Bromine (Br2) reacts with sulfurous acid (H2SO3), producing dithionate ions (S206) and bromide ions, according to the following redox equation: S206" (aq) 4 H* (aq) 2 Br (aq) + 2 H2S03 (aq) Br2(aq) In the above reaction is the H2SO3 acting as an oxidising agent or a reducing agent?

Bromine (Br2) reacts with sulfurous acid (H2SO3), producing dithionate ions (S206) and bromide ions, according to the following redox equation: S206" (aq) 4 H* (aq) 2 Br (aq) + 2 H2S03 (aq) Br2(aq) In the above reaction is the H2SO3 acting as an oxidising agent or a reducing agent?

Chemistry: Principles and Reactions

8th Edition

ISBN:9781305079373

Author:William L. Masterton, Cecile N. Hurley

Publisher:William L. Masterton, Cecile N. Hurley

Chapter3: Mass Relations In Chemistry; Stoichiometry

Section: Chapter Questions

Problem 94QAP: A 100.0-g mixture made up of NaCl03, Na2CO3, NaCl, and NaHCO3 is heated, producing 5.95 g of oxygen,...

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Concept explainers

Stoichiometry

Stoichiometry is a chemical division that evaluates the quantitative content of the chemical process with the help of the reacting molecules or products taking part in the reaction. The term “stoicheion” in “Stoichiometry”, is an old Greek term for "element" whereas “metron” means "measure".

Question

Bromine (Br2) reacts with sulfurous acid (H2SO3), producing dithionate ions (S206-) and bromide ions, according to the following
redox equation:
S206 (aq)
4 H* (aq)
2 Br (aq)
+
2 H2503 (aq)
Br2(aq)
In the above reaction is the H,SO3 acting as an oxidising agent or a reducing agent?

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