A copper rod $(C{u}_{(s)})$ and a $A\frac{g_{(s)}}{A}gC{l}_{(s)}$ rod were immersed in an aqueous solution of $0\mathrm{.}01MCuC{l}_{2(aq)}.$ The two rods were then electrically connected through a voltmeter.

a$.$ Write the cell reaction.

b$.$ Calculate the cell potential under standard conditions.

c$.$ What would be the reading of the voltmeter at the first moment of connection $($assume ideal behavior$).$

d$.$ Describe what actually happens in the above cell.

e$.$ How do you expect the cell potential to change with time? Explain your answer.

f$.$ Calculate the final concentration of $C{u}^{2+}$ when equilibrium has been reached.

g$.$ What experiment do you suggest doing to measure $S$ of the reaction? What sign do you expect $S$ to have? Explain your answer.

$C{u}^{2+}+2e^{-}Cu,E^0=+0\mathrm{.}340V$

$AgC{l}_{(s)}+1e^{-}A{g}_{(s)}+C{l}_{(aq)},E^0=+0\mathrm{.}2224V$