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BIOLOGICAL
THERMODYNAMICS
Presented by
Dr. B. Victor., Ph. D
Email : bonfiliusvictor@gmail.com
Blog: bonvictor.blogspot.com
Presentation outline











Introduction
What is thermodynamics? Definition.
Energy and biological energy needs.
Classes of thermodynamic systems.
Law of conservation of energy-key concepts and
explanation.
Law of degradation of energy – key concepts and
explanation.
Concepts of free energy, entropy and enthalpy.
Summary.
Introduction










All organisms require energy to stay alive.
Organisms are energy transformers.
Organisms take in energy and transduce it to
new forms.
All chemical reactions in cells involve energy
transformations.
For example green plants transform radiant
energy into chemical energy.
Humans are „energy parasites‟.


.

Thermodynamics
• Thermodynamics is simply
the study of energy.
• The science deals with
energy in its various forms
and the conversion of one
form of energy into another
What is thermodynamics?






Thermodynamics is the study of energy
transformations that occur in a collection of
matter.
Thermodynamics is concerned with the
storage, transformation and dissipation of
energy.
Cells store energy, they transform it and they
dissipate to drive unfavorable reactions.
Objectives of thermodynamics


All chemical, physical and biological processes
are ultimately enabled and regulated by the
laws of thermodynamics.
 1.to

understand the relationship between quantities of
heat and work in biological systems.
 2.to understand the influence of energy changes in
biological phenomena.
 3. to predict the effect of temperature on a variety of
physico-chemical and biological phenomena in
systems at equilibrium. e.g. bioreactors.
 4.to understand the biochemical processes.
Biological perspective of
thermodynamics principles


In living cells, thermodynamic changes are
essential for biological functions such as
growth, reproduction photosynthesis and
respiration.
Chemical : photosynthesis.
 Chemical Chemical : cellular respiration.
 Chemical Electrical : Nervous system.
 Chemical Mechanical : Muscles.
 Light
Cells need energy to do all their
work

Biological energy needs
To generate
and maintain
its structure

To generate
To generate concentration
all kinds of and electrical
gradients
movements
across cell
membranes

To maintain To generate
body
Light in some
temperature
animals
Bioenergetics




Bioenergetics is the quantitative study of
energy transductions in living cells.
The „energy industry‟ (production, storage and
use of energy) is central to the economy of the
cell society.
Definition of energy





Energy is defined as the ability to do work.
Organisms take in energy and transduce it to
new forms.
The flow of energy maintains order and life.
Basic types of energy

•Energy in
motion
•Stored
energy
Basic forms of energy
Forms of energy
Energy

Kinetic
energy

Potential
energy

Energy in
motion

Stored
energy

Light, heat, electric
power

Dam, battery
Wood, fossil fuels
Animals are open thermodynamic
systems






The matter flowing into the living system
contains a high energy potential.
The matter flowing out of the system is at a
low energy potential.
The energy changes that occur between these
two mass flow events are used to perform
chemical and physical work processes.
Biological
energy
transformation
s

Energy can be
changed from one form
to another
Plants = Photosynthesis = Starch
• Light energy  Chemical energy

Nerve = Neurotransmission = impulse
• Chemical energy Electrical energy

Eye = Vision = image
• Light energy  Electrical energy

Muscle = movement=power
Chemical energy  Mechanical energy
What is a system?




An assemblage of matter, which can interact
with energy is called a system.
A system is separated from its surroundings by
a boundary. E.g. an organism, a fermenter or a
test tube.

Syste
m

Surrounding
s

Boundary
Classes of thermodynamic
systems


Based on the differentiation between flows of
energy and flow of matter across the system
boundary, thermodynamics distinguishes 3
types of systems:
 1.An

open system exchanges matter and energy
with its environment.
 2.A closed system exchanges only energy with its
environment.
 3.An isolated system exchanges neither matter
nor energy with its environment.
An isolated system




An isolated system has boundary which is
impermeable to both matter and all forms of
energy.
It exchanges neither heat nor matter with its
surroundings.

An isolated system

System boundary
Closed system








A closed system may accept heat from the
surroundings but there is no transfer of matter
between the system and its environment. E.g.
universe.
When heat flows out of the system, the energy
of the system decreases.
When heat flows in, the energy of the system
increases.
If the heat remains constant, it may be called
an isothermal system. e.g. bomb calorimeter.
Open system






An open system is one which can exchange
both energy and matter with its surroundings.
Biological systems are open. E.g. living cells,
living things.
Earth is an open system.

