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Questions
Using the standard electrode potentials, predict if the reaction between the following is feasible:
\[\ce{Ag^+_{ (aq)}}\] and Cu(s)
Using the standard electrode potentials, predict the reaction, if any, that occurs between the following:
\[\ce{Ag^+_{ (aq)}}\] and Cu(s)
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Solution
A reaction is feasible if the value of \[\ce{E{^{\circ}_{cell}}}\] is positive.
According to the question, the reaction is as follows:
\[\ce{Cu_{(s)} + Ag^+_{ (aq)} -> Cu^+_{ (aq)} + Ag_{(s)}}\]
According to this, the cell will be as follows:
\[\ce{Cu_{(s)} | Cu{^{2+}_{(aq)}} || Ag{^+_{(aq)}} | Ag_{(s)}}\]
∴ \[\ce{E^{\circ}_{cell} = E^{\circ}_{Ag^+/Ag} - E^{\circ}_{Cu^{2+}/Cu}}\]
= 0.80 − 0.34
= 0.46 V
Since the value of \[\ce{E{^{\circ}_{cell}}}\] is positive, the reaction is feasible.
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