Balance the following oxidation-reduction reactions, which occur in acidic solution, using the half-reaction method.

a. \(\mathrm{Cu}(s)+\mathrm{NO}_{3}{ }^{-}(a q) \longrightarrow \mathrm{Cu}^{2+}(a q)+\mathrm{NO}(g)\)

b. \(\mathrm{Cr}_{2} \mathrm{O}_{7}{ }^{2-}(a q)+\mathrm{Cl}^{-}(a q) \longrightarrow \mathrm{Cr}^{3+}(a q)+\mathrm{Cl}_{2}(g)\)

c. \(\mathrm{Pb}(s)+\mathrm{PbO}_{2}(s)+\mathrm{H}_{2} \mathrm{SO}_{4}(a q) \longrightarrow \mathrm{PbSO}_{4}(s)\)

d. \(\mathrm{Mn}^{2+}(a q)+\mathrm{NaBiO}_{3}(s) \longrightarrow \mathrm{Bi}^{3+}(a q)+\mathrm{MnO}_{4}{ }^{-}(a q)\)

e. \(\mathrm{H}_{3} \mathrm{AsO}_{4}(a q)+\mathrm{Zn}(s) \longrightarrow \mathrm{AsH}_{3}(g)+\mathrm{Zn}^{2+}(a q)\)

f. \(\mathrm{As}_{2} \mathrm{O}_{3}(s)+\mathrm{NO}_{3}{ }^{-}(a q) \longrightarrow \mathrm{H}_{3} \mathrm{AsO}_{4}(a q)+\mathrm{NO}(g)\)

g. \(\mathrm{Br}^{-}(a q)+\mathrm{MnO}_{4}^{-}(a q) \longrightarrow \mathrm{Br}_{2}(l)+\mathrm{Mn}^{2+}(a q)\)

h. \(\mathrm{CH}_{3} \mathrm{OH}(a q)+\mathrm{Cr}_{2} \mathrm{O}_{7}{ }^{2-}(a q) \longrightarrow \mathrm{CH}_{2} \mathrm{O}(a q)+\mathrm{Cr}^{3+}(a q)\)