The Story of Spontaneity and Energy Dispersal

1. The Story of Spontaneity and Energy Dispersal You never get what you want: 100% return on investment

2. Spontaneity • Spontaneous process are those that occur naturally. • Hot body cools • A gas expands to fill the available volume • A spontaneous direction of change is where the direction of change does not require work to bring it about.

3. Spontaneity • The reverse of a spontaneous process is a nonspontaneous process • Confining a gas in a smaller volume • Cooling an already cool object • Nonspontaneous processes require energy in order to realize them.

4. Spontaneity • Note: • Spontaneity is often interpreted as a natural tendency of a process to take place, but it does not necessarily mean that it can be realized in practice. • Some spontaneous processes have rates sooo slow that the tendency is never realized in practice, while some are painfully obvious.

5. Spontaneity • The conversion of diamond to graphite is spontaneous, but it is joyfully slow. • The expansion of gas into a vacuum is spontaneous and also instantaneous.

6. 2nd Law of Thermodynamics

7. Physical Statements of the 2nd Law of Thermodynamics • Kelvin Statements • “No process is possible in which the sole result is the absorption of heat from a reservoir and its complete conversion into work”

8. “It is impossible for a system to undergo a cyclic process whose sole effects are the flow of an amount of heat from the surroundings to the system and the performance of an equal amount of work on the surroundings.” • “It is impossible for a system to undergo a cyclic process that turns heat completely into work done on the surroundings.”

9. Clausius statement • It is impossible for a process to occur that has the sole effect of removing a quantity of heat from an object at a lower temperature and transferring this quantity of heat to an object at a higher temperature. • Heat cannot flow spontaneously from a cooler to a hotter object if nothing else happens

10. The 2nd Law of Thermodynamics • The 2nd Law of Thermodynamics recognizes the two classes of processes, the spontaneous and nonspontaneous processes.

11. Implications of the 2nd Law • No heat engine can have an efficiency as great as unity • No macroscopic process can decrease the entropy of the universe

12. Are you kidding me? Thermodynamic Cat

13. Hot Reservoir Engine Work Heat Cold Reservoir Heat I approve!

15. What determines the direction of spontaneous change? • The total internal energy of a system does NOT determine whether a process is spontaneous or not. • Per the First Law, energy is conserved in any process involving an isolated system.

16. What determines the direction of spontaneous change? • Instead, it is important to note that the direction of change is related to the distribution of energy. • Spontaneous changes are always accompanied by a dispersal of energy.

17. Energy Dispersal • Superheroes with energy blasts and similar powers as well as the Super Saiyans are impossible characters. • They seem to violate the Second Law of Thermodynamics!

18. Power Genkidama

19. Energy Dispersal • A ball on a warm floor can never be observed to spontaneously bounce as a result of the energy from the warm floor

20. Energy Dispersal • In order for this to happen, the thermal energy represented by the random motion and vibrations of the floor atoms would have to be spontaneously diverted to accumulate into the ball.

21. Energy Dispersal • It will also require the random thermal motion to be redirected to move in a single direction in order for the ball to jump upwards. • This redirection or localization of random, disorderly thermal motion into a concerted, ordered motion is so unlikely as to be virtually impossible.

22. Energy Dispersal and Spontaneity INDEED! • Spontaneous change can now be interpreted as the direction of change that leads to the dispersal of the total energy of an isolated system!

23. Entropy • A state function, denoted by S. • While the First Law can be associated with U, the Second Law may be expressed in terms of the S

24. Entropy and the Second Law • The Second Law can be expressed in terms of the entropy: The entropy of an isolated system increases over the course of a spontaneous change: ΔStot > 0 • Where Stot is the total entropy of the system and its surroundings.

25. Entropy • A simple definition of entropy is that it is a measure of the energy dispersed in a process. • For the thermodynamic definition, it is based on the expression:

26. Hot Reservoir Th qh -w1 w3 Engine w4 -w2 qc Cold Reservoir Tc Entropy as a State Function • To prove entropy is a state function we must show that ∫dS is path independent • Sufficient to show that the integral around a cycle is zero or • Sadi Carnot (1824) devised cycle to represent idealized engine Step 1: Isothermal reversible expansion @ Th Step 2:Adiabatic expansion Th to Tc Step 3:Isothermal reversible compression @ Tc(sign of q negative) Step 4: Adiabatic compression Tcto Th

27. Carnot Engine How is that possible?

28. Carnot Cycle

29. Carnot Cycle Step 1: ΔU=0 Step 2: ΔU=w Step 3: ΔU=0 Step 4: ΔU=-w

30. Efficiency of Heat Engines • Efficiency is the ratio of the work done by an engine in comparison to the energy invested in the form of heat for all reversible engines • All reversible engines have the same efficiency irrespective of their construction.

