For the oxidation of solid elemental sulfur to gaseous sulfur dioxide S (s, rhombic) + O2 (g) -->SO2 (g) calculate the value of AG° at a temperature of 100 °C (373 K) in kJ/mol. Substance AH° (kJ/mol) S° (J/mol K) S(s, rhombic) SO2 (g) 02 (g) 31.88 -269.9 248.5 205.0
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![### Oxidation of Solid Elemental Sulfur to Gaseous Sulfur Dioxide
**Reaction**:
\[ S (s, \text{rhombic}) + O_2 (g) \rightarrow SO_2 (g) \]
**Objective**: Calculate the value of ΔG° at a temperature of 100 °C (373 K) in kJ/mol.
#### Thermodynamic Data Table:
| Substance | ΔH°f (kJ/mol) | S° (J/mol·K) |
|-----------|---------------|--------------|
| S(s, rhombic) | 0 | 31.88 |
| SO₂(g) | -269.9 | 248.5 |
| O₂(g) | 0 | 205.0 |
### Explanation:
- **ΔH°f** refers to the standard enthalpy of formation.
- **S°** represents the standard entropy.
#### Given Options for ΔG°:
- +4597 kJ/mol
- -300.4 kJ/mol (correct answer)
- +300.4 kJ/mol
- -4597 kJ/mol
- -274.2 kJ/mol
**Note**: ΔG° is calculated using the formula:
\[ \Delta G° = \Delta H° - T \Delta S° \]
This exercise requires applying thermodynamic principles to find the correct Gibbs free energy change for the reaction at a given temperature.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F83e4d0e0-41e1-45c9-8283-0ae60fe430d6%2F2d78b940-afbe-4118-82f2-9a5c1bf9f5aa%2Fhwavja9_processed.jpeg&w=3840&q=75)
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