The electrochemical reaction which powers a lead-acid storage battery is as follows:
Pb(s) + PbO₂(s) + 4H⁺(aq) + 2SO₄^2-(aq) $\to$ 2PbSO₄(s) + 2H₂O(l)
A single cell of this battery consists of a Pb electrode and a PbO₂ electrode,each submerged in sulfuric acid.What reaction occurs at the cathode during discharge?

Question

The electrochemical reaction which powers a lead-acid storage battery is as follows:
Pb(s) + PbO₂(s) + 4H⁺(aq) + 2SO₄^2-(aq)

\to

2PbSO₄(s) + 2H₂O(l)
A single cell of this battery consists of a Pb electrode and a PbO₂ electrode,each submerged in sulfuric acid.What reaction occurs at the cathode during discharge?

Quizplus · Accepted Answer

During discharge, the PbO2 electrode (also known as the positive electrode or the anode) releases oxygen and becomes PbSO4. The Pb electrode (also known as the negative electrode or the cathode) gains electrons and becomes PbSO4. This reaction can be represented as:
PbO2(s) + Pb(s) + 2H2SO4(aq) → 2PbSO4(s) + 2H2O(l) + O2(g)
At the cathode, PbO2 is reduced to PbSO4 and loses electrons, while Pb is oxidized to PbSO4 and gains electrons. Therefore, the correct choice is B: PbOSO4 is reduced to PbSO4.

The Electrochemical Reaction Which Powers a Lead-Acid Storage Battery Is →\to→

The Electrochemical Reaction Which Powers a Lead-Acid Storage Battery Is $\to$