The value of ΔG° at 373 K for the oxidation of solid elemental sulfur to gaseous sulfur dioxide 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

We can use the Gibbs-Helmholtz equation to relate ΔG°, ΔH°, and ΔS° at different temperatures:

ΔG° = ΔH° - TΔS°

Substituting the given values, we get:

ΔG° = (-269.9 kJ/mol) - (373 K)(0.0116 kJ/K/mol)
ΔG° = -274.2 kJ/mol

Therefore, the answer is (B), -274.2 kJ/mol.

The Value of ΔG° at 373 K for the Oxidation