Which of the following is correct for repulsive process in real gas ?

Options

A. `Z gt 1`, repulsive forces are dominating
B. `Z lt 1`, repulsive forces are dominating
C. short range interaction
D. long range interactin

Explanation

To solve the question regarding the correct statement for the repulsive process in real gases, we will analyze the compressibility factor (Z) and its implications.

### Step-by-Step Solution:

1. **Understanding the Compressibility Factor (Z)**:
- The compressibility factor (Z) is defined as:
\[ Z = \frac{PV_{\text{real}}}{RT} \]
- Here, \(P\) is the pressure, \(V_{\text{real}}\) is the volume of the real gas, \(R\) is the universal gas constant, and \(T\) is the temperature.

2. **Effect of Temperature on Kinetic Energy**:
- When the temperature of a gas increases, the kinetic energy of the gas molecules also increases.
- Increased kinetic energy results in greater movement of the molecules.

3. **Molecular Movement and Repulsion**:
- As the kinetic energy increases, the molecules tend to move apart from each other.
- This increased separation leads to a repulsive interaction between the molecules.

4. **Volume Considerations**:
- In a repulsive process, as the molecules move apart, the actual volume occupied by the gas becomes greater than the volume predicted by the ideal gas law.
- Therefore, the actual volume (\(V_{\text{actual}}\)) becomes greater than the volume of the real gas (\(V_{\text{real}}\)).

5. **Implications for the Compressibility Factor (Z)**:
- Since \(V_{\text{actual}} > V_{\text{real}}\), it follows that:
\[ Z = \frac{PV_{\text{real}}}{RT} > 1 \]
- This indicates that for a repulsive process in real gases, the compressibility factor (Z) is greater than 1.

6. **Conclusion**:
- Therefore, the correct statement for the repulsive process in real gases is:
\[ \text{Option A: } Z > 1 \]

### Final Answer:
The correct answer is **Option A: Z > 1**.