This document provides an overview of basic thermodynamics concepts including: - Systems, boundaries, surroundings, and the types of thermodynamic systems such as closed, open, isolated, and rigid. - Thermodynamic states, processes, paths, and cycles along with examples of different processes. - The basic definitions of heat, work, internal energy, and enthalpy along with the sign conventions. - The zeroth law of thermodynamics regarding thermal equilibrium and temperature. - The first law of thermodynamics regarding the relationship between heat, work, and changes in internal energy for closed and open systems.

1. Engineering Thermodynamics
Module 1 - Basic Concepts and First law
Lecture 2 of 3 - Basic Concepts 2
Prepared by
Mr.M.Mani Vannan
Assistant Professor
Department of Mechanical Engineering
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2. Unit I - Basic Concepts and First Law
Basic concepts - concept of continuum, comparison of
microscopic and macroscopic approach. Path and point functions.
Intensive and extensive, total and specific quantities. System and
their types. Thermodynamic Equilibrium State, path and process.
Quasi-static, reversible and irreversible processes. Heat and work
transfer, definition and comparison, sign convention.
Displacement work and other modes of work .P-V diagram.
Zeroth law of thermodynamics – concept of temperature and
thermal equilibrium– relationship between temperature scales –
new temperature scales. First law of thermodynamics –
application to closed and open systems – steady and unsteady
flow processes
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3. Thermodynamic System, Boundary and
surrounding s
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.
BOUNDARY SURROUNDINGS
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SYSTEM

4. Types of Thermodynamic system
Closed system or control mass: Only energy
can cross the boundary, but no mass cross the
boundary of the system.
Examples: Pressure Cooker, A gas confined
in piston and cylinder.
Open system or control volume: Both mass
and energy can cross the boundary of a control
volume.
Examples: Air Compressor, Turbine,
Condenser, Nozzle, etc.
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5. Cont..
Isolated system: A closed system that does not communicate
with the surroundings by any means.
Examples:
Rigid system: A closed system that communicates with the
surroundings by heat only.
Adiabatic system: A closed or open system that does not
exchange energy with the surroundings by heat.
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6. Examples of open system
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7. Thermodynamic State, Process and Path
State: Condition of a system at a point
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.
Quasi-Static Process: A quasi-static
process is a thermodynamic process that
happens slowly enough for the system to
remain in internal equilibrium.
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8. Thermodynamic cycle
A thermodynamic cycle is a sequence of different
processes that begins and ends at the same thermodynamic state.
Some sample processes:
 Isothermal process: temperature is constant T = C
 Isobaric process: pressure is constant, P = C
 Isentropic process: entropy is constant, s = C
 Isochoric / isometric process: Volume is constant, v = C
 Adiabatic process: no heat transfer, Q = 0
 Throttling process: enthalpy is constant, h = C
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9. Examples of cycle
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10. Reversible and Irreversible Processes
Sl.No Reversible Processes Irreversible Processes
1. A reversible process is a
process that can be
reversed in order to obtain
the initial state of a system.
An irreversible process is a
thermodynamic process that
cannot be reversed on order
to obtain the initial state of
the system
2. Infinite change occur in the
system
Finite change occur in the
system
3. There is an equilibrium
between the initial state and
the final state of the system
There is no equilibrium
system.
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11. Cont…
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12. Heat (Q)
It is a form of energy which generally
flows from due to temperature difference in
a system. It is denoted by ‘Q’.
1 J = 1 N∙ m : 1 cal = 4.1868 J
1 Btu = 1.0551 kJ
Heat to work Thermal power plant
Work to heat Refrigeration
Heat transferred = Area under the T-s curve
Q > 0 - Heat added to system(+ ve)
Q < 0 - Heat removed from system (-ve)
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13. Work (W)
1.Displacement Work ,Wd = Force(F)  Distance(dx)
W = p.A.dx [Pressure, p= F/A]
W= ʃ p.dv
1 J = 1 N∙ m : 1 cal = 4.1868 J
1 Btu = 1.0551 kJ
Work done = Area under a p-V curve
W > 0 Work done by the system (+ve) or Expansion
W < 0 Work done on the system(-ve) or Compression
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14. Cont..
2.Flow work
WFlow=F.L=p.A.L=p.V (kJ)
WFlow= p.V (kJ/kg)
3.Electrical work, WEle = Vvolt.I
4.Shaft work, Wshaft = ʃ TTorque.dθ
Where, Vvolt = Voltage(V)
I = Current(Amps)
TTorque= Torque (N.m)
θ = Angle of twist(ᵒ)
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15. Internal Energy (ΔU)
Internal energy is the sum of the kinetic and potential
energies of the particles that form the system.
Internal energy is a form of energy measured on a
molecular scale. It can consist of different modes: translational
kinetic energy of individual molecules, rotational energy and
vibrational energies associated with molecules, and
intermolecular forces between molecules.
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16. Cont..
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17. Enthalpy (H)
A thermodynamic quantity equivalent to the total heat
content of a system.
Enthalpy or Total enthalpy H = U + (p.V) or H = m.h
h = u + (p.v) or Cp
. ΔT
Where , h = Specific Enthalpy(kJ)
u = Internal energy of the system(kJ)
p = pressure of the system(N/m2)
v = Specific Volume(m3/kg)
Cp= Specific heat capacity at constant pressure(kJ/kg.K)
ΔT= Change in temperaure(K)
m = Mass of the system(kg)
Specific enthalpy is an intensive property
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18. Zeroth law of Thermodynamics
If A is in thermal equilibrium with B, and B is in thermal
equilibrium with C, then C will be in thermal equilibrium with A.
In other words, all three systems have the same ‘temperature’.
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19. Equilibrium
A state of balance. In an equilibrium state there are no
unbalanced potentials (or driving forces) within the system.
Types of Equilibrium:
1.Thermal equilibrium
2.Mechanical equilibrium
3.Phase equilibrium
4.Chemical equilibrium
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20. Thermal and Mechanical equilibrium
Thermal Equilibrium: If there are no net
flow of thermal energy between them or If
the temperature is the same throughout the
entire system. Thermal equilibrium obeys the
Zeroth law of thermodynamics.
Mechanical Equilibrium: A thermodynamic
system is said to be in mechanical equilibrium
, when there are no unbalanced forces within a
system or with its surrounding. Pressure is
one such force.
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21. Phase and Chemical equilibrium
3.Phase equilibrium: For a water
system represents a point or a line on
the phase diagram (T-P) where two or
more phase of the given system will be
in thermodynamic equilibrium with
each other.
4.Chemical equilibrium: Chemical
equilibrium is the state in which both
reactants and products are present in
Concentrations which have no further
tendency to change with time.
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22. First Law of thermodynamics
The first law of thermodynamics is a version of the law of
conservation of energy, adapted for thermodynamic systems.
It states that “the net heat added(Q) to the system
will be equal to the sum of work done(W) by the
system and internal energy of the system(ΔU)
Q = W + ΔU
W > 0 - Work done by system(+ ve)
W < 0 - Work done on system (- ve)
Q > 0 - Heat added to system(+ ve)
Q < 0 - Heat removed from system (-ve)
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23. Thank you
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