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Chapter two The laws of thermodynamic
3
Chapter one Introduction
1.0 The word thermodynamics
Thermo – is the Greek word meaning hot or heat.
Dynamics -Is the study of matter in motion, from the Greek word meaning power.
1.1 What is thermodynamics as field of study?
Def (1) it is science in which the storage, the transformation and the transfer of energy are studied.
Energy is stored as internal energy, kinetic energy, potential energy and chemical energy. It is
transformed from one of these specifics to another and it is transferred across a boundary as either
heat or work. Thermodynamics is a system of mathematical equations that relate the
transformations and transfer of energy to the material properties such as temperature, pressure and
enthalpy.
Def (2) it is the science of the relationship between heat, work and the properties of systems, it is
concerned with means necessary to convert heat energy from available sources such as fossil fuels
into mechanical work.
1.2 Why do engineers study thermodynamics?
They are concerned with how much heat energy can be effectively converted into work and vice
versa in the case of refrigeration.
1.3 Historical background to the thermodynamics
Man used his muscles as the source of power at the beginning to carry, walk etc.
Later animals were used for carrying purposes and in ploughing fields.
Wind was the next source of power for driving vessels, milling, sawing etc.
Water was the next source of power but its disadvantage was that it was not always
available.
Steam engines were developed in the seventeenth century
Internal combustion engines were next to being developed.
Hydroelectric power was the next
Currently people are turning to solar power.
1.4 What is a thermodynamic system?
Is a definite quantity of matter contained within a closed surface. All matter and space external to
the system is called its surroundings. A system interacts with its surroundings by transferring
energy, not matter across its boundary. If a system does not exchange energy with its surrounding
it is an isolated system.
1.5 Types of energy
Internal energy- it is that energy which results from the random motion of the atoms and
molecules of a body. An internal energy increase does not always result in increase in temperature
Chapter two The laws of thermodynamic
4
of the body e.g. during phase change the temperature does not change. Internal energy is a
property of the substance.
Heat- it is a transient quantity, it describes the energy transfer process through a system of
boundary resulting from temperature difference. Heat ceases to exist when the process of heat
transfer ceases.
Potential energy – If a fluid is at some height Z above a given datum level, then as result of its
mass it possess gravitational potential energy with respect to the datum.
Potential energy per unit mass =gZ…………………………………………1.1
Work- if a system exists in which a force at the boundary of the system is moved through a
distance then work is done by or on the system. Work is therefore a transient quantity, being
descriptive of that process by which a force is moved through a distance.
W = PV………………………………………1.2
Kinetic energy- is the energy that can be obtained from a moving body by slowing it down. The
maximum energy is obtained by slowing the body down to rest
k. e. =1/2mc2 ……………………………………….1.3.
Chapter two The laws of thermodynamic
5
Chapter two
Laws of thermodynamics
2.0 Introduction
The laws of thermodynamics are really statements of thermodynamic behavior. They are natural
laws, which are based on observable phenomena. These are considered as law because they have
never been shown to be contradicted.
2.1 The Zeroth law of thermodynamics.
It states that if two bodies are separately in thermal equilibrium with a third body then they must
be in thermal equilibrium with each other. If bodies B and C are in thermal equilibrium with body
A then bodies B and C must be in thermal equilibrium with each other. By thermal equilibrium is
meant that there is no change of state and hence the zeroth law implies that the bodies A, Band C
will all be at the same temperature.
Thermal Equilibrium
It is observed that a higher temperature object, which is in contact with a lower temperature
object, will transfer heat to the lower temperature object. The objects will approach the same
temperature, and in the absence of loss to other objects, they will then maintain a constant
temperature. They are then said to be in thermal equilibrium. Thermal equilibrium is the subject of
the Zeroth Law of Thermodynamics.
The "zeroth law" states that if two systems are at the same time in
thermal equilibrium with a third system, they are in thermal
equilibrium with each other.
If A and C are in thermal equilibrium with B, then A is in thermal equilibrium with B. Practically
this means that all three are at the same temperature, and it forms the basis for comparison of
temperatures. It is so named because it logically precedes the First and Second Laws of
Thermodynamics.
Application
Measurement of temperature of a body using mercury in glass thermometer, when the
thermometer is steady, it is assumed that the mercury, the glass container and the body whose
temperature is being measured, are all at the same temperature and hence, are in thermal
equilibrium.
2.2 The first law of thermodynamics
Chapter two The laws of thermodynamic
6
Statement 1
Net heat transfer - net work transfer = 0
Net heat transfer = net work transfer
§ Q = § W………………………………………………………………..2.1
Written symbolically § Q = § W § means the summation round the cycle.
The implications of the above statement are that there should be heat transfer for there to be work
done
Statement 2
If the heat transfer is not the same as work then some of the heat has been converted into internal
energy.
Q = U + W …………………………………………………………………2.2
where Q is the heat transfer,
U change of internal energy.
and W is the work transfer.(work done by the system)
Statement 3
The steady flow energy equation is a further statement of the first law of thermodynamics
U1 + p1v1 +2
1
2C
+ gZ1+Q = U2 +p2v2 +2
2
2C
+ gZ2 + W……………………….2.3
Where U = specific internal energy
p1v1 = specific flow work
C = velocity, it gives specific K.E.
Z = height above given datum level ( gives gravitational
potential Energy)
Q = heat transfer
W = work transfer
2.3 The second law of thermodynamics
It is a directional law in that it states that the heat transfer will occur down a temperature gradient
as a natural phenomenon. Heat transfer can occur up the gradient but not without the aid of
external energy e.g. in refrigeration and heat pumps. The second law of thermodynamics is a
general principle which places constraints upon the direction of heat transfer and the attainable
efficiencies of heat engines. In so doing, it goes beyond the limitations imposed by the first law of
thermodynamics.
Chapter two The laws of thermodynamic
7
2.3.1 The concepts of the second law of thermodynamics
Rudolf Claussius (1822-1888)
It is impossible for a self-acting machine, unaided by an external agency, to convey heat
from a body at low temperature to one at a higher temperature.
Lord Kelvin (1824-1907)
We cannot transfer heat into work merely by cooling a body already below the temperature
of the coldest surrounding objects.
Marx Planck (1858-1947)
It is impossible to construct a system, which will operate in a cycle, extract heat from the
reservoir, and do an equivalent amount of work on the surroundings
Kelvin – Planck
It is impossible for heat engine to produce net work in a complete cycle if it exchanges
heat only with bodies at a single fixed temperature.
Second Law: Heat Engines
Second Law of Thermodynamics: It is impossible to extract an amount of heat QH from a hot
reservoir and use it all to do work W. Some amount of heat QC must be exhausted to a cold
reservoir. This precludes a perfect heat engine.
This is sometimes called the "first form" of the second law, and is referred to as the Kelvin-Planck
statement of the second law.
Second Law: Refrigerator
Second Law of Thermodynamics: It is not possible for heat to flow from a colder body to a
warmer body without any work having been done to accomplish this flow. Energy will not flow
spontaneously from a low temperature object to a higher temperature object. This precludes a
perfect refrigerator. The statements about refrigerators apply to air conditioners and heat pumps,
which embody the same principles.
This is the "second form" or Clausius statement of the second law.
Second Law: Entropy
Second Law of Thermodynamics: In any cyclic process the entropy will either increase or remain
the same.
Entropy:
a state variable whose change is defined for a reversible process at temperature T where Q is the
heat absorbed.
T
QS
Entropy: a measure of the amount of energy, which is unavailable to do work.
Entropy: a measure of the disorder of a system.
Entropy: a measure of the multiplicity of a system.
Since entropy gives information about the evolution of an isolated system with time, it is said to
give us the direction of "time's arrow" . If snapshots of a system at two different times shows one
state which is more disordered, then it could be implied that this state came later in time. For an
Chapter two The laws of thermodynamic
8
isolated system, the natural course of events takes the system to a more disordered (higher
entropy) state.
2.3.2 Implications of the second law of thermodynamics.
Heat transfer will only occur, and will always naturally, when a temperature difference
exists, and always naturally down the temperature gradient.
If due to temperature difference, there is heat transfer availability, then work transfer is
always naturally down the temperature gradient.
Temperature can be elevated but not without the expenditure of external energy. Elevation
of temperature cannot occur unaided.
There is no possibility of work transfer if only a single heat energy source or reserve at
fixed temperature is available.
It is useful to note that if work transfer is supplied to a system then this can all be
transformed into heat energy. Examples of this are seen in the cases friction and the
generation of electricity. Heat energy cannot be all transformed into work transfer; there
will always be some loss. Thus work transfer appears to have a higher value than heat
transfer.
No contradiction with the first law of thermodynamics has been demonstrated.
From this second law it follows that inorder to run all the engines and devices in use at
present, and hence to maintain and develop modern industrial society, a source of supply
of suitable fuels is essential it is by burning and consuming these fuels that the various
working substances have their temperatures put up above that of their surroundings, that’s
enabling them to release energy by heat transfer in a natural manner according to the
second law of thermodynamics.
2.4 The third law of thermodynamics
The law suggests that the internal energy of a substance results from the random motion of
the atoms and the molecules which makeup the substance, the motion of the atoms is
associated with the temperature and it develops the idea of an absolute zero temperature
when all random motion ceases. The above considerations led to the development of the
third law of thermodynamics, which is the concept that at absolute zero of the temperature
the entropy of a perfect crystal of a substance is zero.
2.5 Conclusion
The laws of thermodynamics govern the way thermodynamic processes take place.
The zeroth law compares the temperature of two bodies. The first law is a conservation of energy
principle. The second law indicates the direction in which the heat would flow. The third law
gives the relationship between kinetic energy of particles and the temperature of the body.
Chapter two The laws of thermodynamic
9
Chapter three
The properties of the thermodynamic media
3.0 Introduction
The molecules of a gas are in a rapid and random motion such that they fill completely the
container in which they are placed, the rapidly moving molecules continually bombard the surface
of the container and their effect is to produce a force normal to the surface, the number of impacts
per unit time is so large that it appears as if the force is continuous and uniform.
Varying any one of the gas properties such as pressure, temperature, volume, density will witness
the change in other properties.
Heat: is defined as thermal energy transferred across the boundaries of a system mainly because
of temperature difference between the two points. Specifically heat is transferred from a body of
higher temperature to a body in contact, which is at a lower temperature unless aided by
mechanical means to act otherwise.
Specific heat capacity of a body is the amount of heat required to raise one kg of a substance
through one degree.
Specific heat capacity t
Qc
in the limit as 0t , then
dt
dQC
The specific heat capacity is generally found to vary with temperature; they also vary with
pressure and volume. Cp denote the specific heat capacity at constant pressure and at constant
volume it is represented by Cv
For a solid the quantity of heat energy Q = mct
Q = mc(T1-T2)
For a gas of mass m heat added at constant pressure is given by
Q = mcp(T1-T2)……………………………………. .3.1
The heat added at constant volume Q = mcv(T1-T2)…….……………………… ………….3.2
Joule`s law states that the internal energy of a body/ perfect gas is a function of absolute
temperature only.
U = f (T)
But from the first law of thermodynamics the energy supplied to the gas is given by
Q = U + W
U — is internal energy ,
W — is the work done
But at constant volume W = 0
then Q = U
but also at constant volume Q = mCv T
Chapter two The laws of thermodynamic
10
for one kg Q = Cv T
Q = Cv (T2-T1) + k
3.1 Relationship between specific heats
Q = U + W
= m Cv (T2 -T1) + W
but W = P(V2 - V1)
also PV = mRT
W =mR(T2 - T1)
Heat supplied to the system Q = mCv(T2 - T1) + mR(T2 - T1)
But also Q =mCp(T2-T1) for constant pressure
Comparing the two equations above it is deduced that
Cp = Cv + R
Cp - Cv = R……………………………………………………………3.3
3.2 Ratio of specific heats It has been proved that,
constantC
C
v
p
v
p
C
C …………………………………………..………………………….3. 4
is the expansion/ compression index
Cp = Cv
But from above Cp – Cv= R
Dividing through out by Cv
VV
V
V
P
C
R
C
C
C
C
- 1 =R/Cv
1-
RC
V ……………………………………………………………………………3.5
Chapter two The laws of thermodynamic
11
3.3 Partial pressures:
Dalton’s and Gibbs law
The relationship between the partial pressures of the constituent gases is expressed by Dalton`s
law as follows:
The pressure of a mixture of a gas is equal to the sum of the partial pressures of the constituents.
The partial pressure of each constituent is that pressure which the gas would exert if it occupied
alone that volume occupied by the mixture.
The total pressure P= Partial pressure of gas1 + partial pressure of gas 2 + partial pressure gas 3
Thus P = P1 + P2 + P3
Thus from the characteristic gas equation Pv = mRT substituting for the pressure of each gas and
also for the mixture
3
333
2
222
1
111
V
TRm
V
TRm
V
TRm
V
mRT
Since it can be considered as though each gas occupy the same volume, then the volume is
common throughout. The temperature is also common.
MRt = T(m1R1 + m2R2 + m3R3 + etc)………………………………………………………….3. 6
Where m is the total mass of the mixture and R is the gas constant of the mixture.
3.4 The ideal gases
The various laws governing the pressure- volume-temperature relations of gases as discussed in
this section apply accurately only to a hypothetical ideal or perfect gas. A perfect gas is described
as one, in which there is no interaction between the molecules of the gas. The molecules of such a
gas are entirely free and independent of each other’s attraction forces. Hence none of the energy
transferred either to or from an ideal gas has an effect on the internal potential energy.
At high temperature and low pressure gases approach the ideal gas, at low pressure the density
and intermolecular forces become very small. Under this situation the gases obey the law
RT
PV
Where R is the characteristic gas constant whose units are kJ/kgK
Each perfect gas has a different gas constant
For unit mass P v = RT
For m kg Pv = mRT…
the above is known as the characteristic gas equation
for a substance of molecular weight M =m/n, where n is the number of moles, the equation
becomes PV = nMRT
Chapter two The laws of thermodynamic
12
nT
PVMR
Avogadro`s hypothesis states that that the volume of one mole of any gas is the same as the
volume of any other gas at the same temperature and pressure
Thus V/n is the same for all gases at the same temperature and pressure
Thus Tn
PV is constant for all gases
Therefore Tn
PVRMR
0
Where R0 is the molar gas constant or universal gas constant
PV = n R0 T………………………………………………………………………3.7
R0 = 8314, 5J/kmol
3.5 Expansion and compression of ideal gases
Introduction
The state of a working fluid can be identified by its thermodynamic properties, which are
pressure, temperature, volume, internal energy, entropy etc. if two of the properties are chosen
they are enough to define the state of a system and this state is represented by a point situated on
the diagram of the properties shown below.
Fig 3. 1 Pressure volume diagram Fig 3.2 Pressure and Temperature diagram
1
2
3
p1
p2
p3
V1 V2 V2
1
2
3
p1
p2
p3
T1 T2 T2
Chapter two The laws of thermodynamic
13
3.5.1 Reversibility
Definition – when a fluid undergoes a reversible process, both the fluid and its surrounding can
always be restored to their original state.
Conditions of reversibility: The process must be frictionless (no internal friction and mechanical friction).
The differences in pressure between the fluid and its surrounding during the process must
be infinitely small.
