Assertion: In van der Waals equation `(P+(a)/(V^(2)))(V-b)=RT` pressure correction `(a//V^(2))` is due to the force of attraction between molecules.
Reason: Volume of gas molecule cannot be neglected due to force of attraction.

Options

A. If both (`A`) and (`R`) are correct and (`R`) is the correct explanation of (`A`).
B. If both (`A`) and (`R`) are correct, but (`R`) is not the correct explanation of (`A`).
C. If (`A`) is correct, but (`R`) is incorrect.
D. If (`A`) is incorrect, but (`R`) is correct.

Explanation

To solve the given question, we will analyze the assertion and the reason provided, and determine their correctness based on the principles of the van der Waals equation.

### Step-by-Step Solution:

1. **Understanding the van der Waals Equation**:
The van der Waals equation is given by:
\[ \left(P + \frac{a}{V^2}\right)(V - b) = RT \]
Here, \(P\) is the pressure, \(V\) is the volume, \(T\) is the temperature, \(R\) is the universal gas constant, \(a\) is a constant that accounts for the attractive forces between molecules, and \(b\) is a constant that accounts for the volume occupied by the gas molecules themselves.

2. **Analyzing the Assertion**:
The assertion states that the pressure correction term \(\frac{a}{V^2}\) in the van der Waals equation is due to the force of attraction between molecules. This is correct because the term \(\frac{a}{V^2}\) accounts for the attractive forces that reduce the pressure exerted by the gas compared to an ideal gas.

3. **Analyzing the Reason**:
The reason states that the volume of gas molecules cannot be neglected due to the force of attraction. This statement is incorrect. While the volume of gas molecules is indeed taken into account in the van der Waals equation (represented by the term \(b\)), it is not directly related to the force of attraction. The force of attraction is represented by the constant \(a\), while the volume consideration is separate.

4. **Conclusion**:
- The assertion is **correct**: the pressure correction \(\frac{a}{V^2}\) is indeed due to intermolecular attractions.
- The reason is **incorrect**: the volume of gas molecules is not neglected due to the force of attraction; rather, it is a separate consideration in the van der Waals equation.

Thus, we can conclude that the assertion is true, and the reason is false.

### Final Answer:
- Assertion: True
- Reason: False