Question:
In the following reaction, which choice has value twice that of the equivalent weight of the oxidising agent?
\[
\text{SO}_2 + 2\text{H}_2\text{O} \rightarrow \text{S} + 2\text{H}_2\text{O}_2
\]
In the following reaction, which choice has value twice that of the equivalent weight of the oxidising agent?
\[ \text{SO}_2 + 2\text{H}_2\text{O} \rightarrow \text{S} + 2\text{H}_2\text{O}_2 \]
\[ \text{SO}_2 + 2\text{H}_2\text{O} \rightarrow \text{S} + 2\text{H}_2\text{O}_2 \]
Show Hint
The equivalent weight of an oxidizing agent is the mass that can provide one mole of electrons in a redox reaction.
Updated On: Apr 22, 2026
- \( 16 \, \text{g of H}_2\text{O} \)
- \( 10 \, \text{g of O}_2 \)
- \( 32 \, \text{g of O}_2 \)
- \( 64 \, \text{g of H}_2\text{O} \)
Show Solution
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The Correct Option is D
Solution and Explanation
Step 1: Determine the equivalent weight of the oxidizing agent.
The oxidizing agent in this reaction is \( \text{SO}_2 \), and its equivalent weight is determined by the amount of oxygen it can provide in the reaction. The reaction shows that 1 mole of \( \text{SO}_2 \) is reduced to 1 mole of sulfur (S), and 2 moles of \( \text{H}_2\text{O} \) are converted to 2 moles of \( \text{H}_2\text{O}_2 \), with oxygen being released. The equivalent weight of \( \text{SO}_2 \) is the molar mass divided by the number of electrons transferred in the reaction. Since 2 electrons are involved, the equivalent weight of \( \text{SO}_2 \) is half of its molar mass.
Step 2: Find the choice that has twice the equivalent weight.
The molar mass of \( \text{SO}_2 \) is 64 g/mol, so the equivalent weight is: \[ \frac{64}{2} = 32 \, \text{g} \] The choice with twice the equivalent weight is \( 64 \, \text{g of H}_2\text{O} \), which corresponds to option (4).
Step 3: Conclusion.
The correct answer is \( 64 \, \text{g of H}_2\text{O} \), which is option (4).
The oxidizing agent in this reaction is \( \text{SO}_2 \), and its equivalent weight is determined by the amount of oxygen it can provide in the reaction. The reaction shows that 1 mole of \( \text{SO}_2 \) is reduced to 1 mole of sulfur (S), and 2 moles of \( \text{H}_2\text{O} \) are converted to 2 moles of \( \text{H}_2\text{O}_2 \), with oxygen being released. The equivalent weight of \( \text{SO}_2 \) is the molar mass divided by the number of electrons transferred in the reaction. Since 2 electrons are involved, the equivalent weight of \( \text{SO}_2 \) is half of its molar mass.
Step 2: Find the choice that has twice the equivalent weight.
The molar mass of \( \text{SO}_2 \) is 64 g/mol, so the equivalent weight is: \[ \frac{64}{2} = 32 \, \text{g} \] The choice with twice the equivalent weight is \( 64 \, \text{g of H}_2\text{O} \), which corresponds to option (4).
Step 3: Conclusion.
The correct answer is \( 64 \, \text{g of H}_2\text{O} \), which is option (4).
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