicates that the reaction is feasible (spontaneous). Since \( E^\circ_{\text{cell}} = 1.31 \, \text{V} \) is positive, the reaction between \( \text{Fe}^{3+}(aq) \) and \( \text{I}^-(aq) \) is indeed feasible.

### Conclusion
The reaction between \( \text{Fe}^{3+}(aq) \) and \( \text{I}^-(aq) \) is feasible.

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