The spontaneity of a chemical reaction, including polymerization, is determined by the Gibbs free energy change (∆G). For a reaction to be spontaneous, ∆G must be negative:
\( \Delta G = \Delta H - T\Delta S \)
where ∆H is the enthalpy change, ∆S is the entropy change, and T is the temperature in Kelvin.
In the case of spontaneous polymerization:
Even though ∆S is negative, the large negative ∆H ensures that ∆G remains negative, satisfying the condition for spontaneity. Thus, the correct answer is:
\( \Delta G<0, \quad \Delta H<0, \quad \Delta S<0 \)
Correct Answer:
Option 1: ∆G < 0, ∆H < 0, ∆S < 0
Explanation:
1. Gibbs Free Energy (ΔG):
For a spontaneous process, ∆G must be negative (∆G < 0).
2. Enthalpy Change (ΔH):
Polymerization reactions are generally exothermic, so ∆H is usually negative (∆H < 0).
3. Entropy Change (ΔS):
Polymerization reduces the number of independent particles, leading to a decrease in entropy, so ∆S is usually negative (∆S < 0).
4. Relationship between ΔG, ΔH, and ΔS:
∆G = ∆H - T∆S
To ensure ∆G < 0, the magnitude of ∆H must be greater than T∆S.
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