When a silver spoon is kept in an aqueous solution of copper sulphate (CuSO₄), a chemical reaction occurs, resulting in the following observations:

1. Silver spoon turns brownish-red:

* The silver spoon will develop a reddish-brown coating as copper metal is deposited onto its surface. This is because silver is more reactive than copper.

* The reaction is a single displacement reaction where silver (Ag) displaces copper (Cu) from the copper sulphate solution.

2. Blue color of the solution fades:

* The blue color of the copper sulphate solution will gradually fade as the copper ions (Cu²⁺) are reduced to copper metal and deposited on the silver spoon.

3. Formation of Silver ions:

* As silver replaces copper in the solution, silver ions (Ag⁺) are released into the solution.

Here's the chemical equation representing the reaction:

```

2Ag(s) + CuSO₄(aq) → Cu(s) + Ag₂SO₄(aq)

```

Explanation:

* Reactants:

* Silver (Ag) - the silver spoon

* Copper sulphate (CuSO₄) - the aqueous solution

* Products:

* Copper (Cu) - deposited on the silver spoon

* Silver sulphate (Ag₂SO₄) - dissolved in the solution

In summary:

The silver spoon acts as a reducing agent, accepting electrons from copper ions and becoming coated with copper metal. The copper ions lose their blue color as they are reduced, and the solution becomes less blue. Silver ions are released into the solution, causing a change in the composition of the solution.