When heated, CaCO₃ decomposes into CaO and CO₂ according to the following equation: CaCO₃(s) ⇌ CaO(s) + CO₂(g) This is an endothermic reaction in which ∆H° = 178.3 kJ/mol and in which entropy increases, ∆S° = 159 J/mol･K. To what temperature (in °C) must CaCO₃ be heated in a closed container in order to produce CO₂ at an equilibrium pressure of 0.200 atm? (Assume ∆H° and ∆S° do not change appreciably with temperature).

5. The entropy change of the process H20 (s) – H2O () is 22 J/K at 0 °C. Calculate the enthalpy of freezing of water at 0 °C.

What is the standard reaction entropy, ΔS°rxn (in J/K), for the reaction given below?   P4(s)   +   6 F2(g)    →    4 PF3(g)      ΔS°rxn = ?   S°m[P4(s)]  =  41 J/mole·K S°m[F2(g)]  =  203 J/mole·K S°m[PF3(g)]  =  296 J/mole·K

Calcium carbonate decomposes according to the following reaction.   ????3(?)⟺???(?)+??2(?)CaCO3(s)⟺Cao(s)+CO2(g) The tabulated data below was determined at 25 °C.   CaCO3(s) CaO(s) CO2(g) Δ?∘?ΔHf∘ Δ?∘?ΔHf∘, kJ/mol -1206.9 -635.1 -393.5 ?∘S∘ ?∘S∘, kJ/(mol K) 0.0929 0.0382 0.2137 Δ?∘?ΔGf∘ Δ?∘?ΔGf∘, kJ/mol -1128.8 -603.5 -394.4 What is ΔG° at 25 °C for this reaction? Is the reaction spontaneous at 25 °C? What is ΔG° at 1000 °C for this reaction? Is the reaction spontaneous at 1000 °C? Calculate KP for this reaction at 25 °C and 1000 °C.