When sulphur dioxide (SO₂) gas is passed through a hydrogen sulphide (H₂S) solution, a chemical reaction occurs. Based on the provided reference, hydrogen sulfide reacts with sulphur dioxide to form water and Sulphur. This is a significant reaction often demonstrated in chemistry to show the oxidizing and reducing properties of these compounds.
The Chemical Reaction Explained
This reaction is a classic example of an oxidation-reduction (redox) process. Sulphur dioxide acts as an oxidizing agent, while hydrogen sulphide acts as a reducing agent. The sulphur atoms in both reactant molecules change their oxidation states, resulting in the formation of elemental sulphur.
The overall transformation involves the conversion of the two gases (when dissolved) into liquid water and solid sulfur.
Products Formed
The key products of this reaction are:
- Water (H₂O): A common liquid product.
- Sulphur (S): Elemental sulphur is formed. It typically appears as a yellow precipitate, meaning it's a solid that separates from the solution.
Chemical Equation
The balanced chemical equation representing this reaction is:
SO₂(g) + 2H₂S(aq) → 3S(s) + 2H₂O(l)- SO₂(g): Sulphur Dioxide gas (often bubbled through the solution)
- H₂S(aq): Hydrogen Sulphide dissolved in water (aqueous solution)
- S(s): Solid Sulphur (precipitate)
- H₂O(l): Liquid Water
Reaction Summary
| Reactants | Products | Observation |
|---|---|---|
| Sulphur Dioxide | Sulphur | Formation of yellow |
| Hydrogen Sulphide | Water | precipitate |
Passing sulphur dioxide through hydrogen sulphide solution leads to a visible change as solid sulphur forms and settles out of the solution.
