Electrode reactions and changes in a lead storage battery during discharge and recharge

1. A.
   $\text{Pb(s)}$ is reduced
2. B.
   $\text{H}_2\text{SO}_4$ is consumed
3. C.
   $\text{PbSO}_4$ is consumed
4. D.
   $\text{PbO}_2$ is produced

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1. A.
   $\text{PbSO}_4(s) + 2e^- \to \text{Pb}(s) + \text{SO}_4^{2-}(aq)$
2. B.
   $\text{Pb}(s) + \text{SO}_4^{2-}(aq) \to \text{PbSO}_4(s) + 2e^-$
3. C.
   $\text{PbO}_2(s) + 4\text{H}^+(aq) + \text{SO}_4^{2-}(aq) + 2e^- \to \text{PbSO}_4(s) + 2\text{H}_2\text{O}(l)$
4. D.
   $\text{PbSO}_4(s) + 2\text{H}_2\text{O}(l) \to \text{PbO}_2(s) + 4\text{H}^+(aq) + \text{SO}_4^{2-}(aq) + 2e^-$

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1. A.
   $\ Pb$ is oxidised to ${PbSO}_{4}$
2. B.
   $\ {PbSO}_{4}$ is oxidised to ${PbO}_{2}$
3. C.
   $\ {PbSO}_{4}$ is reduced to Pb
4. D.
   $\ {PbO}_{2}$ is reduced to ${PbSO}_{4}$

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1. A.
   $\mathrm{SO_2}$ is evolved
2. B.
   Pb is formed
3. C.
   $\mathrm{H_2SO_4}$ is consumed
4. D.
   $\mathrm{PbSO_4}$ is consumed

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1. A.
   increases by 1
2. B.
   decreases by 1
3. C.
   increases by 2
4. D.
   decreases by 2

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1. A.
   $\mathrm{PbO_{2(s)} + 4H^+_{(aq.)} + SO_4^{2-}{}_{(aq.)} + 2e^- \rightarrow Pb_{(s)} + PbSO_{4(s)} + 2H_2O_{(\ell)}}$
2. B.
   $\mathrm{PbO_{2(s)} + 4H^+\ 2e^- \rightarrow Pb^{2+} + 2H_2O_{(\ell)}}$
3. C.
   $\mathrm{Pb_{(s)} + SO_4^{2-}{}_{(aq.)} \rightarrow PbSO_{4(s)} + 2e^-}$
4. D.
   $\mathrm{PbSO_{4(s)} + 2e^- \rightarrow Pb_{(s)} + SO_4^{2-}{}_{(aq.)}}$

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