Use the table below to answer the question that follow. Part A 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. The value of G° 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, H° for this reaction is -269.9 kJ/mol, and S° is +11.6 J/K.
-274.2
+300.4
-300.4
-4,597
+4,597
Expert Answer
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