Difference between the fluid temperature and its surrounding must be infinitely small.
When a fluid undergoes a reversible process a series of state points can be joined up to
form a line on a diameter of properties.
The work done by a fluid during an irreversible process is given by the area under the P-V
diagram
P1
P2
V1 V2 Volume
pre
ssure
1
2
Fig3.3 Pressure– volume relationship
Work done is the area under graph 1-2 = v
v
1
2
Pdv
3.5.2 The isothermal process
Also known as the constant temperature process
When a gas in the cylinder is compressed from v1 to v2 the temperature of the gas will increase
but if the change takes place slowly there will be a very small change in temperature. In the latter,
when a lapse of time is allowed the temperature will return to its original value. And the process
will approximate an isothermal process.
When the volume of the gas is increased or decreased under such conditions that the temperature
remains constant the absolute pressure will vary inversely with the volume.
Chapter two The laws of thermodynamic
14
Boyles laws
It states that when the temperature of the body is maintained constant as its volume is varied, the
change in absolute pressure is inversely proportional to the volume
V
1P
PV = C
P1V1 = P2V2 …………………………………………………..3.8
P1
P2
V1
V2 Volume
pre
ssure
1
2
Vv
P
PV = C
Fig. P-v Diagram showing work done in an isothermal process
Work done during an isothermal process dvP
V2
V1
w
but V
CP therefore dv
V
C
V2
V1
w
W = C [ ln ] 2
1
v
vInCW
Then PV = C then 1
211
V
VlnVPW ………………………………3.9
Heat transfer during constant temperature process
Q = U + W
Chapter two The laws of thermodynamic
15
But U =0 since there is no temperature change
Q = W
3.5.3 Constant pressure process
If the temperature of the gas is increased by the addition of heat while the gas is allowed to
expand and its pressure is maintained constant, then the volume of the gas will increase in
accordance with Charles law.
Charles law states that:
When energy is supplied to a gas under such conditions that the pressure of the gas is kept
constant, then the volume of the gas will increase in direct proportion to the change in absolute
temperature of the gas.
V T
V/T = constant
V1/T1 =V2/T2………………………………………………………….3.10
Force exerted on the piston = P A
Work done in pushing piston = PAL
But AL = V2- V1
P
V1 V2
L
Area (A) Piston
Fig 3.5 Work done at constant pressure
Work done on the piston = P(V2–V1) ……………………………………………….3.11
Heat transfer Q = U + W…………………………………...……………….3.12
Chapter two The laws of thermodynamic
16
3.5.4 Constant volume process ( isochoric)
Assume that the gas is confined in a closed cylinder so that its volume cannot change as it is
heated or cooled, as the energy to the gas is varied, the absolute pressure will increase
proportionally to the increase in absolute temperature
Combining Charles law and Boyles law
2
22
1
11
T
VP
T
VP Known as the characteristic gas equation
For constant V, V1 =V2
2
2
1
1
T
P
T
P …………………………………………………………….……..3.13
Work done at constant volume W = 0
Heat transfer at constant volume Q = U + W
but W = 0
Q = U
= mC
= mCv(T2- T1)……………………………………….3.14
3.5.5 Adiabatic compression and expansion: Also known as the constant energy process
Def – an adiabatic process occurs when the compression or expansion of a gas takes place without
an heat flow out or into the system ( it occurs very fast)
If a gas expands or is compressed in a cylinder, which is well lagged, and the change takes place
very quickly the conditions are approximately adiabatic. An adiabatic process is a special case of a
polytropic process
Polytropic expansion or compression of gases
PVn = C
All expansions of the above form are polytropic
P1V1n = P2V2
n………………………...…………………3.15
Also PV/T =C then 2
22
1
11
T
VP
T
VP ………………………….………..…………………3.16
From 3.15
1
2
1
2
1
2
V
V
P
P
T
T…………………………………………………3.17
Chapter two The laws of thermodynamic
17
From 3.16 (V2/V1)n = P1/P2
V2/V1 = (P1/P2)1/n
= (P2/P1) –1/n
……………..…………………………………….3.18
substituting into 17, T2/T1 = P2/P1 (P2/P1) –1/n
T2/T1 =P2/P1 n-1/n
……………………….…………………………………………….………3.19
from 2 T2/T1 =P2V2/P1V1
From 1 P2/P1 =V1/V2 n
Then T2/T1 = (V1/V2)n x V2/V1
= (V1/V2)n x (V1/V2)
–1
T2/T1 = ( V1/V2)n-1
…………………………………………………………3.20
3.5.6. For non-flow processes Work done during a polytropic expansion
P1
P2
V1
V2 Volume
pre
ssure
1
2
Vv
P
PVn = C
Work done = area under the curve 1-2
dvP
V2
V1
w
Chapter two The laws of thermodynamic
18
but nV
CP therefore dv
V
C
V2
V1
nw
= C[ V1-n ]
v
v
1
2
1-n
=
n1
VPVP 1122
…………………………….……………………..………………..3.21
=
1n
VPVP 2211
……………………………………………………………………..3.22
ALSO Since PV = mRT W =
1n
TTmR 21
For non-flow processes
Work done during an adiabatic expansion
P1
P2
V1
V2 Volume
pre
ssu
re
1
2
Vv
P
PVγ = C
Work done = area under the curve 1-2
dvP
V2
V1
w
Chapter two The laws of thermodynamic
19
but
V
CP therefore dv
V
C
V2
V1
w
= C[ V1-]v
v
1
2
1-
=
1
VPVP 1122 ………………………..………………..3.23
=
1
VPVP 2211
……………………………………………………………………………………..3.24
ALSO Since PV = mRT W =
1
TTmR 21
Worked examples
QUESTION 1
A petrol engine cylinder has diameter of 9,5 cm and stroke 12,7 cm, clearance volume 230 cm3. If the
temperature at the beginning of the compression is 570C,
Find the temp at the end of compression, and the work done during the compression stroke if the law
of compression is pV1.3
= c. take the initial pressure as 100 kN/m2.
SOLUTION
V2 = VC = 230 X 10-6
V1 = 10 230 0.127095.04
6-2 X X X
= 1130 X 10-6
From 3.111
3.122 VPVP
3.1
2
12
V
V100P
3.1
2230
1130100P
P2
P1
V2=VC V1=VC+VS Volume
pre
ssu
re
2
1
VC VS
Chapter two The laws of thermodynamic
20
= 792.1kN/m2
Temperature
From 2
22
1
11
T
VP
T
VP
11
2212
VP
VPTT
1301100
2307921330T2
X
X
= 532K or 259oC
work done
W = 1n
VPVP 2211
W = 3.0
102301.792101130100 66 XXXX
= -0.23061kJ
= -230.61J
(–)indicates work done on the gas
QUESTION 2
1 m3 of air, initially at 110 kN/m
2 and 15
0C, is compressed according to the law pV
1.3 = c in a
cylinder to a final pressure of 1.4 MN/m2 . Taking R for air = 287 J/kgK and cp = 1005 J/kgK,
determine
a) the volume and temp of air at the end of compression;
b) the work done in compressing the air;
c) the change of internal energy;
d) the heat exchange through the cylinder walls, stating the direction of heat flow.
a) i)
3.1
1
2
112
P
PVV
Chapter two The laws of thermodynamic
21
3.1
1
21400
1101V
= 0.141m3
ii) n
1n
1
212
P
PTT
3.1
13.1
2110
1400288T
= 518 K or 245oC
b) work done
W = 1n
VPVP 2211
W = 3.0
141.014001110 XX
= -291.3kJ
C) U2 – U1 = mcV(T2 – T1)
But RT
PVm =
288287.0
1110
= 1.33
CP - CV = R
Thus Cv = 1.005 - 0.287
= 0.718 kJ/kg
U = 1.33 x 0.718(518 – 288)
= 219.77 kJ/kg
Heat flow Q = W + (U2 – U1)
= –291.3 + 219.6362
= –71.6638 kJ/kg
QUESTION 3
1 kg of a certain gas expands adiabatically in a closed system until its pressure is halved. During the
expansion the gas does 67 kJ of external work and its temp falls from 2400C to 145
0C. Calculate the
value of the adiabatic index and the characteristic constant of the gas.
Chapter two The laws of thermodynamic
22
From
1
1
2
1
2
P
P
T
T
1
2
1
513
418
0.814814814 =
1
2
1
log 0.8 =
1 log
2
1
1 =
5.0log
8.0log
1 = 5.0log
8.0log
- 0.295γ = 1
0.7 = 1
= 1.419
Work done
W =
1
TTmR 21
67 =
1
TTR 21
R =
21 TT
167
R = 418513
419.067
= 0.2955kJ/kg
QUESTION 4
In a closed system, 1 kg of air initially at 100 kN/m2 and 27
0C is compressed adiabatically to 3
MN/m2 and then expanded isothermally back to its original volume. determine the excess of the work
done by the gas over the work done on the gas.Taking R for air = 287 J/kgK and = 1.4.
Chapter two The laws of thermodynamic
23
Given data
m = 1 kg
P1 = 100 kN/m2
T1 = 300K
P2 = 3 000 kN/m2
R = 0.287 kJ/kgK
Final temperature—adiabatic process
1
1
212
P
PTT
4.1
4.0
2100
0003300T
K7858662.792T2
Adiabatic work
W =
1
TTmR 21
W =
14.1
793300287.01
W = –353.573859 kJ
Isothermal work
2
322
V
VlnVPW
But P2V2 = mRT2 2
32
V
VlnmRTW
Also 2
1
2
3
V
V
V
V
From adiabatic process
2
3
1
1
2
2
1
V
V
P
P
V
V
4.114.1
1
1
30100
0003
P2
P1
V2 V1=V1 Volume
pre
ssu
re
2
1
3P3
Chapter two The laws of thermodynamic
24
thus Work 4.11
2 30lnmRTW
4.11
30ln7858662.792287.01W
= 552.7663485 kJ
= 552.8 kJ
Excess of the work done
= 552.7663485 kJ –353.573859kJ
= 199.1924895kJ
Chapter 3
Tutorial questions
1. A volume of 0.5 m3 of gas is expanded in a cylinder from a pressure of 660 kN/m
2 and temp 165
0C
to a pressure of 120 kN/m2 according to the law pV
1.3 = c. Find:-
a) the final volume and temp of air ;
b) the work done by the air during the expansion;
c) the change of internal energy during expansion;
d) the heat exchange through the cylinder walls, stating the direction of heat flow.
Take Cv = 710 J/kg K and R for air = 287 J/kg K.
2. Air is expanded adiabatically from a pressure of 800 kN/m2 to
128 kN/m2. If the final temp is 57
0C, calculate the temp at the beginning of expansion, taking = 1.4.
3.The ratio of compression in a petrol engine is 9 to 1. Find the temp of the gas at the end of
compression if the temp at the beginning is 240C, assuming compression to follow the law pV
n =
constant where n = 1.36.
4.The vol. and temp of a gas at the beginning of expansion are 0.0056 m3 and 183
0C, at the end of
expansion the values are 0.0238 m3 and 22
0C respectively. Assuming expansion to follow the law
pVn = constant, find the value of n.
5. 7.08 litres of air at a pressure of 13.79 bar and temp 3350C are expanded according to the law
pV1.32
= constant, and the final pressure is 1.206 bar. Calculate
i) the vol at the end of expansion
ii) the work transfer from the air
iii) the temp at the end of expansion
Chapter two The laws of thermodynamic
25
iv) the mass of air in the system taking R for air = 287 J/kgK.
6. A perfect is compressed in a cylinder according to the law pV1.3
= constant. The initial condition
of the gas is 1.05 bar, 0.34 m3 and 17
0C. If the final pressure is 6.32 bar, calculate:-
a) the mass of gas in the cylinder;
b) the final volume;
c) the final temperature;
d) the work done to compress the gas;
e) the change in internal energy;
f) the transfer of heat between the gas and cylinder walls.
7. Assume a compression according to the law PV = CONSTANT,
i. Calculate the final volume when 1m3 of gas at 120 k N/m
2 is compressed to a
pressure of 960 k N /m2.
ii. Calculate the initial volume of gas at a pressure of 1.05 bar, which will occupy
a volume of 5.6m3
when it is compressed to a pressure of 42 bar.
iii. 0.25m3 of gas at temperature of 21
0C is heated at constant pressure to a
temperature of 3150C. Calculate the final volume.
8. A closed vessel contains air at a pressure of 140kN/m2 gauge and temperature 20
0C. Find the
final gauge pressure if the air is heated at constant volume to 400C. Take the atmospheric pressure
as 759mm Hg.
9.Taking the characteristic gas constant R for nitrogen as 0.297kJ/kgK., calculate:
i. The mass of 0.05m3 of nitrogen at 550kN/m
2 and 28
0C.
ii. the volume of 1kg of nitrogen at 1MN/m2 at 0
0C.
10.An air reservoir contains 20kg of air at 3200kgkN/m2 gauge and 16
0C. Calculate the new
pressure
and heat energy transfer if the air is heated to 350C. Neglect any expansion of the reservoir, take
the
R for air =0.287kJ/kgK, specific heat at constant volume Cv =0.718kJ/kgK, and atmospheric
pressure = 100kN/m2.
11. heat energy is transferred to 1.36kg of air which causes its temperature to increase from
400C to 468
0C. calculate for two separate cases of heat transfer at a). Constant volume b).
Constant pressure:
i. the quantity of heat energy transfer
ii. the external work done
iii. the increase in internal energy
Take Cv and Cp as 0.718 and 1.005kJ/kgK respectively.
12. A closed vessel of 500cm3 capacity contains a sample of flue gas at 1.015 bars and 20
0C. If
the analysis of the gas by volume is 10% CO2. 8% O2, and 82% n2 calculate the partial
pressure and mass of each constituent in the sample. R for CO2, O2 and N2 =0.189, 0.26
and 0.297kJ/kgK respectively.
13. Gas is expanded in an engine cylinder according to the law Pvn =C. at the beginning of
the expansion the pressure and the volume are 1750kN/m2 and 0.05m
3 respectively, and at
the end of expansion the respective values are 122.5kN/m2 and 0.375m
3. calculate the
value of n.
Chapter two The laws of thermodynamic
26
14. 0.113m3 of air at 8.25 bar is expanded in cylinder until the volume is 0.331m
3 . calculate
the final pressure and the work done if the expansion is ;
i. isothermal,
ii. adiabatic, taking =1.4
15. a gas is expanded in a cylinder behind a gas tight piston. At the beginning of the expansion
the pressure is 36bar, volume 0.125m3 and temperature 510
0C. at the end of expansion the
volume is1.5m3 and the temperature 40
0C. Taking R =0.284kJ/kgK and Cv =0.71kJ/kgK,
calculate;
i. the pressure at the end of expansion.
ii. The index of expansion
iii. The mass of gas in the cylinder,
iv. the change in internal energy,
v. work done by the gas
vi. heat transfer during expansion.
Chapter two The laws of thermodynamic
27
Chapter four
The first law of thermodynamics
4.0 Introduction:
Conservation of mass states that the energy can neither be created nor destroyed but can be
changed from one form to another. The total energy in a system remains constant hence
initial energy of the system plus energy entering the system is equal to the final energy of
the system plus energy leaving the system.
