Question

Which of the following statements is correct for a spontaneous polymerization reaction?

• A. \(∆G<0,∆H<0,∆S<0\)
• B. \(∆G<0,∆H>0,∆S>0\)
• C. \(∆G>0,∆H<0,∆S>0\)
• D. \(∆G>0,∆H>0,∆S>0\)

Answer 1

The Correct Option is A

The spontaneity of a chemical reaction, including polymerization, is governed by the Gibbs free energy change (∆G). A spontaneous reaction requires a negative ∆G:

\( \Delta G = \Delta H - T\Delta S \)

where ∆H represents enthalpy change, ∆S is the entropy change, and T is the temperature in Kelvin.

For spontaneous polymerization:

• ∆H<0: The process is exothermic; energy is released as bonds form between monomers.
• ∆S<0: Polymerization creates a more ordered structure from monomers, reducing entropy.

Despite a negative ∆S, the significant negative ∆H ensures a negative ∆G, fulfilling the spontaneity condition. Therefore, the correct answer is:

\( \Delta G<0, \quad \Delta H<0, \quad \Delta S<0 \)