1. Maximum Work 1 Often reactions are not carried out in a way that does useful work. –As a spontaneous precipitation reaction occurs, the free energy of the system decreases and entropy is produced, but no useful work is obtained. –In principle, if a reaction is carried out to obtain the maximum useful work, no entropy is produced.

2. Maximum Work 2 Often reactions are not carried out in a way that does useful work. –It can be shown that the maximum useful work, w max, for a spontaneous reaction is  G. –The term free energy comes from this result.

3. Free Energy Change During Reaction 3 As a system approaches equilibrium, the instantaneous change in free energy approaches zero. –Figure 19.9 illustrates the change in free energy during a spontaneous reaction. –As the reaction proceeds, the free energy eventually reaches its minimum value. –At that point,  G = 0, and the net reaction stops; it comes to equilibrium.

4. Relating  G o to the Equilibrium Constant 4 The free energy change when reactants are in non-standard states (other than 1 atm pressure or 1 M) is related to the standard free energy change,  G o, by the following equation. –Here Q is the thermodynamic form of the reaction quotient.

5. Relating  G o to the Equilibrium Constant 5 The free energy change when reactants are in non- standard states (other than 1 atm pressure or 1 M) is related to the standard free energy change,  G o, by the following equation. –  G represents an instantaneous change in free energy at some point in the reaction approaching equilibrium.

6. Relating  G o to the Equilibrium Constant 6 The free energy change when reactants are in non- standard states (other than 1 atm pressure or 1 M) is related to the standard free energy change,  G o, by the following equation. –At equilibrium,  G=0 and the reaction quotient Q becomes the equilibrium constant K.

7. Relating  G o to the Equilibrium Constant 7 The free energy change when reactants are in non- standard states (other than 1 atm pressure or 1 M) is related to the standard free energy change,  G o, by the following equation. –At equilibrium,  G=0 and the reaction quotient Q becomes the equilibrium constant K.

8. Relating  G o to the Equilibrium Constant 8 This result easily rearranges to give the basic equation relating the standard free-energy change to the equilibrium constant. –When K > 1, the ln K is positive and  G o is negative. –When K < 1, the ln K is negative and  G o is positive.

9. Spontaneity and Temperature Change 9 All of the four possible choices of signs for  H o and  S o give different temperature behaviors for  G o. HoHo SoSo GoGo Description –+– Spontaneous at all T +–+ Nonspontaneous at all T ––+ or – Spontaneous at low T; Nonspontaneous at high T +++ or – Nonspontaneous at low T; Spontaneous at high T

10. Calculation of  G o at Various Temperatures 10 In this method you assume that  H o and  S o are essentially constant with respect to temperature. –You get the value of  G T o at any temperature T by substituting values of  H o and  S o at 25 o C into the following equation.

11. A Problem To Consider 11 Find the  G o for the following reaction at 25 o C and 1000 o C. Relate this to reaction spontaneity. So:So: 38.292.9213.7 J/K Hfo:Hfo: -635.1-1206.9-393.5 kJ