Matter exchange

Open system

Energy exchange
The first law of thermodynamics






Law of conservation of
energy – this law was put
forward by Robert Mayer in
1941.
The first law states that “
the total energy of a
system plus its
environment remains
constant”.
This law declares that “
energy is neither created
nor destroyed in the
universe and it allows to be
exchanged between a
system and its
surroundings”.
Key concepts of first law








The sum of the energy before the conversion
is equal to the sum of the energy after
conversion.
The total quantity of energy in the universe
remains constant.
The energy conversion is never 100% efficient.
Ecological efficiencies vary from 1% to 56%
depending on organisms.
Some energy is wasted in increasing the
disorder or entropy.
Explanation of the first law






Light is a form of energy. It can be transformed
in to work, heat or potential energy of
food, depending on the situation, but none of it
is destroyed.
Plants convert light energy from the sun into
high energy compounds that help to build cell
material.
When animals eat plants, their stomach and
intestines break down the compounds for
further use.
Free energy (∆G) concept








Free energy refers to the amount of energy
available during a chemical reaction to do cellular
work.
The free energy concept was developed by
Willard Gibbs in 1870s.
The Gibbs free energy is a thermodynamic
quantity which can be used to determine, if a
reaction is spontaneous or not.
Gibbs free energy equation = ∆G=∆H -T∆S


Where ∆G=Gibbs free energy in KJ
∆H=enthalpy change
T = temperature in Kelvin K =273+oC
∆S=entropy change (in KJ K -1)
Gibbs free energy











The driving force of a chemical as two
components
∆H is the drive toward stability (enthalpy)
∆ S is the drive toward disorder (entropy)
∆ G is the net driving force of a chemical
reaction.
∆ G values depend upon temperature,
pressure and the concentration of the
reactants and products.
If ∆ G<0 = the reaction is spontaneous.
If ∆ G>0 = the reaction is non-spontaneous.
Significance of ∆G







The sign ∆G is a predictive element.
- ∆G  reaction favorable
(exergonic, spontaneous)
+ ∆G  reaction not
favorable(endergonic, non-spontaneous).
∆G =0 reaction at equilibrium (no change).
Second law of thermodynamics






Also called law of the
degradation of energy
or law of entropy.
This law was
developed in 1850s
by German Physicist
Rudolf Clausius.
This law states that “a
system and its
surroundings always
proceed to a state of
maximum disorder or
maximum entropy”.
Explanation of second law






Living systems are ordered, while the natural
tendency of the universe is to move toward
systems of disorder with unavailable energy.
The second law is an important indicator of the
direction of the reaction.
All reactions proceed in a direction with
increase in entropy and decrease in free
energy.
Concept of entropy (∆ S)








The word entropy (from the Greek entrope =
change ) is a measure of the unavailable energy
resulting from transformations
The term is used as a general index of the
molecular disorder associated with energy
degradation.
Second law implies that the entropy of the
universe is increasing because energy
conversions are not 100% efficient. i.e. some heat
is always released.
Second law also implies that if a particular system
becomes more ordered, its surroundings become
more disordered.
Concept of entropy (∆ S) -2











Entropy =unavailable energy or molecular
disorder.
Entropy is the capacity factor for thermal energy.
It is a function of state.
It is a function of the degree of disorder in the
system.
„Entropy tends to increase‟ = a change to a more
disordered state at a molecular level.
„no process is 100% efficient‟
High S value = high degree of disorder in a
system.
Concept of enthalpy (∆H)




Enthalpy is defined as a change in heat
content or heat of formation of a system.
The change in enthalpy is given by ∆H= ∆U +P
∆V
 Where







∆U= internal energy change
P=pressure
V=volume
∆U= the change in internal energy of a system is
equal to the heat added to the system minus the work
done by the system.
∆U=Q - W
Where Q= heat added to the system
 W=work done by the system
Two types of biochemical
reactions
Exergonic reaction (catabolic
reactions)

Endergonic reaction (Anabolic
reactions)

∆G is negative

∆G is positive

∆H is less than zero

∆H is greater than zero

Increase in stability

Decrease in stability

Spontaneous

Non-spontaneous

Movement towards equilibrium

Movement away from equilibrium

Coupled to ATP formation

Coupled to ATP utilization

Catabolism

Anabolism
Summary










Thermodynamic laws describe the flows and
interchanges of heat, energy and matter.
Almost all chemical and biochemical
processes are as a result of transformation of
energy.
Laws can provide important insights into
metabolism and bioenergetics.
The energy exchanges between the system
and the surroundings balance each other.
There is a hierarchy of energetics among
organisms:
About the presenter










Dr. B.Victor is a highly experienced postgraduate
professor, recently retired from the reputed educational
institution - St. Xavier‟ s
College(Autonomous), Palayamkottai, India-627001.
He was the dean of sciences and assistant controller of
examinations.
He has more than 32 years of teaching and research
experience
He has taught a diversity of courses and published 45
research articles in reputed national and international
journals.
Send your comments to : bonfiliusvictor@gmail.com
Biological thermodynamics

