AP Chemistry
9.3 Gibbs Free Energy and Thermodynamic Favorability
The thermal decomposition of calcium carbonate is represented by the equation below.
\[ \text{CaCO}_3(s) \rightleftharpoons \text{CaO}(s) + \text{CO}_2(g) \]
For this reaction, \(\Delta H^\circ = +176\text{ kJ/mol}_{\text{rxn}}\) and \(\Delta S^\circ = +160\text{ J/}(\text{mol}_{\text{rxn}}\cdot\text{K})\). Assuming that \(\Delta H^\circ\) and \(\Delta S^\circ\) are constant over the temperature range, at approximately what temperature does the reaction transition from thermodynamically unfavorable to thermodynamically favorable under standard conditions?
\[ \text{CaCO}_3(s) \rightleftharpoons \text{CaO}(s) + \text{CO}_2(g) \]
For this reaction, \(\Delta H^\circ = +176\text{ kJ/mol}_{\text{rxn}}\) and \(\Delta S^\circ = +160\text{ J/}(\text{mol}_{\text{rxn}}\cdot\text{K})\). Assuming that \(\Delta H^\circ\) and \(\Delta S^\circ\) are constant over the temperature range, at approximately what temperature does the reaction transition from thermodynamically unfavorable to thermodynamically favorable under standard conditions?
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