Chapter 19, Problem 7E

The following sketch is of a voltaic cell consisting or two standard electrodes tor two metals, M and N.

   $\begin{array}{l}{\text{M}}^{\text{z+}}\left(\text{aq}\right)+{\text{ze}}^{\text{-}}\to M\left(s\right)E°M*\text{*/M}\\ {\text{M}}^{\text{z+}}\left(\text{aq}\right)+{\text{ze}}^{\text{-}}\to \text{M}\left(\text{s}\right)E{°}_{M**/M}\end{array}$

Use the standard reduction potentials of these halfreactions to answer the questions that follow:

   ${\text{Ag}}^{\text{+}}\left(\text{aq}\right)+e^{-}\to \text{Ag}\left(s\right)$

   $Z{n}^{2+}\left(\text{aq}\right)+2{\text{e}}^{\text{-}}\to \text{Zn}\left(\text{s}\right)$

   ${\text{Cu}}^{\text{2+}}\left(\text{aq}\right){\text{+2e}}^{\text{-}}\to \text{Cu}\left(\text{s}\right)$

   ${\text{Al}}^{\text{3+}}\left(\text{aq}\right)+3e^{-}\to \text{Al}\left(\text{s}\right)$

a. Determine which pair of these half-cell reactions with the largest positive cell potential, and calculate its value.
b. Determine which pair of thses haplf-cell reactions leads to the cell potenital, and caluclate its value. Which couple is at the anode and which is at the cathode?