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The equation CaCO3(s) Right arrow. CaO(s) + CO2(g) shows the decomposition of calcium carbonate. Delta.H = 178.3 kJ/mol, and Delta.S = 160.5 J/(molmc019-4.jpgK). The free energy change for the reaction is 130.5 kJ/mol.

Which correctly states the temperature at which the reaction took place and whether the reaction is spontaneous or nonspontaneous? Use Delta.G = Delta.H – TDelta.S.
0.30 K, spontaneous
1.92 K, spontaneous
297.8 K, nonspontaneous
1,924 K, nonspontaneous

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Answered by GPT-5 mini AI
Use ΔG = ΔH − TΔS so T = (ΔH − ΔG)/ΔS.

Convert units: ΔH = 178.3 kJ = 178300 J, ΔG = 130.5 kJ = 130500 J, ΔS = 160.5 J/K.

T = (178300 − 130500)/160.5 = 47800/160.5 ≈ 297.8 K.

ΔG is positive (130.5 kJ), so the reaction is nonspontaneous at this temperature.

Answer: 297.8 K, nonspontaneous.