KNOWLEDGE INSTITUTE OF TECHNOLOGY. · Process 1-2: vapor refrigerant is compressed to a relatively...
Transcript of KNOWLEDGE INSTITUTE OF TECHNOLOGY. · Process 1-2: vapor refrigerant is compressed to a relatively...
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KNOWLEDGE INSTITUTE OF
TECHNOLOGY.
DEPARTMENT OF MECHANICAL
ENGINNERING
ENGINEERING THERMODYNAMICS
BY
Mr.V.Karthikeyan
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ENGINEERING
THERMODYNAMICS
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OBJECTIVES
To familiarize and to understand the fundamentals of
thermodynamics and to perform thermal analysis on their
behaviour and performance.
OUTCOMES
You can able to apply the Thermodynamic Principles to
Mechanical Engineering Application.
Apply mathematical fundamentals to study the properties of
steam, gas and gas mixtures.
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Text Book & Reference Book
Nag.P.K. - Engineering Thermodynamics
Cengel. Y and M.Boles, "Thermodynamics - An Engineering
Approach", 7th Edition, Tata McGraw Hill, 2010.
Table and Charts
Steam Table,
Mollier Chart,
Compressibility Chart,
Psychrometric Chart.
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ETD FUNDAMENTALS BASED SUBJECTS
Thermal Engineering- IV Sem
Heat and Mass Transfer- V Sem
Gas Dynamics and Jet Propulsion- VI Sem
Power Plant Engineering- VII Sem
Elective
Refrigeration and Air conditioning- VI Sem
Thermal Turbo Machines- VII Sem
Advanced I.C. Engines- VIII Sem
Design of Heat Exchangers- VIII Sem
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INTRODUCTION
The name thermodynamics stems from the Greek words therme (heat) and dynamis (power).
Thermodynamics is the science of energy transfer and its effects on a physical properties.
The application of thermodynamic laws and principles are found in all field of energy technologies.
Refrigeration System
Steam and nuclear power plants
Internal Combustion Engine
Gas Turbine
Air Conditioning
Gas Dynamics
Jet Propulsion
Compressor
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7
Steam power plants
Fundamentals
Coal, Natural Gas,
Nuclear, Biofuel,
Waste Fuel
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SIMPLE IMPULSE TURBINE PRINCIPLE
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REFRIGERATION SYSTEM
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BASIC CONCEPTS
DIMENSIONS AND UNITS
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DENSITY AND SPECIFIC GRAVITY
Specific gravity: The ratio of the density of a substance to the density of some standard substance at a specified temperature (usually water at 4°C).
Density
Specific weight: The weight of a unit volume of a substance.
Specific volume
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SI UNITS
The SI unit prefixes are used in all branches of engineering.
Work = Force Distance
1 J = 1 N∙m
1 cal = 4.1868 J
1 Btu = 1.0551 kJ
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PRESSURE Pressure: A normal force exerted by a fluid per unit area
Absolute pressure: The actual pressure at a given position. It is measured relative to absolute vacuum (i.e., absolute zero pressure).
Gage pressure: The difference between the absolute pressure and the local atmospheric pressure. Most pressure-measuring devices are calibrated to read zero in the atmosphere, and so they indicate gage pressure.
Vacuum pressures: Pressures below atmospheric pressure.
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SYSTEMS System: A quantity of matter or a region in space chosen for study.
Surroundings: The mass or region outside the system
Boundary: The real or imaginary surface that separates the system from its surroundings.
The boundary of a system can be fixed or movable. ME
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TYPES OF SYSTEM Closed system
Open System
Isolated System
Closed system (Control mass):
A fixed amount of mass, and no mass can cross its boundary.
Open system (control volume):
Both mass and energy can cross the boundary of a control volume.
It usually encloses a device that involves mass flow such as a compressor, turbine, or nozzle.
Isolated Sysem
A system which is not affected by the surrounding. No heat, work and mass transfer take place.
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PROPERTIES
OF A SYSTEM
Property: Any characteristic of a system.
Some familiar properties are pressure P, temperature T, volume V, and mass m.
