Chapter 14, Problem 44QP

The zinc-silver oxide battery, although expensive, is used to power satellite systems because of its light weight. Unbalanced half-reactions that occur in this battery are

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

Which equation represents the oxidation half-reaction? Which represents the reduction half-reaction? Add electrons to the appropriate side of each equation to account for the chance in oxidation number.