In thermodynamics, a spontaneous reaction is one that occurs naturally without needing to be driven by external forces. The spontaneity of a reaction is primarily determined by the Gibbs free energy change (∆G). For a reaction to be spontaneous, the Gibbs free energy change must be negative (i.e., ∆G<0 ). The Gibbs free energy is related to the enthalpy change (∆H) and the entropy change (∆S) by the equation: ∆G=∆H−T∆S where T is the absolute temperature in Kelvin. For polymerization reactions, typically they involve the formation of long-chain molecules from smaller monomer units. During this process: Enthalpy Change (∆H) : Generally, polymerization reactions are exothermic (release heat), so ∆H is often negative. Entropy Change (∆S) : Polymerization leads to a decrease in randomness since individual monomers form a more ordered polymer. Therefore, ∆S is usually negative. Given that a spontaneous reaction requires ∆G<0, and considering the typical characteristics of polynomial reactions, the correct conditions should be: ‌∆G<0 ‌∆H<0 ‌∆S<0 So, option A ∆G<0,∆H<0,∆S<0 is the correct one for a spontaneous polymerization reaction.