Chapter 19, Problem 19.47QP

A silver oxide–zinc cell maintains a fairly constant voltage during discharge (1.60 V). The button form of this cell is used in watches, hearing aids, and other electronic devices. The half-reactions are

$\begin{array}{l}\text{Zn}(s)+2{\text{OH}}^{-}(aq)\stackrel{}{\to }\text{Zn}{(}_{\text{OH}}(s)+2{\text{e}}^{-}\\ {\text{Ag}}_2\text{O}(s)+{\text{H}}_2\text{O}(l)+2{\text{e}}^{-}\stackrel{}{\to }2\text{Ag}(s)+2{\text{OH}}^{-}(aq)\end{array}$

Identify the anode and the cathode reactions. What is the overall reaction in the voltaic cell?