In van der Waals equation of state for a non-ideal gas , the term that accounts for intermolecular forces is

Options

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

Answer

To solve the question regarding the Van der Waals equation of state for a non-ideal gas, we will follow these steps:

### Step-by-Step Solution:

1. **Understand the Van der Waals Equation**:
The Van der Waals equation is a modification of the ideal gas law to account for the behavior of real gases. The equation is given by:
\[ \left( P + \frac{a}{V_m^2} \right) (V_m - b) = RT \]
where \( P \) is the pressure, \( V_m \) is the molar volume, \( T \) is the temperature, \( R \) is the universal gas constant, \( a \) is a measure of the attractive forces between particles, and \( b \) is the volume occupied by the gas particles themselves.

2. **Identify the Terms**:
In the equation, the term \( \frac{a}{V_m^2} \) accounts for the intermolecular forces. The parameter \( a \) is specifically included to correct for the attractive forces between gas molecules, which are not considered in the ideal gas law.

3. **Conclusion**:
Therefore, the term that accounts for intermolecular forces in the Van der Waals equation is \( \frac{a}{V_m^2} \).

4. **Final Answer**:
The answer to the question is the term \( \frac{a}{V_m^2} \).