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Thermodynamics

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Title: Thermodynamics


1
Thermodynamics(Study of Heat )
Dr. Shaun Wyngaardt (Room 511)
2
Other members of the PHY1024F Team
Course Convenor Dr. Azwinndini Muronga (rm 406)
3
Other members of the PHY1024F Team
Course Tutor ???
4
Other members of the PHY1024F Team
Lab Coordinators Drs. Rudolph Nchodu (rm. 504)
Shaun Wyngaardt (511)
5
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6
Web Information
  • Course content can be found at
  • http//www.phy.uct.ac.za/courses/phy1024f

7
Consultation Times
  • Dr Wyngaardt (Tuesdays Thursdays)
  • 1300-1400 room 511.
  • Course Tutor ???

8
Skill which you with Master
  • Construction of scientific models
  • Develop problem solving techniques
  • Develop the ability to perform experiments, do
    measurements, and interpret the data.

9
Scientific Terminology
The Moon is made of Cheese
  • Scientific Statement
  • Scientific Facts
  • Scientific Theories/Models
  • Scientific Law

10
Physical Systems
  • An isolated part of the universe which is being
    investigated.
  • Why do we isolate things in science?

11
ThermoDynamics
Temperature/Heat
Movement/Change
12
Outline
  • Week 1
  • Temperature, Thermal expansion, Heat transfer,
    Zeroth Law of thermodynamics
  • Week 2
  • Thermal processes (1st law of TD).
  • The Kinetic theory of gasses
  • Week 3
  • The 2nd Law of Thermodynamics the Physics
    behind Heat engines.

13
Thermodynamic system
  • Thermodynamic systems are
  • Macroscopic (size of everyday things)
  • Homogeneous (same composition and structure
    throughout material)
  • Isotropic (identical physical properties in all
    directions)
  • Uncharged (no net electric charge)
  • Chemically inert (no chemical processes)
  • Experiences no change in its total mechanical
    energy (no stress or strain on the system).

14
Thermal properties of a system
  • What is temperature?
  • Macroscopic description
  • a measure of the hotness/coldness of a body

15
  • In Physics we distinguish between temperature and
    heat.
  • Heat is defined as the transfer (donation) of
    internal energy between different objects (in
    contact with each other) at different
    temperatures (Objects in thermal contact).
  • Heat transfer -gt state of thermal equilibrium
    (same temperature).

16
Zeroth Law of thermodynamics
  • If systems A and B are in thermal equilibrium
    with system C then A and B are in thermal
    equilibrium with each other.

A
C
B
17
Zeroth Law of thermodynamics
  • If system A and B are in thermal equilibrium with
    system C then A and B are in thermal equilibrium
    with each other.

A
B
18
Measures of temperature and heat
  • Heat Energy transferred Joule
  • Other units of heat energy include Calories (cal)

19
  • Is the human body a good thermometer?
  • Most materials respond to temperature changes by
    expanding when heated or contracting when cooled.

http//home.howstuffworks.com/therm1.htm
20
Temperature scales
  • Two commonly used temperature scales
  • Fahrenheit scale - Daniel Fahrenheit arbitrarily
    decided that the freezing and boiling points of
    water would be separated by 180 degrees, and he
    pegged freezing water at 32 degrees. So he made a
    thermometer, stuck it in freezing water and
    marked the level of the mercury on the glass as
    32 degrees. Then he stuck the same thermometer in
    boiling water and marked the level of the mercury
    as 212 degrees. He then put 180 evenly spaced
    marks between those two points.
  • Celsius scale - Anders Celsius arbitrarily
    decided that the freezing and boiling points of
    water would be separated by 100 degrees, and he
    pegged the freezing point of water at 100
    degrees. (His scale was later inverted, so the
    boiling point of water became 100 degrees and the
    freezing point became 0 degrees.)

21
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22
Absolute zero temperature
  • When a gas is cooled its pressure drops.
  • Gasses which are not near its liquefaction
    temperature follow a linear temperature pressure
    relationship of the form

23
Temperature in degrees Celsius
Pressure
24
Kelvin scale
25
Classroom Exercise
  • Like the Kelvin scale, the Rankine scale is an
    absolute temperature scale absolute is zero
    degrees Rankine (0oR). However, the units of this
    scale are the same are the size as those on the
    Fahrenheit scale rather than the celcius scale.
    What is the numerical value of the triple point
    of water (25oC) on the Rankine scale.

26
K
oC
27
Thermal properties of Macroscopic Objects
28
Thermal expansion in solids and liquids
  • Most objects expand when heated.
  • This expansion need to be considered in various
    engineering and architectural structures such as
    railway lines, windows pains, etc.
  • Amount of thermal expansion depends on the
    material which is heated.

29
  • Quantifying thermal expansion experimental we
    find that

30
  • Quantifying thermal expansion experimental we
    find that

31
  • Quantifying thermal expansion experimental we
    find that

32
  • Thermal expansion depends on the initial length
    of the rod.

33
  • Thermal expansion depends on the initial length
    of the temperature change.

