Statement-`1`: A real gas behaves as an ideal gas at high temperature and low pressure .
Statement-`2`: Liquid state of an ideal gas is impossible.

Options

A. Statement -`1` is True , Statement -`2` is True , Statement -`2` is correct explanation for Statement - `1`
B. Statement -`1` is True , Statement -`2` is True , Statement -`2` is not correct explanation for Statement - `1`
C. Statement -`1` is True , Statement -`2` is True , Statement -`2` is False.
D. Statement -`1` is False , Statement -`2` is True .

Answer

To analyze the statements provided in the question, we will evaluate each statement individually and then determine their relationship.

### Step 1: Evaluate Statement 1
**Statement 1**: A real gas behaves as an ideal gas at high temperature and low pressure.

- At high temperatures, the kinetic energy of gas molecules increases significantly. This increase in kinetic energy means that the molecules move faster and are less influenced by intermolecular forces.
- At low pressures, the gas molecules are further apart, which reduces the effect of intermolecular attractions and repulsions.
- Therefore, under these conditions (high temperature and low pressure), the behavior of a real gas approaches that of an ideal gas, where the gas follows the ideal gas law (PV = nRT) more closely.

**Conclusion for Statement 1**: True.

### Step 2: Evaluate Statement 2
**Statement 2**: Liquid state of an ideal gas is impossible.

- An ideal gas is defined as a hypothetical gas that perfectly follows the ideal gas law and has no intermolecular forces acting between its molecules.
- Liquefaction (the process of a gas turning into a liquid) requires the presence of intermolecular attractions to bring the molecules close enough together to form a liquid state.
- Since ideal gases do not have intermolecular attractions, they cannot condense into a liquid state.

**Conclusion for Statement 2**: True.

### Step 3: Analyze the Relationship Between the Statements
- Both statements are true, but they address different aspects of gas behavior.
- Statement 1 discusses the conditions under which real gases behave like ideal gases, while Statement 2 explains a fundamental property of ideal gases regarding their inability to exist in a liquid state.
- Therefore, while both statements are true, Statement 2 does not provide a correct explanation for Statement 1. They are independent truths about gas behavior.

### Final Conclusion
- Statement 1: True
- Statement 2: True
- Statement 2 is not a correct explanation for Statement 1.

---