1. Thermodynamics Lecture Series Capturing the Lingo
Assoc. Prof. Dr. Jaafar Jantan aka DR. JJ
Applied Science Education Research
Applied Science, UiTM, Shah Alam
Journey towards
Enrichment and
Balance utilizing
Arts and Sciences in
Teaching & Learning
Deep Impact Mission: Flyby camera capturing the image when impactor spacecraft collides with Tempel 1 on July 3rd.
Dr. J.J.
Voice: Website:
Copyright DRJJ, ASERG, FSG, UiTM, 2004

2. Copyright DRJJ, ASERG, FSG, UiTM, 2004
“Education is the kindling of a flame, not the filling of a vessel” - Socrates.
“Learning is not a spectator sport.
You do not learn much just sitting in classes listening to teachers, memorizing prepackaged assignments, and spitting out answers. You must talk about what you are learning, write reflectively about it, relate it to past experiences, and apply it to your daily lives. You must make what you learn part of yourselves.”
  -Source:"Implementing the Seven Principles: Technology as Lever" by Arthur W. Chickering and Stephen C. Ehrmann
11/28/2018
Copyright DRJJ, ASERG, FSG, UiTM, 2004
Copyright DRJJ, ASERG, FSG, UiTM, 2004

3. Copyright DRJJ, ASERG, FSG, UiTM, 2004
Learning
Objectives/Intended Learning Outcome:
At the end of this session, participants should be able to:
State, discuss and apply the terminologies used in thermodynamics to daily life.
State and identify origins and transformations of the many different forms of energy
State and discuss the characteristics and description of changes from and to a system
State and discuss the zeroth law of thermo.
11/28/2018
Copyright DRJJ, ASERG, FSG, UiTM, 2004
Copyright DRJJ, ASERG, FSG, UiTM, 2004

4. Basic Concepts of Thermodynamics – The science of Energy
CHAPTER 1
Basic Concepts of Thermodynamics –
The science of Energy

5. FIGURE 1–5 Some application areas of thermodynamics.
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FIGURE 1–5 Some application areas of thermodynamics.
1-1

6. Steam Power Plant

7. FIGURE 1–13 System, surroundings, and boundary.
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FIGURE 1–13 System, surroundings, and boundary.
1-3

8. Copyright © The McGraw-Hill Companies, Inc
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FIGURE 1–14 Mass cannot cross the boundaries of a closed system, but energy can.
1-4

9. Dynamic Energies cross in and out
Systems
Win
Wout
Dynamic Energies cross in and out
NO VOLUME CHANGE
Vinitial = Vfinal
V = constant
Qin
Qout
A rigid tank

10. NO dynamic energy transfer
Systems
NO mass transfer
min = mout = 0
NO dynamic energy transfer
Ein = Eout = 0
An isolated system

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FIGURE 1–17 A control volume may involve fixed, moving, real, and imaginary boundaries.
1-5

12. Open system devices Throttle Heat Exchanger
Copyright DRJJ, ASERG, FSG, UiTM, 2004

13. The system can be either open or closed. The concept of a property
Properties
Properties:
Temperature
Pressure
Volume
Internal energy
Entropy
System
The system can be either open or
closed. The concept of a property
still applies.

14. First Law of Thermodynamics
System expands
Movable boundary position gone up
System
System
A change has taken place.

15. NOT ADDITIVE OVER THE SYSTEM.
Classes of properties
Extensive
MASS, m
VOLUME, V
ENERGY, E
ADDITIVE OVER
THE SYSTEM.
Intensive
TEMPERATURE, T
PRESSURE, P
DENSITY
Specific properties
NOT ADDITIVE OVER THE SYSTEM.

16. Box with 3 sections after equilibrium Intensive: not size independent
Classes of properties
Box with 3 sections after equilibrium
Intensive: not size independent
 = 1 = 2 = 3 = V/m
e = e1 = e2 = e3 = E/m
T, P
Extensive: Total :
V = V1 + V2 + V3
E = E1 + E2 + E3
m = m1 + m2 + m3

17. State A set of properties describing the condition of a system
States
State
A set of properties describing the condition of a system
A change in any property, changes the state of that system

18. Equilibrium A state of balance
States
Equilibrium
A state of balance
Thermal – temperature same at all points of system
Mechanical – pressure same at all points of system at all time
Phase – mass of each phase about the same
Chemical – chemical reaction stop

19. States
State postulate
Must have 2 independent intensive properties to specify a state:
Pressure & specific internal energy
Pressure & specific volume
Temperature & specific enthalpy

20. Processes and cycles

21. First Law of Thermodynamics
Properties will change indicating change of state
System
E1, P1, T1, V1 To
E2, P2, T2, V2
Win
Wout
Mass in
Mass out
Qin
Qout

22. FIGURE 1–25 A process between states 1 and 2 and the process path.
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FIGURE 1–25 A process between states 1 and 2 and the process path.
1-6

23. FIGURE 1–28 The P-V diagram of a compression process.
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FIGURE 1–28 The P-V diagram of a compression process.
1-7

24. Thermodynamic process
State 1
State 2 p V T

25. Example: Heating water
Heat supplied by electricity or combustion. T1
T1+dT
T1+2dT T2 ….

26. Theater System analysis of the slow heating process:
Energy in via electricity
or gas combustion
System Boundary
Neglect vapor loss
Twater
Theater
Assume no heat
losses from sides
and bottom.

