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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:

$\mathrm{Ag}(\mathrm{s})$ and $\mathrm{Fe}^{3+}(\mathrm{aq})$
✓

Answer

The possible reaction between $\mathrm{Ag}(\mathrm{s})$ and $\mathrm{Fe}^{3+}(\mathrm{aq})$ is given by, $\text{Ag}_{(\text{s})}+2\text{Fe}^{3+}_{(\text{aq})}\rightarrow\text{Ag}^{+}_{(\text{aq})}+\text{Fe}^{2+}_{(\text{aq})}$ $\text{Oxidation half equation:}\ \ \ \ \ \ \ \text{Ag}_{(\text{s})}\xrightarrow{\ \ \ \ \ \ }\text{Ag}^{+}_{(\text{aq})}+\text{e}^-;\ \ \text{E}^\circ=-0.80\text{V}\\\text{Reduction half equation:}\ \ \text{Fe}^{3+}_{(\text{aq})}+\text{e}^-\xrightarrow{\ \ \ \ \ }\text{Fe}^{2+}_{(\text{aq})};\ \ \ \ \ \ \ \ \text{E}^\circ=+0.77\text{V}\\\overline{\ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ }\\\ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \text{Ag}^{}_{(\text{s})}+\text{Fe}^{3+}_{(\text{aq})}\xrightarrow{\ \ \ \ \ }\text{Ag}^{+}_{(\text{aq})}+\text{Fe}^{2+}_{(\text{aq})};\ \ \ \text{E}^\circ=-0.03\text{V}$Here, E° for the overall reaction is negative. Hence, the reaction between $\mathrm{Ag}(\mathrm{s})$ and $\mathrm{Fe}^{3+}(\mathrm{aq})$ is not feasible.

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