Which of the following represents correcty the changes in thermodynamic properties during the formation of 1 mole of an ideal binary solution :

Options

A.
B.
C.
D.

Answer

To solve the question regarding the changes in thermodynamic properties during the formation of 1 mole of an ideal binary solution, we will analyze the changes in Gibbs free energy (ΔG), entropy (ΔS), and enthalpy (ΔH).

### Step-by-Step Solution:

1. **Understanding the Formation of an Ideal Solution**:
- An ideal binary solution is formed when a solute and a solvent are mixed. In this case, we assume that the interactions between the solute and solvent are similar to the interactions between the solute-solute and solvent-solvent.

2. **Change in Gibbs Free Energy (ΔG)**:
- The formation of a solution is generally a spontaneous process. For a spontaneous process, the change in Gibbs free energy (ΔG) is negative.
- Therefore, we can conclude that:
\[ \Delta G < 0 \]

3. **Change in Entropy (ΔS)**:
- Entropy is a measure of randomness or disorder in a system. When a solute is dissolved in a solvent, the number of particles in the solution increases, leading to greater randomness.
- Thus, the change in entropy (ΔS) is positive:
\[ \Delta S > 0 \]

4. **Change in Enthalpy (ΔH)**:
- For an ideal solution, it is assumed that there is no heat absorbed or released during the mixing process. This means that the change in enthalpy (ΔH) is zero:
\[ \Delta H = 0 \]

5. **Summary of Thermodynamic Changes**:
- Based on the analysis:
- ΔG < 0 (negative)
- ΔS > 0 (positive)
- ΔH = 0 (zero)

6. **Identifying the Correct Option**:
- Now, we need to find the option that correctly represents these changes. The correct representation should indicate that ΔG is negative, ΔS is positive, and ΔH is zero.

### Conclusion:
The correct representation of the changes in thermodynamic properties during the formation of 1 mole of an ideal binary solution is:
- ΔG < 0
- ΔS > 0
- ΔH = 0