Physical chemistry and thermodynamic

1. PHYSICAL CHEMISTRY
THERMODYNAMIC

3. CHEMISTRY
• A Branch of science which deals with the structure,
properties constituents and change which takes place is
known as chemistry.
• Origin of chemistry -: Chemes means black color.
Egyptian called black earth as “chemi ” and in early age
the study of chemical science was known as chemistry.
• Antoine Lavoisier (1743, 1794) is known as father of
Modern Chemistry

4. • Born: August 26, 1743, Paris, France
• Died: May 8, 1794, Paris, France

5. Antoine Lavoisier

6. WHAT IS PHYSICAL CHEMISTRY?
If we look around us, chemical reactions are taking place everywhere.
1. When we strike a match to light our grills, a chemical reaction occurs.
2. If we mix milk with baking powder in our favorite recipe, a reaction happens.
3. Why do some reactions create heat?
4. How is it that certain reactions proceed fast while others move very slow?
All of these questions and more can be solved within
the field of physical chemistry.

7. THE TERM "PHYSICAL CHEMISTRY" WAS COINED BY MIKHAIL LOMONOSOV IN 1752
PHYSICAL
CHEMISTRY

8. PHYSICAL
CHEMISTRY
• Physical Chemistry is the branch of chemistry
dealing with the principles and methodologies of
both chemistry and physics and is the study of
how chemical structure impacts physical
properties of a substance.

9. PHYSICAL CHEMISTRY
Physical chemistry gives us information that how light behaves like particle in
the form of Quantum. it also tells us that what sort of order of reaction a
molecule possess?
it shows that how ripening of fruits is takes place and what phenomenon is
going on and how photons are get converted into mass. how energy is
produced from different resources and can be used for benefits of human kind

10. PHYSICAL CHEMISTRY
• Physical Chemistry includes study of the physical properties of many different types of substances and on different scales
(levels of physical detail).
• That is, it includes study of the following scales of chemical properties of materials:
1. Macroscopic:
Macroscopic properties of substances describe how relatively large quantities of the substance behave as a group,
• Example; melting points and boiling points, thermal conductivity, specific heat capacity
• Microscopic:
Microscopic properties of substances concern details of their physical properties observable only using the magnification
provided by microscopes
• Example; the shapes and structures of crystals

11. PHYSICAL CHEMISTRY
• For example, a theory may attempt to explain why certain atoms in a molecule
behave a certain way. In addition to this primary purpose, physical chemistryoffers
many branches within the field that have their own unique purposes:
1. Electrochemistry is a branch of physical chemistry that asks how do atoms,
electrons, and ions mingle in an electrical current?
2. Photochemistry asks what happens when you use light in a chemical reaction?
3. Thermochemistry asks why did this chemical reaction produce heat?
4. Spectroscopy asks what happens to matter that emits radiation?

12. WHAT IS
PHYSICAL
CHEMISTRY?
– Physical chemistry is the study of the underlying physical principles
that govern the properties and behavior of chemical systems.
• What is Chemical Systems?
– A chemical system can be studied from either a microscopic or a
macroscopic viewpoint.
The microscopic viewpoint is based on the
concept of molecules.
The macroscopic viewpoint studies large-scale
properties of matter without explicit use of the
molecule concept.
Chemical
Systems

13. Physical
Chemistry
Analytical
Chemistry
Biochemistry
Chemistry
Organic
Chemistry
Inorganic
chemistry

14. Thermodynamics
4 BRANCHES
OF PHYSICAL
CHEMISTRY
Quantum
Chemistry
Statistical
Mechanics
Kinetics
Thermodynamics is a
macroscopic
science that studies the
interrelationships of the
various equilibrium
properties
of a system and the
changes in equilibrium
properties in processes.
Molecules and the
electrons and nuclei
that compose them do
not obey classical
mechanics. Instead,
their motions are
governed by the laws of
quantummechanics.
Application of quantum
mechanics to atomic
structure, molecular
bonding,
and spectroscopygives
us quantumchemistry.
The molecular and
macroscopic levels are
related to each other by
the branch of science
called statistical
mechanics. Statistical
mechanics gives insight
into why the laws of
thermodynamics hold
and allows calculation
of macroscopic
thermodynamic
properties from
molecular properties.
Kinetics is the study of
rate processes such as
chemical reactions,
diffusion,and
the flow of charge in an
electrochemical cell.
Kinetics uses relevant
portions of
thermodynamics,
quantum chemistry,
and statistical
mechanics.

