Chapter 14, Problem 42QP

The reaction that occurs in a lead-acid battery is as follows:

$\text{Zn}\left(s\right)+{\text{2MnO}}_{\text{2}}\left(s\right)+2{\text{NH}}_4^{+}\left(aq\right)\to {\text{Zn}}^{\text{2+}}\left(aq\right)+{\text{Mn}}_{\text{2}}{\text{O}}_3\left(s\right)+2{\text{NH}}_{\text{3}}\left(aq\right)+{\text{H}}_{\text{2}}\text{O}\left(l\right)$

What gets oxidized in this battery? What gets reduced? What is the oxidizing agent? What is the reducing agent?