When a solution of `CHCl_(3)` and acetone is formed, the solution is non-ideal with ………deviation from Raoult's law. The vapour pressure of such a solution will be ………….than the corresponding ideal solution.

Answer

To solve the question regarding the behavior of a solution formed by CHCl₃ (chloroform) and acetone, we need to analyze the interactions between the molecules in the solution and how they deviate from Raoult's law.

### Step-by-Step Solution:

1. **Identify the Components**:
- The solution consists of two components: CHCl₃ (chloroform) and acetone (C₃H₆O).

2. **Understand the Intermolecular Interactions**:
- When CHCl₃ and acetone are mixed, hydrogen bonding occurs between the oxygen atom of acetone and the hydrogen atom of CHCl₃. This interaction is stronger than the individual interactions between the molecules of CHCl₃ (CHCl₃-CHCl₃) and acetone (acetone-acetone).

3. **Determine the Type of Deviation**:
- In solutions where the solute-solvent interactions (AB interactions) are stronger than the solvent-solvent (AA) and solute-solute (BB) interactions, the solution exhibits a negative deviation from Raoult's law. This is because the stronger AB interactions lead to a lower tendency for the molecules to escape into the vapor phase.

4. **Conclude the Effect on Vapor Pressure**:
- Due to the negative deviation from Raoult's law, the vapor pressure of the solution will be lower than that of an ideal solution. This is because the stronger interactions in the solution reduce the number of molecules that can escape into the vapor phase.

5. **Fill in the Blanks**:
- The solution is non-ideal with **negative** deviation from Raoult's law. The vapor pressure of such a solution will be **less** than the corresponding ideal solution.

### Final Answer:
- The solution is non-ideal with **negative** deviation from Raoult's law. The vapor pressure of such a solution will be **less** than the corresponding ideal solution.