Question
Using the standard electrode potentials given in the Table, predict if the reaction between the following is feasible:
Fe3+(aq) and I-(aq).
Fe3+(aq) and I-(aq).
✓
Answer
The possible reaction between Fe3+(aq) + I-(aq) is given by, $2\text{Fe}^{3+}_{(\text{aq})}+2\text{I}^-_{(\text{aq})}\rightarrow2\text{Fe}^{2+}_{(\text{aq})}+\text{I}_{2(\text{s})}$
$\text{Oxidation half equation:}\ \ \ \ \ \ \ \ \ \ 2\text{I}^-_{(\text{aq})}\xrightarrow{\ \ \ \ \ \ \ }\text{I}_{2(\text{s})}+2\text{e}^-;\ \ \text{E}^\circ=-0.54\text{V}\\\text{Reduction half equation:}\ [\text{Fe}^{3+}_{(\text{aq})}+\text{e}^-\xrightarrow{\ \ \ \ \ \ }\text{Fe}^{2+}_{(\text{aq})}]\times2;\ \ \text{E}^\circ=+0.77\text{V}\\\overline{\ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ }\\ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ 2\text{Fe}^{3+}_{(\text{aq})}+2\text{I}^-_{(\text{aq})}\xrightarrow{\ \ \ \ \ \ \ \ }2\text{Fe}^{2+}_{(\text{aq})}+\text{I}_{2(\text{s})};\ \ \text{E}^\circ=+0.23\text{V}$
E° for the overall reaction is positive. Thus, the reaction between
$\text{Fe}^{3+}_{(\text{aq})}$ and $\text{I}^-_{(\text{aq})}$ is feasible.Need a full question paper?
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