31. Refrigeration/ Heat pump

32. Refrigeration

33. Coefficient of performance (COP or β or c) • COP describes the qc in this case as the minimum energy to be supplied to a refrigeration-like system in order to generate the required entropy to make the system work.

34. SUPERENGINE?

35. Hot Reservoir w Engine Work qh Heat -qc Cold Reservoir Heat Carnot Cycle - Thermodynamic Temperature Scale • The efficiency of a heat engine is the ratio of the work performed to the heat of the hot reservoir e=|w|/qh • The greater the work the greater the efficiency • Work is the difference between the heat supplied to the engine and the heat returned to the cold reservoir w = qh -(-qc) = qh + qc • Therefore, e =|w|/qh = ( qh + qc)/qh = 1 + (qc/qh)

36. Hot Reservoir w Engine Work qh Heat -qc Cold Reservoir Heat Carnot Cycle - Thermodynamic Temperature Scale • William Thomson (Lord Kelvin) defined a substance-independent temperature scale based on the heat transferred between two Carnot cycles sharing an isotherm • He defined a temperature scale such that qc/-qh= Tc/Th • e = 1 - (Tc/Th ) • Zero point on the scale is that temperature where e = 1 • Or as Tc approaches 0 e approaches 1 • Efficiency can be used as a measure of temperature regardless of the working fluid • Applies directly to the power required to maintain a low temperature in refrigerators • Efficiency is maximized • Greater temperature difference between reservoirs • The lower Tc, the greater the efficiency

37. Entropy • For a measurable change between two states, • In order to calculate the difference in entropy between two states, we find a reversible pathway between them and integrate the energy supplied as heat at each stage, divided by the temperature.

38. Example

39. Change in entropy of the surroundings: ΔSsur • If we consider a transfer of heat dqsur to the surroundings, which can be assumed to be a reservoir of constant volume. • The energy transferred can be identified with the change in internal energy • dUsur is independent of how change brought about (U is state function • Can assume process is reversible, dUsur= dUsur,rev • Since dUsur = dqsur and dUsur= dUsur,rev, • dqsurmust equal dqsur,rev • That is, regardless of how the change is brought about in the system, reversibly or irreversibly, we can calculate the change of entropy of the surroundings by dividing the heat transferred by the temperature at which the transfer takes place.

40. Change in entropy of the surroundings: ΔSsur • For adiabatic change, qsur = 0, so DSsur = 0

41. Entropy changes: Expansion • Entropy changes in a system are independent of the path taken by the process • Total change in entropy however depends on the path: • Reversible process: ΔStot= 0 • Irreversible process: ΔStot> 0

42. Entropy changes: Phase Transitions • Trouton’s rule: • An empirical observation about a wide range of liquids providing approximately the same standard entropy of vaporization, around 85/88/90 J/mol K.

44. Entropy of gas mixing

45. Third Law of Thermodynamics • At T = 0, all energy of thermal motion has been quenched, and in a perfect crystal all the atoms or ions are in a regular, uniform array. • The localization of matter and the absence of thermal motion suggest that such materials also have zero entropy. • This conclusion is consistent with the molecular interpretation of entropy, because S = 0 if there is only one way of arranging the molecules and only one microstate is accessible (the ground state).

46. Third Law of Thermodynamics The entropy of all perfect crystalline substances is zero at T = 0.

47. Nernst heat theorem • The entropy change accompanying any physical or chemical transformation approaches zero as the temperature approaches zero: ΔS 0 as T 0 provided all the substances involved are perfectly crystalline.

48. Lewis statement • If the entropy of each element in some crystalline state be taken as zero at the absolute zero of temperature, every substance has a finite positive entropy—but at the absolute zero of temperature the entropy may become zero, and does so become in the case of perfect crystalline substances.

49. Unattainable absolute zero William Francis Giauque, 1895–1982, was an American chemist who discovered that ordinary oxygen consists of three isotopes. He received the 1949 Nobel Prize in chemistry for pioneering the process of adiabatic demagnetization to attain low temperatures. • Giauque’s adiabatic demagnetization has led to temperatures of less than 0.000001 K (1 μK) in the nuclear spins of a magnetizablesystem. • Opposing laser beams that effectively stop the translational motion of atoms have achevedan effective temperature of 3 × 10−9 K (3 nK) (Saubamea and friends)

50. Third-Law entropies or Absolute Entropies • These are entropies reported on the basis that S(0) = 0.