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Thermodynamics Chapter 19.

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Presentation on theme: "Thermodynamics Chapter 19."— Presentation transcript:

1 Thermodynamics Chapter 19

2 Spontaneous Processes and Entropy
Thermodynamics lets us predict whether a process will occur but gives no information about the amount of time required for the process. A spontaneous process is one that occurs without outside intervention.

3 Figure: 19-03

4

5 Entropy The driving force for a spontaneous process is an increase in the entropy of the universe. Entropy, S, can be viewed as a measure of randomness, or disorder.

6 Figure: 19-05

7

8 Figure: 19-08

9 Ssolid < Sliquid << Sgas
Positional Entropy A gas expands into a vacuum because the expanded state has the highest positional probability of states available to the system. Therefore, Ssolid < Sliquid << Sgas

10 Figure: 19-14

11 The Second Law of Thermodynamics
. . . in any spontaneous process there is always an increase in the entropy of the universe. Suniv > 0 for a spontaneous process.

12 Figure: 19-11a,b

13

14 G means +Suniv Free Energy
G = H  TS (from the standpoint of the system) A process (at constant T, P) is spontaneous in the direction in which free energy decreases: G means +Suniv

15 Effect of H and S on Spontaneity

16 Figure: 19-T04

17 The Third Law of Thermodynamics
. . . the entropy of a perfect crystal at 0 K is zero. Because S is explicitly known (= 0) at 0 K, S values at other temps can be calculated.

18 Free Energy Change and Chemical Reactions
G = standard free energy change that occurs if reactants in their standard state are converted to products in their standard state. G = npGf(products)  nrGf(reactants)

19 Entropy and Enthalpy

20 Free Energy and Pressure
G = G + RT ln(Q) Q = reaction quotient from the law of mass action.

21 Free Energy and Equilibrium
G = RT ln(K) K = equilibrium constant This is so because G = 0 and Q = K at equilibrium.

22

23

24 Figure: 19-18

25 Temperature Dependence of K
ln(K) = -Ho/R*(1/T) + So/R y = mx + b (H and S  independent of temperature over a small temperature range)

26 Reversible v. Irreversible Processes
Reversible: The universe is exactly the same as it was before the cyclic process. Irreversible: The universe is different after the cyclic process. All real processes are irreversible -- (some work is changed to heat).

27 END


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