The discussion centers on the oxidation reaction of sulfur dioxide (SO2) to sulfuric acid (H2SO4). Participants explore the chemical processes involved, questioning whether the transformation should be classified as oxidation or reduction, particularly in light of the addition of hydrogen and oxygen atoms.
Participants express disagreement regarding the classification of the reaction as oxidation or reduction. Multiple competing views remain, with some supporting oxidation based on oxidation states and others advocating for reduction based on the addition of hydrogen.
Participants reference formal oxidation states and the roles of different elements in the reaction, but there are unresolved assumptions regarding the definitions of oxidation and reduction in this context.
I meant previously it was SO2(no hydrogen atom) and then it became H2SO4 (two hydrogen atoms)so it should be reduction why it is written in my textbook that SO2 is oxidised when it get converted into H2SO4?Borek said:I don't think I have ever heard about a method of producing sulfuric acid that uses hydrogen, can you elaborate?
gracy said:I meant previously it was SO2(no hydrogen atom) and then it became H2SO4 (two hydrogen atoms)so it should be reduction
Ok.So two hydrogen atoms and two oxygen atom ,so tie then why oxidation not reduction?Borek said:Why do you ignore two added oxygen atoms?
So we should say sulfur is oxidized rather than SO2 is oxidized.Bystander said:Formal oxidation states for oxygen are always -2. Minus eight for oxygen, plus two for two hydrogens, leaves plus six for sulfur. Compare that to plus four for sulfur in sulfur dioxide, and the sulfur has been further oxidized.
gracy said:Ok.So two hydrogen atoms and two oxygen atom ,so tie then why oxidation not reduction?
OK I understood.Bystander said:The starting state is sulfur dioxide, and it has been further oxidized.