Chemistry

Chemistry

Problem

When the engine of a vehicle containing a lead–acid battery is running, the lead–acid battery is charged up by the following reactions: anode: PbSO4(s)+2H2O(l)→PbO2(s)+2e−+4H+(aq)+SO42−(aq)\text{PbSO}_4(\text{s}) + 2\text{H}_2\text{O}(\text{l}) \rightarrow \text{PbO}_2(\text{s}) + 2\text{e}^- + 4\text{H}^+(\text{aq}) + \text{SO}_4^{2-}(\text{aq}) cathode: PbSO4(s)+2e−→Pb(s)+SO42−(aq)\text{PbSO}_4(\text{s}) + 2\text{e}^- \rightarrow \text{Pb}(\text{s}) + \text{SO}_4^{2-}(\text{aq}) Lead(II) sulfate occurs as an insoluble coating on the surface of both metal electrodes.

Browse the problem library