This document discusses key concepts in thermodynamics and heat transfer, including:
1. It defines temperature and heat, and explains why touching a hot rack burns but hot air does not due to their different energy contents.
2. It reviews common units of heat measurement and conversions between them.
3. It outlines the contributions of important historical figures in thermodynamics and the development of the absolute temperature scale.
4. It describes the primary mechanisms of heat transfer as conduction, convection, and radiation.
This ppt is more useful for Civil Engineering students.
I have prepared this ppt during my college days as a part of semester evaluation . Hope this will help to current civil students for their ppt presentations and in many more activities as a part of their semester assessments.
I have prepared this ppt as per the syllabus concerned in the particular topic of the subject, so one can directly use it just by editing their names.
This ppt is more useful for Civil Engineering students.
I have prepared this ppt during my college days as a part of semester evaluation . Hope this will help to current civil students for their ppt presentations and in many more activities as a part of their semester assessments.
I have prepared this ppt as per the syllabus concerned in the particular topic of the subject, so one can directly use it just by editing their names.
the branch of physical science that deals with the relations between heat and other forms of energy (such as mechanical, electrical, or chemical energy), and, by extension, of the relationships between all forms of energy.
First law of thermodynamics as taught in introductory physical chemistry (includes general chemistry material). Covers concepts such as internal energy, heat, work, heat capacity, enthalpy, bomb calorimetry, Hess's law, thermochemical equations, bond energy, and heat of formations.
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3. Temperature and Heat
• Everyone has a qualitative understanding of temperature, but it is not
very exact.
• Question: Why can you put your hand in a 400 F oven and not get
instantly burned, but if you touch the metal rack, you do?
• Answer: Even though the air and the rack are at the same
temperature, they have very different energy contents.
4. Units of Heat
• J - Joules
• Cal - calorie
• Btu - British Thermal Unit
• Conversions:
1 cal =4.186 J
1Btu = 252 cal
5. Thermodynamics
Contributions made by:
• Benjamin Thompson (1753-1814) - (Count Rumford)
• Sadi Carnot (1796-1832)
• James Joule (1818-1889)
• Rudolf Clausius (1822-1888)
• William Thompson (1824-1907) - (Lord Kelvin)
• Robert Boyle (1627-1691)
• Charles (1746-1823)
• Gay-Lussac (1778-1823)
• Amedeo Avogadro (1776-1856)
• Daniel Bernoulli (1700-1782)
• John Dalton (1766-1844)
• Ludwig Boltzmann (1844-1906)
• J. Willard Gibbs (1939-1903)
• James Clerk Maxwell (1831-1879)
5
6. Construction of a Temperature Scale
• Absolute or Kelvin Scale
•K=C+273
32
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CelsiuswantandFahrenheitknowweIf
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9. Heat Transfer Mechanisms
1. Conduction: (solids--mostly) Heat transfer without mass transfer.
2. Convection: (liquids/gas) Heat transfer with mass transfer.
3. Radiation: Takes place even in a vacuum.
11. Convection
• Typically very complicated.
• Very efficient way to transfer energy.
• Vortex formation is very common feature.
12. Radiation
• Everything that has a temperature radiates energy.
• Method that energy from sun reaches the earth
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13. Specific Heat
• Observational Fact: It is easy to change the temperature of some things (e.g. air)
and hard to change the temperature of others (e.g. water)
• The amount of heat (Q) added into a body of mass m to change its temperature
an amount T is given by
Q=m C T
• C is called the specific heat and depends on the material and the units
used.
• Note: since we are looking at changes in temperature, either Kelvin or
Celsius will do.
14. Heat Capacity of Ideal Gas
• CV = heat capacity at constant volume
CV = 3/2 R
• CP = heat capacity at constant pressure
CP = 5/2 R
• For constant volume
Q = nCVΔT = ΔU
• The universal gas constant R = 8.314 J/mol·K
15. Work Done by a Gas
• Work=(Force)x(distance)
=Fy
• Force=(Presssure)x(Area)
• W=P(Ay)
=PV
16. The Laws of Thermodynamics
• First law: The change in the internal energy ΔU of a system is equal to the heat Q
added to a system plus the work W done by the system
ΔU = Q + W
• Secondlaw: It is not possible to convert heat completely into work without some
other change taking place.
• The “zeroth” law: Two systems in thermal equilibrium with a third system are in
thermal equilibrium with each other.
• Third law: It is not possible to achieve an absolute zero temperature
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17. First law
Isothermal Process
• An isothermal process is a constant temperature process. Any heat
flow into or out of the system must be slow enough to maintain
thermal equilibrium
• For ideal gases, if ΔT is zero, ΔU = 0
• Therefore, Q = W
• Any energy entering the system (Q)
• must leave as work (W)
18. First law
Isobaric Process
• An isobaric process is a constant pressure process. ΔU, W, and Q are
generally non-zero, but calculating the work done by an ideal gas is
straightforward
W = P·ΔV
• Water boiling in a saucepan is an example of an isobar process
19. First law
Isochoric Process
• An isochoric process is a constant volume process. When the volume
of a system doesn’t change, it will do no work on its surroundings. W
= 0
ΔU = Q
• Heating gas in a closed container is an isochoric process
20. Primary Results
• Internal energy U directly related to the average molecular kinetic energy
• Average molecular kinetic energy directly related to absolute temperature
• Internal energy equally distributed among the number of degrees of
freedom (f) of the system
(NA = Avogadro’s Number)
20
21. Other Primary Results
2. Maxwell derives a relation for the molecular speed distribution f (v):
3. Boltzmann contributes to determine the root-mean-square of the
molecular speed
Thus relating energy to the temperature for an ideal gas
21