15. Electrochemistry (study
of the interaction of
atoms, molecules, ions
and electric current)
Photochemistry (study
of the chemical effects
of light;
photochemical
reactions)
Surface chemistry
(study of chemical
reactions at
interfaces)
Chemical Kinetics
(study of rates of
chemical reactions)
Thermodynamics/Ther
mochemistry (study of
how heat relates to
chemical change)
Quantum
Mechanics/Quantum
Chemistry (study of
quantum mechanics
and how it relates to
chemical phenomena)
Spectroscopy (study
of spectra of light or
radiation)

16. THERMODYNAMICS/THERMOCHEMISTRY
(study of how heat relates to chemical change)
• The word ‘thermodynamics’ comes from the two Greek words
 ‘dynamic’ comes from the Greek word dunamikos, which means movement
 thermo means energy or temperature i.e. ‘thermometer’,
• Thermodynamics is the scientific study of work, heat, and the related
properties of chemical and mechanical systems.

17. Laws of Thermodynamics:
0th, 1st, 2nd, 3rd
dynamics – changes
(motion)
thermo – heat

18. Open system Closed system
Isolated system
Example:

19. THERMODYNAMIC SYSTEM
An important concept in thermodynamics is the thermodynamic system. A thermodynamic
system is one that interacts and exchanges energy with the area around it (transformation
of energy). A system could be as simple as a block of metal or as complex as a compartment
fire. Outside the system are its surroundings. The system and its surroundings comprise the
universe.
Systems:
A region of the universe that we direct our attention to.
Surroundings:
Everything outside a system is called surroundings.
Boundary:
The boundary or wall separates a system from its
surroundings.
UNIVERSE

20. UNIVERSE
 System – part of world have special
interest/quantity of matter
 Surroundings – where we make our
observations/Everything other than
system
 Boundary ---- imaginary or physical
thing that separate system and
surrounding

22. ENERGY TRANSFER IS STUDIED IN THREE TYPES
OF SYSTEMS:
Opensystems
Open systems can exchange both matter and energy with an outside system. They are portions of larger
systems and in intimate contact with the larger system. Your body is an open system.
Closedsystems
Closed systems exchange energy but not matter with an outside system. Though they are typically
portions of larger systems, they are not in complete contact. The Earth is essentially a closed system; it
obtains lots of energy from the Sun but the exchange of matter with the outside is almost zero.
Isolatedsystems
Isolated systems can exchange neither energy nor matter with an outside system. While they may be
portions of larger systems, they do not communicate with the outside in any way. The physical universe
is an isolated system; a closed thermos bottle is essentially an isolated system (though its insulation is
not perfect).
Heat can be transferred between open systems and between closed systems, but not between
isolated systems.

23. EXAMPLE

24. 4 LAW OF
THERMODYNAMIC
• There are 4 laws to thermodynamics, and they
are some of the most important laws in all of
physics. The laws are as follows

25. THE ZEROTH
LAW
Two systems that are each found to be
in thermal equilibrium with a third
system will be found to be in thermal
equilibrium with each other.
It is so called because only after the first,
second, and third laws of thermodynamics had
been formulated was it realized that the zeroth
law is needed for the development of
thermodynamics.
Moreover, a statement of the zeroth law
logically precedes the other three.The
zeroth law allows us to assert the existenceof
temperature as a state function.

26. ZEROTH LAW OF
THERMODYNAMICS
• The Zeroth law is so named as it came after the other 3. Laws
1, 2, and 3 had been around for a while before the
importance of this law had been fully understood. It turned
out that this law was so important and fundamental that it
had to go before the other 3, and instead of renaming the
already well known 3 laws they called the new one the Zeroth
law and stuck it at the front of the list.
• Zeroth law :- it gives you information about mass / energy.
• If assume water bucket in which you put cup of tea … so if
water is in thermal equilibrium with tea. And tea is in thermal
equilibrium with surrounding then you have to say water is in
equilibrium with surrounding . That is what zeroth law is
• Basically, if A=B and C=B then A=C. This may seem so
obvious that is doesn’t need stating but without this law we
couldn’t define temperature and we couldn’t build
thermometers.

