Consider the following reaction: caco3(s)→cao(s)+co2(g).estimate δg∘ for this reaction at each of the following temperatures. (assume that δh∘ and δs∘ do not change too much within the given temperature range.)a. 285 kδg∘ =b.1025 kδg∘=c.1475 kδg∘ =

a) ΔG° = 132.5 kJ

b) ΔG° = 13.68 kJ

c) ΔG° = -58.58 kJ

Explanation:

The values of the enthalpy of formation(H°f) and the entropy (S°) for the substances in the reaction are:

CaCO₃(s): H°f = -1206.9 kJ/mol   S° = 92.9 J/K.mol

CaO(s): H°f = -635.09 kJ/mol  S° = 39.75 J/K.mol

CO₂(g): H°f = -393.51 kJ/mol   S° = 213.74 J/K.mol

ΔH° = ∑n*H°f,products - ∑n*H°f,reactants (where n is the number of moles)

ΔH° = (-393.51 + (-635.09)) - (-1206.9) = 178.3 kJ

ΔS° = ∑n*S°,products - ∑n*S°,reactants

ΔS° = (213.74 + 39.75) - 92.9 = 160.59 J/K = 0.1606 kJ/K

ΔG° = ΔH° - TΔS°

a) ΔG° = 178.3 - 285*0.1606 = 132.5 kJ

b) ΔG° = 178.3 - 1025*0.1606 = 13.68 kJ

c) ΔG° = 178.3 - 1475*0.1606 = -58.58 kJ

it’s previous models   because when i picked that son of a gun’s answer it was wrong look for previous models because they might make it a different letter