AP Chemistry
9.3 Gibbs Free Energy and Thermodynamic Favorability
A student investigates the thermodynamic parameters for the decomposition of a liquid compound at \(298\text{ K}\), as represented by the balanced equation below:
\[ 2\,\text{XO}(l) \rightarrow 2\,\text{X}(s) + \text{O}_2(g) \]
Based on the data in the table, what is the value of the standard Gibbs free energy change, \(\Delta G^\circ\), for the reaction at \(298\text{ K}\)?
\[ 2\,\text{XO}(l) \rightarrow 2\,\text{X}(s) + \text{O}_2(g) \]
| Thermodynamic Parameter | Value |
|---|---|
| \(\Delta H^\circ\) | \(-40.2\text{ kJ/mol}_{\text{rxn}}\) |
| \(\Delta S^\circ\) | \(+100.\text{ J}/(\text{mol}_{\text{rxn}}\cdot\text{K})\) |
Based on the data in the table, what is the value of the standard Gibbs free energy change, \(\Delta G^\circ\), for the reaction at \(298\text{ K}\)?
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