27. FIRST LAW OF THERMODYNAMICS
• Energy can neither be created nor destroyed. It can only change forms. In any process, the total energy of the
universe remains the same. For a thermodynamic cycle the net heat supplied to the system equals the net work
done by the system.
• The first law of thermodynamics basically states that energy is conserved; it can neither be created nor
destroyed, just changed from one for to another,
• “The total amount of energy in an isolated system is conserved.”
• it's simply says that energy is conserved. You neither create energy nor destroy energy.
• The energy in a system can be converted to heat or work or other things, but you always have the same total
that you started with.
• As an analogy, think of energy as indestructible blocks. If you have 30 blocks, then whatever you do to or with
the blocks you will always have 30 of them at the end. You can't destroy them, only move them around or divide
them up, but there will always be 30. Sometimes you may lose one or more, but they still have to be taken
account of because Energy is Conserved.

28. SECOND LAW OF THERMODYNAMICS
• The entropy of an isolated system not in equilibrium will tend to increase over time,
approaching a maximum value at equilibrium.
• There are no such device which develop 100% work. Nothing is in world which convert
energy one form to another form with no such losses. There has to be some losses. And
that's why , no one is 100% efficient
• This is possibly the most famous (among scientists at least) and important laws of all science.
It states;
• “The entropy of the universe tends to a maximum.”
• In other words Entropy either stays the same or gets bigger, the entropy of the universe can
never go down.

29. ENTROPY AND ENTHALPY
• Both entropy and enthalpy are thermodynamically properties of a system.
Entropy is a measure of disorder or randomness of a system. An ordered
system has low entropy. A disordered system has high entropy.
• Enthalpy is defined as the sum of internal energy of a system and the product
of the pressure and volume of the system. The change in enthalpy is the sum
of the change in the internal energy and the work done.
• Enthalpy has the units of heat, joules.
• Entropy has the units of heat divided by temperature, joules per kelvin.

30. THE THIRD LAW
• The third law provides an absolute reference point for measuring entropy,
saying that
• “As the temperature of a system approaches absolute zero (−273.15°C, 0 K),
then the value of the entropy approaches a minimum.”
• The value of the entropy is usually 0 at 0K, however there are some cases
where there is still a small amount of residual entropy in the system.
• Third law :- there are no such device which has zero entropy

31. SUMMARY OF THE LAWS OF THERMODYNAMICS
• 0. This is the Game: you’re here, you are part of the system
• 1. You Can’t Win: you can’t get more energy out of the system than you put
into it.
• 2. You Can’t Break Even: any transfer of energy will result in some waste of
energy unless a temperature of absolute zero can be achieved.
• 3. You Can’t Get Out of the Game: you cannot achieve absolute zero.
• Stated simply: There’s no such thing as a free lunch.

32. • Video Link
• https://youtu.be/-x2TomNak6o

33. REFERENCES
• https://en.wikipedia.org/wiki/Antoine_Lavoisier
• http://www.vidyagyaan.com/general-knowledge/science/basic-chemistry-element-terms-and-definitions/
• https://images.app.goo.gl/XrGqyrjf2KR9MwA59
• https://study.com/academy/lesson/what-is-physical-chemistry-definition-examples.html
• https://en.wikipedia.org/wiki/Physical_chemistry
• https://www.britannica.com/science/physical-chemistry
• http://www.chemistryexplained.com/Ny-Pi/Physical-Chemistry.html#ixzz5lOA2FueI
• https://www.ivyroses.com/Chemistry/What-is-Physical-Chemistry.php
• https://study.com/academy/lesson/what-is-physical-chemistry-definition-examples.html
• http://www.chemistry2011.org/branchesofchemistry
• https://astro.ins.urfu.ru/sites/default/files/upload_files/temp/1/%5BPaul_M._S._Monk%5D_Physical_Chemistry_Understandin(BookSee.org).pdf (page 40)
• https://www.thoughtco.com/thermodynamics-definition-602127