Chapter 18, Problem 18.139CP

Consider the following half-reactions and values:

$\begin{array}{l}{\text{Ag}}^{+}\left(aq\right)+{\text{e}}^{-}\to \text{Ag}\left(s\right)E^{°}=0.80\text{V}\\ {\text{Cu}}^{+}\left(aq\right)+2{\text{e}}^{-}\to \text{Cu}\left(s\right)E^{°}=0.34\text{V}\\ {\text{Pb}}^{2+}\left(aq\right)+2{\text{e}}^{-}\to \text{Pb}\left(s\right)E^{°}=-0.13\text{V}\end{array}$

(a) Which Of these metals or ions is the strongest oxidizing agent? Which is the strongest reducing agent?

(b) The half-reactions can be used to construct three different galvanic cells. Tell which cell delivers the highest voltage, identify the anode and cathode, and tell the direction of electron and ion flow.

(c) Write the cell reaction for part (b), and calculate the values of $E°$ , $△G°$ (in kilojoules), and K for this reaction at $25°\text{C}$ .

(d) Calculate the voltage for the cell in part (b) if both ion concentrations are 0.010 M.