Consider the reaction: CaCO3(s) → CaO(s) + CO2(g). Estimate ΔG° for this reaction at each temperature and predict whether or not the reaction is spontaneous. (Assume that ΔH° and ΔS° do not change too much within the given temperature range.) a. 298 K b. 1055 K c. 1455 K.

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1. Identify the given reaction: \( \text{CaCO}_3(s) \rightarrow \text{CaO}(s) + \text{CO}_2(g) \). This is a decomposition reaction.
2. Recall the Gibbs free energy equation: \( \Delta G^\circ = \Delta H^\circ - T\Delta S^\circ \).
3. Determine the standard enthalpy change (\( \Delta H^\circ \)) and the standard entropy change (\( \Delta S^\circ \)) for the reaction from standard tables.
4. For each temperature (298 K, 1055 K, 1455 K), substitute the values of \( \Delta H^\circ \), \( \Delta S^\circ \), and the given temperature \( T \) into the Gibbs free energy equation to calculate \( \Delta G^\circ \).
5. Analyze the sign of \( \Delta G^\circ \) for each temperature: if \( \Delta G^\circ < 0 \), the reaction is spontaneous; if \( \Delta G^\circ > 0 \), the reaction is non-spontaneous.