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/ 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

A decomposition reaction is the breakdown of the chemical reactant into its product. The equation of calcium carbonate is nonspontaneous and takes place at 297.8 K. Thus, option C is correct.

What is a nonspontaneous reaction?

A nonspontaneous reaction occurs when the product formation is not favored under the normal conditions of the reaction system and is accompanied by endothermic reactions that are characterized by decreased entropy.

The temperature for the reaction, CaCO₃(s) → CaO(s) + CO₂(g) is calculated by,

Given,

ΔH = 178.3 kJ/mol

ΔS = 160.5 J/

ΔG = 130.5 kJ/mol

ΔG = ΔH – TΔS

130.5 = 178.3 - T(160.5)

= 0.29781

= 297.81 K

The entropy, enthalpy, and temperature of the system are in positive values, and hence, the system proceeds in the reverse direction depicting a nonspontaneous reaction.

Therefore, the reaction occurs at 297.81 K and is a nonspontaneous reaction.

Learn more about the nonspontaneous reaction here:

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