During recharge, the reaction at the cathode is A. $\text{Pb(s)} + \text{SO}_4^{2-}(aq) \rightarrow \text{PbSO}_4(s) + 2e^-$ B. $\text{PbSO}_4(s) + 2e^- \rightarrow \text{Pb(s)} + \text{SO}_4^{2-}(aq)$ C. $\text{Pb(s)} + \text{SO}_4^{2-}(aq) + 4\text{H}^+ + 2e^- \rightarrow \text{PbSO}_4(s) + 2\text{H}_2\text{O}(l)$ D. $\text{PbSO}_4(s) + 2\text{H}_2\text{O}(l) \rightarrow \text{PbO}_2(s) + \text{SO}_4^{2-}(aq) + 4\text{H}^+(aq) + 2e^-$

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During recharge, the reaction at the cathode is A - VCE - SSCE Chemistry - Question 12 - 2021 - Paper 1

Question 12

During recharge, the reaction at the cathode is A. $\text{Pb(s)} + \text{SO}_4^{2-}(aq) \rightarrow \text{PbSO}_4(s) + 2e^-$ B. $\text{PbSO}_4(s) + 2e^- \rightarr... show full transcript

Worked Solution & Example Answer:During recharge, the reaction at the cathode is A - VCE - SSCE Chemistry - Question 12 - 2021 - Paper 1

Step 1

A. Pb(s) + SO₄²⁻(aq) → PbSO₄(s) + 2e⁻

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Answer

This reaction represents the discharge of the battery rather than the recharge that occurs at the cathode.

Step 2

B. PbSO₄(s) + 2e⁻ → Pb(s) + SO₄²⁻(aq)

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Answer

This reaction correctly reflects the reduction of lead sulfate to lead at the cathode during recharge.

Step 3

C. Pb(s) + SO₄²⁻(aq) + 4H⁺ + 2e⁻ → PbSO₄(s) + 2H₂O(l)

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Answer

This is not the correct reaction for the cathode; it depicts a different scenario involving proton exchange.

Step 4

D. PbSO₄(s) + 2H₂O(l) → PbO₂(s) + SO₄²⁻(aq) + 4H⁺(aq) + 2e⁻

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Answer

This is the correct reaction occurring at the cathode during recharge of the lead-acid battery.

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