Using the standard electrode potentials given in the Table, predi…

Question

Using the standard electrode potentials given in the Table, predict if the reaction between the following is feasible:

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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