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Annonn Annonn
wrote...
Posts: 116
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A month ago
The following is the overall reaction that occurs during discharge of a lead-acid battery:
PbO2(s) + Pb(s) + 2HSO4-(aq) + 2H+(aq) → 2PbSO4(s) + 2H2O(l)

What is the correctly balanced anode half reaction for the battery?

PbO2(s) + SO42-(aq)  + 2e-→ 2PbSO4(s)

Pb(s) + HSO4-(aq) → PbSO4(s) + H+(aq) + 2e-

PbO2(s) + HSO4-(aq) + 3H+(aq) + 2e- → PbSO4(s) + 2H2O(l)

Pb(s) + HSO4-(aq) + 2e- → PbSO4(s) + H+(aq)

PbO2(s) + HSO4-(aq) + 3H+(aq) → PbSO4(s) + 2H2O(l) + 2e-
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Valued Member
A month ago
Solution given down
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