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