34
  • Hence the linear thermal expansion of a rod is
    given by

Expansion coefficient
35
Thermal expansion of an area
36
Thermal expansion of an area
37
Thermal expansion of a volume
38
Coefficients of thermal expansion
  • http//hypertextbook.com/physics/thermal/expansion

39
Thermal expansion in kettles
40
Exercise 1
  • A surveyor uses a steel measuring tape that is
    exactly 50.0 km long at a temperature of 20
    degrees C. What is its length on a hot summer day
    when the temperature is 35 degrees C?

41
Exercise 2
  • A glass flask with a volume 200 cm3 is filled to
    the brim with mercury at 20 oC. How much mercury
    overflows when the temperature of the system is
    raised to 100 oC? The coefficient of linear
    expansion of the glass is 0.4 X 10-5 K-1, while
    the volume expansion of mercury is 18 X 10-5 K-1.

42
Calorimetry
  • When heat is transferred two things could happen
  • Temperature could change
  • System could undergo a phase change (melting
    ice).
  • Convention Heat transfer to a system is while
    heat transfer from a system is -

43
Case 1 Temperature change
44
Case 1 Temperature change
45
Case 1 Temperature change
specific heat capacity
46
Case 1 Temperature change
of moles
Molecular mass
47
Case 1 Temperature change
Molar specific heat capacity
48
Phase change
  • Solid lt-gtLiquidlt-gtGaslt-gtPlasma
  • The temperature of a system undergoing a phase
    change remain the same.
  • The amount of heat energy required for a phase
    change depend on the amount (mass) of the
    substance we have.

49
Phase change
  • Hence

Latent heat
50
Processes of heat transfer
  • There are 3 way to transfer heat
  • Conduction
  • Convection
  • Radiation

51
Heat Conduction
Heat energy moves
52
Heat Conduction
Heat energy moves
53
Heat Conduction
Heat energy moves
54
Heat Conduction
Heat energy moves
55
Heat Convection
  • The transfer of heat by means of the mass
    movement of molecules from one place to another.

56
Heat Convection
57
Heat Convection
58
Radiation of Heat Energy
  • Both the transfer of heat through conduction and
    convection require the present of matter.
  • How does heat energy move through empty space
    from the hot sun to earth?

59
Radiation of Heat Energy
  • All hot objects above absolute zero (0K) emit
    ELECTROMAGNETIC RADIATION in one form or another
    (microwaves, radiowaves, light, x-rays).
  • The rate of radiation is given by the
    Stephan-Boltzmann equation

60
Radiation of Heat Energy
  • Stephan-Boltzmann equation

61
Radiation of Heat Energy
62
Radiation of Heat Energy
  • Radiation correction due to the colour of the
    radiating object.

63
Radiation of Heat Energy
  • Radiation can be absorbed from the environment
    surrounding an object, thus increasing its
    temperature.
  • At the same time the object could emit radiation
    to its surroundings

64
Thermal effects in an Ideal gas
  • Robert Boyle 1660 (Gas consists of particles)

65
Thermal effects in an Ideal gas
  • Robert Boyle 1660
  • At constant temperature he observed that

66
  • Furthermore this constant depends linearly on the
    temperature
  • The value of PV also depends on the amount of gas
    particles in the container.

67
  • Avogadros number of particles (atoms/molecules)

68
Idea Gas Relationships
69
Exercise 3
  • When excessive heat is produced within the body,
    it must be transferred to the skin and dispersed
    if the body interior is to be maintained at the
    normal value of 37.0 degrees Celsius. One
    possible mechanism for transfer is conduction
    through body fat. Suppose that heat travels
    through 0.030 m of fat in reaching the skin,
    which has a total surface area of 1.7 m2 and a
    temperature of 34.0 degrees Celsius. Find the
    amount of heat that reaches the skin in half an
    hour (1800 s) K(Fat) 0.2 J/(s.moC).

70
Thermal Processes and the 1st Law of
Thermodynamics
  • We reap the practical benefits of thermodynamic
    processes on a daily basis.
  • Examples include driving cars, turning on an air
    conditioner, cooking a meal,
  • Central to all processes in the Conservation of
    Energy (energy transforms from one form to
    another)

71
Thermal Processes
  • Four main thermodynamic quantities to play around
    with (Temperature, Pressure, Volume, and Heat).
  • Thermal processes are characterised by keeping
    one of these 4 quantities fixed.

72
Thermal Processes
  • Four thermodynamic processes include
  • Isothermal process Temperature of system is
    fixed.
  • Isobaric process Pressure is fixed.
  • Isochoric process Volume is fixed.
  • Adiabatic process hardly no heat is transfer to
    or from the system (Thermus flask).

73
Thermal systems have Internal Energy
Particles inside container have internal kinetic
energy
74
1st law of Thermodynamics
  • We can change the internal energy by
  • doing work on it or
  • heating it.
  • Conversion Work done on the system is and work
    done by the system is -.

75
1st law of Thermodynamics
Change in internal energy
Heat applied to the system
Work done by the system on surroundings
76
Work done by system on surroundings
77
Work done by gas in Isobaric process
P Constant
78
Work done by gas in Isochoric process
V Constant
79
Work done by gas in Isothermal process
T Constant
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