The lead-acid battery used in automobiles utilizes the following redox reaction:
PbO₂(s) + Pb (s) + 2 HSO₄^- (aq) + 2 H₃O⁺ (aq) $\rightarrow$ 2 PbSO₄(s) + 4 H₂O (l) E°= 2.04 VWhat mass of H₂ being oxidized by O₂ under standard acid conditions would be required to give the same amount of electrons as one mole of lead oxide?(If needed, refer to Table 17-1 in the text)

Question

The lead-acid battery used in automobiles utilizes the following redox reaction:
PbO₂(s) + Pb (s) + 2 HSO₄^- (aq) + 2 H₃O⁺ (aq)

\rightarrow

2 PbSO₄(s) + 4 H₂O (l) E°= 2.04 VWhat mass of H₂ being oxidized by O₂ under standard acid conditions would be required to give the same amount of electrons as one mole of lead oxide?(If needed, refer to Table 17-1 in the text)

Quizplus · Accepted Answer

The Answer of The lead-acid battery used in automobiles utilizes the following redox reaction: PbO₂(s) + Pb (s) + 2 HSO₄^- (aq) + 2 H₃O⁺ (aq) $\rightarrow$ 2 PbSO₄(s) + 4 H₂O (l) E°= 2.04 VWhat mass of H₂ being oxidized by O₂ under standard acid conditions would be required to give the same amount of electrons as one mole of lead oxide?(If needed, refer to Table 17-1 in the text)

The Lead-Acid Battery Used in Automobiles Utilizes the Following Redox →\rightarrow→

The Lead-Acid Battery Used in Automobiles Utilizes the Following Redox $\rightarrow$