1. Chapter: 01
BASIC CONCEPTS

2. Objectives
Identify the unique vocabulary associated with thermodynamics through the precise definition of basic concepts to form a sound foundation for the development of the principles of thermodynamics.
Review the metric SI and the English unit systems.
Explain the basic concepts of thermodynamics such as system, state, state postulate, equilibrium, process, and cycle.
Review concepts of temperature, temperature scales, pressure, and absolute and gage pressure.
Introduce an intuitive systematic problem-solving technique.

3. What is Mechanical Engineering?
Before we start learning Thermodynamics…
What is Engineering?
What is Mechanical Engineering?
What is the place of Thermodynamics in Mechanical Engineering?

4. What is Engineering?
Resources
ENGINEERING
Good Life

5. What is Mechanical Engineering?
Machines
Power
Resources
Good Life

6. What is the place of Thermodynamics in Mechanical Engineering?
Machines
Power
Resources 6
Good Life

7. What is the place of Thermodynamics in Mechanical Engineering?
Thermal Engineering
Power
Fuel
SPECIAL
MACHINES
Pump
Water
Cool
Stuff
Good Effects
Power

8. What is THERMODYNAMICS?
It is the science of energy.
The name thermodynamics stems from the Greek words therme (heat) and dynamis (power).

9. Points to remember:
Conservation of energy principle: During an interaction, energy can change from one form to another but the total amount of energy remains constant.
Energy cannot be created or destroyed.

10. Application Areas of Thermodynamics

11. SYSTEMS ~ thermodynamic system
A quantity of matter or a region in space chosen for study.

12. Thermodynamic system

13. SYSTEMS ~ thermodynamic system
System: A quantity of matter or a region in space chosen for study.
Surroundings: The mass or region outside the system
Boundary: The real or imaginary surface that separates the system from its surroundings.
The boundary of a system can be
fixed or movable.

14. SYSTEMS AND CONTROL VOLUMES
Systems may be considered to be closed or open.
Closed system (Control mass): A fixed amount of mass, and no mass can cross its boundary.

15. Open system (control volume): A properly selected region in space.
It usually encloses a device that involves mass flow such as a compressor, turbine, or nozzle.
Both mass and energy can cross the boundary of a control volume.
Control surface: The boundaries of a control volume. It can be real or imaginary.
An open system (a control volume) with one inlet and one exit.

16. Open system (control volume): A properly selected region in space.
It usually encloses a device that involves mass flow such as a compressor, turbine, or nozzle.
An open system (a control volume) may have one/ multiple inlet and one / multiple exit.

17.  Why do we have to study STATE of a system?
What happens to the system when there is some mass or energy transfer?
What the changes that the systems undergo during this exchange?

18. How to define STATE OF A SYSTEM?
List of relevant characteristics :
PROPERTIES
Quantify each Property.

19. How to define STATE OF A SYSTEM?
Example: M V p T
=700 gm
= 0.8 lit
= 1 bar
= 250

20. VIEW POINT m V p T =700 gm = 0.8 lit = 1 bar = 250
This quantification follows MACROSCOPIC view point.

21. MACROSCOPIC / MICROSCOPIC VIEW POINT
Classical thermodynamics: A macroscopic approach to the study of thermodynamics that does not require a knowledge of the behavior of individual particles.
It provides a direct and easy way to the solution of engineering problems and it is used in our study.
Statistical thermodynamics: A microscopic approach, based on the average behavior of large groups of individual particles.
It is used in our study only in the supporting role.

22. Continuum
Matter is made up of atoms that are widely spaced in the gas phase. Yet it is very convenient to disregard the atomic nature of a substance and view it as a continuous, homogeneous matter with no holes, that is, a continuum.
The continuum idealization allows us to treat properties as point functions and to assume the properties vary continually in space with no jump discontinuities.
This idealization is valid as long as the size of the system we deal with is large relative to the space between the molecules.
This is the case in practically all problems.
In this text we will limit our consideration to substances that can be modeled as a continuum.
Despite the large gaps between molecules, a substance can be treated as a continuum because of the very large number of molecules even in an extremely small volume.

23. PROPERTIES OF A SYSTEM Property: Any characteristic of a system.
Primitive properties: Some familiar properties – Area A, pressure P, volume V, and mass m.
Thermodynamic Properties: T, E, S
Derived: Enthalpy H, Bulk-Modulus

24. PROPERTIES OF A SYSTEM
CLASSIFICATION: β B A
EXTENSIVE
INTENSIVE

25. PROPERTIES OF A SYSTEM SPECIFIC PROPERTIES (denoted by small letters)
CLASSIFICATION:
EXTENSIVE
INTENSIVE
NOTE: There are properties which may be neither extensive nor intensive.
SPECIFIC PROPERTIES (denoted by small letters)
= An extensive properties / mass
NOTE: Temperature (T), time (t) exceptions

26. PROPERTIES OF A SYSTEM Property: Any characteristic of a system.
Some familiar properties are pressure P, temperature T, volume V, and mass m.
Properties are considered to be either intensive or extensive.
Intensive properties: Those that are independent of the mass of a system, such as temperature, pressure, and density.
Extensive properties: Those whose values depend on the size—or extent—of the system.
Specific properties: Extensive properties per unit mass.

