The value of ΔG° at 373 K for the oxidation of solid elemental sulfur to gaseous sulfur dioxide, S (s, rhombic) + O₂ (g) → SO₂ (g)
Is ________ kJ/mol. At 298 K, ΔH° for this reaction is -269.9 kJ/mol, and ΔS° is +11.6 J/K.

Question

Quizplus · Accepted Answer

To find ΔG° at 373 K, use the equation ΔG° = ΔH° - TΔS°. Convert ΔS° to kJ (11.6 J/K = 0.0116 kJ/K). ΔG° = -269.9 kJ/mol - (373 K)(0.0116 kJ/K) = -274.2 kJ/mol.

The Value of ΔG° at 373 K for the Oxidation