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

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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

Solution:

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

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