Assertion: Compressibility factor `(Z)` for non ideal gases is always greater than `1`.
Reason: Non-ideal gases always exert higher pressure than expected.

Options

A. If both (`A`) and (`R`) are correct and (`R`) is the correct explanation of (`A`).
B. If both (`A`) and (`R`) are correct, but (`R`) is not the correct explanation of (`A`).
C. If (`A`) is correct, but (`R`) is incorrect.
D. Both (`A`) and (`R`) are incorrect.

Explanation

To solve the assertion and reasoning question, we will analyze both the assertion and the reason provided.

### Step-by-Step Solution:

1. **Understanding the Assertion**:
- The assertion states that the compressibility factor \( Z \) for non-ideal gases is always greater than 1.
- The compressibility factor \( Z \) is defined as:
\[ Z = \frac{PV}{nRT} \]
- For ideal gases, \( Z = 1 \). For non-ideal gases, \( Z \) can be either greater than 1 or less than 1 depending on the interactions between gas molecules.

2. **Analyzing the Compressibility Factor**:
- If \( Z > 1 \), it indicates that the gas is less compressible than an ideal gas, often due to repulsive forces between molecules.
- If \( Z < 1 \), it indicates that the gas is more compressible than an ideal gas, often due to attractive forces between molecules.
- Therefore, the assertion that \( Z \) is always greater than 1 is incorrect.

3. **Understanding the Reason**:
- The reason states that non-ideal gases always exert higher pressure than expected.
- In the van der Waals equation for real gases, the pressure is modified by a term that accounts for intermolecular forces:
\[ P + \frac{a n^2}{V^2} = \frac{nRT}{V - nb} \]
- Here, \( a \) accounts for attractive forces, and \( b \) accounts for the volume occupied by gas molecules.
- While non-ideal gases can exert higher pressure due to repulsive forces, there are conditions under which the pressure can be lower than expected due to attractive forces dominating.
- Thus, the reason that non-ideal gases always exert higher pressure than expected is also incorrect.

4. **Conclusion**:
- Since both the assertion and the reason are incorrect, the correct answer is that both A and R are incorrect.

### Final Answer:
Both the assertion and the reason are incorrect.

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