27. Theater System analysis for the water under equilibrium processes:
Heating via an equilibrium process
Energy In
Twater
Theater
Reversed process of slow cooling, which is reversible for the water
Energy Out

28. Processes & Equilibrium States
What is the
state of the
system along
the process
path? p V T S1 S2
Process Path

29. Thermodynamic process
State 1
State 2
Process 1 p V
Process 2

30. P1 P2 Process Path I Process Path II State 1 State 2
Thermodynamic cycles P1 P2
State 1
State 2
Process Path I
Process Path II

31. Example: A steam power cycle.
Turbine
Mechanical Energy
to Generator
Heat
Exchanger
Cooling Water
Pump
Fuel
Air
Combustion
Products
System Boundary
for Thermodynamic
Analysis

32. Types of Energy

33. Dynamic System Changes occuring within system
Types of Energy
Dynamic
Heat, Q
Work, W
Energy of moving mass, Emass
Crosses in and out of system’s boundary
System
Internal, U
Kinetic, KE
Potential, PE
Changes occuring within system

34. Internal, U Sensible, Relates to temperature change Latent
Types of Energy
Internal, U
Sensible,
Relates to temperature change
Latent
Relates to phase change

35. Copyright © The McGraw-Hill Companies, Inc
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FIGURE 1–32 The various forms of microscopic energies that make up sensible energy.
1-8

36. Kinetic Changes with square of velocity
Types of Energy
Kinetic
Changes with square of velocity
KE = (mv2)/2, kJ; ke = v2/2, kJ/kg
If velocity doubles,
KE = (m(2v)2)/2 = (4mv2)/2, kJ
If decrease by ½, then
KE = (m(v/2)2)/2 = (mv2)/8, kJ

37. Potential Changes with vertical position,
Types of Energy
Potential
Changes with vertical position,
PE = mg(yf - yi) = mgh, kJ; pe = gh, kJ/kg
If position above reference point doubles,
PE = mg(2h), kJ; pe = g2h, kJ/kg
If decrease by ½, then
PE = mgh/2, kJ; pe = gh/2, kJ/kg

38. APPLICATION OF THE EQUILIBRIUM PRINCIPLE
Zeroth Law of Thermodynamics
Heat, and Temperature
Copyright DRJJ, ASERG, FSG, UiTM, 2004

39. Temperature & heat...

40. Our sense of the direction of
Heat & temperature
Large body
at constant
temperature T1
T2<T1
Our sense of the direction of
heat flow - from high to low temperature.

41. Temperature and heat are related.
For metals, high
heat flow - diathermal
materials. T1 T2
For nonmetals, low
heat flow - insulating.

42. Caloric definition of temperature
Isolating
boundaries

43. Bring systems into thermal contact and surround
with an isolating -- adiabatic -- boundary.
Initial configuration of the closed, combined
systems with a diathermal wall between the two. T1 T2

44. Heat is observed to flow from the subsystem at the higher temperature to that with the lower temperature. T1 T2

45. The final observed state of the total system is that when the temperatures are equal. Heat flow from subsystem 1 to subsystem 2 decreases in time.
T1,final
T2,final

46. Zeroth Law of Thermodynamics...

47. Thermal equilibrium T1 T2
T1,final
T2,final
Initial State:
Final State:

48. Demonstration of the Zeroth Law
Two subsystems in equilibrium with a third subsystem
Adiabatic
Diathermal B D A C

49. The Zeroth Law
Two systems in thermal equilibrium with a third system are in thermal equilibrium with each other.

50. FIGURE 1–41 The greenhouse effect on earth.
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FIGURE 1–41 The greenhouse effect on earth.
1-11

51. Copyright © The McGraw-Hill Companies, Inc
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FIGURE 1–45 P versus T plots of the experimental data obtained from a constant-volume gas thermometer using four different gases at different (but low) pressures.
1-12

52. FIGURE 1–47 Comparison of temperature scales.
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FIGURE 1–47 Comparison of temperature scales.
1-13

53. FIGURE 1–51 Absolute, gage, and vacuum pressures.
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FIGURE 1–51 Absolute, gage, and vacuum pressures.
1-14

54. Copyright © The McGraw-Hill Companies, Inc
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FIGURE 1–55 The pressure is the same at all points on a horizontal plane in a given fluid regardless of geometry, provided that the points are interconnected by the same fluid.
1-15

55. FIGURE 1–57 The basic manometer.
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FIGURE 1–57 The basic manometer.
1-16

56. FIGURE 1–61 Schematic for Example 1–8.
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FIGURE 1–61 Schematic for Example 1–8.
1-17

57. FIGURE 1–63 The basic barometer.
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FIGURE 1–63 The basic barometer.
1-18

58. Copyright © The McGraw-Hill Companies, Inc
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FIGURE 1–75 Some arrangements that supply a room the same amount of energy as a 300-W electric resistance heater.
1-19

59. Copyright © The McGraw-Hill Companies, Inc
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FIGURE 1–39 Ground-level ozone, which is the primary component of smog, forms when HC and NOx react in the presence of sunlight in hot calm days.
1-9

60. Copyright © The McGraw-Hill Companies, Inc
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FIGURE 1–40 Sulfuric acid and nitric acid are formed when sulfur oxides and nitric oxides react with water vapor and other chemicals high in the atmosphere in the presence of sunlight.
1-10

61. FIGURE 1–7 The definition of the force units.
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FIGURE 1–7 The definition of the force units.
1-2