4.1 Energy forms in thermodynamics:
Gravitational potential energy, for unit mass of fluid potential energy =gz where z is some
height above a given datum.
Kinetic energy, k.e. = C2/2 where C is the velocity of flow of the fluid.
Internal energy U –all fluids store energy. The energy stored within the fluid results from
the internal motion of the atoms and molecules.
Heat received or rejected (Q)- in an system a fluid can have a direct reception or rejection
of heat through the system boundary. Heat received is positive heat rejected is negative.
External work done (W)
In any system a fluid can do external work or have external work done on it, transferred
through the system boundary. External work done by the system is positive, external work
done on the system is negative.
4.2 The-closed system: The substance enclosed by the system will possess internal energy U, there could also be
some other random energies, which are electrical, magnetic and surface tension but these
forms of energy will be neglected as being insignificantly small.
In a closed system the sum of all the energies possessed by the contained substance called
the total energy E:
E = U + P.e + K.e
Process carried out on a closed system:
E1 = initial energy of the contained substance
E2= final total energy of the contained substance
Q = heat transferred to or from the substance.
W = work transferred to or out of the system.
E1 +Q = E2 + W
4.3 The non-flow energy equation:
It was stated that the sum of all energies possessed by the contained substances was called
total energy E, where
E = U + P.E + K.E
Chapter two The laws of thermodynamic
28
If the substance is considered to be at rest then there is no turbulence. In this case the random
potential and kinetic energy will be zero. Thus for a substance at rest the contained energy will be
only internal energy then equation 1 becomes.
U1 + Q = U2 + W
Q = U2-U1 + W………………………………………………..4.1
4.4 The open system:
The purpose here is to examine the two flow open system in which an equal mass of fluid
per unit time is entering and leaving the system. This is known as the continuity of mass
flow.
Q
W
Input Output
Fig 4.1 energy balance in an open system
Entering
1. internal energy (U)
2. displacement or flow energy (PV)
3. kinetic energy (KE)
4. Gravitational potential ( PE)
Leaving
1. U2
2. KE2
3. P2V2
4. PE2
As the fluid enters the system let the total actual energy of the fluid in the system= E1
after passing through the system as the fluid leaves let the total energy of the fluid mass
remaining in the system = E2 in its passage through the system, let the fluid mass transfer heat
=Q. and the transfer work = W. for two flow open systems:
Fluid mass entering the system =U1 + P1V1 + KE1 + Q1
Energy of fluid mass leaving the region = U2 + P2V2 + PE2 + KE2
Chapter two The laws of thermodynamic
29
from the principle of conservation of energy
U1 + E1 +P1V1 + KE1 + PE1 + Q = U2 + E2 + P2V2 + KE2 + PE2 +W
But U + PV = H = enthalpy
E1 + H1 + PE1 + KE1 + Q = E2 + H2 + PE2 + KE2 + W
Q - W = (E2-E1) + (H2-H1) + (KE2-KE1) + (PE2-PE1)
4.5 The steady flow energy equation
In a stead flow system it is considered that the mass rate of the fluid throughout the system is
constant. It is further considered that the total fluid mass in the system remains constant
For unit mass through the system
U1 + P1V1 +2
C21 + Q + Z1 = U2 + P2V2 +
2
C22 2 + W + Z2 …………. ….4.2
`for most industrial applications the difference in height is negligible Z2-Z1=0
and also U + PV = H
H1 + 2
C21 + Q = H2 +
2
C22 + W………………. ….. . 4.3
W
Q
P1, V1, C1, U1
Entry
P2, V2, C2, U2
Exit
Z2
Z2
Datum
Fig 4.2 energy balance in a steady flow
Chapter two The laws of thermodynamic
30
Worked example 1
A turbine operating under steady flow conditions receives steam at the flowing state; pressure,
13.8 bar, specific volume 0.143m3/kg, specific internal energy 2590 kJ/kg,
velocity 30 m/s. the state of the steam leaving the turbine is as flows: pressure 0.35 bar,
specific volume 4.37m3, specific internal energy 2360 kJ/kg, velocity 90m/s. heat is
rejected to the surroundings at the rate of 0.25 kW and the rate of steam flow through
the turbine is 0.38 kg/s. calculate the power developed in the turbine.
Given data
Entering Leaving
P1 = 1 380 kN/m2 P2 = 35 kN/m
2
V1 = 0.143 m3/kg V2 = 4.37m
3/kg
U1 = 2 590 kJ/kg U2 = 2 360 kJ/kg
C1 = 30 m/s C2 = 90 m/s
= – 0.25 kJ/s
Q = = 38.0
25.0 – 0.657894736kJ/kg
W = (U1 – U2) + (P1V1 – P2V2) + 3
22
21
102
CC
+ Q
= 2 590 – 2 360 + 1 380 x 0.143 – 35 x 4.37 + 3
22
102
9030
– 0.658
= 270.1321kJ/kg
P = W = 270.1321 x 0.38
= 102.65 kW
Q• Q
•
Q•
Q•
m•
2.In the turbine of a gas turbine unit the gases
= – 0.25 kJ/s
Q =
= – 0.657894736kJ/kg
38.0
25.0
m•
Chapter two The laws of thermodynamic
31
Chapter four
Tutorial Questions
The first law of thermodynamics
1.A nozzle is a device for increasing the velocity of a steadily flowing
fluid . At the inlet to a certain nozzle the specific enthalpy of the fluid is 3025 kJ/kg
and the velocity is 60m/s. at exit from the nozzle the specific enthalpy is 2790 kJ/kg
the nozzle is horizontal and there is negligible heat loss from it. Calculate
The velocity of the fluid at exit.
The rate of flow of fluid when the inlet area is 0.1m2 and the specific volume at inlet is
0.19m3 /kg
The exit area of the nozzle when the specific volume at the exit is 0.5m3/kg
[688m/s; 31.6kg/s; 0.0229m2.] esatop
2.In the turbine of a gas turbine unit the gases flow through the turbine at 17 kg/s and the power
developed by the turbine is 14000kW . The specific enthalpies of the gases at
inlet and outlet are 1200kJ/kg and 360kJ/kg respectively, and the velocities of the
gases at inlet and outlet are 60m/s and 150m/s respectively. Calculate the rate at which
heat is rejected from the turbine. Find also the area of the inlet pipe given that the
specific volume of the gases at the inlet is 0.5m3/kg
[119.34KJ/s 0.142m3 ]
Chapter two The laws of thermodynamic
32
Chapter five
The second law of thermodynamics
5.0 Engine cycles and thermal efficiency
During a cycle there will be some heat transfer and work transfer to and from the substance. After
performing the cycle, if the substance returns to its original state then from the first law of
thermodynamics.
§ Q = § W
Thus for the cycle the net work transfer = net heat received- net heat rejected
Thermal efficiency receivedheatnet
doneworknet
Net work done = positive work – negative work
Specific steam consumption kWinoutputPower
hr/kgsteamofflowmass
Specific fuel consumption kWinoutputPower
uesdfuelofflowmass
Chapter two The laws of thermodynamic
33
5.1 The Carnot cycle for the gas
Carnot`s principle states that no engine can be more efficient than a reversible engine working
between the same limits of temperature
Carnot conceived of a cycle made up of thermodynamically reversible process.
Figs 5.1 P-V diagram for Carnot cycle
1-2 isothermal expansion
Work done =P1V1lnV2/V1 = mRT1lnV2/V1
for the isothermal process, Q = W
therefore heat received =mRT1lnV2/V1
2-3 adiabatic expansion
work done =P2V2-P3V3 = mR(T2-T3)
( – 1) ( – 1)
for the adiabatic process Q = 0, there is no heat transfer.
Chapter two The laws of thermodynamic
34
3-4 isothermal compression
Work done = P3V3ln V4/V3 = - P3V3ln V3/V4
= - mRT3lnV3/V4
for the isothermal process, Q = W
Therefore heat rejected = mRT3lnV3/V4
4-1 adiabatic compression
Work done = P4V4- P1V1 = -(P1V1-P4V4)
( – 1) ( – 1)
for the adiabatic Q = 0, no heat transfer during the process
This process returns the cycle to the starting point 1
Net work done per cycle = § W
= area under 1-2 + area under 2-3- area under 3-4 – area 4-1
= area 1 2 3 4
= area enclosed by cycle
§ W =mRT1lnV2/V1+ mRln(T2-T3) - mRT3lnV3/V4 – mR(T1-T4)
( – 1) ( – 1)
now T1 = T2 and T3 = T4 from the isothermals
therefore mR(T2-T3) = mR(T1-T4)
( – 1) ( – 1)
from the above equation
§ W = mRT1lnV2/V1-mRT3ln V3/V4
For the adiabatic 1-4
T1/T4 = (V4/V1) ( – 1)
For the adiabatic 2-3
T2/T3 = (V3/V2) ( – 1)
But T1 =T2 and T3 =T4
Therefore T1/T4 =T2/T3
Hence, from equations above
V4/V1 =V3/V2 or V2/V1 = V3/V4
Substituting equation 6 into equation 2
§ W =mRlnV2/V1(T1-T3)
Chapter two The laws of thermodynamic
35
Thermal efficiency = heat received – heat rejected
heat received
from the above analysis thermal efficiency = mRT1ln(V2/V1) –mRT3ln(V3/V4)
mRT1ln(V2/V1)
= mRln(V2/V1) (T1-T3)
mRln(V2/V1) T1
Since V2/V1 = V3/V4
Therefore thermal = T1 –T3
T1
= Max. absolute temp.– min. absolute temp.
Max. absolute temp .
5.1.1 Carnot efficiency using T-s diagram
Carnot showed the most efficient possible cycle is one with all the heat supplied at one fixed
temperature and then all the heat is rejected at a lower fixed temperature. The cycle therefore
consists of two isothermals joined with two adiabatic
1
23
4
A B
T1
T2
S
T
Fig 5.2 Carnot cycle on a T-s diagram
1-2 isentropic expansion from T1 to T2
2-3 isothermal heat rejection
3-4 isentropic compression from T2 to T1
4-1 isothermal heat supply
The cycle is completely independent of the substance used
The cycle efficiency = - W = Q/Q1
Q1
Chapter two The laws of thermodynamic
36
From the graph the gross heat supplied Q1 is given by the area 41BA4
Q1 =T1( sB-sA)
The net heat supplied Q is given by the area 41234
Q =(T1-T2) (sB-sA)
Hence the carnot cycle efficiency = T1-T2) (sB-sA)
T1( sB-sA)
= (T1-T2)
T1
5.20 Entropy
It is the property of a body, which is defined as Q/T
From the first law of thermodynamics the work transfer in a reversible process
W rev = PdV
The second law provides the corresponding expression for heat transfer which can be
written as
Q rev = T s , s is the change in entropy
Entropy is an abstract property it can not be measured but can only be calculated, entropy
like enthalpy can be treated in three stages of the formation of vapour from the liquid.
The energy of the liquid can be expressed as Q = mc
And for unit mass Q = cθ, for θ = T And for constant pressure Q = cpl T
Dividing by T Q/T = cpl T/T
S = cpl T/T
To calculate the total change in entropy between given temperatures
S = m cpl T/T
s2 –s1 =cpl ln (T2/T1) ………………………………….[5.1]
Change in entropy for a vapour
S = mcpv T/T
s2 –s1 = cpv ln (T2/T1)
s2 –sf = cpv ln (T2/T1)
s2 = sf + cpv ln (T2/T1)………………………………….[5.2]
Chapter two The laws of thermodynamic
37
Entropy of steam
s2 –sg =cps ln (T2/T1)
s2 = sg + cps ln (T2/T1)…………………………………………….[5.3]
5.2.1 Change of entropy for a gas
from the first law of thermodynamics
Q = U +W where U = cv T and W =P V
Q = cv T + P V Dividing by T
Q = cv T + P V T T T
From pv = RT then P/T = R/v put in above equation
Q = cv T + R V T T V
S = cv T + R V T V
S = cv T + R V T V
s2-s1 =cvln (T2/T1) +Rln( V2/V1)………………………………………[5.4]
but cp- cv =R
Substituting s2-s1 =cvln (T2/T1) +( cp- cv) ln( V2/V1)
s2-s1 =cvln (T2/T1) + cp ln( V2/V1) - cv ln( V2/V1)……………….. [5.5]
s2-s1 =cvln{ (T2/T1)(V1/V2) } + cp ln( V2/V1)
And from P1V1/T1 =P2V2/T2; T2V1 = P2/P1
T1V2
s2-s1 =cvln (P2/P1) + cp ln( V2/V1)……………………[5.6]
But also cv = cp-R put into equation [5.4]
s2-s1 =cPln (T2/T11) -R ln (T2/T11) + R ln( V2/V1)
s2-s1 =cPln (T2/T11) + R ln{( V2/V1)(T1/T2)}
Chapter two The laws of thermodynamic
38
From P1V1/T1 =P2V2/T2; T1V2 = P1/P2
T2V1
s2-s1 =cPln (T2/T11) +R ln (P1/P2) ……………………………………… [5.7 ]
5.2.2 Change of entropy at constant pressure
From equation [5.4]
s2-s1=cvln(T2/T1)+Rln(V2/V1)…………………………………………… [5.8]
from equation [5.6] p1=p2
s2-s1 = cp ln( V2/V1)…………………………………………………… [5.9]
from equation [5.7]
s2-s1 =cPln (T2/T11)…………………………………………………… [5.10]
5.2.3 Change of entropy at constant temperature
from equation [5.6]
s2-s1 =cvln (P2/P1) + cp ln( V2/V1)………………………………… [5.11]
from equation [5.4]
s2-s1 =Rln( V2/V1)…………………………………………………. . [5.12]
from equation [5.7]
s2-s1 = R ln (P1/P2) ………………………………………………… [5.13]
5.2.4 Change of entropy at constant volume
from equation [5.7]
s2-s1 =cP ln (T2/T11) +R ln (P1/P2)………………………………… [5.14]
from equation [7]
s2-s1 =R ln (P1/P2)…………………………………………………. [5.15]
from equation [4]
s2-s1 =cvln (T2/T1) ………………………………………………… [5.16]
5.2.5 Change of entropy during a polytropic process
Q = –n x polytropic work
–1
Q = –n x P V
–1
dividing by T
Q = –n x P V from pv = RT, P/T =R/V
T –1 T
Chapter two The laws of thermodynamic
39
s = –n x R V
–1 V
s2-s1 = –n x R ln(V2/V1) ………………………………………..[5.17]
–1
From cp –cv =R and cp/cv =
R = cv(–1) put into [5.17]
s2-s1 = –n x cv( –1) ln(V2/V1)
–1
s2-s1 = cv (–n ) ln(V2/V1) ……………………………….. [5.18]
but from P1V1n =P2V2
2
V2/V1 = (P1/P2)1/n
Putting into [5.18]
s2-s1 = cv (–n ) ln(P1/P2) 1/n
s2-s1 = cv ( –n ) ln(P1/P2) ……………………………………………[5.19]
n
from T2/T1 = (V2/V1)n-1
, V2/V1 =( T2/T1 )1/(n-1)
put into equation [18]
s2-s1 = cv ( –n ) ln( T2/T1 )1/(n-1)
s2-s1 = cv ( –n ) ln( T2/T1 ) …………………………………………[5.20]
n-1
Worked example A rigid vessel contains 0.5 kg of a perfect gas of specific heat at constant volume 1.1 kJ/kg K. A
stirring paddle is inserted into the vessel; and 11 kJ of work are done on the paddle by the stirrer
motor. Assuming that the vessel is well lagged and that the gas is initially at the temperature of the
surroundings, which are at 17 oC, calculate the effectiveness of the process.
