Table of Contents
- 1 How can SO2 act as both oxidizing as well as reducing agent but it prefers to show reducing behavior more?
- 2 Why SO2 can act as oxidizing as well as reducing agent but SO3 can act as oxidizing agent only?
- 3 Can SO2 be an oxidizing agent?
- 4 Can so2 be oxidized and reduced?
- 5 Is SO2 a reducing agent?
- 6 Is H2SO4 a reducing agent or an oxidizing agent?
- 7 What is the oxidation number of sulphur in H2SO4?
How can SO2 act as both oxidizing as well as reducing agent but it prefers to show reducing behavior more?
SO2 can act as both oxidizing as well as reducing agent since it has +4 oxidation state which is exactly between its highest oxidation state +6 and lowest oxidation state +2 ,Thus it can change its oxidation number either from +4 to-2(reduction) and +4 to+6 (oxidation) .
Why SO2 can act as both oxidising and reducing agent?
Why SO2 can act as oxidising as well as reducing agent but H2S act as only reducing agent. In SO2, S is in oxidation state with +4 charge and the highest oxidation state is +6. So, it acts as both oxidising as well as reducing agent. Therefore, it acts only as a reducing agent.
Why SO2 can act as oxidizing as well as reducing agent but SO3 can act as oxidizing agent only?
=> This is because in SO2 , Sulphur has vacant d orbital but this is not so in SO3 . Hence it acts only as an oxidizer . If SO3 acted as a reducing agent , it would achieve an oxidation higher than what is already has in SO3 . Thus, it can act only as an oxidizing agent.
Is H2SO4 an oxidizing agent or reducing agent?
it is always an oxidizing agent. In H2SO4 sulphur is in +6 oxidation state. As sulphur is already in it’s maximum possible oxidation state in H2SO4, further loss of electrons is not possible. So it can’t act as a reducing agent.
Can SO2 be an oxidizing agent?
The sulfur dioxide acts as a reducing agent as well as an oxidizing agent.
Why H2SO4 Cannot act as reducing agent?
Sulphur cannot increase its oxidation number beyond +6.
Can so2 be oxidized and reduced?
Reduction of higher oxides 2 CaSO4 + 2 SiO2 + C → 2 CaSiO3 + 2 SO2 + CO.
Why so2 is a reducing agent?
i) Sulphur dioxide is reducing agent because sulphur has d-orbital so it can easily expand its oxidation state +4 to +6 and thus behave as reducing agent.
Is SO2 a reducing agent?
Can no act as both oxidising and reducing agent?
Hydrogen peroxide (H2O2) acts as both oxidising and reducing agent.
Is H2SO4 a reducing agent or an oxidizing agent?
Answer Wiki. It’s always an oxidizing agent. In H2SO4 sulphur is in +6 oxidation state. To act a a reducing agent one should lose electrons i.e; the atom should go from lower positive oxidation state to higher positive oxidation state.
Why is sulphur an oxidising agent in s O2?
In S O2, sulphur having oxidation state +4 so it can lose its two more electrons to attain +6 oxidation state. Therefore it can lose and gain electron therefore it acts as oxidising as well as reducing agent.
What is the oxidation number of sulphur in H2SO4?
In H2SO4 sulphur is in +6 oxidation state. To act a a reducing agent one should lose electrons i.e; the atom should go from lower positive oxidation state to higher positive oxidation state.
What is the difference between h2h2s and SO2?
H2S acts only as reducing agent while SO2 can act both as reducing agent and oxidising agent.