AP Chemistry
9.3 Gibbs Free Energy and Thermodynamic Favorability
9.2 Absolute Entropy and Entropy Change
Methanol is synthesized industrially according to the following equation:
\[ \text{CO}(g) + 2\,\text{H}_2(g) \rightarrow \text{CH}_3\text{OH}(g) \quad \Delta H^\circ_{rxn} = -90.0\text{ kJ/mol}_{rxn} \]
The standard molar entropies of the substances involved in the reaction are provided in the table below.
Assuming that \(\Delta H^\circ\) and \(\Delta S^\circ\) are constant over the temperature range, what is the value of \(\Delta G^\circ_{rxn}\) at \(500\text{ K}\)?
\[ \text{CO}(g) + 2\,\text{H}_2(g) \rightarrow \text{CH}_3\text{OH}(g) \quad \Delta H^\circ_{rxn} = -90.0\text{ kJ/mol}_{rxn} \]
The standard molar entropies of the substances involved in the reaction are provided in the table below.
| Substance | \(S^\circ\ (\text{J}/(\text{mol}\cdot\text{K}))\) |
|---|---|
| \(\text{CO}(g)\) | \(200\) |
| \(\text{H}_2(g)\) | \(130\) |
| \(\text{CH}_3\text{OH}(g)\) | \(240\) |
Assuming that \(\Delta H^\circ\) and \(\Delta S^\circ\) are constant over the temperature range, what is the value of \(\Delta G^\circ_{rxn}\) at \(500\text{ K}\)?
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