The van der Waals' equation accounts for :

Options

A. the intermolecular forces only
B. the actual volume of the molecules only
C. both the intermolecular forces and the molecular volume
D. neither the intermolecular forces nor the molecular volume.

Answer

**Step-by-Step Solution:**

1. **Understanding the Question:**
The question asks what the van der Waals' equation accounts for in the context of real gases. We need to identify the factors that the equation corrects for compared to the ideal gas law.

2. **Identifying the Components of the van der Waals Equation:**
The van der Waals equation is given by:
\[ \left(P + \frac{a n^2}{V^2}\right)(V - nB) = nRT \]
- Here, \(P\) is the pressure of the gas.
- \(V\) is the volume of the gas.
- \(n\) is the number of moles.
- \(R\) is the universal gas constant.
- \(T\) is the temperature.
- \(a\) and \(b\) are constants specific to each gas.

3. **Analyzing the Corrections Made by the Equation:**
- The term \(\frac{a n^2}{V^2}\) accounts for the **attractive forces** between gas molecules (intermolecular forces).
- The term \(nB\) accounts for the **volume occupied by the gas molecules** themselves (intermolecular volume).

4. **Conclusion:**
The van der Waals equation accounts for both the intermolecular forces and the volume occupied by the gas molecules. Therefore, the correct answer to the question is that it accounts for **both the intermolecular forces and the intermolecular volume**.

**Final Answer:**
The van der Waals' equation accounts for both the intermolecular forces and the intermolecular volume.

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