Use the first law of thermodynamics

$\Delta Q = \Delta U + \Delta W$

where:

• $\Delta Q$ = heat supplied to the system
• $\Delta W$ = work done by the system
• $\Delta U$ = change in internal energy

Match each process with its defining condition

(I) Adiabatic

In an adiabatic process, no heat is exchanged.

$\Delta Q = 0$

So,

$\text{(I)} \to (2)$

(II) Isothermal

In an isothermal process, temperature remains constant. For an ideal gas, internal energy depends only on temperature, so:

$\Delta U = 0$

Hence,

$\text{(II)} \to (4)$

(III) Isochoric

In an isochoric process, volume remains constant, so no work is done:

$\Delta W = 0$

Therefore,

$\text{(III)} \to (1)$

(IV) Isobaric

In an isobaric process, pressure remains constant. In general, heat supplied, work done, and change in internal energy are all non-zero.

So,

$\Delta U \ne 0,\quad \Delta W \ne 0,\quad \Delta Q \ne 0$

Hence,

$\text{(IV)} \to (3)$

Final matching

Compare with options

This corresponds to Option B.