Solution
Q + W = U2 +U1 but Q = 0 , W = 11 kJ
Giving
W = mCv(T2 – T1)
11 = 0.5 x 1.1 x (T2 – 290)
T2 = 310K = 37 oC
Chapter two The laws of thermodynamic
40
Change in entropy
s2 – s1 = Cvln(T2/T1) = 1.1 x ln(310/290)
= 0.07336 kJ/kg K
Increase in specific energy
= (U2 +U1) – To(s2 – s1)
= 1.1(310 – 290) – (290 x 0.07336)
= 0.7256 kJ/kg
therefore
effectiveness = gssurroundinofenergyinloss
systemaofenergyinincrease
effectiveness = 11
5.07256.0 = 0.033 or 3.3%
Tutorial questions
Second law of thermodynamics
1. The overall expansion ratio of a Carnot cycle is 15. The temperature limits of the cycle are
2600C and 21
0C. Determine;
The volume ratios of the isothermal and adiabatic processes
The thermal efficiency of the cycle
=1.4 [3.39; 44.8%] RJ
2. 0.23kg of gas is taken through a cycle whose temperature limits are 3000C and 50
0C if the
volume ratio of the isothermal processes is2.5:1 determine for the cycle,
the thermal efficiency
the net work done
the work ratio
Take =1.4 R =0.28kJ/kgK [43.6%; 14.75kJ; 0.2] RJ
3. Steam at a pressure of 1.9MN/m2 and with temperature of 250
0C is expanded isentropically
to a pressure of 0.3MN/m2. it is further expanded hyperbolically to a pressure of 0.12MN/m
2.
using tables determine;
the final condition of steam
the change of specific entropy during the hyperbolic process
Chapter two The laws of thermodynamic
41
[0.954; 0.5727kJ/kgK, an increase] RJ
4. A quantity of gas as an initial pressure, volume, and temperature of 1.1bar, 0.16m3 and 18
0C,
respectively. It is compressed isothermally to pressure of 6.9bar. Determine the change of
entropy. Take R =0.3kJ/kgK [-111kJ/K]
5. 1kg of dry saturated steam at 22bar is throttled to a pressure of 7bar, then expanded at constant
entropy to a pressure of 1.4bar. calculate;
the degree of superheat at 7bar
the increase in entropy
the dryness fraction at 1.4bar [15.80C, 0.4848kJ/kgK, 0.9217] REEDS
Chapter two The laws of thermodynamic
42
Chapter six
Gas engine cycles 6.0 Introduction
Gas engine cycles are ideal gas cycles the working media is assumed to be air. In studying this
chapter the students should be able to calculate the change in thermodynamic property at each
turning point. From which the heat supplied, heat rejected work done and the thermal efficiency
can be calculated.
6.1. Constant pressure cycle
Also known as the [isobaric] cycle, heat is added and rejected at constant pressure
Fig 6.1 P-v and T-s for constant pressure cycle
1-2 adiabatic compression according to the law PV = C
at point 1 assume that P1 V1 T1
1
1
2
2
1
V
V
T
T
1
2
112
V
VTT
= T1( rv)
-1
where 2
1
V
Vr
also 2211 VPVP
2
112
V
VPP
Chapter two The laws of thermodynamic
43
2-3 constant pressure heat addition
P3 = P2
2
2
3
3
T
V
T
V
T3 =T2 V3/V2 =V3/V2T1 rv(-1)
3-4 adiabatic expansion according to the law PV = C
i
4
3
3
4
V
V
T
T
4-1 constant pressure heat rejection
T4 =T1V4/V1
It follows that V4/V1 = V3/V2 =constant pressure ratios
This could also be obtained from the fact that since V1/V2 =V4/V3 = rv then
V4/V1 = V3/V2
Also P4V4
=P3V3
Then P4 =P3 (V3/V4) = P3/r
v
Net work done by the system= area under 2-3 + area under 3-4 – area under 4-1 – area1-2
= 1
VP-VP - )V-(VP -
1
)VP-V(P )V-(VP 1122
1414433
232
= 1
VP-VP-VP-VP)V-(VP )V-(VP 11224433
141232
1
T-T-T-TmR)T-(TmR )T-mR(T 1243
1423
1
T-T-T-T)T-(T )T-(TmR 1243
1243
1
11)T-(T )T-(TmR 1243 but PCR
1
)T-(T )T-(TmC 1243P
Work done = heat received – heat rejected
= mcp (T3-T2)- mcp(T4-T1)
= mcp (T3-T2)-(T4-T1)
Chapter two The laws of thermodynamic
44
Net work done =heat received x thermal efficiency
Thermal efficiency = 1- heat rejected
heat received
= 1-mcp(T4-T1)
mcp(T3-T2
= 1- (T4-T1)
(T3-T2)
6.2. Constant volume Also known as an otto cycle heat is added and rejected at constant volume
fig 6.2 T-s and P-V for constant volume cycle
1-2 adiabatic compression of the gas according to the law PV = C
assume that the thermodynamic properties at 1 are P1, V1, T1
T1/T2 = (V2/V1) -1
T2 = T1(V1/V2) -1
where, r v =V1/V2 , the adiabatic compression , volume ratio
=V4/V3, adiabatic expansion, volume ratio
also P1V1 = P2V2
P2 =P1(V1/V2)
=P1 rv
2- 3 constant volume heat addition
V3 =V2 since the volume remains constant
P3/T3 =P2/T2
T3 = T2 P3/P2 = T1P3/P2 r-1
v from 2
3-4 adiabatic expansion of the gas according to the law PV =C
T3/T4 =(V4/V3)-1
= r-1
v
Chapter two The laws of thermodynamic
45
T4 =T3/ r-1
v
= T1(P3/P2) r-1
v/ r-1
v
= T1(P3/P2) from 3
AlsoP4V4 =P3V3
P4 =P3 (V3/V4)
= P3/rv
4-1 constant volume heat rejection
and also from the constant volume process
P4/T4 = P1/T1
T4 = T1 (P4/P1) = T1P3/P2 from above
from the above then it follows that P4/P1 =P3/P2
Net work done = area under 3-4 – area under 1-2
= P3V3 –P4V4 – P2V2 –P1V1
-1 -1
= P3V3 –P4V4 – P2V2 –P1V1
-1
= m R {( T3-T4)-(T2-T1)} Since pv =mRT
-1
6. 3.Diesel cycle
heat is added at constant pressure and then released at constant volume
fig 6.3 P-V and T-s for the diesel cycle
1-2 adiabatic compression according to the law PV =C
2-3 constant pressure heat addition P2 =P3
3-4 adiabatic expansion according to the law PV =C
4-1 constant volume heat rejection V4 =V1
the cycle is sometimes referred to as the modified constant pressure cycle
assume that at point 1, P1,V1,T1, are known
Chapter two The laws of thermodynamic
46
1. P1,V1,T1
2. T1/T2 =(V2/V1) -1
T2 T1 (V2/V1) -1
Also P1V1 = P2V2
P2 = P1( V1/V2)
2. P3 =P2 pressure remains the same
V3/T3 =V2/T3
T3 =T2 V3/V2 =V3/V2T1 rv -1
= T1 rv -1
= V3/V2 cut off ratio
3. T4/T3 = (V3/V4) -1
T4 = T3(V3/V4) -1
Now V3/V4 =V3/V1 since V4 = V1 and
V3/V1 =V3 V2 =/rv
V2 V1
T4 =T3( /rv) -1
= T1 rv-1
-1
rv-1
T4 = T1 -1
= T1
and also P4V4 = P3V3
P4 = P3( V3/V4) =P3 (/ rv)
Work done during the process= area under2-3 + area under 3-4 –area under 1-2
=P2(V2-V3) +(P3V3 –P4V4) – P2V2 –P1V1
-1 -1
= P2(V2-V3) + (P3V3 –P4V4) –P2V2 –P1V1
-1
6.4. The dual combustion cycle
Heat is added at constant pressure and at constant volume hence the name dual. Heat is then
rejected at constant volume, it is a modified diesel cycle
Chapter two The laws of thermodynamic
47
1-2 isentropic compression
2-3 reversible constant volume heating
3-4 reversible constant pressure heat addition
4-5 isentropic expansion
4-6 reversible constant volume cooling
1
2
34
5
p
vv1
v2=v3
p3=p4
The heat is supplied in two parts first at constant volume and then at constant pressure
Heat supplied =mcv(T3-T2) + mcp(T4-T3)
Heat rejected = mcv(T5-T1)
Net work done = area under 3-4 + area under 4-5 – area under 1-2
= P3(V4-V3) +P4V4 –P5V5) – (P2V2 –P1V1)
( –1 ) ( –1)
= P3(V4-V3) +(P4V4 –P5V5) – (P2V2 –P1V1)
( –1)
= mR{T4-T3) +{(T4-T5)-T2-T1)}
( –1)
or net work = heat received – heat rejected
=mcv(T3-T2) +mcp(T4-T3) –mcv(T5-T1)
Thermal efficiency =1 - heat rejected
Heat received
=1 - mcv(T5-T1)
mcv(T3-T2) +mcp(T4-T3)
=1- (T5-T1)
(T3-T2) + (T4-T3)
Chapter two The laws of thermodynamic
48
6.5. Gas turbine cycles
combustion chamber
air compressor
2 3
turbine
coupling shaft
1 4
air intake exhaust
2s2
1
3
4s
4
p2
p2
T
s
fig 6.5 T-s diagram for gas turbine
The basic gas turbine unit is that which operates on an open cycle in which a rotary compressor is
coupled to a turbine. Air is drawn into the compressor, and after compression it is passed into the
combustion chamber where energy is supplied in the form of sprayed fuel. The resulting hot gases
expand through the turbine to the atmosphere.
1-2 represents irreversible adiabatic compression
2-3 constant pressure heat supply in the combustion chamber
3-4 irreversible adiabatic expansions
1-2s represents the ideal isentropic process between same pressures p1=p2
3-4s represents the ideal isentropic expansion between the same pressures
Assume that the kinetic energy through the system is negligible compared with enthalpy changes
Chapter two The laws of thermodynamic
49
Applying the flow equation to each part of the cycle for unit mass
Compressor work input =cpa(T2-T1)
For combustion chamber heat supplied =cpc(T3-T2)
For the turbine work output =cpt(T3-T4)
Net work output =cpt(T3-T4)- cpa(T2-T1)
The thermal efficiency = net work output
heat supplied
= cpt(T3-T4)- cpa(T2-T1)
cpc(T3-T4)
cpa is the specific heat capacity at constant pressure for entering compressor
cpc is the specific heat capacity at constant pressure for fuel in the combustion chamber
cpt is the specific heat capacity at constant pressure for combustion products in the turbine
isentropic efficiency of the compressor is defined as the ratio of work in put required in isentropic
compression between p1 and p2 to the actual work required
compressor isentropic efficiency c = cp(T2s –T1)
cp(T2-T1)
= (T2s –T1)
(T2-T1)
Isentropic efficiency of the turbine is defined as the ratio of the actual work to the isentropic work
output between the same pressures
Turbine isentropic efficiency = cp(T3-T4)
cp(T3-T4s)
= (T3-T4)
(T3-T4)
Worked Example
A closed cycle gas turbine unit operating with maximum and minimum temperatures of 760oC and
20oC has a pressure ratio of 7:1. Calculate the ideal cycle efficiency and the work ratio.
T2 = 293 x (7) 0.4/1.4
= 510.9 K
Then heat supplied
Q = Cp(T3 –T2)
= 1.005(1033 – 510.9)
= 52407 kJ/kg
T4 = 1033/(7) 0.4/1.4
= 592.4 K
Chapter two The laws of thermodynamic
50
Then heat rejected
Q = Cp(T4 –T1)
= 1.005(592.4 - 293)
= 300.9 kJ/kg
thus cycle efficiency = pliedsupHeat
rejectedHeatpliedsupHeat
= 7.524
8.223
7.524
9.3007.524
= 42.7%
The net work output is equal to the net heat supplied
i.e. net work output = 223.8 kJ/kg
Gross work output = Cp(T3 – T4)
= 1.005(1033 – 592.4)
= 442.8 kJ/kg
Work ratio = outputworkgross
outputworknet
= 8.442
8.223= 0.505
Worked example
In a dual combustion cycle the maximum temperature is 20000C and the maximum pressure is 70
bar. Calculate the cycle efficiency and the mean effective pressure when the pressure and
temperature at the beginning of the compression are 1 bar and 170C respectively. The compression
ratio is 18/1 (63.6%; 10.46bar) T.D. Eastop
Solution
P2 = P1x (18)1.4
= 1 x (18)1.4
= 57.2 bar
T2 = T1x (18)0.4
= 290 x (18)0.4
= 921.5 K
Also 2
3
2
3
P
P
T
T
T3 = K6.11292.57
70923
And 012.26.1129
2273
T
T
V
V
3
4
3
4
i.e. 945.8012.2
18
V
V
4
5
Chapter two The laws of thermodynamic
51
Then T5 =
4.0
5
44
V
VT
= 946.2 K
Heat supplied = Cv(T3 – T2) + Cp(T4 – T3)
= 0.718(1123 – 921.5) + 1.005(2273 -11296)
= 1293.8 kJ/kg
Heat rejected = Cv(T5 –T1)
= 0.718(946.2 - 290)
= 471.2 kJ/kg
Net heat supplied = net work output
= 1293.8 – 471.2
= 822.6 kJ/kg
then, cycle efficiency
= %6.63or636.0pliedsupheat
outputworknet
now kg/m8323.0101
290287
P
RTV 3
51
11
V2 –V1 = (.8323/18) – 0.8323 = 0.7861 m3/kg
mean effective pressure = 12 VV
1000outputworknet
= 5107861.0
10006.822
= 10.46 bar
Chapter two The laws of thermodynamic
52
Chapter six
Gas power cycles Tutorial Questions
1. The pressure, volume and temperature at the beginning of the compression of a constant
volume (otto) cycle are 105kN/m2, 0.002m
3 and 25
0C respectively. The maximum
temperature of the cycle is 1250 0C. The volume ratio of the cycle is 8:1. The cycle is
repeated 4000times/min. determine for the cycle,
the theoretical output in kilowatts;
the thermal efficiency;
the mean effective pressure;
the carnot efficiency within the same temperature limits
take cp =1.007kJ/kgK.cv =0.717kJ/kgK [54.3kW; 57%; 465.1kN/m2; 80.4% ] R.JOEL
2. 0.5 kg of air is taken through constant pressure cycle. The pressure and temperature at the
beginning of the adiabatic compression are 96.5kN/m2 and temperature 15
0C, respectively.