27. IMPORTANCE OF DIMENSIONS AND UNITS
Any physical quantity can be characterized by dimensions.
Some basic dimensions such as mass m, length L, time t, and temperature T are selected as primary or fundamental dimensions, while others such as velocity V, energy E, and volume V are expressed in terms of the primary dimensions and are called secondary dimensions, or derived dimensions.
Metric SI system: A simple and logical system based on a decimal relationship between the various units.
English system: It has no apparent systematic numerical base, and various units in this system are related to each other rather arbitrarily.

28. Some SI and English Units
Work = Force  Distance
1 J = 1 N∙m
1 cal = J
1 Btu = kJ
The SI unit prefixes are used in all branches of engineering.
The definition of the force units.

29. W weight
m mass
g gravitational acceleration
A body weighing 60 kgf on earth will weigh only 10 kgf on the moon.
The relative magnitudes of the force
units newton (N), kilogram-force
(kgf), and pound-force (lbf).
The weight of a unit mass at sea level.

30. Dimensional homogeneity
All equations must be dimensionally homogeneous.
To be dimensionally homogeneous, all the terms in an equation must have the same unit.
All non primary units (secondary units) can be formed by combinations of primary units.
Force units, for example, can be expressed as

31. STATE OF A SYSTEM T m p T =1 kg = 4 bar = 250
Point representing the state m p T
=1 kg
= 4 bar
= 250
Properties are known as Thermodynamic Co-ordinates. m p
Such a geometric space is known as Thermodynamic State Space

32. STATE OF A SYSTEM The Question arises:
Which Properties are required to define a state of a system?
How many?
Is it always possible to represent by a point?

33. STATE POSTULATE
We know from experience that we do not need to specify all the properties in order to fix a state (all of the properties are not independent of one another). Once a sufficient number of properties (the independent subset) are specified, the rest of the properties assume certain values automatically. That is, specifying a certain number of properties is sufficient to fix a state. The number of properties (independent intensive) required to fix the state of a system is given by the state postulate:
The state of a simple compressible system is completely specified by two independent, intensive properties.

34. STATE OF A SYSTEM YES / NO The Question arises:
Which Properties are required to define a state of a system?
How many?
Is it always possible to represent by a point?
YES / NO

35. STATE AND EQUILIBRIUM

36. STATE AND EQUILIBRIUM STATE = A state in EQUILIBRIUM
A SYSTEM AT TWO DIFFERENT STATES.
STATE
= A state in EQUILIBRIUM
= A point in state space
= All properties are uniquely defined.

37. STATE AND EQUILIBRIUM Thermodynamics deals with equilibrium states.
Equilibrium: A state of balance.
In an equilibrium state there are no unbalanced potentials (or driving forces) within the system.
Thermal equilibrium: If the temperature is the same throughout the entire system.
Mechanical equilibrium: If there is no change in pressure at any point of the system with time.
Chemical equilibrium: If the chemical composition of a system does not change with time, that is, no chemical reactions occur.
A system at two different states.
A closed system reaching thermal equilibrium.

38. What is the ‘way’ followed by the system?
CHANGE of STATE:
PROCESS
SYSTEM, INITIAL STATE, FINAL STATE i f i f
What is the ‘way’ followed by the system?

39. QUASI-STATIC PROCESS

40. CHANGE of STATE: PROCESS QUASI-STATIC PROCESS f f i i PATH followed by

41. QUASI-STATIC PROCESS ~ similar example

42. PROCESSES
Process: Any change that a system undergoes from one equilibrium state to another.
Path: The series of states through which a system passes during a process.
To describe a process completely, one should specify the initial and final states, as well as the path it follows, and the interactions with the surroundings.
Quasi-static or quasi-equilibrium process: When a process proceeds in such a manner that the system remains infinitesimally close to an equilibrium state at all times.

43. PROCESSES
Process diagrams plotted by employing thermodynamic properties as coordinates are very useful in visualizing the processes.
Some common properties that are used as coordinates are temperature T, pressure P, and volume V (or specific volume v).
The prefix iso- is often used to designate a process for which a particular property remains constant.
Isothermal process: A process during which the temperature T remains constant.
Isobaric process: A process during which the pressure P remains constant.
Isochoric (or isometric) process: A process during which the specific volume v remains constant.
The P-V diagram of a compression process.

44. CYCLIC PROCESS: initial state = final state
Cycle: A process during which the initial and final states are identical. i f f i
CYCLIC PROCESS: initial state = final state

45. CHANGE of PROPERTIES during a PROCESS:1
= Does not depend on the PATH 2 V
= True for any PATH
PROPERTIES: POINT FUNCTION

46. CHANGE of PROPERTIES during a PROCESS:
If ɸ is a Property... p i 2
= dɸ is an exact differential
Give example of dx and dA (=ydx) area 1 V
PROPERTIES: POINT FUNCTION

47. The Steady-Flow Process
The term steady implies no change with time. The opposite of steady is unsteady, or transient.
A large number of engineering devices operate for long periods of time under the same conditions, and they are classified as steady-flow devices.
Steady-flow process: A process during which a fluid flows through a control volume steadily.
Steady-flow conditions can be closely approximated by devices that are intended for continuous operation such as turbines, pumps, boilers, condensers, and heat exchangers or power plants or refrigeration systems.
During a steady-flow process, fluid properties within the control volume may change with position but not with time.
Under steady-flow conditions, the mass and energy contents of a control volume remain constant.

48. THANK YOU