Question:
What is the oxidation state of S in the sulphur containing product of the following reaction?
$\mathrm{SO}_3^{2-} (aq) + \mathrm{Br}_2(l) + \mathrm{H}_2O \to$
What is the oxidation state of S in the sulphur containing product of the following reaction?
$\mathrm{SO}_3^{2-} (aq) + \mathrm{Br}_2(l) + \mathrm{H}_2O \to$
$\mathrm{SO}_3^{2-} (aq) + \mathrm{Br}_2(l) + \mathrm{H}_2O \to$
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Track oxidation numbers to identify products in redox reactions.
Updated On: May 19, 2025
- $+6$
- $+4$
- $+2.5$
- $+2$
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The Correct Option is A
Solution and Explanation
Sulfur in $\mathrm{SO}_3^{2-}$ is +4; bromine oxidizes S to +6 in product
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