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Old May 5th, 2012, 12:31 PM
crythicky
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Default IIT Lecture Notes PDF

Sir I am searching for the Indian Institute of Technology Lecture Notes so please can you give me the notes and tell me from where I can download the PDF of IIT Lecture Notes and provide me the link that can give me the free download?
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Old May 5th, 2012, 06:20 PM
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Default Re: IIT Lecture Notes PDF

It is very difficult to get the notes online if you want to get the notes then you should contact to student of that particular IIT.
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Old February 15th, 2014, 12:27 PM
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Here I am giving you lecturer notes for Engineering Thermodynamics course offer by Indian institute of technology college in zip file with it …. Some content is given below :

Engineering Thermodynamics lecturer notes :

Types of Thermodynamic Systems
There are three types of thermodynamic systems :
a) Closed System
b) Open System and
c) Isolated System

BASIC CONCEPTS
AND
DEFINITIONS
Thermodynamics is the science of energy transfer which deals with the relations among heat, work and properties of systems.
The name ‘thermodynamics’ is derived from the Greek words therme, meaning ‘heat’ and dynamis meaning power. Thus, thermodynamics is basically the study of heat and power.

1.1 Application Area of Thermodynamics
Energy transfer is present in almost all the engineering activities. Hence, the principles of thermodynamics are playing vital role in designing all the engineering equipments such as internal combustion engines, rockets, jet engines, thermal and nuclear power plants, refrigerators etc.

1.2 Statistical and Classical Thermodynamics
Statistical Thermodynamics is microscopic approach in which, the matter is assumed to be made of numerous individual molecules. Hence, it can be regarded as a branch of statistical mechanics dealing with the average behaviour of a large number of molecules.
Classical thermodynamics is macroscopic approach. Here, the matter is considered to be a continuum without any concern to its atomic structure.
Consider a gas in a container. Pressure exerted at the wall of the container is the average force per unit area due to the collision of the gas molecules on the wall surface. To determine this pressure, we need not know the behaviour of individual molecules of the gas. This approach is macroscropic approach. However, the results obtained from macroscopic and statistical study of matter.

1.3 Thermodynamic Systems and Surroundings
A Thermodynamic system is defined as a quantity of matter or a region in space whose behaviour is being investigated.
Everything external to the system is defined as surroundings. In its usual context the term ‘surroundings’ is restricted to the regions in the immediate vicinity which has a detectable influence on the system.
Boundary is the surface which separates the system from its surroundings. It may be fixed or moving and real or imaginary.

Fig.1.1 Thermodynamic System, boundary, surroundings
1.3.1 Types of Thermodynamic Systems
There are three types of thermodynamic systems :
a) Closed System
b) Open System and
c) Isolated System
In closed system, attention is focused on a fixed mass. Energy in the form of heat and work (The terms heat and work will be defined in the chapter 2.) can cross the boundary of the system. But there is no mass flow across the boundary. Hence, the possibility of change in volume is always there in the closed systems.

Fig.1.2 Closed system

In open system, both matter and energy can cross the boundary. Here, the behaviour of a fixed region in space called control volume is investigated and hence, there is no change in volume. The surface of the control volume is known as control surface.

Fig.1.3 Open system

A system that exchanges neither energy nor matter with its surroundings is known as an isolated system.


Fig.1.2 Isolated system

1.4 Thermodynamic Properties
In all thermodynamic problems energy transfer to or from the system is observed. To receive, store and deliver energy a working substance is present within the system. The characteristics which can be used to describe the condition of the system are known as properties.
Thermodynamic properties are classified into two categories : intensive and extensive. Intensive properties are independent of quantity of matter or mass whereas extensive properties are dependent on mass
Consider a vessel containing air. If a membrane is assumed to be introduced into the vessel, such that it is divided into two equal parts. The properties remaining unchanged such as pressure and temperature are intensive properties. Volume of air will be reduced to half of its initial value. Hence, it is an extensive property.

