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Redox Reactions — Chemistry STD 11 Science — Question

Gujarat BoardEnglish MediumSTD 11 ScienceChemistryRedox Reactions3 Marks
Question
Using the standard electrode potentials given in the Table, predict if the reaction between the following is feasible:

$\mathrm{Fe}^{3+}(\mathrm{aq})$ and $\mathrm{l}^{-}(\mathrm{aq})$.
✓

Answer

The possible reaction between $\mathrm{Fe}^{3+}(\mathrm{aq})$ and $\mathrm{l}^{-}(\mathrm{aq})$. 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.

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