Final answer:
Calculation of change in enthalpy and entropy for a reaction requires standard enthalpy and entropy values which are not provided for the specific reaction in question. The provided data refers to different reactions and doesn't allow for the calculation of the heat and disorder change for the formation of calcium titanate at 1000 K.
Step-by-step explanation:
The question relates to calculating the change in enthalpy (ΔH) and change in entropy (ΔS) for a specific chemical reaction at a certain temperature, which in this case is 1000 K. However, the provided information in the reference section is inconsistent with the question posed by the student, mentioning different reactions and enthalpy changes that do not pertain to the reaction between calcium oxide (CaO) and titanium dioxide (TiO₂) to form calcium titanate (CaTiO₃).
For accurate calculations, we would require the standard enthalpy of formation and standard entropy values for all the reactants and products involved in the correct reaction. This data can usually be found in thermodynamic tables. The enthalpy change (ΔH) for the reaction would be calculated by subtracting the sum of the enthalpies of formation of the reactants from the sum of the enthalpies of formation of products. The entropy change (ΔS) can be calculated in a similar fashion, using standard entropy values.
The mention of an exothermic reaction where CaCO3 (s) decomposes into CaO (s) and CO₂ (g) giving an enthalpy change (ΔH) of 177.8 kJ/mol and an entropy change (ΔS) of 160.5 J/K·mol, hints at the kind of data needed for the actual calculation. To compute these changes for a different temperature (such as 1000 K), the temperature dependence of ΔH and ΔS might need to be considered, and the values may need to be adjusted accordingly using standard thermodynamic equations.