A : The specific heat of an ideal gas is zero in an adiabatic process.
R : Specific heat of a gas is process independent.

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 question, we need to analyze both the assertion (A) and the reason (R) provided.

### Step-by-Step Solution:

1. **Understanding the Assertion (A)**:
- The assertion states that "The specific heat of an ideal gas is zero in an adiabatic process."
- In an adiabatic process, there is no heat exchange with the surroundings (ΔQ = 0).
- The specific heat (C) can be defined as the amount of heat added per unit mass per degree of temperature change. For an adiabatic process, since ΔQ = 0, we can conclude that the specific heat C must also be zero.

2. **Understanding the Reason (R)**:
- The reason states that "Specific heat of a gas is process independent."
- This statement is actually false. The specific heat of a gas can vary depending on the process it undergoes (e.g., constant pressure, constant volume, adiabatic, isothermal). For example, the specific heat at constant pressure (Cp) is different from the specific heat at constant volume (Cv).

3. **Evaluating the Truth of A and R**:
- From our analysis:
- Assertion A is true because specific heat in an adiabatic process is indeed zero.
- Reason R is false because specific heat is not process independent; it varies with the type of thermodynamic process.

4. **Conclusion**:
- Since the assertion is true and the reason is false, we conclude that the correct answer is option 3.

### Final Answer:
The correct answer is 3: Assertion is true, but Reason is false.

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