1.5 Thermodynamic State and Equilibrium
When a system does not undergo any change, all the properties have fixed values. This condition is known as a thermodynamic state.
The word equilibrium means balance. An equilibrium state of a thermodynamic system is a state that can not be changed without any interaction with its surroundings. The factors that cause a change without any interactions with its surroundings are:

1. Pressure difference
2. Temperature difference
3. Chemical reaction
If a system is balanced in all respects, it is in a state of thermodynamic equilibrium. Balanced in all respects means :

• There should not be any temperature difference within the system, so that the system is thermally balanced.
• No pressure difference exists between any two points within the system (Neglecting gravitational effects) and between the system and surroundings, so that it is mechanically balanced.
• No chemical reaction is taking place, so that it is chemically balanced.
• If two phases are involved, mass of each phase remains constant so that phase equilibrium is achieved.
Hence, for a system in a state of thermodynamic equilibrium, there is no change in any macroscopic property.

1.6 Processes and Cycles
When a system is taken from one equilibrium state to another, the change is known as process. The series of intermediate states through which a system passes during a process is called the path of the process. If all these intermediate states are equilibrium states, the process is known as quasi equilibrium or quasi-static process.
Consider a certain quantity of gas taken in a frictionless piston cylinder arrangement as shown in Fig 1.5. The system is in thermodynamic equilibrium so that there is no unbalanced force acting on piston.

Fig.1.5 Illustration for thermodynamic equilibrium

The moment the weight is removed from the piston, mechanical equilibrium does not exist and as a result the piston is moved upward until mechanical equilibrium is restored again. Therefore the actual process occurs only when equilibrium does not exist.

As shown in Fig.1.5.a, if the entire weight on the piston is removed at once, the deviation from the equilibrium is high and the expansion is rapid. For such a process the intermediate states are not equilibrium states and hence the process would be non-quasi-equilibrium.
If the weight is assumed to be made of a large number of small pieces as shown in

Fig.1.5.b and taken off one by one, the deviation from equilibrium is less. The process could be considered quasi-equilibrium.
A thermodynamic system is said to undergo a cycle, if it is taken through a number of processes such that, the final state of the last process is identical with the initial state of the first process in all respects. For cycles net change in any property is zero.

1.7 Point and Path Functions
Thermodynamic functions are classified into two categories namely point and path functions. Point functions are those for which the change depends on only the end states and not on the path followed. Hence point functions are inexact differentials
Path functions are those for which the change depends not only on the end states but also on the path followed. Hence path functions are exact differentials
In can be observed the change in any property during a process depends only on end states. Therefore all the properties are point functions.
.
To demonstrate path and point functions, let us consider two stations A and B on a hill as shown in the Fig.1.6. While moving from station A to station B, let the distance traveled and increase in height from the mean sea level are observed. Distance traveled in path 1 is different from that in path 2. Hence it may be regarded as path function. But the change in height is same in both path 1 and path 2, therefore it is a point function.

Fig.1.6 Illustration of point and path functions


1.8 State Postulate and Property Diagrams
As mentioned earlier, properties are meant for describing the state of a system. To fix a state, all the properties need not be specified. If any two independent intensive properties are specified, rest of the properties automatically assumes certain values.
This is known as state postulate.

Fig.1.7 property diagram of equilibrium and non equilibrium processes
Consider pressure and specific volume (Volume per unit mass) are the two independent, intensive properties, describing the state of a compressible system. On a p-V diagram the state will assume a point as represented in the Fig.1.7(a). Let the system be taken to another state such that all the intermediate states are equilibrium states. The curve connecting the initial state and final state, passing through all the intermediate states is indicating the path of the process. In non-quasi-equilibrium process as the intermediate status can not be defined, the path is denoted by dashed line as given in Fig.1.7(b)

Fig. 1.8 Thermodynamic cycle on a property diagram
Fig.1.8 indicates a system undergoing a cycle consisting of three quasi-equilibrium processes.

1.9 Temperature and Zeroth Law
Maxwell defined the temperature of a system as its Thermal state considered with reference to its ability to communicate heat to other bodies.
When a hot body is brought into contact with a cold body, the hot body becomes cooler and the cold body becomes hotter. After sufficient time, the temperature of both the bodies will be equal. At that point, the two bodies are said to have reached thermal equilibrium.
Consider three bodies A, B and C. If the bodies A and B are in thermal equilibrium with C when brought into contact separately, they are also in thermal equilibrium with each other. This concept is known as zeroth law of thermodynamics.

Several properties of materials are found to be varying with temperature in a predictable way. This variation is used to measure temperature. In mercury thermometers, expansion of mercury with temperature is used for temperature measurement.

