Use the first law of thermodynamics

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

For quasi-static expansion/compression,

$\Delta W = P\,\Delta V$

so for an isobaric process,

$\Delta Q = \Delta U + P\Delta V$

Hence,

$(A)\; \text{Isobaric} \to (IV)$

Isochoric process

In an isochoric process, volume is constant, so

$\Delta V = 0 \implies \Delta W = P\Delta V = 0$

Therefore,

$\Delta Q = \Delta U$

Hence,

$(B)\; \text{Isochoric} \to (II)$

Adiabatic process

In an adiabatic process, no heat is exchanged:

$\Delta Q = 0$

Hence,

$(C)\; \text{Adiabatic} \to (III)$

Isothermal process

In an isothermal process for an ideal gas, temperature remains constant, so internal energy does not change:

$\Delta U = 0$

Therefore from the first law,

$\Delta Q = \Delta W$

Hence,

$(D)\; \text{Isothermal} \to (I)$

Final matching

$(A)-(IV),\ (B)-(II),\ (C)-(III),\ (D)-(I)$

This corresponds to Option B.