Answer:
I. Kindly, see the attached image.
II. The reaction is exothermic.
III. - 51.88 kJ/mol.
IV. The reaction is spontaneous.
Explanation:
I. Draw a possible potential energy diagram of the reaction. Label the enthalpy of the reaction.
In an exothermic reaction, the energy of the reactants is higher than that of the products.
Kindly see the attached image to show you the potential energy diagram of the reaction.
II. Is the reaction endothermic or exothermic? Explain your answer.
If the sign is positive, the reaction is endothermic.
If the sign is negative, the reaction is exothermic.
Herein, ΔH = - 33.1 kJ/mol, so the reaction is exothermic.
III. What is the Gibbs free energy of the reaction at 25°C?
∵ ΔG = ΔH - TΔS.
Where, ΔG is the Gibbs free energy change (J/mol).
ΔH is the enthalpy change (ΔH = - 33.1 kJ/mol).
T is the temperature (T = 25°C + 273 = 298 K).
ΔS is the entorpy change (ΔS = 63.02 J/mol.K = 0.06302 J/mol.K).
∴ ΔG = ΔH - TΔS = (- 33.1 kJ/mol) - (298 K)(0.06302 J/mol.K) = - 51.88 kJ/mol.
IV. Is the reaction spontaneous or nonspontaneous at 25°C?
The sign of ΔG indicates the spontaneity of the reaction:
If ΔG < 0, the reaction is spontaneous.
If ΔG = 0, the reaction is at equilibrium.
If ΔG > 0, the reaction is nonspontaneous.
Herein, ΔG = - 51.88 kJ/mol, so the reaction is spontaneous.