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Biological thermodynamics

  • 1. BIOLOGICAL THERMODYNAMICS Presented by Dr. B. Victor., Ph. D Email : bonfiliusvictor@gmail.com Blog: bonvictor.blogspot.com
  • 2. Presentation outline         Introduction What is thermodynamics? Definition. Energy and biological energy needs. Classes of thermodynamic systems. Law of conservation of energy-key concepts and explanation. Law of degradation of energy – key concepts and explanation. Concepts of free energy, entropy and enthalpy. Summary.
  • 3. Introduction       All organisms require energy to stay alive. Organisms are energy transformers. Organisms take in energy and transduce it to new forms. All chemical reactions in cells involve energy transformations. For example green plants transform radiant energy into chemical energy. Humans are „energy parasites‟.
  • 4.  . Thermodynamics • Thermodynamics is simply the study of energy. • The science deals with energy in its various forms and the conversion of one form of energy into another
  • 5. What is thermodynamics?    Thermodynamics is the study of energy transformations that occur in a collection of matter. Thermodynamics is concerned with the storage, transformation and dissipation of energy. Cells store energy, they transform it and they dissipate to drive unfavorable reactions.
  • 6. Objectives of thermodynamics  All chemical, physical and biological processes are ultimately enabled and regulated by the laws of thermodynamics.  1.to understand the relationship between quantities of heat and work in biological systems.  2.to understand the influence of energy changes in biological phenomena.  3. to predict the effect of temperature on a variety of physico-chemical and biological phenomena in systems at equilibrium. e.g. bioreactors.  4.to understand the biochemical processes.
  • 7. Biological perspective of thermodynamics principles  In living cells, thermodynamic changes are essential for biological functions such as growth, reproduction photosynthesis and respiration. Chemical : photosynthesis.  Chemical Chemical : cellular respiration.  Chemical Electrical : Nervous system.  Chemical Mechanical : Muscles.  Light
  • 8. Cells need energy to do all their work Biological energy needs To generate and maintain its structure To generate To generate concentration all kinds of and electrical gradients movements across cell membranes To maintain To generate body Light in some temperature animals
  • 9. Bioenergetics   Bioenergetics is the quantitative study of energy transductions in living cells. The „energy industry‟ (production, storage and use of energy) is central to the economy of the cell society.
  • 10. Definition of energy    Energy is defined as the ability to do work. Organisms take in energy and transduce it to new forms. The flow of energy maintains order and life.
  • 11. Basic types of energy •Energy in motion •Stored energy
  • 12. Basic forms of energy
  • 13. Forms of energy Energy Kinetic energy Potential energy Energy in motion Stored energy Light, heat, electric power Dam, battery Wood, fossil fuels
  • 14. Animals are open thermodynamic systems    The matter flowing into the living system contains a high energy potential. The matter flowing out of the system is at a low energy potential. The energy changes that occur between these two mass flow events are used to perform chemical and physical work processes.
  • 15. Biological energy transformation s Energy can be changed from one form to another Plants = Photosynthesis = Starch • Light energy  Chemical energy Nerve = Neurotransmission = impulse • Chemical energy Electrical energy Eye = Vision = image • Light energy  Electrical energy Muscle = movement=power Chemical energy  Mechanical energy
  • 16. What is a system?   An assemblage of matter, which can interact with energy is called a system. A system is separated from its surroundings by a boundary. E.g. an organism, a fermenter or a test tube. Syste m Surrounding s Boundary
  • 17. Classes of thermodynamic systems  Based on the differentiation between flows of energy and flow of matter across the system boundary, thermodynamics distinguishes 3 types of systems:  1.An open system exchanges matter and energy with its environment.  2.A closed system exchanges only energy with its environment.  3.An isolated system exchanges neither matter nor energy with its environment.
  • 18. An isolated system   An isolated system has boundary which is impermeable to both matter and all forms of energy. It exchanges neither heat nor matter with its surroundings. An isolated system System boundary
  • 19. Closed system     A closed system may accept heat from the surroundings but there is no transfer of matter between the system and its environment. E.g. universe. When heat flows out of the system, the energy of the system decreases. When heat flows in, the energy of the system increases. If the heat remains constant, it may be called an isothermal system. e.g. bomb calorimeter.
  • 20. Open system    An open system is one which can exchange both energy and matter with its surroundings. Biological systems are open. E.g. living cells, living things. Earth is an open system. Matter exchange Open system Energy exchange
