Consider the following statements
I. In an isothermal process for an ideal gas, `triangleV=0`
II.In an isothermal expansion, `triangleW=0`.Choose the correct option.

Options

A. Statement I Is correct
B. Statement II Is correct
C. Both the statements are correct
D. Both the statements are Incorrect

Answer

To solve the problem, we need to analyze the two statements given regarding isothermal processes in ideal gases.

### Step 1: Understand the Isothermal Process
An isothermal process is defined as a thermodynamic process in which the temperature remains constant. For an ideal gas, this means that the internal energy change (ΔU) is zero because ΔU depends only on temperature for an ideal gas.

### Step 2: Analyze Statement I
The first statement claims that in an isothermal process for an ideal gas, ΔV = 0.
- **Analysis**: This statement is incorrect. While the temperature is constant, the volume can change. According to the ideal gas law (PV = nRT), if the temperature (T) is constant and the pressure (P) changes, the volume (V) must also change to maintain the equation. Therefore, ΔV is not necessarily zero.

### Step 3: Analyze Statement II
The second statement claims that in an isothermal expansion, ΔW = 0.
- **Analysis**: This statement is also incorrect. In an isothermal expansion, work done (W) is given by the formula W = nRT ln(V_final/V_initial). Since V_final is greater than V_initial in an expansion, the work done is positive and not zero. Therefore, ΔW is not zero.

### Conclusion
Both statements are incorrect.

### Final Answer
Both statements are wrong.