The pressure ratio o9f the compression is 6:1. Constant pressure heat addition occurs after the
adiabatic compression until the volume is doubled. Determine for the cycle,
the thermal efficiency;
the heat received
the net work done
the work ratio
the mean effective pressure
[40%; 241kJ; 96.4kJ; 0.466; 134.3kN/m2 ] R. JOEL
4. An engine working on an ideal Diesel cycle has a clearancevolume of 0.000 25m3. it has a
bore and stroke 0f 152.5mm and 200mm, respectively. At the beginning of the adiabatic
compression the air in the cyclinder has a pressure of 100kN/m2 and a temperature of 20
0C
respectively. The maximum temperature of the cycle is 10900C ,. Determine,
The temperature and pressure at the end of the adiabatic compression;
the temperature and pressure at the end of an adiabatic expansion
the thermal efficiency of the cycle
take =1.4 [6060C;4680kN/m
2; 269
0C;185kN/m
2 63.3% ] R. JOEL
5. A continuous combustion constant pressure gas turbine takes in air at a pressure of 93KN/m2
with a temperature of 20 0C .A rotary air compressor compresses the air to a pressure of 552
kN/m2 with an isentropic efficiency of 83%.The compressed air is passed to a combustion
chamber in which its temperature is increased to 8700C .From the combustion chamber the
high temperature air passes into a gas turbine in which it is expanded to 93kN/m2 with an
isentropic efficiency of 80%.For an air flow of 10 kg/s and neglecting the fuel mass as
small, determine:
(a) the net power output of the plant if the turbine is coupled to the
compressor;
(b) the thermal efficiency of the plant;
(c) the work ratio.
Take, =1.4 and cp =1.00kJ/kgK
[(a) 1310KW; (b) 21%; (c) 0.36]
Chapter two The laws of thermodynamic
53
Chapter seven
Vapour power cycles:
Chapter two The laws of thermodynamic
54
7.0 Introduction
The steam power plant is the plant, which is used to convert water into steam, whose kinetic
energy is used to drive the turbine. The turbine in turn is coupled to the generator, which is used to
generate electricity. The main components of a steam power plant are as flows:
1. the boiler
2. the turbine
3. the condenser
4. the feed pump
5. extraction pump
6. cooling tower
7. the economizer
fig 7.1 major components of a steam power plant
7.1 Vapours
Formation of steam
When water is put into a boiler it absorbs heat at constant pressure, steam bubbles are formed near
the heating surface and they rise through the water, however the water around is cold hence it
absorbs heat energy from the steam bubbles, which immediately collapse. Finally the steam
bubbles can escape from the boiling surface. The mass is in extreme state of turbulent called
boiling. it will be noted that as boiling temperature ceases to rise. The temperature remains
constant despite the increase in heat being added (saturation temperature). As the steam breaks
away from the water surface it will carry with it droplets of water. The steam with these droplets is
called wet steam. Further heating to the wet steam will convert the droplets tom dry steam, which
is then known as dry saturated steam. This makes the end of the constant temperature heat
addition. Further addition of heat to this steam result in the formation of superheated steam. And
there is a sudden increase of temperature.
Chapter two The laws of thermodynamic
55
7.1.1 Stages in the formation of steam
Temp,
tsup liquid water vapour
water/ steam superheated steam
boiling point dry saturated
tf
hf enhalpy of steam
hg
hsup
fig. 7.2 formation of steam from water
Stage 1
Warming phase, temperature rise to saturation temperature. The energy supplied, is the liquid
Enthalpy hf in kJ/kg
Stage 2
It starts with water at saturation temperature tf at the beginning and a dry saturated steam at
saturated temperature at the end. The energy required, is the enthalpy of evaporation, hfg
Stage 3
Formation of superheated steam, temperature rise as the energy is added, superheat enthalpy
Liquid enthalpy
For 1kg of water, the specific liquid enthalpy is written as hf, the accurate value of hf at any given
saturation temperature corresponding to any given constant pressure given from steam tables, also
hf = mc
Enthalpy of evaporation
Dryness fraction of steam x, quality of steam is the fraction of dry steam to the total mass of wet
steam
x = mass of dry steam present
total mass of water and steam
Chapter two The laws of thermodynamic
56
= ms
mw + ms
= v/vg …………………………………………………………………………….7.1
VfVg
c=0 c=1
fig 7.3 dryness fraction of steam
Specific enthalpy of wet steam
hwet = hf + x ( hg-hf) …………………………………………7.2
hwet = hf + x hfg
Enthalpy of superheated steam
hsup = hg + cp (tsup –tf ) cp specific heat capacity of superheated steam
Chapter two The laws of thermodynamic
57
Formation of the T-s or T-h diagrams
When experiments are performed at different pressures the temperature enthalpy diagrams will be
as shown in the first diagram. As the operating pressure increases the boiling temperature also
increases.
If points 2,6,10,13,14, 11,7, 3 are joined with a smooth curve the second diagram is formed. At
point c is that pressure which will ensure that the water suddenly changes into gas without passing
through the vapor phase, it is known as the critical pressure and temperature point.
Curve ac is the liquidous line, and cb is the gaseous line. The second graph is the one applied
when dealing with different cycles
7.2 The Rankine cycle
T
h
T
h
Vapor
phase
Gaseous
phase
Liquid
phase
c
12 3
4
5
6 7
8
9
10 11
1213 14
ab
Chapter two The laws of thermodynamic
58
Fig 7.4 Rankine cycle with superheat
1-2 water is being pumped into the boiler with volume V and pressure P2,
2-3 in the boiler water is converted into steam at pressure P2, with volume V3 which is then
fed into the turbine.
3-4 the steam is expanded frictionless adiabatic ally in the engine or turbine.
4-1 steam after expansion, is passed from the turbine into a condenser in the condenser the
volume of the steam is reduced.
2-3 shows constant pressure formation of steam in the boiler
3-4 isentropic expansion of steam in the turbine
4-1 constant pressure and temperature formation of steam.
1-2 pumping of water into the boiler at constant volume.
Heat supplied to unit mass of water in the boiler = h3 –h2
Specific work done in the turbine = h3 –h4
Feed pump work = ( p2- p1) v1
where v1 is the specific volume of water
net work done/cycle = (h3 –h2) -( p2- p1) v1
total energy of water entering the boiler at 2 h2 = liquid enthalpy at 1 + work done by pump
h2 = h1 +( p2- p1) v1
Heat transfer required in the boiler = ( h3 - h1 )+( p2- p1) v1
Thermal efficiency of the cycle = workdone per cycle
heat received per cycle
Thermal efficiency of rankine cycle = (h3-h4)- ( p2- p1) v1
( h3 - h1 )+( p2- p1) v1
if the feed pump work is neglected, then the efficiency
= (h3-h4) …………..7.3
( h3 - h1)
to calculate h4, from s3= s4 isentropic expansion in the turbine
then s4 = sf + x4 sfg x4 =( s4-sf)/sfg
therefore h4 = hf + x4 hfg
Chapter two The laws of thermodynamic
59
7.3 The reheat cycle:
The pressure ratio through the turbine can be considerable, therefore after partial expansion in
high pressure side of the turbine, the partially wet steam is fed back to the boiler were it is
reheated at constant pressure to a higher temperature it is then passed to the lower pressure
side of the turbine, the expansion which follows is largely dry and superheated.
The reheat cycle reduces erosion and corrosion by wet steam. It also results in higher thermal
efficiency.
fig7.5 reheat cycle
Work done in the turbine = ( h3-h4) +(h5-h6)
S3 = S4 Isentropic expansion in the high pressure side of the turbine
S5 =S6 Isentropic expansion in the low pressure side of the turbine
Work done by the pump = v1(P2-P1)
Heat supplied in the boiler = (h3- h2) + (h5 –h4)
Net work output = work done by turbine – work of pump
=( h3-h4) +(h5-h6) - v1(P2-P1)
also h2 = h1 + v1(P2-P1)
thermal efficiency = net work
heat supplied
= h3-h4) +(h5-h6) - v1(P2-P1)
(h3- h2) + (h5 –h4)
Neglecting work done by the pump
Thermal efficiency = h3-h4) +(h5-h6)
(h3- h2) + (h5 –h4)………………………….7.4
7.4 The regenerative cycle:
Also known as the feed heat
The steam is made to expand from condition 1 through the turbine. At the pressure corresponding
to point 5, aquantity of steam, say ykg per kg of steam supplied from the boiler, is bled off for
feed heating purposes. The rest of the steam,(1-y)kg,completes the expansion and is exhausted at
state 4. This amount of steam is then condensed and pumped to the same pressure as the feed
Chapter two The laws of thermodynamic
60
steam, y kg is such that, after the mixing and being in the second feed pump the condition is
defined by state 7
The heat to be supplied in the boiler is given by =h1-h7
to determine the bled pressure when one or more feed heaters are used this can be based on the
assumption that the bleed steam temperature to obtain maximum efficiency the arithmetic mean of
the temperatures at 4 and 7
t –bleed =(t4 + t7)/2
Fig 7.6 T-s diagram for regenerative cycle
m5 =y, m2 = (1-y)
h2(1-y) +yh5 =h6
y = h6-h2
h5-h2
also s3 = s5 = s4
heat supplied in the boiler = h3-h7
total work output -W = -W35 –W54
= h3-h5 +(1-y)(h5-h4)
cycle efficiency = h3-h5 +(1-y)(h5-h4) …………………………..7.5
(h3-h7)
Chapter two The laws of thermodynamic
61
Worked Example
In a regenerative cycle employing three closed feed heaters the steam is supplied to the turbine at
42 bar and 5000C and is exhausted to the condenser pressure at 0.035 bar. The bled steam for
feed heating is taken at a pressure of 15, 4, and 0.5 bar. Assuming ideal process and neglecting
pump work, calculate,
The fraction of the boiler steam bled at each stage;
the power output of the plant per unit mass flow rate of the boiler steam;
the cycle efficiency
T.D Eastop
i) using the tables and h-s chart:
h1 = 3443 kJ/kg, h2 = 3127 kJ/kg
h3 = 2815 kJ/kg h4 = 2458 kJ/kg
h5 = 2114 kJ/kg h6 = 112 kJ/kg
h7 = 340 kJ/kg h8 = 605 kJ/kg
h9 = 845 kJ/kg
Applying an energy balance to each feed heater assuming that the bleed steam fractions are y1, y2
and y3 as shown in the figure:
3127y1 + (1 - y1)605 = 845
i.e. y1 = 0.0952
2815y2 + (1 – 0.0952 - y2)340 = (1 – 0.0952)605
Chapter two The laws of thermodynamic
62
i.e. y2 = 0.0969
2155y3 + (1 – 0.0952 – 0.0969 – y3)112 = (1 – 0.0952 – 0.0969)340
i.e. y3 = 0.02
BOILER
42 bar
PPP
P
9 8 7
6
y 1kg/s
y 2kg/s
y 3kg
/s
15 bar
4 bar
0.5 b
ar
TURBINE
5
(1-y1-y2-y3)kg/s
CONDENSER
0.035bar
42 bar
500oC
1 kg/s
1
1 kg/s
23
4
ii) Power output per unit mass flow rate of boiler steam is given by
Power output = (h1 –h2) + (1 - y1)(h2 –h3) + (1 - y1 – y2)(h3 –h4) + (1 - y1 – y2 – y3)(h4–h5)
=(3443-3127)+(1-0.0952)(3127-2815)+(1-0.0952-0.0969)(2815-2458)+(1-0.0952-0.0969-
0.0902)(2585-2114)
i.e. Power output = 1 133.6 kW per kg/s
iii) heat supplied per unit mass of boiler steam
= h1 –h9 = 3443 – 845 = 2598 kJ/kg
then, cycle efficiency = 1134/2558 = 43.6%
Chapter two The laws of thermodynamic
63
Tutorial Questions
Vapor power cycle
1. Steam at a pressure of 30 bar and temperature of 2500C is fed into a steam turbine from the
boiler. In the turbine the steam is expanded isentropically to a pressure of 1 bar. The steam is then
exhausted into the condenser where it is condensed but not under cooled. The condensate is then
pumped back into the boiler, determine
the dryness fraction of the steam after expansion;
the Rankine efficiency
[0.823; 23.88] R.J
2. Steam at 1.7MN/m2 and with a temperature of 250
0C is fed into a steam engine in which it is
expanded adiabatically to arelease pressure of 0.35MN/m2. From this pressure it is released at
constant volume to a condenser pressure of 50kN/m2.the steam is then exhausted from the engine
into the condenser where it is condensed but not undercooled the condensate is then pumped back
into the boiler. The stem flow rate is 1500kg/h determine
the power output of the turbine
the Rankine efficiency
the Carnot efficiency for the same temperature limits of the cycle
[ 187kW; 17.4%; 32.25%]R.J
3. In a steam turbine plant, the initial pressure and temperature of the steam are 3MN/m2
and
3200C, respec tively and the exhaust pressure is 0.06NM/m
2 . after isentropic expansion to
1MN/m2 the steam is reheated isobarically to 250
0C and after further isentropic expansion in the
turbine to 0.4MN/m2 it is again reheated isobarically to a temperature of 200
0C. the steam is
finally expanded isenropically in the turbine to exhaust pressure. Determine,
thermal efficiency of the arrangement
[ 26.5%] RJ
Chapter two The laws of thermodynamic
64
Chapter eight
Refrigeration cycles
8.0 Introduction
In general refrigeration is defined as any process of heat removal, specifically it is defined as the
branch of science that deals with the process of reducing and maintaining the temperature of a
space or material below the temperature of the surrounding.
Fig. 8.1 T-s refrigeration cycles
Chapter two The laws of thermodynamic
65
8.1 Components of vapor refrigeration cycle
1.Compressor
Work is input by a compressor, which increases the pressure of the vapour and also the
temperature through isentropic compression in the ideal cycle.
2.The condenser.
From the compressor the vapour enters the condenser, where heat is extracted, resulting in
saturated liquid. The heat extracted is released to the surrounding.
3. Expansion valve
The pressure of the saturated vapour is then reduced through the expansion valve or the
Throttle valve. The expansion takes place at constant enthalpy.
4. Evaporator
From the expansion valve the refrigerant enters the evaporator, where it absorbs heat from
the refrigerated space. This was the actual refrigeration of the items takes place. The items
release the heat to the refrigerant, resulting in them getting cooler and the refrigerant
getting hotter.
8.2 The refrigeration cycle
1-2 isentropic compression in the compressor
s1 = s2 , for an isentropic compression
work done by the pump= h2- h1
to find h1; at pressure p1
s1 = sf + x1 sfg
x1 = (s1 - sf )/ sfg
then, h1 = hf + x1 hfg
to get h2, at pressure p2, assume the temperature at 2 to be t2 and the saturation
temperature at p2 to be tf , then,
the degree of superheat = t2 - tf
if (t2 - tf ) 15 K, choose the value h, under this column
if (t2 - tf ) > 15 K choose the h, value under the 30K value.
2-3 heat rejection in the condenser,
heat rejected = h2 – h3
h3 = hf at p2
3-4. Expansion of the refrigerant at constant enthalpy.
h3 = h4
also x4 =( h4 – hf1)/ hfg1
Chapter two The laws of thermodynamic
66
4-1 constant pressure heat addition to the refrigerant
Refrigerating effect = h1 – h4
Coeffient of performance C.O.P. = heat absorbed from the refrigerated space.
