Question:
What happens during the discharge of a lead storage battery?
What happens during the discharge of a lead storage battery?
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On discharge both plates turn to PbSO4 and sulfuric acid is used up.
Updated On: Oct 1, 2026
- \(\text{SO}_2\) is evolved
- Pb is formed
- \(\text{H}_2\text{SO}_4\) is consumed
- \(\text{PbSO}_4\) is consumed
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The Correct Option is C
Solution and Explanation
Step 1: Understanding the Concept:
In a lead storage battery the anode is Pb and the cathode is \(\text{PbO}_2\), both dipping in dilute \(\text{H}_2\text{SO}_4\).
Step 2: Detailed Explanation:
Overall discharge reaction:
\[ \text{Pb} + \text{PbO}_2 + 2\text{H}_2\text{SO}_4 \rightarrow 2\text{PbSO}_4 + 2\text{H}_2\text{O} \]
Sulfuric acid is used up, which also lowers the density of the electrolyte.
No \(\text{SO}_2\) gas is produced. Pb is a reactant, not a product, during discharge. \(\text{PbSO}_4\) is formed on discharge, and consumed only during recharging.
Step 3: Final Answer:
\(\text{H}_2\text{SO}_4\) is consumed, option (C).
Final Answer:
Discharge uses up sulfuric acid. \[ \boxed{\text{(C) }\text{H}_2\text{SO}_4\ \text{is consumed}} \]
In a lead storage battery the anode is Pb and the cathode is \(\text{PbO}_2\), both dipping in dilute \(\text{H}_2\text{SO}_4\).
Step 2: Detailed Explanation:
Overall discharge reaction:
\[ \text{Pb} + \text{PbO}_2 + 2\text{H}_2\text{SO}_4 \rightarrow 2\text{PbSO}_4 + 2\text{H}_2\text{O} \]
Sulfuric acid is used up, which also lowers the density of the electrolyte.
No \(\text{SO}_2\) gas is produced. Pb is a reactant, not a product, during discharge. \(\text{PbSO}_4\) is formed on discharge, and consumed only during recharging.
Step 3: Final Answer:
\(\text{H}_2\text{SO}_4\) is consumed, option (C).
Final Answer:
Discharge uses up sulfuric acid. \[ \boxed{\text{(C) }\text{H}_2\text{SO}_4\ \text{is consumed}} \]
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