The reactions in a lead-acid battery are Positive terminal: (mathrm{PbO}_{2}+mathrm{HSO}_{4}^{-}+3 mathrm{H}^{+}+2 mathrm{e}^{-} ightarrow) [mathrm{PbSO}_{4}+2 mathrm{H}_{2} mathrm{O}]

The reactions in a lead-acid battery are Positive terminal: \(\mathrm{PbO}_{2}+\mathrm{HSO}_{4}^{-}+3 \mathrm{H}^{+}+2 \mathrm{e}^{-} \rightarrow\)

\[\mathrm{PbSO}_{4}+2 \mathrm{H}_{2} \mathrm{O}\]

Negative terminal: \(\quad \mathrm{HSO}_{4}^{-}+\mathrm{Pb} \rightarrow \mathrm{PbSO}_{4}+\mathrm{H}^{+}+2 \mathrm{e}^{-}\)

If a certain battery supplies \(1.0 \times 10^{8}\) electrons per second to the negative terminal and the battery contains 3. 00 moles of electrolytic solution (which means the solution contains 3. 00 moles of \(\mathrm{HSO}_{4}^{-}\)), what fraction of the solution undergoes a chemical reaction each second? \(\cdot\)\(\cdot\)