Heat energy equivalent of the energy supplied by comp.
= refrigerating effect ……………….. 8.1
heat of compression
Chapter two The laws of thermodynamic
67
8.3. The absorption refrigerating cycle
fig 8.2 diagrammatic presentation of absorption
it replaces the compressor in the conventional refrigerating cycle with an absorber, pump, heat
exchanger and a generator.
Saturated low-pressure refrigerant enters the absorber, where it is absorbed in aweak carrier
solution. Heat is released in the process. In the absorber the temperature is maintained low by
removing heat Q`A. The much stronger solution leaves the absorber and is pumped into the
higher condenser pressure using little power., it goes through the heat exchanger which
increases its temperature and enters the generator, the added heat boils off the refrigerant
which then passes off into the condenser. The remaining weak carrier solution is then returned
Chapter two The laws of thermodynamic
68
from the generator to the absorber. To be recharged with the refrigerants on its way to the
absorber the temperature of the carrier solution is reduced in the heat exchanger. And its
pressure is reduced in the regulating valve.
From the condenser the refrigerant is passed through the expansion valve where its pressure is
reduced before being fed into the evaporator where absorbs heat from the refrigerated space
and is then fed into the absorber.
The solutions normally used are that of ammonia in water or water and lithium bromide for air
conditioning.
The concentration fraction of liquid ammonia x` = mass of NH3 liquid
Mass of mixture
Concentration of vapour ammonia x`` = mass NH3 vapour
Mass of mixture
Enthalpy of liquid mixture = hL, enthalpy of vapour mixture =hv
fig 8.3 concentration versus temperature
Chapter two The laws of thermodynamic
69
8.4 Gas refrigeration cycle
fig. 8.4 T-s diagram for gas refrigeration cycle
1-2 the refrigerant absorbs heat from the refrigerated space at constant pressure
2-3 isentropic compression in the compressor
3-4 the gas releases heat at constant pressure
4-1 isentropic expansion in the turbine to a low exit temperature
The net work input to the plant W =W14 + W23
Applying steady – flow energy equation
W14 = -(h4- h1 ) and W23 =h3-h2
For a perfect gas
W 41 =cp(T4- T1) and W23 =cp(T3- T2)
The refrigerating affects Q1 = (h2-h1)
= cp(T2-T1)
The actual cycle would be as shown below
Chapter two The laws of thermodynamic
70
T
3
3s
4
2
1S 1
S
Fig. T-s diagram for gas turbine
The cycle would have W23 = cp(T3-T2)
W34 = -cp(T4-T1)
Isentropic efficiency of the compressor c = T3s –T2 ……………………………… 8.2
T3-T2
Isentropic efficiency of the turbine T = T4- T1 ………………… 8.3
T4- T1s
Then the refrigerating effect Q1 =cp (T2-T1)
Worked Example
In a refrigerating plant using R12 the vapour leaves the evaporator dry saturated at 1.826 bar and
is compressed to 7.449 bar. The temperature of the vapour leaving the compressor is 45ºC and the
liquid leaves the condenser at 25ºC and is throttled to the evaporator pressure calculate:
the refrigerating effect
the specific work input
the COPref
Solution
i) h1 = 180.5 kJ/kg
After compression the refrigerant is superhe
ated by (45 – 30) = 15K at 7.449 bar therefore
from tables,
h2 = 210.63 kJ/kg
also h3 = 59.7 kJ/kg = h4
the refrigerating effect = h1 – h4
= 180.67 – 59.7
= 121. 27 kJ/kg
T
S
2
3
41
45oC
30oC25oC
-15oC
Chapter two The laws of thermodynamic
71
ii) Work in put = h2 – h1 = 210.63 – 180.97 = 29.66 kJ/kg
iii) COPref = 66.29
27.121
put in Work
effect ingRefrigerat
= 4.09
Chapter two The laws of thermodynamic
72
Chapter eight
Refrigeration
Tutorial questions
1. A heat pump using ammonia as a refrigerant operates between saturation temperatures 6 and
38ºC. the refrigerant is compressed isentropically from dry saturation and there is 6K of
undercooling in the condenser, calculate
the COPhp
the mass flow of refrigerant per kilowatt power input
the heat available per kilowatt power input
( 8.77; 25.03kg/h; 8.77Kw) eastop
2. Freon 12 leaves the condenser of the refrigerating plant as saturated liquid at 5.673 bar. The
evaporator pressure is 1.509 bar and the refrigerant leaves the evaporator at this pressure and at a
temperature-50C. Calculate,
the dryness fraction of the refrigerant as it enters the evaporator
the refrigerating effect per kg
Chapter two The laws of thermodynamic
73
Chapter nine
Nozzles and Jet propulsion 9.0 Nozzles A nozzle is a duct of whose cross-sectional area varies with length such that when a fluid is
passed through it is either accelerated or decelerated.
Applications;
Steam and gas turbines
Jet engines
Rocket motors
Inflow measurements
General nozzle shapes
Convergent divergent nozzle, at the entry the area of the nozzle converges down to the
throat and then diverges up to the exit
Convergent nozzle, the cross-sectional area converges from entry down to the exit.
Diffuser, is the opposite of the above the fluid is decelerated and the pressure is increased.
entryexit
throat
convergent divergent
fig 9.1 divergent- convergent nozzle
9.2 Flow analysis
A1, c1
P1,V1,T1,
h1
A2, c2
P2,V2,T2h1
Neglecting change in potential energy and putting W =0 since no work is done in the nozzle, the
steady flow energy equation for the nozzle becomes
h1 + c12/2 +Q = h2+c2
2/2………………………………………………………………9.1
The time taken by the substance to pass through the nozzle is very small hence there is little time
for heat exchange. Hence Q =0
Chapter two The laws of thermodynamic
74
The above equation becomes
h1 + c12/2 = h2+c2
2/2
c22 - c1
2 = h1 - h2
2
but c2 >> c1
therefore c2 = 2(h1-h2)1/2
………………………………………………………………9.2
for gas,
h1-h2 =cp(T1-T2) = R(T1-T2)………………….……………………………….9.3
( -1)
Since cp = R…………………………………………………………………………9.4
( -1)
substituting equation 9. 3 into 9. 2
c= {2 R(T1-T2)}………………………………………………….9.5
(-1)
since Pv = mRT, then
c= {2 P1V1(1- P2V2)}………………………………………….9.6
(-1) P1V1
At any section of the nozzle
.
m v =AC
Where .
m = mass flow rate in kg/s
v =specific volume in m3/kg
A = the crosssectional area in m2
C = velocity in m/s
9.2 Steam turbines
Chapter two The laws of thermodynamic
75
INLET
Cai = is the absolute velocity at inlet, is the velocity of steam as is leaves the nozzle
The nozzles are inclined at an angle to the plane of rotation of the turbine blade
U = is the mean blade speed at the mean height of the blades
Cri = is the velocity of steam relative to the blades is obtained by compounding U and Cai.
It is inclined at angle to the plane of rotation, if the steam enters without shock then the
angle must be the inlet angle of the blades
Cwi = is the velocity of whirl at inlet is the component of Cai in the plane of rotation
Cfi = is the velocity of flow at inlet is the component of Cai along the axis of rotation
OUTLET
Cre = is the exit relative velocity, at an angle to the plane of rotation, which also the exit
angle of the blade
U= is still the mean velocity of the blades
Cae= is the absolute velocity at exit is obtained by compounding U and Cre
It is inclined at an angle to the plane of rotation.
Cwe= is the velocity of whirl at exit it is the component of Cae in the plane of rotation.
Cfe = is the velocity of flow at exit, is the component of Cae along the axis of rotation
9.3.1 The combination of inlet and outlet velocity triangles.
CfiCai
UCwi
Cri
CreCaeCfe
Cwe U
EXIT
INLET
Direction of
motion
Φβ
θ
θα
Fig 9.3 Velocity diagram for impulse turbine
Axis of rotation
Plane of rotation
Chapter two The laws of thermodynamic
76
-CweCwe
CfiCri
CaiCre
U
Cae
Cfe
Change of velocity of whirl
= -Cwe-Cwi= -(Cwe+Cwi)
A Bβ α Φ θ
Cfi-Cfe
fig 9.4 combination of inlet and outlet velocity triangles
The exit velocity triangle remains as originally shown. The inlet velocity triangle is drawn sa the
other half of the parallelogram of velocities the original triangle is shown dotted. Absolute
velocities start at A. For no friction Cri = Cre
Work done by the blades
The whirl velocities are the effective part in producing motion in the blades
From Newton`s
The force to change the velocity of whirl of steam
Force = rate of change of momentum
=mass x change of velocity change in V = – Cwe – Cwi
= .
m x[-(Cwi +Cwe)] m is the mass flow rate in kg/s
The negative sign shows that this force acts in opposite direction to that of rotation, then the actual
force being exerted on the blades
F = .
m (Cwi + Cwe)
Work done = force x distance
Power = force x mean velocity
= .
m U( Cwi + Cwe)
Kinetic energy of the steam supplied = C2
ai J/kg steam/s
2
Blade or diagram efficiency = work done by blade/kg steam
energy supplied /kg steam
Chapter two The laws of thermodynamic
77
= U(Cwi + Cwe)
C2ai
2
= 2U( Cwi + Cwe)
C2ai
The velocity of flow is that velocity which passes the steam across the blades, this also causes
end thrust along the turbine shaft.
End thrust force =mass rate x change of velocity
= .
m (Cfe –Cfi)
9.3.2 The blade height
The blade height at any particular section of turbine will be a function of the following
Mass flow rate in kg/s
specific volume of steam in m3/kg
the area through which the steam is passing in m2
the velocity of steam as it passes the section in m/s
For a given section we have
.
m v = AC
9.3.3 Blade height for impulse turbine
p
Cri
psi
nθ
θ
Cri
Cfi = Crisinθ
θ
(a)
(b)
Cfi=Cri Sin
For an impulse turbine blade row,let,
Chapter two The laws of thermodynamic
78
M=mass flow of steam,kg/s
V=specific volume of the steam,m3/Kg
N=number of blades covered by nozzles
P=pitch of blades,m(taken at mean blade height)
H=blade height,m
=blade inlet angle
Cri=relative velocity of steam at inlet,m/s
Cfi=velocity of flow at inlet,m/s
Then,from equatin (1) .
m v =AC
=N p sin
=NPH x Cri sin , which from equation (2)
=N P H Cfi
H =.
m v
NPCfi
NP= circumference at the mean blade diameter
=d
Where d = mean blade diameter, m.
(b) Reaction turbine
In this case, let,
D =mean blade diameter, m.
Then, since the reaction turbine has full admission, from equations (3) and (5)
H = .
m v
d Cfi
9.4.0 Jet propulsion
Aircraft propulsion is achieved by using a heat engine to drive an airscrew or propeller, or by
allowing a high-energy fluid to expand and leave the aircraft in a rear direction as a high velocity
jet. In the propeller type of aircraft engine the propeller takes a large mass flow and gives it a
moderate velocity backwards relative to the aircraft. In the jet engine the aircraft induces a
comparatively small airflow
and gives it high velocity backwards relative to the aircraft. In both
cases the rate of change of momentum of the air provides a reaction forward thrust which propels
the engine.
9.4.1 Turbojets
Ca turbojet Cj
Chapter two The laws of thermodynamic
79
Air craft velocity, Ca
Thrust per unit mass flow rate = Cj – Ca
Propulsive power, thrust power per unit mass flow rate = Ca( Cj – Ca)
The above is the rate at which work is done inorder to keep the air craft moving.
The net work output from the engine is given by the increase in kinetic energy
( Cj2 -Cj
2)/2
the work output can be divided into two:
It provides the thrust work as given by Ca( Cj – Ca)
Gives the air a kinetic energy (Cj-Ca)2/2
Ca( Cj – Ca) +(Cj-Ca)2/2 =CaCj -Ca
2 +Cj
2/2 +Ca
2/2 –2CjCa/2
Therefore workoutput = C2j –C
2a
2
the propulsive efficiency p = thrust work
rate at which work is done on the air in the air craft
= 2 Ca( Cj – Ca)
C2j –C
2a
= 2Ca
Cj + Ca
9.4.1The ram jet Is the simplest form of jet engine. In this engine the air is compressed by the conversion of
the kinetic energy of the atmospheric air relative to the aircraft, it is known as the ram
effect. Fuel is burnt in the compressed air stream at approximately constant pressure and
the hot gases are allowed to expand through the nozzle reaching a high velocity backwards
relative to the aircraft
Fuel ramjet velocity nozzle
Ca
1 2 3 4
Chapter two The laws of thermodynamic
80
air inlet exhaust
1 2 3 4
T PI
P2=P3
I 3
T2=T1 2
2S P1=P4
4S 4
1
S
The ramjet velocity is Ca, the air enters the diffuser with a kinetic of =C2
a/2 per unit mass
Assuming isentropic, using flow equation
h1 +C2a/2 = hi +Ci
2/2
cpT1 +C2a/2 = cp(Ti + C
2i/2) =cpToi
C2a/2 = cp (Toi –T1)
Toi –T1 = C2a/2 cp
The total pressure Poi is the pressure the air attains when the diffusion process is isentropic, when
the procee is irreversible, though still approximately adiabatic, then the total pressure attained
isPo2 which is less than Poi
The kinetic energy available, C2a/2 is the same whether or not the process is irreversible the
temperatures remain the same Toi =To2
To2 –To1 =Ca2/2cp
Intake efficiency = Tt2s –T1
Tt2 – T1
Worked Example
Chapter two The laws of thermodynamic
81
A convergent–divergent nozzle expands air at 6.89 bar and 427oC into a space at 1 bar. The throat
area of nozzle is 650 mm2 and the exit area is 975mm
2. the exit velocity is found to be 680m/s
when the inlet velocity is negligible. Assuming that friction in the convergent portion is
negligible, calculate:
i) the mass flow through the nozzle, stating whether the nozzle is underexpanding or
overexpanding;
ii) the nozzle efficiency and the coefficient of velocity
Solution
i) 5283.04.2
2
p
p 4.0
4.1
1
c
therefore,
pc = 6.89 x 0.583 x 3.64 bar
also,
Tc = K3.5832.1
700
2.1
T1
And, Cc = s/m4833.5832874.1
Vc = kg/m459.01064.3
3.583287 3
5
Therefore,
Mass flow rate =
610459.0
6504830.684 kg/s
To determine whether the nozzle is underexpanding or overexpanding it is necessary to
find the correct exit pressure
V2 = kg/m97.010684.0
975680 3
6
Also.
