AP Chemistry
9.3 Gibbs Free Energy and Thermodynamic Favorability
The decomposition of a solid metal carbonate is represented by the following equation:
\[ \text{MCO}_3(s) \rightleftharpoons \text{MO}(s) + \text{CO}_2(g) \]
For this process, \(\Delta H^\circ = +88\text{ kJ/mol}_{rxn}\) and \(\Delta S^\circ = +110\text{ J/}(\text{mol}_{rxn}\cdot\text{K})\). Assuming that \(\Delta H^\circ\) and \(\Delta S^\circ\) do not change significantly with temperature, at approximately what minimum temperature does the reaction become thermodynamically favorable under standard conditions?
\[ \text{MCO}_3(s) \rightleftharpoons \text{MO}(s) + \text{CO}_2(g) \]
For this process, \(\Delta H^\circ = +88\text{ kJ/mol}_{rxn}\) and \(\Delta S^\circ = +110\text{ J/}(\text{mol}_{rxn}\cdot\text{K})\). Assuming that \(\Delta H^\circ\) and \(\Delta S^\circ\) do not change significantly with temperature, at approximately what minimum temperature does the reaction become thermodynamically favorable under standard conditions?
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