Question

$2Ag^{+}\left(\right.aq\left.\right)+Cu\left(\right.s\left.\right)\rightleftharpoonsCu^{2 +}\left(\right.aq\left.\right)+2Ag\left(\right.s\left.\right)$
The standard potential $E^\circ $ for this reaction is 0.46 V. Which change will increase the potential the most?

• A. Doubling the $\left[\right.Ag^{+}\left]\right.$
• B. Halving the $\left[\right.Cu^{2 +}\left]\right.$
• C. Doubling the size of the Cu(s) electrode
• D. Decreasing the size of the Ag electrode by one-half

Answer 1

Answer: (A)

$E=E^\circ -\frac{0.059}{2}log\frac{\left[\right. C u^{2 +} \left]\right.}{\left[\right. A g^{+} \left]\right.^{2}}$
The cell potential will increase the most by doubling the concentration of $Ag^{+}$ ion.