`CH_3-Cl+NaI overset("Acetone")iff CH_3-I+NACl`
Above equilibrium is more towards right because

Options

A. Nal s more reaction than NaCl
B. `CH_(3)` is more reactive than `CH_(3)`Cl
C. NaCl is less soluble than Nal in acetone
D. It is Finkelstein's reaction

Answer

To understand why the equilibrium of the reaction \( CH_3-Cl + NaI \overset{\text{Acetone}}{\iff} CH_3-I + NaCl \) shifts towards the right, we can analyze the factors involved in this reaction step by step.

### Step-by-Step Solution:

1. **Understanding the Reaction**:
The reaction involves the substitution of chlorine in methyl chloride (\( CH_3-Cl \)) with iodine from sodium iodide (\( NaI \)), resulting in the formation of methyl iodide (\( CH_3-I \)) and sodium chloride (\( NaCl \)).

2. **Lattice Energy vs. Solvation Energy**:
- **Lattice Energy** is the energy required to break the ionic lattice of a compound. It is influenced by the charge and size of the ions.
- **Solvation Energy** is the energy released when ions are solvated or dissolved in a solvent.

3. **Comparison of Lattice Energies**:
- For \( NaCl \) and \( NaI \):
- The lattice energy of \( NaCl \) is greater than that of \( NaI \) because the chloride ion (\( Cl^- \)) is smaller than the iodide ion (\( I^- \)). Therefore, \( NaCl \) has a stronger ionic bond due to the smaller size of \( Cl^- \), leading to higher lattice energy.

4. **Solvation in Acetone**:
- When these salts are dissolved in acetone, the solvation energy plays a crucial role.
- The solvation energy of \( NaI \) is greater than its lattice energy, allowing it to dissolve easily in acetone.
- Conversely, the solvation energy of \( NaCl \) is less than its lattice energy, making it less soluble in acetone, which can lead to the precipitation of \( NaCl \).

5. **Le Chatelier's Principle**:
- According to Le Chatelier's principle, if a system at equilibrium is subjected to a change, the system will adjust to counteract that change.
- As \( NaCl \) precipitates out of the solution, the equilibrium shifts to the right to produce more \( NaCl \) and thus favors the formation of \( CH_3-I \).

6. **Conclusion**:
- The reaction proceeds in the forward direction because \( NaI \) is soluble in acetone, while \( NaCl \) precipitates out, driving the equilibrium towards the formation of \( CH_3-I \).

### Final Answer:
The equilibrium shifts towards the right because the solvation energy of \( NaI \) is greater than its lattice energy, allowing it to dissolve easily in acetone, while \( NaCl \) precipitates due to its higher lattice energy compared to its solvation energy.