Question
Using the standard electrode potentials given in the Table, predict if the reaction between the following is feasible:
Ag(s) and Fe3+(aq).
Ag(s) and Fe3+(aq).
✓
Answer
The possible reaction between Ag(s) and Fe3+(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 Ag(s) and Fe3+(aq) is not feasible.
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