Gibbs free energy change for the reaction at 29°C. is equal to -1378.93 KJ.
<h3>What is Gibbs's free energy?</h3>
Gibbs free energy can be described as the enthalpy of the system minus the product of the temperature and entropy.
If the chemical reaction can be carried out under constant temperature ΔT = 0:
ΔG = ΔH – TΔS
The above equation is known as the Gibbs-Helmholtz equation.
ΔG > 0 non-spontaneous and endergonic and ΔG < 0 spontaneous and exergonic, ΔG = 0 is representing equilibrium.
Given the ΔS = -364 J/K, ΔH = -1269.8 KJ, T = 29°C = 29 + 273 = 302 K
ΔG = - 1269 - 302 × 364
ΔG = -1269 KJ - 109.93 KJ
ΔG = - 1378.93 KJ
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Your question is incomplete, most probably the complete question was,
2Ca(s)+O₂(g) → 2CaO(s)
ΔH∘rxn= -1269.8 kJ; ΔS∘rxn= -364.6 J/K
For this problem, assume that all reactants and products are in their standard states.
Calculate the free energy change for the reaction at 29°C.
