Lecture Notes Alan D. Earhart Southeast Community College Lincoln, NE Chapter 16 Thermodynamics: Entropy, Free Energy, and Equilibrium John E. McMurry Robert C. Fay CHEMISTRY Fifth Edition Copyright © 2008 Pearson Prentice Hall, Inc.
Chapter 16/2 Spontaneous Processes Spontaneous Process: A process that, once started, proceeds on its own without a continuous external influence.
Copyright © 2008 Pearson Prentice Hall, Inc.Chapter 16/3 Spontaneous Processes
Copyright © 2008 Pearson Prentice Hall, Inc.Chapter 16/4 Enthalpy, Entropy, and Spontaneous Processes State Function: A function or property whose value depends only on the present state, or condition, of the system, not on the path used to arrive at that state. Enthalpy Change ( H): The heat change in a reaction or process at constant pressure; H = E + P V. Entropy (S): The amount of molecular randomness in a system.
Copyright © 2008 Pearson Prentice Hall, Inc.Chapter 16/5 Enthalpy, Entropy, and Spontaneous Processes = kJ H vap CO 2 (g) + 2H 2 O(l)CH 4 (g) + 2O 2 (g) H 2 O(l)H 2 O(s) H 2 O(g)H 2 O(l) 2NO 2 (g)N2O4(g)N2O4(g) = kJ H°H° = kJ H fusion = kJ H°H° = kJ H°H° Endothermic: Exothermic: Na 1+ (aq) + Cl 1- (aq)NaCl(s) H2OH2O
Copyright © 2008 Pearson Prentice Hall, Inc.Chapter 16/6 Enthalpy, Entropy, and Spontaneous Processes S = S final - S initial
Copyright © 2008 Pearson Prentice Hall, Inc.Chapter 16/7 Enthalpy, Entropy, and Spontaneous Processes
Copyright © 2008 Pearson Prentice Hall, Inc.Chapter 16/8 Enthalpy, Entropy, and Spontaneous Processes
Copyright © 2008 Pearson Prentice Hall, Inc.Chapter 16/9 Entropy and Probability S = k ln W k = Boltzmann’s constant = 1.38 x J/K W =The number of ways that the state can be achieved.
Copyright © 2008 Pearson Prentice Hall, Inc.Chapter 16/10 Entropy and Temperature Third Law of Thermodynamics: The entropy of a perfectly ordered crystalline substance at 0 K is zero.
Entropy and Temperature
Copyright © 2008 Pearson Prentice Hall, Inc.Chapter 16/12 Standard Molar Entropies and Standard Entropies of Reaction Standard Molar Entropy (S°): The entropy of 1 mole of a pure substance at 1 atm pressure and a specified temperature.
Copyright © 2008 Pearson Prentice Hall, Inc.Chapter 16/13 Standard Molar Entropies and Standard Entropies of Reaction cC + dDaA + bB S° = S°(products) - S°(reactants) S° = [cS°(C) + dS°(D)] - [aS°(A) + bS°(B)] ReactantsProducts
Copyright © 2008 Pearson Prentice Hall, Inc.Chapter 16/14 Standard Molar Entropies and Standard Entropies of Reaction Using standard entropies, calculate the standard entropy change for the decomposition of N 2 O 4. 2NO 2 (g)N2O4(g)N2O4(g) - (1 mol) S° = 2 S°(NO 2 (g)) - S°(N 2 O 4 (g)) K mol J S° = J/K K mol J S° = (2 mol)
Copyright © 2008 Pearson Prentice Hall, Inc.Chapter 16/15 Entropy and the Second Law of Thermodynamics First Law of Thermodynamics: In any process, spontaneous or nonspontaneous, the total energy of a system and its surroundings is constant. Second Law of Thermodynamics: In any spontaneous process, the total entropy of a system and its surroundings always increases.