1.10 Temperature Scales
Freezing point of water known as ice point and boiling point of water known as steam point are taken as the reference states for all types of temperature scales.
The various types as temperature scales in use are :
a) Celsius scale
b) Fahrenheit scale
c) Kelvin scale
d) Rankine scale


Reference state Celsius Kelvin Fahrenheit Rankine
Steam point 100 373 212 672
Ice point 0 273 32 492
Absolute Zero -273 0  460 0

1.11 Homogeneous and Heterogeneous Systems
Matter can exist in any one of the three phases namely solid, liquid and gas. A system consisting of a single phase is known as homogeneous systems. If the matter exists in more than one phase, the system is known as heterogeneous system.
1.12 Pure Substances
Substances of fixed chemical composition throughout are known as pure substances.
That is, pure substances have homogenous and invariable chemical composition irrespective of the phase or phases in which they exist.
Example
a. Atmosphere air
b. Water
c. Nitrogen
d. Water-steam mixture
e. Product of combustion.
Though, mixture of water and steam is considered a pure substance, air and liquid air cannot be, since, the chemical composition of liquid air differs from that of gaseous air.
1.13 The Ideal Gas
Based on the experimental work carried out by Boyle, Charles and Gay-Lussac, pressure, temperature and specific volume of many gases at low pressure and moderate temperature are related by the following equation.
pv = RT where R=
This equation is known as equation of state of an ideal gas. The term R is known as characteristic gas constant and Ru universal gas constant. In SI unit Ru= 8.314 kJ/kgmol.K.
1.14 Concept of continuum
In microscopic approach the substance is assumed to be continuously distributed, ignoring the space between the molecules. This is known as continuum hypothesis.
Since the matter is treated as continuous, the density at a point can be defined as

Where v’ is the smallest volume for which a definite value of the ratio exists. Below the limiting value of v’ , the fluctuation in average density will be high and a definite value for the ratio becomes impossible, with the mean free path* of the molecules approaching the order of magnitude of the dimension of the vessel.

* mean free path is the distance traveled between two consecutive collisions of a molecule.


Exercises
1. Identify the type of the systems given below.
a) Reciprocating air compressor
b) Steam turbine in a steam power plant
c) Pressure cooker
d) Radiator of an automobile engine
e) A can of soft drink cooled inside the refrigerator

2. In ____________system control volume approach is employed.
3. Define a quasi-equilibrium process.
4. Define intensive and Extensive properties. Give examples.
5. What is the state postulate ?
6. What is zeroth law of thermodynamics ?
7. When does the concept of continuum become invalid ?
8. In which type of system neither mass nor energy is allowed to cross the boundary.
9. What is meant by thermodynamic equilibrium?
10. What is meant by a control surface?
11. What is meant by microscopic and macroscopic approach?
12. Universal gas constant = Characteristic Gas constant Molecular weight (T/F)
13. What is an open system? Give examples.
14. Define a closed system. Give examples.
Attached Files
File Type: zip IIT Engineering Thermodynamics lecturer note.zip (2.00 MB, 4 views)
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  #4  
Old February 24th, 2014, 11:54 AM
Sashwat's Avatar
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Default Re: IIT Lecture Notes PDF

Here I am giving you lecturer notes for Joint entrance examination for admission in Indian institute of Technology College in PDF file with it …. Some content is given below:

Order & Degree of a Di erential Equation
Order of a derivative
Number of times the dependent variable is di erentiated is de ned
the order of the derivative
Order of a derivative
Order of a DE is de ned as the order of the higest order derivative
occurring in the DE

Order & Degree
Degree of a DE
Degree of a DE is power over the highest order derivative provided
the DE is a polynomial in derivatives of dependent variable i.e.
1 DE is free from radicals over the di erential coe cients
2 DE is free from denominators
So that the DE becomes a polynomial in derivatives of the
dependent variables

Solution to a di erential equation can be of two types
Generala : General solution is the solution to a D.E containing
arbitrary independent constants.
Particular : Particular solution of a D.E is de ned as the solution
without any arbitrary constants i.e. those arbitrary constants are
evaluated by given extra condition.

Orthogonal Trajectories
Definition

Orthogonal TrajectoriesAny curve which cuts every member of a
given family of curves at right angle, is called an orthogonal
trajectory of the family
For e.g. Each straight line passing through the origin, y = mx is an
orthogonal trajectory of the family of the circles x2+y2 = a2











Attached Files
File Type: pdf IIT JEE lecturer notes.pdf (359.9 KB, 4 views)
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