Match List - I with List - II.

List-I	List-II
(A) Spontaneous process	(I) $$\Delta H < 0$$
(B) Process with $$\Delta P = 0, \Delta T = 0$$	(II) $$\Delta G_{T,P} < 0$$
(C) $$\Delta H_{reaction}$$	(III) Isothermal and isobaric process
(D) Exothermic Process	(IV) [Bond energies in reactants] - [Bond energies in products]

Choose the correct answer from the options given below

We need to match chemical thermodynamics concepts from List-I with List-II.

Consider (A) the spontaneous process: a process is spontaneous when the Gibbs free energy change is negative at constant temperature and pressure, i.e., $$\Delta G_{T,P} < 0$$. This matches with (II).

Next, the process with $$\Delta P = 0, \Delta T = 0$$ indicates constant pressure and constant temperature, defining an isothermal and isobaric process. This corresponds to (III).

For (C), the reaction enthalpy $$\Delta H_{reaction}$$ can be calculated using bond energies as: $$\Delta H_{reaction}$$ = [Bond energies in reactants] - [Bond energies in products]. This matches with (IV). In contrast, an exothermic process releases heat, meaning $$\Delta H < 0$$, which corresponds to (I).

Therefore, the final matching is A → (II), B → (III), C → (IV), and D → (I). The correct answer is Option B.