Properties are considered to be either intensive or extensive.
Intensive properties: Those that are independent of the mass of a system, such as temperature, pressure , Specific Volume and density.
Extensive properties: Those whose values depend on the mass, Mass, volume, total energy, weight. Criterion to differentiate
intensive and extensive
properties.
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STATE AND EQUILIBRIUM
Thermodynamics deals with equilibrium states.
Equilibrium: A state of balance.
In an equilibrium state there are no unbalanced potentials (or driving forces) within the system.
Thermal equilibrium: If the temperature is the same throughout the entire system.
Mechanical equilibrium: If there is no change in pressure or un balance force at any point of the system with time.
Phase equilibrium: If a system involves two phases and when the mass of each phase reaches an equilibrium level and stays there.
Chemical equilibrium: If the chemical composition of a system does not change with time, that is, no chemical reactions occur.
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PROCESSES Process: Any change that a system undergoes from one equilibrium state to
another.
Path: The series of states through which a system passes during a process.
To describe a process completely, one should specify the initial and final states, as well as the path it follows, and the interactions with the surroundings.
Quasistatic or quasi-equilibrium process: When a process proceeds in such a manner that the system remains infinitesimally close to an equilibrium state at all times.
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CONTINUUM Matter is made up of atoms that are
widely spaced in the gas phase. Yet it is very convenient to disregard the atomic nature of a substance and view it as a continuous, homogeneous matter with no holes, that is, a continuum.
The continuum idealization allows us to treat properties as point functions and to assume the properties vary continually in space with no jump discontinuities.
This idealization is valid as long as the size of the system we deal with is large relative to the space between the molecules.
This is the case in practically all problems.
In this text we will limit our consideration to substances that can be modeled as a continuum.
Despite the large gaps between molecules, a substance can be treated
as a continuum because of the very
large number of molecules even in an
extremely small volume.
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MACROSCOPIC & MICROSCOPIC
APPROACH
Classical thermodynamics: A macroscopic approach to the study of thermodynamics that does not require a knowledge of the behavior of individual particles.
It provides a direct and easy way to the solution of engineering problems.
Statistical thermodynamics: A microscopic approach, based on the average behavior of large groups of individual particles.
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REVERSIBLE AND IRREVERSIBLE
PROCESSES
A reversible process is defined as a process
that can be reversed without leaving any trace
on the surroundings That is, both the system and
the surroundings are returned to their initial
states at the end of the reverse process. This is
possible only if the net heat and net work
exchange between the system and the
surroundings is zero for the combined
Irreversible Process
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CHARACTERISTIC GAS EQUATION
General Gas Equation
pV/ T = C
pV = mRT
Specific Heat Capacity (C)
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BASICS OF REFRIGERATION
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BASICS
Second law of thermodynamics
Clausius statement
Heat vs Temperature
Relation Between Pressure & temperature
Boiling point and Freezing point (Phase Change)
Latent Heat
Critical point
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REFRIGERATION
Process of removing heat from a
substance under controlled
conditions.
Also process of reducing heat and
maintaining the temp. of a body
below the general temp. of its
surroundings.
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COEFFICIENT OF PERFORMANCE
• The efficiency of a refrigerator is expressed
in terms of the Coefficient of performance
(COP).
• COP of Refrigerator can be greater than
unity
innet
LR
W
QCOP
,inputWork
effect Cooling
Input Required
Output Desired
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TONNE OF REFRIGERATION
1 tonne of refrigeration is the rate of heat
removal required to freeze a metric ton
(1000 kg) of water at 0°C in 24 hours.
Based on the heat of fusion being 333.55
kJ/kg
1 tonne of refrigeration = 13,898 kJ/h = 3.861
kW.
