Question
Using the standard electrode potentials given in the Table, predict if the reaction between the following is feasible:
✓
Answer
The possible reaction between Ag+(aq) + Cu(s) is given by,
$2\text{Ag}^+_{(\text{aq})}+\text{Cu}_{(\text{s})}\rightarrow2\text{Ag}_{(\text{s})}+\text{Cu}^{2+}_{(\text{aq})}$
$\text{Oxidation half equation:}\ \ \ \ \ \ \ \ \text{Cu}_{(\text{s})}\xrightarrow{\ \ \ \ \ }\text{Cu}^{2+}_{(\text{aq})}+2\text{e}^-;\ \ \text{E}^\circ=-0.34\text{V}\\\text{Reduction half equation:}\ \ [\text{Ag}^+_{(\text{aq})}+\text{e}^-\xrightarrow{\ \ \ \ \ }\text{Ag}_{(\text{s})}]\times2;\ \ \ \text{E}^\circ=+0.80\text{V}\\\overline{\ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ }\\\ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ 2\text{Ag}^+_{(\text{aq})}+\text{Cu}_{(\text{s})}\xrightarrow{\ \ \ \ \ }2\text{Ag}_{(\text{s})}+\text{Cu}^{2+};\ \ \ \text{E}^\circ=+0.46\text{V}$
E° positive for the overall reaction is positive. Hence, the reaction between Ag+(aq) and Cu(s) is feasible.
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