1. We match each statement in List-I with the thermodynamic process in List-II.

2. (A) Pressure varies inversely with volume of an ideal gas.

For an ideal gas in an isothermal process, temperature remains constant, so $PV = \text{constant}$ Thus, $P \propto \frac{1}{V}$ So, (A) $\to$ (III) Isothermal process.

3. (B) Heat absorbed goes partly to increase internal energy and partly to do work.

From the first law of thermodynamics, $\Delta Q = \Delta U + W$ In an isobaric process (constant pressure), when heat is supplied, part of it increases internal energy and part is used in expansion work. So, (B) $\to$ (IV) Isobaric process.

4. (C) Heat is neither absorbed nor released by a system.

This is the definition of an adiabatic process: $Q = 0$ So, (C) $\to$ (I) Adiabatic process.

5. (D) No work is done on or by a gas.

Work done by a gas is $W = \int P\, dV$ If volume does not change, $dV=0$, hence $W=0$ This is an isochoric process. So, (D) $\to$ (II) Isochoric process.

6. Final matching:

• $A \to III$
• $B \to IV$
• $C \to I$
• $D \to II$

This corresponds to Option D.

7. Comparison with stored answer

Stored correct answer: D

Our derived answer: D

Hence, the answer agrees with the stored correct answer.