The document is a presentation on thermodynamics, covering essential concepts such as open, closed, and isolated systems, as well as key thermodynamic processes and laws. It explains the first law of thermodynamics, the classification of processes, and introduces concepts like spontaneous and non-spontaneous processes, entropy, and the Carnot cycle. The presentation concludes with the significance of these principles in understanding energy transfer and state changes within thermodynamic systems.

1. PRESENTATION ON THERMODYNAMICS
PRESENTED TO
NARGIS ARA
ASSOCIATE PROFESSOR
DEPARTMENT OF PHARMACY
UNIVERSITY OF DEVELOPMENT ALTERNATIVE

2. Group Members
Name ID
1. Farzana Akter Jami 032182014
2. Srijita Dafadar 032182010
3. Mst Rammi Khatun 032182012
4. Shamima Nasrin Bithi 032182011
5. Rakibul Hasan 032182015

3. INTRODUCTORY
 The word thermodynamics was
coined in 1840 from Greek word
therme meaning heat and dynamis
meaning power.
 It is the science of the relationship
between heat, work, temperature and
energy.
 It deals with the transfer of energy
from one place to another and from
one form to another.

4. BASIC CONCEPTS AND
THERMODYNAMIC TERMS
 System – Part of the universe which is
under thermodynamic study i.e. to
study the effect of temperature,
pressure etc.
 Boundary – Which separates the
system and the surroundings.
 Surroundings - Everything that
external to the system.
Universe = System + Surroundings

5. THERMODYNAMIC TERMS
Types of system
1. Open System:
Here mass and energy both can be exchanged with
surroundings.
Example: Hot tea in open cup.
2. Closed System:
There is only exchange of energy with
surroundings, no exchange of mass takes place.
Example: Hot tea placed in a closed tea pot.
3. Isolated System:
There is neither exchange of energy nor mass with
surroundings.
Example: Tea placed in a thermo flask.

6. CLASSIFICATION OF SYSTEM ON THE BASIS OF
NATURE OF CONSTITUENTS
Homogenous system:
All the constituents are present in the same
phase and composition of system is uniform
throughout.
Example: Sea water. Sea water is nothing but
water. However it is composed of many
minerals which we can’t see.
Heterogeneous system:
It contains two or more phases and the
composition is uniform throughout.
Example: Water with ice floating in it.

7. INTENSIVE AND EXTENSIVE
PROPERTIES
Intensive Properties:
Do not depend on the size of
the system or quantity of
matter present in it. Depend on
the nature of substance present
in it.
Extensive Properties:
Depend on the quantity of
matter present in the system.

8. PROCESS
When state of system changes then process is
said to occur. The first and last state of process
are called initial and final state respectively.
There are certain processes in which particular
state variable is kept constant.
Isothermal Processes:
Temperature of the system remains constant.
Heat can flow from system to surrounding
and vice versa to keep the temp. constant.
Here dT= 0.
Adiabatic Processes:
Does not exchange heat with the
surroundings
Here dq= 0.

9. TYPES OF PROSSESES
Isobaric Processes:
Where the pressure stays constant.
Here dP= 0.
Isochoric Processes:
Volume of the system remains constant.
Here dV= 0.
Cyclic Processes:
Here the system undergoes series of changes
and finally returns to it’s initial state. Internal
energy will be 0.
Here dE= 0, dV= 0.

10. 1st LAW OF THERMODYNAMICS
Law of Conservation of Energy
 Energy can neither be created nor destroyed although it may
be converted from one form to other.
 The total energy of an isolated system remains constant though
it may change from one form to another.
 The internal energy of a system changes due to heat and work:
∆E = q – W
 Another illustration of the law, the net energy of a closed
system = (heat transfer to the system – work done by the
system)
 The mathematical statement of the First law :
∆E = q - P×∆V

11. SOME SPECIAL FORMS OF 1ST LAW OF
THERMODYNAMICS
1. For a Cyclic process,
∆E = 0, q = w
2. For an adiabatic process,
dq = 0, ∆E = - w
3. For an Isochoric Process,
dV = 0, ∆E = q
4. For an Isobaric Process,
dP = 0, ∆E = q

12. SPONTANEOUS PROCESS AND NON
SPONTANEOUS PROCESS
Spontaneous Process:
The process which can take place by itself or initiation.
Example: 1. Evaporation of water in open vessel,
2. Dissolution of Salt in water,
3. Flow of water down a hill.
Non Spontaneous Process:
The process which can not take place itself.
Example: 1. Dissolution of sand in water,
2. Flow of water up the hill.
Spontaneity: The quality or state of being spontaneous.

13. REVERSIBLE AND IRREVERSIBLE PROCESS
Reversible Process:
A process that can be reversed in order to
obtain the initial state of a system. Infinite
changes occur in this system. There is
equilibrium between the initial and final state
of the system.
Irreversible Process:
A thermodynamic process that can not be
reversed in order to obtain the initial state of
the system. Finite changes occur.

14. ENTROPY
 Entropy is a thermodynamic state
quantity that is measure of the
randomness or disorder of the
molecules of the system.
 The symbol of Entropy is S.
 It is a state function: its path
independent
S Final −Sinitial = ∆S
∆S=
𝑞
𝑇

15. 2nd LAW OF THERMODYNAMICS
 Whenever a spontaneous process takes place, it is accompanied by
an increase in the total energy of the universe(system+surrounding).
 Another form – All natural or spontaneous process are
thermonamically irreversible in character.
3rd LAW OF THERMODYNAMICS
At absolute zero the entropy of a pure crystal is also zero.

16. CARNOT CYCLE
The cycle process which occurred
under reversible conditions is
referred to as the Carnot Cycle.
 (1-2) Reversible Isothermal
Expansion (Heat Addition)
 (2-3) Reversible Adiabatic
Expansion
 (3-4) Reversible Isothermal
Compression (Heat Rejection)
 (4-5) Reversible Adiabatic
Compression

17. THANK YOU FOR BEING WITH US