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Asked by Altaf Last Modified
Answer In a lead-acid storage battery, such as the lead-acid car battery, the reactions at the cathode and anode during discharge (when the battery is in use) and charging are as follows:
During Discharge:
At the cathode (positive electrode): PbO2(s) + 4H+(aq) + SO4^2-(aq) + 2e^- → PbSO4(s) + 2H2O(l)
At the anode (negative electrode): Pb(s) + SO4^2-(aq) → PbSO4(s) + 2e^-
In simpler terms, during discharge, lead dioxide (PbO2) at the cathode combines with sulfuric acid (H2SO4) and protons (H+) from the acid to form lead sulfate (PbSO4) and water. At the anode, lead (Pb) reacts with sulfate ions (SO4^2-) to form lead sulfate and releases electrons.
During Charging:
At the cathode (positive electrode): PbSO4(s) + 2H2O(l) → PbO2(s) + 4H+(aq) + SO4^2-(aq) + 2e^-
At the anode (negative electrode): PbSO4(s) + 2e^- → Pb(s) + SO4^2-(aq)
During charging, the reactions are essentially reversed. Lead sulfate on the cathode is converted back to lead dioxide, sulfuric acid, and water, while lead sulfate on the anode is converted back to lead and sulfate ions.
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