Thermodynamics II. Copyright The McGraw-Hill Companies, Inc. Permission required for reproduction or display.

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1 Thermodynamics II Copyright The McGraw-Hill Companies, Inc. Permission required for reproduction or display. 1

Spontaneous Physical and Chemical Processes A waterfall runs downhill A lump of sugar dissolves in a cup of coffee At 1 atm, water freezes below 0 o C and ice melts

2 Spontaneous Physical and Chemical Processes A waterfall runs downhill A lump of sugar dissolves in a cup of coffee At 1 atm, water freezes below 0 o C and ice melts above 0 o C Heat flows from a hotter object to a colder object A gas expands in an evacuated bulb Iron exposed to oxygen and water forms rust spontaneous nonspontaneous 2

3 spontaneous nonspontaneous 3

4 Does a decrease in enthalpy mean a reaction proceeds spontaneously? Spontaneous reactions CH 4 (g) + 2O 2 (g) H + (aq) + OH - (aq) CO 2 (g) + 2H 2 O (l) ΔH = kj/mol H 2 O (l) ΔH = kj/mol H 2 O (s) H 2 O (l) ΔH = 6.01 kj/mol NH 4 NO 3 (s) H 2 O NH 4 + (aq) + NO 3 - (aq) ΔH = 25 kj/mol 4

5 Entropy (S) is a measure of the randomness or disorder of a system. order S disorder S ΔS = S f - S i If the change from initial to final results in an increase in randomness S f > S i ΔS > 0 For any substance, the solid state is more ordered than the liquid state and the liquid state is more ordered than gas state S solid < S liquid << S gas H 2 O (s) H 2 O (l) ΔS > 0 5

6 Entropy W = number of microstates S = k ln W ΔS = S f - S i ΔS = k ln W f W i W f > W i then ΔS > 0 W f < W i then ΔS < 0 6

7 Processes that lead to an increase in entropy (ΔS > 0) 7

8 Example: Br 2 (l) Br 2 (g) Example: I 2 (s) I 2 (g) ΔS > 0 ΔS > 0 8

9 How does the entropy of a system change for each of the following processes? (a) Condensing water vapor Randomness decreases Entropy decreases (ΔS < 0) (b) Forming sucrose crystals from a supersaturated solution Randomness decreases Entropy decreases (ΔS < 0) (c) Heating hydrogen gas from 60 C to 80 C Randomness increases Entropy increases (ΔS > 0) (d) Subliming dry ice Randomness increases Entropy increases (ΔS > 0) 9

10 Entropy State functions are properties that are determined by the state of the system, regardless of how that condition was achieved. Examples: energy, enthalpy, pressure, volume, temperature, entropy Review Potential energy of hiker 1 and hiker 2 is the same even though they took different paths. 10

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12 First Law of Thermodynamics Energy can be converted from one form to another but energy cannot be created or destroyed. Second Law of Thermodynamics The entropy of the universe increases in a spontaneous process and remains unchanged in an equilibrium process. Spontaneous process: Equilibrium process: ΔS univ = ΔS sys + ΔS surr > 0 ΔS univ = ΔS sys + ΔS surr = 0 12

13 Entropy Changes in the System (ΔS sys ) The standard entropy of reaction (ΔS 0 rxn ) is the entropy change for a reaction carried out at 1 atm and 25 0 C. aa + bb cc + dd ΔS rxn = [ cs (C) + ds (D) ] - [ as (A) + bs (B)] ΔS rxn = Σ ns (products) - Σ ms (reactants) What is the standard entropy change for the following reaction at 25 C? 2CO (g) + O 2 (g) 2CO 2 (g) S (CO) = J/K mol S (O 2 ) = J/K mol S (CO 2 ) = J/K mol ΔS rxn = 2 x S (CO 2 ) [2 x S (CO) + S (O 2 )] ΔS rxn = [ ] = J/K mol 13

14 Entropy Changes in the System (ΔS sys ) When gases are produced (or consumed) If a reaction produces more gas molecules than it consumes, ΔS > 0. If the total number of gas molecules diminishes, ΔS < 0. If there is no net change in the total number of gas molecules, then ΔS may be positive or negative BUT ΔS will be a small number. What is the sign of the entropy change for the following reaction? 2Zn (s) + O 2 (g) 2ZnO (s) The total number of gas molecules goes down, ΔS is negative. 14

15 Entropy Changes in the Surroundings (ΔS surr ) Exothermic Process ΔS surr > 0 Endothermic Process ΔS surr < 0 15

16 Third Law of Thermodynamics The entropy of a perfect crystalline substance is zero at the absolute zero of temperature. S = k ln W W = 1 S = 0 16

17 Gibbs Free Energy Spontaneous process: Equilibrium process: ΔS univ = ΔS sys + ΔS surr > 0 ΔS univ = ΔS sys + ΔS surr = 0 Gibbs free energy (G) For a constant temperature and constant pressure process: ΔG = ΔH sys -TΔS sys ΔG < 0 ΔG > 0 ΔG = 0 The reaction is spontaneous in the forward direction. The reaction is nonspontaneous as written. The reaction is spontaneous in the reverse direction. The reaction is at equilibrium. 17

18 The standard free-energy of reaction (ΔG rxn ) is the freeenergy change for a reaction when it occurs under standardstate conditions. ΔG rxn ΔG rxn aa + bb cc + dd = [ cδg f (C) + dδg (D) ] - [ aδg f (A) + bδg f (B) ] f = Σ nδg f (products) - Σ mδg f (reactants) Standard free energy of formation (ΔG ) is the free-energy f change that occurs when 1 mole of the compound is formed from its elements in their standard states. ΔG of any element in its stable form is zero. f 18

19 19

20 What is the standard free-energy change for the following reaction at 25 0 C? 2C 6 H 6 (l) + 15O 2 (g) 12CO 2 (g) + 6H 2 O (l) ΔG rxn = Σ nδg f (products) - Σ mδg f (reactants) ΔG rxn = [ 12ΔG (CO 6ΔG 2 ) + (H 2 O) ] - [ 2ΔG (C 6 H 6 )] f f ΔG rxn = [ 12x x ] [ 2x124.5 ] = kj/mol Is the reaction spontaneous at 25 C? ΔG = kj/mol < 0 spontaneous f 20

21 ΔG = ΔH - TΔS 21

22 Temperature and Spontaneity of Chemical Reactions CaCO 3 (s) CaO (s) + CO 2 (g) Equilibrium Pressure of CO 2 ΔH = kj/mol ΔS = J/K mol ΔG = ΔH TΔS At 25 C, ΔG = kj/mol ΔG = 0 at 835 o C 22

Chapter 19. Entropy, Free Energy, and Equilibrium

Chapter 19. Entropy, Free Energy, and Equilibrium Chapter 19 Entropy, Free Energy, and Equilibrium Spontaneous Physical and Chemical Processes A waterfall runs downhill A lump of sugar dissolves in a cup of coffee At 1 atm, water freezes below 0 0 C and