Question:
One mole of aqueous $ \text{SO}_3^{2-} $ is completely reacted with 2 moles of $ \text{Br}_2 (l) $. What is the oxidation state (s) of S in the product formed?
One mole of aqueous $ \text{SO}_3^{2-} $ is completely reacted with 2 moles of $ \text{Br}_2 (l) $. What is the oxidation state (s) of S in the product formed?
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Oxidation reactions often involve an increase in oxidation states. Check the change in oxidation number to identify the correct oxidation state.
Updated On: May 9, 2025
- \( 0, +5 \)
- \( +6 \)
- \( -2, +4 \)
- \( +4 \)
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The Correct Option is B
Solution and Explanation
In the reaction, \( \text{SO}_3^{2-} \) is oxidized to \( \text{SO}_4^{2-} \), where sulfur is in the +6 oxidation state. Since there is no reduction of sulfur in this case, the oxidation state of sulfur in the product is \( +6 \).
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