Statement-1: The amount of work done in the isothermal expansion is greater than work done in the adiabatic system for same final volume.
Statement-2: In the adiabatic expansion of a gas temperature and pressure both decrease due to decrease in internal energy of the system.

Options

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

Explanation

To solve the problem, we need to analyze both statements and their implications regarding isothermal and adiabatic processes.

### Step-by-step Solution:

1. **Understanding Isothermal Expansion**:
- In an isothermal process, the temperature of the system remains constant. According to the ideal gas law, for a fixed amount of gas, the product of pressure (P) and volume (V) remains constant (PV = constant).
- The work done (W) during an isothermal expansion from volume V1 to V2 can be calculated using the formula:
\[ W = nRT \ln\left(\frac{V_2}{V_1}\right) \]
- Here, \(n\) is the number of moles, \(R\) is the gas constant, and \(T\) is the absolute temperature.

2. **Understanding Adiabatic Expansion**:
- In an adiabatic process, there is no heat exchange with the surroundings. The relationship between pressure and volume is given by:
\[ PV^\gamma = \text{constant} \]
- Here, \(\gamma\) (gamma) is the heat capacity ratio (C_p/C_v).
- The work done during adiabatic expansion can be calculated, but it is generally less than that of isothermal expansion for the same change in volume because the internal energy of the gas decreases, leading to a drop in temperature and pressure.

3. **Comparison of Work Done**:
- When comparing the work done in both processes for the same final volume, the area under the PV curve for the isothermal process is larger than that for the adiabatic process.
- This is because, in isothermal expansion, the gas does work by absorbing heat from the surroundings, while in adiabatic expansion, the gas does work at the expense of its internal energy.

4. **Evaluating Statement-1**:
- Statement-1 claims that the work done in isothermal expansion is greater than that in adiabatic expansion for the same final volume. This is true based on the analysis above.

5. **Evaluating Statement-2**:
- Statement-2 states that in adiabatic expansion, both temperature and pressure decrease due to a decrease in internal energy.
- This is also true because, in an adiabatic process, the gas does work on the surroundings, which results in a decrease in internal energy, leading to a drop in temperature and pressure.

6. **Conclusion**:
- Both statements are true, and Statement-2 correctly explains Statement-1. Therefore, the correct answer is that both statements are true, and Statement-2 supports Statement-1.

### Final Answer:
Both Statement-1 and Statement-2 are true, and Statement-2 explains Statement-1.

---