In Vander Waal’s equation of state for a non-ideal gas, the term that accounts for intermolecular forces is

Options

A. (V - b)
B. (RT)-1
C. `(P + (a)/(V^(2)))`
D. RT

Answer

To solve the question regarding the term in Van der Waals equation that accounts for intermolecular forces, we can follow these steps:

### Step-by-Step Solution:

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

2. **Identify the Terms**:
In this equation, the term \(\frac{a n^2}{V^2}\) is added to the pressure \(P\). This term accounts for the attractive forces between the gas molecules.

3. **Explain the Role of the Term**:
The term \(\frac{a n^2}{V^2}\) represents the correction for intermolecular forces. In an ideal gas, we assume no intermolecular forces, but in real gases, these forces affect the pressure exerted by the gas on the walls of the container.

4. **Conclusion**:
Therefore, the term that accounts for intermolecular forces in the Van der Waals equation is:
\[ \frac{a n^2}{V^2} \]

### Final Answer:
The term that accounts for intermolecular forces in Van der Waals equation is \(\frac{a n^2}{V^2}\).

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