A : The change in intermal energy does not depend on the path of process.
R : The internal energy of an ideal gas is independent to the configurationof its molecules.

Options

A. If both Assertion & Reason are true and the reason is the correct explantion of the assertion, then mark(1)
B. If both Assertion & Reason are true but the reason is not the correct explanation of the assertion, then mark (2).
C. If Assertion is true statement but Reason is false, then mark (3).
D. If both Assertion and Reason are false statements, then mark (4)

Answer

To solve the assertion-reason question, we will analyze both the assertion (A) and the reason (R) provided.

### Step 1: Analyze the Assertion (A)
The assertion states: "The change in internal energy does not depend on the path of the process."

- **Explanation**: The change in internal energy (ΔU) is a state function. This means that it only depends on the initial and final states of the system, not on how the system transitions from one state to another. Therefore, the assertion is **true**.

### Step 2: Analyze the Reason (R)
The reason states: "The internal energy of an ideal gas is independent of the configuration of its molecules."

- **Explanation**: For an ideal gas, the internal energy is a function of temperature and the number of moles of gas. It can be expressed as ΔU = nCvΔT, where Cv is the specific heat capacity at constant volume, which varies depending on whether the gas is monatomic, diatomic, or polyatomic. Thus, the internal energy does depend on the type of gas and its molecular configuration. Therefore, the reason is **false**.

### Step 3: Conclusion
Since the assertion is true and the reason is false, we conclude that:

- **Assertion (A)**: True
- **Reason (R)**: False

Thus, the correct answer to the question is that the assertion is true, but the reason is false.

### Final Answer
Assertion (A) is true, and Reason (R) is false.

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