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REFRIGERANT
Working fluid used in the refrigeration cycle
Heat carrying medium which during their
cycle in a refrigeration system absorbs heat
from a low temp. system and delivers it to a
higher temp. system
• Halocarbon compounds (R11, R12)
• Azeotropes
• Hydrocarbons (R50, R170)
• Inorganic compounds (R717, R718)
• Unsaturated Organic compounds (R1120, R1130)
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Thermodynamic Properties
o Critical Temperature & Pressure - High
o Boiling point – Low
o Freezing point – Low
o Enthalpy of Vaporization - High
o Thermal Conductivity - High
o Coefficient of Performance - High
PROPERTIES OF REFRIGERANTS M
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REFRIGERATOR M
EC
H-K
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VAPOR-COMPRESSION REFRIGERATION
CYCLE
► There are four principal
control volumes involving
these components:
►Evaporator
►Compressor
►Condenser
►Expansion valve
► Most common refrigeration cycle in use today
All energy transfers by work and heat are taken as positive
in the directions of the arrows on the schematic and energy
balances are written accordingly.
Two-phase
liquid-vapor mixture
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THE VAPOR-COMPRESSION
REFRIGERATION CYCLE
Process 4-1: two-phase liquid-vapor
mixture of refrigerant is evaporated
through heat transfer from the
refrigerated space.
Process 1-2: vapor refrigerant is
compressed to a relatively high
temperature and pressure requiring
work input.
Process 2-3: vapor refrigerant
condenses to liquid through heat
transfer to the cooler surroundings. Process 3-4: liquid refrigerant
expands to the evaporator pressure.
►The processes of this cycle are
Two-phase
liquid-vapor mixture
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REVERSED CARNOT CYCLE M
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IDEAL VAPOR COMPRESSION
REFRIGERATION (VCR) CYCLE
1-2 Isentropic compression in a compressor
2-3 Constant-pressure heat rejection in a
condenser
3-4 Throttling in an expansion device
4-1 Constant-pressure heat absorption in an
evaporator
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P
h
THE IDEAL VCR CYCLE ON THE P-H DIAGRAM
2 1m h h &
2 3m h h &
1 4m h h &
3 4h h1
23
4
1-2: Isentropic compression
2-3: Isobaric heat rejection
3-4: Isenthalpic expansion
4-1: Isobaric heat addition
/in inq Q m & & /c cw W m & &
/out outq Q m & &
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PROPERTIES OF PURE
SUBSTANCE
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PURE SUBSTANCE
A substance that has a fixed chemical composition
throughout is called a pure substance.
Water, nitrogen, helium, and carbon dioxide
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PHASES
Solid liquid gas
ice water steam
One species of molecules can aggregate into several forms, known as phases.
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FORMATION OF STEAM M
EC
H-K
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P-V DIAGRAM M
EC
H-K
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Saturated Liquid line , Saturated Vapour line,
Saturated solid line
Triple line(Where all the three phases solid, liquid,
and gas exist in equilibrium)
P-T Diagram (Triple point)
0.01 C or 273.16 K , 0.00611 Bar
Solid to Vapour (below triple point pr) –SUBLIMATION
Critical Point
221.2 bar
374.15 C
Liquid to Vapour (No Liquid- Vapour Mixture)
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P-T DIAGRAM
Fusion Curve
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T- V DIAGRAM
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T- S & H-S DIAGRAM
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P-V-T DIAGRAM M
EC
H-K
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DRYNESS FRACTION OF STEAM
Dryness fraction of steam
(Quality of a vapour) x = mass of
vapour/total mass of the mixture
= mg/mg+mf
x=1 (saturated vapour line)
x=0 (saturated liquid line)
Wet steam
Dry steam
Superheated steam V> vg = superheated steam
V = vg = dry steam
v < vg = wet steam
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Properties of steam at 1 Mpa
Saturated steam has a entropy of 6.76 kj/kg K. what
are its pr,temp,v,h.
Find the enthalpy, entropy and volume of steam at
1.4 Mpa, 3800C
Determine the Condition of Steam
(Dry,wet,Superheater)
10 bar, 0.22 m3/kg
15 bar, 2250C
2000C , 2790.9 kJ/kg
1200C , 7 kJ/kg K
Find the enthalpy and entropy of steam when the
pressure is 2 Mpa and sp. Volume is 0.09 m3/kg
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