Simple behaviour under all conditions of real gas is governed by the equation

Options

A. `pV=muRT`
B. `(p+(a)/V^(2))(V-b)=muRT`
C. `pV="constant"`
D. `pV^(gamma)="constant" `

Explanation

To determine the equation that governs the simple behavior of real gases under all conditions, we need to analyze the options provided.

### Step-by-Step Solution:

1. **Understanding the Options**:
- The first option refers to the ideal gas equation, which is \( PV = nRT \). This equation is applicable to ideal gases but does not accurately describe real gases under all conditions, especially at high pressures and low temperatures.

2. **Evaluating the Second Option**:
- The second option presents the equation \( (P + \frac{a}{V^2})(V - b) = RT \). This is known as the Van der Waals equation, which accounts for the volume occupied by gas molecules (b) and the intermolecular forces (a). This equation is specifically designed to describe the behavior of real gases under various conditions, making it a strong candidate.

3. **Examining the Third Option**:
- The third option states \( PV = \text{constant} \), which applies to isothermal processes for an ideal gas. This does not represent the behavior of real gases under all conditions.

4. **Looking at the Fourth Option**:
- The fourth option \( PV^\gamma = \text{constant} \) describes an adiabatic process, which is also specific to ideal gases and does not apply to real gases in general.

5. **Conclusion**:
- After evaluating all options, the second option, which is the Van der Waals equation, is the correct answer. It accurately describes the behavior of real gases under various conditions.

### Final Answer:
The equation that governs the simple behavior of real gases under all conditions is the Van der Waals equation:
\[ (P + \frac{a}{V^2})(V - b) = RT \]