In the van der Waals equation
`(P + (n^(2)a)/(V^(2)))(V - nb) = nRT`
the constant a reflects the actual volume of the gas molecules.

Explanation

To solve the question regarding the van der Waals equation and the constants \( a \) and \( b \), we will analyze the equation step by step.

### Step 1: Understand the van der Waals equation
The van der Waals equation is given by:
\[ \left( P + \frac{n^2 a}{V^2} \right) (V - nb) = nRT \]
Here, \( P \) is the pressure, \( V \) is the volume, \( n \) is the number of moles, \( R \) is the universal gas constant, and \( T \) is the temperature.

### Step 2: Identify the constants \( a \) and \( b \)
In the van der Waals equation:
- The constant \( a \) accounts for the attractive forces between gas molecules. It corrects the pressure term to account for these intermolecular attractions.
- The constant \( b \) represents the volume occupied by the gas molecules themselves. It is often referred to as the "excluded volume," which is the volume that cannot be occupied by other gas molecules due to the presence of the gas molecules themselves.

### Step 3: Analyze the statement
The statement claims that "the constant \( a \) reflects the actual volume of the gas molecules." This is incorrect. Instead, it is the constant \( b \) that reflects the actual volume occupied by the gas molecules.

### Step 4: Conclusion
Thus, the statement is false. The correct interpretation is:
- Constant \( a \): Reflects the magnitude of attractive forces between gas molecules.
- Constant \( b \): Reflects the actual volume of the gas molecules (the excluded volume).

### Final Answer
The statement is false because constant \( a \) reflects the intermolecular forces of attraction, while constant \( b \) reflects the actual volume of the gas molecules.

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