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Title: Thermodynamics Chapter 1


1
Thermodynamics
2
Chapter Summary
1-14
  • The first law of thermodynamics is simply an
    expression of the conservation of energy
    principle, and it asserts that energy is a
    thermodynamic property.
  • The second law of thermodynamics asserts that
    energy has quality as well as quantity, and
    actual processes occur in the direction of
    decreasing quality of energy.

3
Chapter Summary
1-15
  • A system of fixed mass is called a closed system,
    or control mass, and a system that involves mass
    transfer across its boundaries is called an open
    system, or control volume.

4
Chapter Summary
1-16
  • The mass-dependent properties of a system are
    called extensive properties and the others,
    intensive properties. Density is mass per unit
    volume, and specific volume is volume per unit
    mass.

5
Chapter Summary
1-17
  • The sum of all forms of energy of a system is
    called total energy, which is considered to
    consist of internal, kinetic, and potential
    energies. Internal energy represents the
    molecular energy of a system and may exist in
    sensible, latent, chemical, and nuclear forms.

6
Chapter Summary
1-18
  • A system is said to be in thermodynamic
    equilibrium if it maintains thermal, mechanical,
    phase, and chemical equilibrium.

7
Chapter Summary
1-19
  • Any change from one state to another is called a
    process.
  • A process with identical end states is called a
    cycle.

8
Chapter Summary
1-20
  • During a quasi-static or quasi-equilibrium
    process, the system remains practically in
    equilibrium at all times.

9
Chapter Summary
1-21
  • The state of a simple, compressible system is
    completely specified by two independent,
    intensive properties.

10
Chapter Summary
1-22
  • Force per unit area is called pressure, and its
    unit is the pascal. The absolute, gage, and
    vacuum pressures are related by

11
Chapter Summary
1-23
  • Small to moderate pressure differences are
    measured by a manometer, and a differential fluid
    column of height h corresponds to a pressure
    difference of where ? is the fluid density
    and g is the local gravitational acceleration.

12
Chapter Summary
1-24
  • The atmospheric pressure is measured by a
    barometer and is determined from where h is
    the height of the liquid column above the free
    surface.

13
Chapter Summary
1-25
  • The zeroth law of thermodynamics states that two
    bodies are in thermal equilibrium if both have
    the same temperature reading even if they are not
    in contact.

14
Chapter Summary
1-26
  • The temperature scales used in the SI and the
    English system today are the Celsius scale and
    the Fahrenheit scale, respectively.

15
Chapter Summary
1-27
  • The absolute temperature scale in the SI is the
    Kelvin scale, which is related to the Celsius
    scale by

16
Chapter Summary
1-28
  • In the English system, the absolute temperature
    scale is the Rankine scale, which is related to
    the Fahrenheit scale by

17
Chapter Summary
1-29
  • The magnitudes of each division of 1 K and 1 0C
    are identical, and so are the magnitude of each
    division of 1 R and 10F. Therefore,and

18
Chapter Summary
1-30
  • An important application area of thermodynamics
    is the biological system. Most diets are based on
    the simple energy balance the net energy gained
    by a person in the form of fat is equal to the
    difference between the energy intake from food
    and the energy expended by exercise.

19
1
CHAPTER
BasicConcepts ofThermodynamics
20
Applications of Thermodynamics
1-1
21
Crossing Closed-System Boundries
1-2
Energy, not mass, crosses closed-system boundries
  • (Fig. 1-13)

22
Closed System with Moving Boundry
1-3
23
Crossing Control Volume Boundaries
1-4
Mass and Energy Cross Control Volume Boundaries
24
Systems Internal Energy
1-5
Systems Internal Energy Sum of Microscopic
Energies
  • (Fig. 1-19)

25
Quasi-Equilibrium, Work-Producing Devices
1-6
Quasi-Equilibrium, Work-Producing Devices Deliver
the Most Work
  • (Fig. 1-30)

26
Compressed Process P-V Diagram
1-7
  • (Fig. 1-31)

27
Absolute, Gage, and Vacuum Pressures
1-8
  • (Fig. 1-36)

28
The Basic Manometer
1-9
29
Temperature Scales Comparison
1-10
  • (Fig. 1-48)

30
Many Ways to Supply the Same Energy
1-11
Ways to supply a room with energy equalling a
300-W electric resistance heater
  • (Fig. 1-52)

31
Bomb Calorimeter Used to Determine Energy
Content of Food
1-12
  • (Fig. 1-53)

32
Chapter Summary
1-13
  • Thermodynamics is the science that primarily
    deals with energy.

33
Chapter Summary
1-14
  • The first law of thermodynamics is simply an
    expression of the conservation of energy
    principle, and it asserts that energy is a
    thermodynamic property.
  • The second law of thermodynamics asserts that
    energy has quality as well as quantity, and
    actual processes occur in the direction of
    decreasing quality of energy.

34
Chapter Summary
1-15
  • A system of fixed mass is called a closed system,
    or control mass, and a system that involves mass
    transfer across its boundaries is called an open
    system, or control volume.

35
Chapter Summary
1-16
  • The mass-dependent properties of a system are
    called extensive properties and the others,
    intensive properties. Density is mass per unit
    volume, and specific volume is volume per unit
    mass.

36
Chapter Summary
1-17
  • The sum of all forms of energy of a system is
    called total energy, which is considered to
    consist of internal, kinetic, and potential
    energies. Internal energy represents the
    molecular energy of a system and may exist in
    sensible, latent, chemical, and nuclear forms.

37
Chapter Summary
1-18
  • A system is said to be in thermodynamic
    equilibrium if it maintains thermal, mechanical,
    phase, and chemical equilibrium.

38
Chapter Summary
1-19
  • Any change from one state to another is called a
    process.
  • A process with identical end states is called a
    cycle.

39
Chapter Summary
1-20
  • During a quasi-static or quasi-equilibrium
    process, the system remains practically in
    equilibrium at all times.

40
Chapter Summary
1-21
  • The state of a simple, compressible system is
    completely specified by two independent,
    intensive properties.

41
Chapter Summary
1-22
  • Force per unit area is called pressure, and its
    unit is the pascal. The absolute, gage, and
    vacuum pressures are related by

42
Chapter Summary
1-23
  • Small to moderate pressure differences are
    measured by a manometer, and a differential fluid
    column of height h corresponds to a pressure
    difference of where ? is the fluid density
    and g is the local gravitational acceleration.

43
Chapter Summary
1-24
  • The atmospheric pressure is measured by a
    barometer and is determined from where h is
    the height of the liquid column above the free
    surface.

44
Chapter Summary
1-25
  • The zeroth law of thermodynamics states that two
    bodies are in thermal equilibrium if both have
    the same temperature reading even if they are not
    in contact.

45
Chapter Summary
1-26
  • The temperature scales used in the SI and the
    English system today are the Celsius scale and
    the Fahrenheit scale, respectively.

46
Chapter Summary
1-27
  • The absolute temperature scale in the SI is the
    Kelvin scale, which is related to the Celsius
    scale by

47
Chapter Summary
1-28
  • In the English system, the absolute temperature
    scale is the Rankine scale, which is related to
    the Fahrenheit scale by

48
Chapter Summary
1-29
  • The magnitudes of each division of 1 K and 1 0C
    are identical, and so are the magnitude of each
    division of 1 R and 10F. Therefore,and

49
Chapter Summary
1-30
  • An important application area of thermodynamics
    is the biological system. Most diets are based on
    the simple energy balance the net energy gained
    by a person in the form of fat is equal to the
    difference between the energy intake from food
    and the energy expended by exercise.
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