C2 = s/m680TT10052 21
21 TT = 230 K
2T = 700 – 230 = 470 K
therefore,
p2 = bar39.11097.0
4702875
since the actual back pressure is 1 bar the nozzle is underexpanding.
ii) For isentropic expansion between pressures of 6.89 bar and 1.39,
58.139.1
89.6
T
T 4.14.0
2
1
i.e. T2 = K44358.1
700
Chapter two The laws of thermodynamic
82
21 TT = 700 – 443 = 257 K
Then,
Nozzle efficiency = 100257
230 = 89.5%
And,
Coefficient of velocity = 985.0 = 0.946
Worked Example
A turbo air craft is traveling at 625 km/h in atmospheric conditions of 0.45 bar and –26oC. The
compressor pressure ratio is 8, the air mass flow rate is 45 kg/s, and the maximum allowable cycle
temperature is 800oC. The compressor, turbine, and jet pipe stagnation isentropic efficiencies are
0.85, o.89, and 0.9 respectively, the mechanical efficiency of the drive is 0.98, and the combustion
efficiency is 0.99. Assuming a convergent propulsion nozzle, a loss of stagnation pressure in the
combustion chamber of 0.2 bar, and a fuel of calorific value 43 300 kJ/kg, calculate:
i) the require nozzle exit area;
ii) the net thrust developed;
iii) the air-fuel ratio
iv) the specific fuel consumption.
For gasses in the turbine and propulsion nozzle take γ = 1.333 and Cp = 1.15 kJ/kg K;
for the combustion process assume an equivalent Cp value of 1.15 kJ/kg K.
Solution
i) Kinetic energy at inlet = 23600
1000925
21
= 33 kJ/kg
= cp(T01 – T0)
i.e. T01 = (-26 + 273) + (33/1.005) = 279.85 K
then, 247 + (279.85 - 247) x 0.9 = 276.6 K
therefore, p01 = 0.45 x
5.3
247
6.276
= 0.5585 bar
For the process in the compressor:
T02s = T01 x 80.4/1.4
= 1.8115 T01
i.e. T02s = 279.85 x 1.8115 = 506.9 K
then, T02 - T01 =
85.0
85.2799.506 = 267.16 K
i.e. T02 = 279.85 + 267.16 = 547 K
Chapter two The laws of thermodynamic
83
Also, p02 =8 x p01 = 8 x 0.6685 = 5.348 bar
Therefore, p03 = 5.348 – 0.2 = 5.148 bar
cpg(T03 – T04) = cpa(T02 – T01)/0.98
i.e.(T03 – T04) = 98.015.1
16.267005.1
= 238.2 K
therefore T04 1073 – 238.2 = 834.8 K
and, (T03 – T04s) = 89.0
8.8341073 = 267.7 K
i.e. T04s = 1073 – 267.7 = 805.3 K
then, 333.0
333.1
04
03
3.805
1073
p
p
= 3.154
i.e. p04 = 5.148/3.154 = 1.632 bar
For an isentropic nozzle,
333.0
333.1
04
c
333.2
2
p
p
= 0.5398
pc = 1.632 x 0.5398 = 0.881 bar
Since the back pressure is 0.45 bar the nozzle is underexpanding. The actual exit nozzle pressure,
p5 is slightly different from the above since there is friction in the nozzle.
800
-26
2s
0
2
1s
1
3
4
54s
5s
0.45 bar
Tem
per
ature
/(oC
)
Entropy/(S)
Chapter two The laws of thermodynamic
84
Assuming that since the nozzle is choked the actual temperature at exit is the critical temperature,
333.2
2
T
T
04
c = 0.8573
i.e. T5 = Tc = 834.8 x 0.8573 = 715.6 K
therefore
T5s = 9.0
6.7158.8348.834
= 702.4 K
And, 333.0
333.1
5
04
4.702
8.834
p
p
= 1.996
i.e. p5 =0.8176 bar
Then, 55
108176.0
6.715287v
= 2.5146 m
3/kg
And, 6.715287333.1c5 = 523.5m/s
Therefore
Nozzle exit area = 5.523
455146.2 = 0.216 m
2
ii) momentum thrust = a5 ccma
=
3600
109255.52345
3
=11 996 N
and, Pressure thrust = (0.8176 – 0.45) x 105 x 0.216
= 7940 N
i.e. total thrust = 11 996 + 7 940 = 19 936 N
= 19.94 kN
iii) Heat supplied = 45 x 1.15 x (1073 – 547)
= 27 220 kJ/kg
therefore, mass flow rate of fuel = 3004399.0
20027
Chapter two The laws of thermodynamic
85
= 0.635 kg/s
ie. Air-fuel ratio = 635.0
45 = 70.87
iv) specific fuel consumption = 936.19
635.0 = 0.0319 kg/kN s
Chapter nine
Chapter two The laws of thermodynamic
86
Tutorial questions
1. Air enters the nozzle at a pressure of 3 MN/m
2 and with a temperature of 400
0C. it leaves at
a pressure of 0.5 MN/m2. the exit area is 5000 mm
2 the expansion through the nozzle is
adiabatic according to the law PV =C. Determine
the mass flow through the nozzle
the throat area
the mach number at the exit
take =1.4 and R = 0.287 KJ/kgK [15.86 kg/s, 3390mm2, 1.55 ]
2. Air enters the nozzle with a pressure of 700kN/m2 and with a temperature of 180
0C. Exit
pressure is 100kN/m2. the law connecting pressure and specific volume during the expansion in
the nozzle is PV1.3
= C. Dtermine the velocity at exit from the nozzle takeCp =1.006kJ/kgK and
Cv = 0.717kJ/kgK [576m/s]
3. Steam leave as the nozzle of a single stage impulse turbine with a velocity of 1000m/s. the
nozzles are inclined at an angle of 24o to the direction of motion of the turbine blades. The mean
blade speed is 400m/s. and the blade inlet and exit angles are equal. The steam enters the blades
without shock and the flow over the blades is considered to be frictionless.
Determine i) the inlet angles of the blades
ii) the force exerted on the blade in the direction of their motion
iii) the power developed when the steam flow rate is at 4000kg/h
39o, 1.133kN, 453.2kW
Chapter ten
Effects of temperature change
10.Introduction
Chapter two The laws of thermodynamic
87
When matter is subjected to heat energy, the particles which make up the body absorbs the heat
energy and they start vibrating showing that the inter –atomic/ inter molecular forces holding the
particles will be weakened
Weakening of solid particles will result in the formation of liquid
Further addition of heat to liquid would result in the formation of gas
The degree of vibration of particles of a substance is a measure of its temperature
10.1 Thermal expansion and contraction
It is the increase in size or reduction in size of a body when heat is added or subtracted
Most substances increase in size when they are being subjected to heat energy
Their size is reduced when they are cooled, with the exception of water, which expands when it is
cooled to 4 oC
10.2. Linear Expansion It is the increase in length when a body is subjected to heat energy
Coefficient of Linear Expansion ()
It is the increase in length per unit length per degree rise in temperature
The change in length L of a solid bar when heated or cooled through a temperature change t is
given by the experimental relation L = lo t
t
1
Lo
-----------------------------------------------------------(10.1)
l = change in length
lo = original length
t = change in temperature
Final length L1 = l0 + l
By transposing in (1) for l ,
l = lo t
L1 = lo + lo t
= l0(1+ t)
but t = (1 – 2)
L1 = l0 { 1+ (2 – 1)}---------------------------------------------------------------(10.2)
10.3 Superficial expansion / area expansion ()
It is the increase in area per unit area per degree rise in temperature
= t
1
A
A
0
---------------------(10.3)
Chapter two The laws of thermodynamic
88
A1 = a1b1
a1 = a0 + a
= a0{1+ (2 – 1)} but for 1degree ;
a1 = a0(1+)
b1 = b0(1+ )
A1 = a1b1 = a0(1+) b0(1+ )
= a0b0(1+ )2
= a0b0(1+2 +
2)
but = small change
then 2 would be approaching 0
A1 = a0b0(1+ 2)
For temperature change of ( 2 -1)
A1 = a0b0{1+ 2 (2 -1 )}--------------------------------------------------(10.4)
10.4 Volumetric or cubical expansion
It is the increase in volume of an object when subjected to heat energy
Coefficient Of Cubical Expansion () It is the increase in volume per unit volume per degree rise in temperature
V1 = a1b1c1
But a1 = ao + a
b1 = bo + b
c1 = co + c
for change in length of one side a,
a1 = ao{1 + (2 – 1)} but for 1o
a1 = ao (1 + )
b1 = bo (1 + )
c1 = co (1 + )
V1 = a1b1c1
= ao (1 + ) bo (1 + ) co (1 + )
= aoboco(1 + )3
= aoboco{1 + 3 + 32 +
3}
A0
b1
a1a0
b0
A1
Chapter two The laws of thermodynamic
89
but is very small therefore 32 and
3 approach
zero
giving V1 = aoboco{1 + 3 }
for a change in temperature from 1 to 2
V1 = aoboco{1 + 3 (2– 1)}
V1 = Vo{1 + 3 (2 – 2)} but = 3
V1 = Vo{1 + (2 – 2)}----------------------------------------(10.5)
10.5 Change of phase
All matter exists in one of the three states viz. solid, liquid and gas.
Heating a solid enough will result in the formation of a liquid and further application of heat will
result in the formation of gas.
Enthalpy
It is the energy content of a given mass of a substance. Units are J/kg K.
Specific heat capacity
It is the energy, which is required to raise the temperature of 1 kg of a body by 1 degree.
Latent heat
It is that amount of energy which when added or subtracted from a body system will cause a phase
change at a constant temperature.
Sensible heat
It is the amount of energy which when supplied to a body will cause a temperature rise.
c1
co
b1
b2
a1
ao
Vo
V1
Chapter two The laws of thermodynamic
90
SOLID
SOLID
&
LIQUID
LIQUID
&
GASLIQUID
GAS
ENTHALPY
TE
MP
ER
AT
UR
E O
C
Latent
heat
of
fusion
Latent
heat of
Vapour-
isation
``
In general if an amount of heat Q produces a rise in temperature t in a body of mass m and
specific heat capacity c and the same heat produces the same rise in temperature in a mass mw of
water then mw is the water equivalent of the body, thus:
Q = cm t = cwmw t
i.e. equivalent mass of water, mw = mc
c
w
WORKED EXAMPLES
QUESTION 1
AN 80 mm Ø aluminium piston fits into a cast iron cylinder with uniform radial clearance of 0.75
mm at room temperature. Determine the percentage increase in area of the gap between piston and
cylinder at 130°c. For aluminium, =24x10-6
/K and for Cylinder, =10X10-6
/K.
Area of piston = r2 = x 40
2 = 5027mm
2
Area of cylinder = r2= x 40.75
2 =5217mm
2
Initial gap area = x 40.752 - 40
2
=190.3 mm2
Coefficient of superficial expansion for aluminium is,
= 2 = 2 x24 x10-6
/k
Change in temperature = (130oC -15
oC)= 115
oC
Chapter two The laws of thermodynamic
91
Increase in area of piston =2tAo
=2 x 24 x 10-6/k x 5027 x 115 = 27.8mm2
Increase in cylinder area =2 x 10 x 10-6/k x 52217 x 115
=12 mm2
Change in area of cylinder gap
=27.8 mm2 – 12 mm
2
=15.8mm2
Percentage increase =15.8/190.3 x 100
= 8.3 %
QUESTION 2
A steel tank of mass 50 kg contains 200 kg of water at 15 oC. A further 100 kg of water is poured
into the tank at 95 oC. If the specified heat capacity of steel is 0.44 kJ/kg K, calculate the final
temperature of the water in the tank.
Let t be the final temperature of the mixture.
Heat given up by the liquid poured in the tank
= mct
= 4.2 x 100 x (95 – t)kJ
Heat gained by steel tank = mc t
=.45 x 50 x (t -15)KJ
=22.5 (t – 15)KJ
Heat gained by water in tank = mc t
= 4.2 x 200 x (t – 15)
Equating heat given up by the water poured into the heat taken by the tank and water then =
4.2 x 100 x (95 – t) = (22.5 (t – 15)) + 4.l2 x 200 (t – 15)
= 862.5 (t – 15)
t = 41.3 oC.
QUESTION 3
Calculate the heat required to convert 8 Kg of ice -10 oC to water at 60
oC. The specific Heat
capacity of ice is 2.1 KJ/Kg K and its latent heat is 335KJ/Kg.
Heat required to raise temperature of the ice from -10 oC to melting point 0
oC
= mct
= 2.1 x 8 x 10
=168 KJ
Heat to melt the ice at constant temperature = mass x latent heat
= 8 x 335
=2680 KJ
Chapter two The laws of thermodynamic
92
Heat to raise temperature of 8 Kg of water from 0 oC to 60
oC
= mct
= 8 x4.2 x 60
= 20166 KJ
Total Heat required = 2016KJ + 2680KJ + 168KJ
= 4864 KJ
Chapter ten
Tutorial questions
1.A duralumin piston slides in a cast iron cylinder at 20 oC. At this temperature, there is a radial
clearance of 0.13m and the piston diameter is 100 mm. Determine the area of gap at 20 oC and
also when the temperature is raised to 120 oC. When the coefficient of linear expansion is 22.5 x
10 -6
/k. [20mm²]
2. How much heat energy would be required to convert 20g of ice at -15 oC into water at 40
oC
take the relative specific heat capacity of ice as 0.5 and the specific enthalpy of fusion as
335kJ/Kg [10.69 KJ]
Chapter two The laws of thermodynamic
93
3 .A glass flask of volume 200 cm ³ is first filled with mercury at 20ºC. How much mercury will
over flow when the temperature of the system is raised to 100ºC? The coefficient of cubical
expansion of glass is 1.2 x 10 -6
and mercury is 18 x 10 -5
. [27 cm ³]
4.A refrigerator produces ice by evaporation of to liquid ammonia. How much liquid ammonia
must be evaporated to convert 500g of water at 15ºC to ice at -5ºC. If no heat energy is
transmitted through the outside walls the refrigerator.
Specific enthalpy of fusion of ice is 335 KJ/Kg and specific heat capacity of ice is 2.1 KJ/Kg.
[204.25 KJ]
Chapter two The laws of thermodynamic
94
Chapter eleven
Heat transfer 11.0 Introduction
The laws of heat transfer find application in many engineering fields i.e. in process engineering,
manufacturing and in everyday life. Heat transfer is by virtue of temperature difference between
parts of material. There are three ways by which heat can be transferred. These are conduction,
convection and radiation.
11.1 Heat Transfer By Conduction
It is the main mode of heat transfer in solid materials. Heat transfer by conduction occurs by
virtue of temp difference between parts of a material. It also takes place in liquids and gasses.
11.2 Mechanism of Conduction
source
of
heat
particles Figure 11.1.
The particles, which are in contact with the source of heat, absorb heat energy through contact. As
the particles get heated, they start vibrating, thereby getting in contact with the adjacent particles
thus passing heat to the next particle until the energy is distributed within the material.
Conduction within a solid material is the transfer of internal energy. This energy is the kinetic
energy of the constituent molecules, atoms and particles of the material. This kinetic energy is
proportional to the absolute temperature. Metals are generally considered as good conductors of
heat. Materials such as glass, wood, wool, paper, and asbestos are poor conductors or insulators. A
good conductor of heat has a high thermal conductivity. Good conductors of heat are usually good
electrical conductors.
11.3 Fourier’s Rate Equation Of Conduction
Molecular collision leads to energy transfer to regions of low kinetic energy. Under steady state
conditions, a molecule will pass on the same amount of energy as it receives.
The figure shows a section of a rod through which heat is flowing.
If the temperature T2 and T1 of a section are kept for a sufficient long time the temperature at
points within the rod is found to decrease uniformly with distance from the hot to the cold face.
However at each point the temperature remains constant with time. This condition is the steady
state.