Copyright © 2008 Pearson Prentice Hall, Inc.Chapter 16/16 Entropy and the Second Law of Thermodynamics S total > 0The reaction is spontaneous. S total < 0The reaction is nonspontaneous. S total = 0The reaction mixture is at equilibrium. S total = S sys + S surr or S total = S system + S surroundings
Entropy and the Second Law of Thermodynamics s surr - H s surr T 1 s surr = T - H
Copyright © 2008 Pearson Prentice Hall, Inc.Chapter 16/18 Free Energy G = H - T S = -T S total Free Energy: G = H - TS G = H - T S S = S sys Using: s surr = T - H S total = S sys + S surr
Copyright © 2008 Pearson Prentice Hall, Inc.Chapter 16/19 Free Energy G < 0The reaction is spontaneous. G > 0The reaction is nonspontaneous. G = 0The reaction mixture is at equilibrium. Using the second law and G = H - T S = -T S total
Copyright © 2008 Pearson Prentice Hall, Inc.Chapter 16/20 Free Energy
Copyright © 2008 Pearson Prentice Hall, Inc.Chapter 16/21 Standard Free-Energy Changes for Reactions Thermodynamic Standard State: Most stable form of a substance at 1 atm pressure and at a specified temperature, usually 25 °C; 1 M concentration for all substances in solution. G° = H° - T S°
Copyright © 2008 Pearson Prentice Hall, Inc.Chapter 16/22 Standard Free-Energy Changes for Reactions Calculate the standard free-energy change at 25 °C for the Haber synthesis of ammonia using the given values for the standard enthalpy and standard entropy changes: S° = J/K 2NH 3 (g)N 2 (g) + 3H 2 (g) = kJ H° = kJ G° = H° - T S° 1000 J 1 kJ K J xx= kJ K
Copyright © 2008 Pearson Prentice Hall, Inc.Chapter 16/23 Standard Free Energies of Formation G° = G° f (products) - G° f (reactants) G° = [c G° f (C) + d G° f (D)] - [a G° f (A) + b G° f (B)] ReactantsProducts cC + dDaA + bB
Copyright © 2008 Pearson Prentice Hall, Inc.Chapter 16/24 Standard Free Energies of Formation
Copyright © 2008 Pearson Prentice Hall, Inc.Chapter 16/25 Standard Free Energies of Formation Using table values, calculate the standard free-energy change at 25 °C for the reduction of iron(III) oxide with carbon monoxide: 2Fe(s) + 3CO 2 (g)Fe 2 O 3 (s) + 3CO(g) - [(1 mol)( kJ/mol) + (3 mol)( kJ/mol)] G° = kJ G° = [2 G° f (Fe(s)) + 3 G° f (CO 2 (g))] - [1 G° f (Fe 2 O 3 (s)) + 3 G° f (CO(g))] G° = [(2 mol)(0 kJ/mol) + (3 mol)( kJ/mol)]
Copyright © 2008 Pearson Prentice Hall, Inc.Chapter 16/26 Free Energy Changes and the Reaction Mixture G = G° + RT ln Q G = Free-energy change under nonstandard conditions. For the Haber synthesis of ammonia: 2NH 3 (g)N 2 (g) + 3H 2 (g) Q p = NH 3 P 2 H2H2 P N2N2 P 3
Copyright © 2008 Pearson Prentice Hall, Inc.Chapter 16/27 Free Energy Changes and the Reaction Mixture C2H4(g)C2H4(g)2C(s) + 2H 2 (g) Q p = C2H4C2H4 P H2H2 P 2 Calculate ln Q: Calculate G for the formation of ethylene (C 2 H 4 ) from carbon and hydrogen at 25 °C when the partial pressures are 100 atm H 2 and 0.10 atm C 2 H 4. = ln
Copyright © 2008 Pearson Prentice Hall, Inc.Chapter 16/28 Free Energy Changes and the Reaction Mixture Calculate G: = 68.1 kJ/mol + G = 39.6 kJ/mol (298 K)(-11.51) 1000 J 1 kJ K mol J G = G° + RT ln Q
Copyright © 2008 Pearson Prentice Hall, Inc.Chapter 16/29 Free Energy and Chemical Equilibrium G = G° + RT ln Q Q >> 1RT ln Q >> 0 G > 0 The total free energy decreases as the reaction proceeds spontaneously in the reverse direction. When the reaction mixture is mostly products: Q << 1RT ln Q << 0 G < 0 The total free energy decreases as the reaction proceeds spontaneously in the forward direction. When the reaction mixture is mostly reactants:
Free Energy and Chemical Equilibrium At equilibrium, G = 0 and Q = K. G° = -RT ln K G = G° + RT ln Q
Copyright © 2008 Pearson Prentice Hall, Inc.Chapter 16/32 Free Energy and Chemical Equilibrium Calculate K p at 25 °C for the following reaction: Calculate G°: CaO(s) + CO 2 (g)CaCO 3 (s) - [(1 mol)( kJ/mol)] G° = kJ/mol = [(1 mol)( kJ/mol) + (1 mol)( kJ/mol)] G° = [ G° f (CaO(s)) + G° f (CO 2 (g))] - [ G° f (CaCO 3 (s))]
Copyright © 2008 Pearson Prentice Hall, Inc.Chapter 16/33 Free Energy and Chemical Equilibrium Calculate K: = G° = -RT ln K kJ/mol ln K = (298 K) 1000 J 1 kJ K mol J = 1.4 x Calculate ln K: RT -G°-G° ln K = K = e