For the process S₈ (rhombic)$\to$ S₈ (monoclinic)at 110°C,$\Delta$H = 3.21 kJ/mol and $\Delta$S = 8.70 J/K . mol (at 110°C). Which of the following is correct?

Question

Quizplus · Accepted Answer

To determine spontaneity, we use the Gibbs free energy equation: ΔG = ΔH - TΔS. Given ΔH = 3.21 kJ/mol (or 3210 J/mol for consistency with ΔS units) and ΔS = 8.70 J/K·mol at 110°C (or 383K), ΔG = 3210 J/mol - (383K)(8.70 J/K·mol) = 3210 J/mol - 3331.1 J/mol = -121.1 J/mol. Since ΔG is negative, the reaction is spontaneous, making the monoclinic form stable at 110°C.

For the Process S8 (Rhombic) →\to→ S8 (Monoclinic)at 110°C Δ\DeltaΔ H = 321 KJ/mol And S8

For the Process S₈ (Rhombic) $\to$ S₈ (Monoclinic)at 110°C $\Delta$ H = 321 KJ/mol And S₈