Sulfur dioxide (SO2) is oxidized to sulfuric acid (H2SO4) during the chemical reaction, despite the addition of hydrogen atoms. The oxidation state of sulfur changes from +4 in SO2 to +6 in H2SO4, indicating that oxidation occurs. The discussion clarifies that the addition of oxygen atoms plays a crucial role in this process, as oxygen is an electron acceptor while hydrogen acts as an electron donor. Therefore, the conversion from SO2 to H2SO4 is correctly classified as oxidation.
PREREQUISITESChemistry students, educators, and professionals involved in chemical engineering or environmental science who seek to deepen their understanding of oxidation-reduction reactions and sulfuric acid production.
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.