Statement -I : There is no change in enthalpy of an ideal gas during compression at constant temperature.
Statement-II: Enthalpy of an ideal gas is a function of temperature and pressure.

Options

A. Statement-I is true, statement-II is true and statement-II is correct explanation for statement-I
B. Statement-I is true, statement-II is true and statement-II is NOT correct explanation for statement-I
C. Statement -I is false, statement-II is true.
D. Statement-I is true, statement-II is false

Answer

To solve the question, we need to analyze both statements regarding the enthalpy of an ideal gas during compression at constant temperature.

### Step-by-step Solution:

**Step 1: Analyze Statement-I**
- Statement-I claims that there is no change in the enthalpy of an ideal gas during compression at constant temperature.
- For an ideal gas, the enthalpy (H) is given by the equation:
\[ H = U + PV \]
where \(U\) is the internal energy, \(P\) is the pressure, and \(V\) is the volume.
- At constant temperature, the internal energy \(U\) of an ideal gas depends only on temperature and remains constant if the temperature does not change.
- During isothermal compression, while the pressure and volume change, the temperature remains constant, which means the internal energy does not change.
- Since \(H\) also depends on \(U\) and \(PV\) (where \(PV\) changes with pressure and volume), but at constant temperature, the enthalpy change (\(\Delta H\)) can be shown to be zero for an ideal gas.

**Conclusion for Statement-I:**
- Statement-I is **True**.

**Step 2: Analyze Statement-II**
- Statement-II states that the enthalpy of an ideal gas is a function of temperature and pressure.
- For an ideal gas, the enthalpy is primarily a function of temperature alone, as the internal energy is a function of temperature only.
- While pressure can influence the enthalpy in real gases, for an ideal gas, the enthalpy change is independent of pressure at constant temperature.
- Therefore, the enthalpy of an ideal gas does not depend on pressure in the same way it does for real gases.

**Conclusion for Statement-II:**
- Statement-II is **False**.

### Final Conclusion:
- Statement-I is True, and Statement-II is False. Thus, the correct answer is that Statement-I is true and Statement-II is false.

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