= G0p G0r ΔG – If G0p < G0r , -ve ΔG If G0p > G0r , +ve ΔG So G0p = G0r , =0 ΔG Gibbs energy, Pure Reactant Pure Product Table below show the properties about enthalpy change, entropy change, and change in free energy. If is negative, the forward reaction is spontaneous. ∆G If is 0, the system is at equilibrium. If is positive, the reaction is ∆G ∆G spontaneous in the reverse direction Enthalpy Change Entropy Change Spontaneous Reaction? Exothermic (ΔH < 0) Increase (ΔS > 0) Yes, < 0 ΔG Exothermic (ΔH < 0) Decrease (ΔS < Only at low temps, if |T < ΔS| 0) |ΔH| Endothermic (ΔH > Increase (ΔS > 0) Only at high temps, if T > ΔS ΔH 0) Endothermic (ΔH > Decrease (ΔS < No, > 0 ΔG 0) 0) When 300 mL of oil and 900 mL of water are agitated in a container, emulsification occurs. However, the system quickly reverts back into two separate phases as agitation stops. Explain, in terms of entropy and surface free energy,
ΔG = G0p – G0r If G0p < G0r , ΔG -ve If G0p > G0r , ΔG +ve So G0p = G0r , ΔG =0 Gibbs energy, Pure Reactant Pure Product Table below show the properties about enthalpy change, entropy change, and change in free energy. If ∆G is negative, the forward reaction is spontaneous. If ∆G is 0, the system is at equilibrium. If ∆G is positive, the reaction is spontaneous in the reverse direction Enthalpy Change Entropy Change Spontaneous Reaction? Exothermic (ΔH < 0) Increase (ΔS > 0) Yes, ΔG < 0 Exothermic (ΔH < 0) Decrease (ΔS < 0) Only at low temps, if |T ΔS| < |ΔH| Endothermic (ΔH > 0) Increase (ΔS > 0) Only at high temps, if T ΔS > ΔH Endothermic (ΔH > 0) Decrease (ΔS < 0) No, ΔG > 0 When 300 mL of oil and 900 mL of water are agitated in a container, emulsification occurs. However, the system quickly reverts back into two separate phases as agitation stops. Explain, in terms of entropy and surface free energy,
Chan_Ming_See_A140285.docx