Chapter two The laws of thermodynamic
95
Experiments have shown that:-
The rate of heat flow Q at steady state is proportional to area A and temperature difference T2—T1
is inversely proportional to the change in length .
12 TTA
Q
12 TTkA
Q
TkAQ
A is the area of transfer, m2.
T1 is the inlet face temperature.
T2 is the outlet face temperature.
is the change in thickness.
k is the coefficient of thermal conductivity
of the material (W/m K) Figure 11.2.
– negative sign shows that the temperature is
decreasing with increase in distance.
11.4 Conduction through A Flat Plate
The transfer of heat by conduction is found to depend upon: -
The area through, which heat transfer, takes place. The temperature difference of the two faces through which the heat is passing.
The time taken for heat transfer.
The thickness of material through which the heat is passing.
The greater the area and temperature difference, the greater would be the heat transfer. The heat
transfer is, therefore, inversely proportional to the thickness of wall. Consider a flat plate, or wall
thickness and heat transfer area A. Let the temperatures of its faces be T1 and T2. This is shown
on figure below
Quantity of heat required
12 ttkA
A
T1
T2
Q
Chapter two The laws of thermodynamic
96
21 TTkA
Q ------------------------11.1
t1
t2
Direction of
heat transfer Q
Heat transfer
area A
Figure 11.3.
11.5 Conduction through A Composite Wall
Consider the composite wall shown in figure 4. In this case there are three layers.
t1
2 3
t2
k2k1 k3
t3
t4
1
Direction of
heat transfer Q
Heat transfer
area A
Figure 11.4.
If Q is passing through this wall, then Q is passing through each wall.
Chapter two The laws of thermodynamic
97
Thus
1
211 ttAkQ
……………………………………..1
2
322 ttAkQ
…….……………………..………..2
3
432 ttAkQ
………………………………..……..3
Transposing equations 1, 2 and 3 gives,
Ak
Qtt
1
121
………………………….…………………..4
Ak
Qtt
2
232
……………………………………………..5
Ak
Qtt
3
343
……………………………………………..6
Adding equations 4, 5 and 6 gives,
3
3
2
2
1
141
kkkA
Qtt ……………………………….7
From equation 7,
2
2
2
2
1
1
41
kkk
TTAQ
------------------------11.2
Therefore in general for n number of layers,
k
TTAQ 1n1 -----------------------11.3
Chapter two The laws of thermodynamic
98
Thus the heat transfer per second can be calculated. When this is known, by substitution in
equations 1, 2 and 3 the interface temperatures can be calculated.
11.6 Surface and Overall Heat Transfer
Now there must be a temperature difference a surface and its surroundings for heat transfer to
occur.
As before if heat transfer Q passes through wall, then Q passes through each layer of the wall.
Let ta1 = ambient temperature (temperature of surrounding) on inlet side
t1 = inlet surface temperature
t2 = interface temperature
t3 = exit face temperature
ta2 = temperature of surrounding on outlet side
t2
k1
t1
k2
t3
ta2Inlet surface
film
a1
Outlet surface
film
Direction of
heat transfer Q
21
Figure 11.5.
Q = Us1A(ta1-t1)
= Us2A(t3-ta2)
U is called the surface transfer coefficient and has units W/m2K
2a2
2
1
1
1a
2a1aU
1
kkU
1
A
Qtt
Chapter two The laws of thermodynamic
99
2a2
2
1
1
1a
2a1a
U
1
kkU
1
ttAQ
= UA(ta1-ta2)…………………………………………11.4
2a2
2
1
1
1a U
1
kkU
1
1U …………………………11.5
= Overall transfer coefficient sometimes called the U coefficient value.
11.7 Conduction through A Thin Cylinder
A thin cylinder may be one whose internal surface area is almost the same as its external surface
area. From heat transfer point of view, if this is the case, then the area through which the heat is
passing is always very nearly the same. For a thin cylinder of radius r, (either external or internal)
and thickness x, then the area of heat transfer for a length of cylinder L = 2rL.
21 TTkA
Q
21 ttrL2k
Q
Figure 11.6.
11.8 Conduction through A Thick Cylinder
Let L be the length of the cylinder. The internal surface area of a thick cylinder is much smaller
than the external surface area. The fig shows a thick cylinder of internal radius r1 and external
radius r2 with internal and external temperatures t2 and t2 respectively. Assume that the heat is
flowing from the inside to the outside. Consider the elementary cylinder of radius r and thickness
r, let the change across this elementary cylinder t.
t1
r1 t2L
Chapter two The laws of thermodynamic
100
t2
t1
r2
r1
r
Q Q
r
r
Figure 11.7.
Hence the heat transfer r
tkAQ
r
trL2kQ
Make t the subject,
rL2k
rQt
rr
1
L2k
Qt
2r
1r
2t
1t
1
212
r
rln
L2k
Qtt
1
212
r
rln
L2k
Qtt
1r2rln
ttL2kQ 21
Chapter two The laws of thermodynamic
101
k
ln
ttL2Q
12r
r21
-------------------------------------11.6
11.9 Heat Transfer through A Composite Cylinder
Similarly Q is given by,
321
41
k
ln
k
ln
k
ln
ttL2Q
34
23
12
rr
rr
rr
t1
t4
r1
r4
r2
r3
Qt2
t3
Figure 11.8.
For inner cylinder
t1— t2 = (Q/2Lk1) ln r2/r1 ……………………………………..1
For intermediate cylinder
T2— t3 = (Q/2Lk2) ln r3/r2 ……………………………………..2
For outer cylinder
T3— t4 = (Q/2Lk3) ln r4/r3 ……………………………………..3
Adding equations 1, 2 and 3 gives,
321
41k
ln
k
ln
k
ln
L2
Qtt 3
42
31
2r
rr
rr
r
Chapter two The laws of thermodynamic
102
321
41
k
ln
k
ln
k
ln
ttL2Q
34
23
12
rr
rr
rr
----------------------------------------------------------11.6
11.10 heat transfer by convection
It is the name given to gross motion of fluid itself so that fresh fluid is continuously available for
heating or cooling.
Mechanism
Air next to the source of heat is heated by conduction, due to its contact with the hot surface. The
heated mass of air will expand, increasing its volume and density decreasing. The cool air around
with higher density will displace the warm air, which is forced to rise. The cool air gets in touch
with hot surface and become warm by conduction. This process continues with heat getting
distributed within the fluid.
Types Of Convection Transfer
Natural convection — is the movement of fluid caused by differences in density
resulting from temperature differences.
Forced convection — is produced by mechanical means e.g. by fans.
Newton’s Law Of Cooling
The heat transfer from one fluid to another through a wall is understood by studying
how heat is transferred from one to a wall and vice versa.
Newton’s law of cooling states that:
Heat transfer from a solid surface of area A at temperature tw to a fluid of
temperature t is given by:
Q = hA(tw — t) ------------------------11.7
h is the heat transfer coefficient with units W/m2K. h depends on the properties of
the fluid and its velocity.
Transfer Of Heat From Fluid A To
Fluid B Through A Wall.
In fluid the temperature decreases
suddenly from tA to t1 and in fluid B,
temperature decreases rapidly from t2
to tB. this is due to the thin film close
to the wall where transfer is by
conduction.
k
Fluid A
Ta
t1
Direction of
heat transfer Q
Tbt2
Fluid B
Chapter two The laws of thermodynamic
103
X is thickness of wall.
K is thermal conductivity.
Figure 11.9.
Considering unit surface area
From fluid A to the wall the rate of heat transfer is,
1a
A
A ttk
Q
A
AA1aA
khwhere,tthQ
From wall to fluid B
b2
B
B ttk
Q
B
BBb2B
khwhere,tthQ
Transmission through the wall per unit area
21 ttk
Q
For steady state, heat transfer flowing from fluid A to the wall = heat flowing
through the wall = heat flowing through from wall to the wall.
Q = hA(tb — t1) = hB(t2 — tb) =
21 ttk
Expressing in terms of temperature,
Chapter two The laws of thermodynamic
104
(ta — t1) = Ah
Q
(t1 — t2) =
k
Q
(t2 — tb) = Bh
Q
Adding the corresponding sides,
(tA — tB) = Q + Q + Q
hA k hB
X
(tA — tB) = Q 1 + X + 1
hA k hB
Q = (tA — tB)_______
1 + X + 1
hA k hB --------------------------11.8
Q = U(tA — tB)
1 = 1 + X + 1
U hA k hB
U is the overall heat transfer coefficient has the same units as h.
11.11 transmission of heat by radiation
Chapter two The laws of thermodynamic
105
Thermal radiation consists of electromagnetic waves emitted due to the agitation of
the molecules of substance. These waves are similar to the light waves in that they
are propagated in a straight line at the speed of light. It requires no medium to be
transmitted. Heat energy from the sun to the earth is mainly transmitted by radiation
because the space between is largely vacuum.
Radiation striking a body (absorptivity )
Reflected from the body (reflectivity )
Transmitted through the wall (transmissivity )
The emissivity of a body radiating energy at a temperature t is equal to the to the
absorptivity (α) of the body when receiving energy from the source from
temperature t.
The Boltzmann’s law
States that the emissive power of the black body is directly proportional to the
fourth power of its absolute temperature.
EB = s AT4
Where s is Boltzmann’s constant = 5.67-8
Wm2/K
4
Energy absorbed by a grey body,
E = s T4
Where is the emissivity of the body.
The heat transfer from the body to its surroundings per square metre is given by,
Q = s(T14— T2
4) -----------------------------11.9
Worked Example
In a small furnace, the heat loss to the surroundings is to be kept down to 1 700 W/m
2. The
internal temperature of 150 mm firebrick wall which lines the furnace is 650oC, and the
temperature of the air surrounding the furnace is 25oC. Neglecting the temperature drop through
the steel casing, calculate the thickness of exterior lagging required. Take the thermal conductivity
of the firebrick 1W/mK, the thermal conductivity of the lagging as 1.2W/mK and the convection
heat transfer coefficient of the lagging surface as 20W/m2K. Radiation from the lagging surface
Chapter two The laws of thermodynamic
106
may be ignored. Estimate also the temperature of the outer surface of the lagging.
lm
Lagging
Steel
shell
Fire
brick
0.150m
25°C
650°C
Figure 11.10.
For conduction through the fire brick Q = 1700W/m2
1650kAQ
)1..(..........m/W
15.0
6501Q 21
For conduction through the lagging
)2..(..........m/W
2.1Q 221
For convection from the lagging surface
25hAQ 2
)3..(..........m/W2520Q 22
From (1)
15.01700650 1
From (2)
2.1
170021
From (3)
20
11700252
Adding:
2.1
05.015.0170025650
thus 05.015.01700
625
2.1
l = 0.201 m
For temperature of the lagging surface, from equation (3)
1700 = 20(2 – 25)
Chapter two The laws of thermodynamic
107
2 = 1100C
Worked Example
A steel pipe shown in Figure 1 carries steam at 260 oC. The atmospheric temperature is 15
0C. The
heat transfer coefficient for the inside and outside surfaces are 550 and 15W/m2K respectively,
and the thermal conductivities of steel, diatomaceous earth and asbestos felt are 50, 0.09, and
0.07W/mK respectively. Calculate:
The rate of heat loss by the steam per unit length of pipe
The temperature of the outside surface.
Diatomaceous Earth
Asbestos Felt
Ø 3
14
Ø 1
94
Ø 1
14 Ø
100
Steel
all dimensions are in milimetres
Figure 11.11.
Rate of heat loss Q
aafdesta
as
h
1
k
ln
k
ln
k
ln
h
1
ttL2Q
34
23
12
rr
rr
rr
15
1
07.0
ln
09.0
ln
50
ln
500
1
1526012Q
097.0157.0
057.0097.0
05.0057.0
Q = 116W
Rate of heat loss per meter length of pipe = 116W
0675.0
15t116Q 4
Chapter two The laws of thermodynamic
108
t4 = (116 x 0.0675) + 15
= 22.8oC
Temperature of outside surface = 22.8oC
Chapter eleven
Tutorials
1.Calculate the quantity of heat conducted per minute through a circular disc of diameter 127 mm
19mm thick hen the temperature drop across he thickness of the plate is 5oC. Take the coefficient
of thermal conductivity as 150W/mK. [30kJ]
2.A cold storage compartment is 4.5m long by 4m wide by 2.5m high. The four walls, ceiling and
floor are covered to a thickness of 150mm with insulating material, which has a coefficient of
thermal conductivity of 5.8 x 10-2
W/mK. Calculate the quantity of heat leaking through the
insulation per hour when the inside and the outside face temperatures of the material is 15oC and –
5oC respectively. [2.185MJ or 2185kJ]
3.One side of a refrigerated cold chamber is 6m long by 3.7m high and consist of 168mm
thickness of cork between outer and inner walls of wood. The outer wood wall is 13mm thick and
its outside face temperature is 20oC, the inner wood wall is 35mm thick and its inside face
temperature is –3oC.Taking the coefficient of thermal conductivity of the cork and wood as 0.042
and 0.2W/mK respectively, calculate:
Chapter two The laws of thermodynamic
109
(a) the heat transfer per second per square metre of surface area, [5.318J]
(b) the total heat transfer through the chamber side per hour, [425kJ]
(c) the interface temperatures. [19.2oC , -2.07
oC ]
4.Hot gasses at 280oC flow on one side of metal plate of 10mm thickness and air at 35
oC flows on
the other side. The heat transfer coefficient the gasses is 31.5 W/m2K and that of air is 32W/m
2K.
The coefficient of thermal conductivity of the metal plate is 50W/mK. Calculate:
(a) the overall heat transfer coefficient, [15.82W/m2K]
(b) the heat transfer from gasses to air per minute per square metre of plate area.
[232.7kJ ]
5.The wall of a cold room consists of a layer of cork sandwiched between outer and inner walls of
wood, the wood walls being each 30 mm thick. The inside atmosphere of the room is maintained
at –20oC when the external atmospheric temperature is 25
oC, and the heat loss through the wall is
42W/m2. Taking the thermal conductivity of cork and wood as 0,2W /m K and 0.05 W/mK
respectively, and the rate of heat transfer between each exposed wood surface and their respective
atmospheres as 15W/m2k, calculate;
(a) the temperatures of the exposed surfaces, [22.2oC , -17.2
oC]
(b) the temperatures of the interfaces, [15.9oC , -10.9
oC]
(c) the thickness of the cork. [31.9mm]
6.A flat circular plate is 500 mm diameter. Calculate the theoretical quantity of heat radiated per
hour when its temperature is 215oC and the temperature of its surrounds is 45
oC. Take the value of
the radiation constant as 5.67 X 10-11
kJ/m2sK
4
[1862kJ]
7.The steam drum of a water-tube boiler has hemispherical ends, the diameter is 1.22m and the
overall length is 6m. Under steaming conditions the temperature of the shell lagging was 230oC
and the temperature of the surrounds was 51oC. The temperature of the cleading after lagging was
69oC and the surrounds 27
oC. Assuming 75% of the total shell area to be lagged and taking the
radiation constant as 5.67X10-11
kJ/m2sK
4, estimate the saving in heat energy per hour due to
lagging. [167MJ]
Chapter two The laws of thermodynamic
110