  • 21. The first law of thermodynamics    Law of conservation of energy – this law was put forward by Robert Mayer in 1941. The first law states that “ the total energy of a system plus its environment remains constant”. This law declares that “ energy is neither created nor destroyed in the universe and it allows to be exchanged between a system and its surroundings”.
  • 22. Key concepts of first law     The sum of the energy before the conversion is equal to the sum of the energy after conversion. The total quantity of energy in the universe remains constant. The energy conversion is never 100% efficient. Ecological efficiencies vary from 1% to 56% depending on organisms. Some energy is wasted in increasing the disorder or entropy.
  • 23. Explanation of the first law    Light is a form of energy. It can be transformed in to work, heat or potential energy of food, depending on the situation, but none of it is destroyed. Plants convert light energy from the sun into high energy compounds that help to build cell material. When animals eat plants, their stomach and intestines break down the compounds for further use.
  • 24. Free energy (∆G) concept     Free energy refers to the amount of energy available during a chemical reaction to do cellular work. The free energy concept was developed by Willard Gibbs in 1870s. The Gibbs free energy is a thermodynamic quantity which can be used to determine, if a reaction is spontaneous or not. Gibbs free energy equation = ∆G=∆H -T∆S  Where ∆G=Gibbs free energy in KJ ∆H=enthalpy change T = temperature in Kelvin K =273+oC ∆S=entropy change (in KJ K -1)
  • 25. Gibbs free energy        The driving force of a chemical as two components ∆H is the drive toward stability (enthalpy) ∆ S is the drive toward disorder (entropy) ∆ G is the net driving force of a chemical reaction. ∆ G values depend upon temperature, pressure and the concentration of the reactants and products. If ∆ G<0 = the reaction is spontaneous. If ∆ G>0 = the reaction is non-spontaneous.
  • 26. Significance of ∆G     The sign ∆G is a predictive element. - ∆G  reaction favorable (exergonic, spontaneous) + ∆G  reaction not favorable(endergonic, non-spontaneous). ∆G =0 reaction at equilibrium (no change).
  • 27. Second law of thermodynamics    Also called law of the degradation of energy or law of entropy. This law was developed in 1850s by German Physicist Rudolf Clausius. This law states that “a system and its surroundings always proceed to a state of maximum disorder or maximum entropy”.
  • 28. Explanation of second law    Living systems are ordered, while the natural tendency of the universe is to move toward systems of disorder with unavailable energy. The second law is an important indicator of the direction of the reaction. All reactions proceed in a direction with increase in entropy and decrease in free energy.
  • 29. Concept of entropy (∆ S)     The word entropy (from the Greek entrope = change ) is a measure of the unavailable energy resulting from transformations The term is used as a general index of the molecular disorder associated with energy degradation. Second law implies that the entropy of the universe is increasing because energy conversions are not 100% efficient. i.e. some heat is always released. Second law also implies that if a particular system becomes more ordered, its surroundings become more disordered.
  • 30. Concept of entropy (∆ S) -2        Entropy =unavailable energy or molecular disorder. Entropy is the capacity factor for thermal energy. It is a function of state. It is a function of the degree of disorder in the system. „Entropy tends to increase‟ = a change to a more disordered state at a molecular level. „no process is 100% efficient‟ High S value = high degree of disorder in a system.
  • 31. Concept of enthalpy (∆H)   Enthalpy is defined as a change in heat content or heat of formation of a system. The change in enthalpy is given by ∆H= ∆U +P ∆V  Where      ∆U= internal energy change P=pressure V=volume ∆U= the change in internal energy of a system is equal to the heat added to the system minus the work done by the system. ∆U=Q - W Where Q= heat added to the system  W=work done by the system
  • 32. Two types of biochemical reactions Exergonic reaction (catabolic reactions) Endergonic reaction (Anabolic reactions) ∆G is negative ∆G is positive ∆H is less than zero ∆H is greater than zero Increase in stability Decrease in stability Spontaneous Non-spontaneous Movement towards equilibrium Movement away from equilibrium Coupled to ATP formation Coupled to ATP utilization Catabolism Anabolism
  • 33. Summary      Thermodynamic laws describe the flows and interchanges of heat, energy and matter. Almost all chemical and biochemical processes are as a result of transformation of energy. Laws can provide important insights into metabolism and bioenergetics. The energy exchanges between the system and the surroundings balance each other. There is a hierarchy of energetics among organisms:
  • 34. About the presenter      Dr. B.Victor is a highly experienced postgraduate professor, recently retired from the reputed educational institution - St. Xavier‟ s College(Autonomous), Palayamkottai, India-627001. He was the dean of sciences and assistant controller of examinations. He has more than 32 years of teaching and research experience He has taught a diversity of courses and published 45 research articles in reputed national and international journals. Send your comments to : bonfiliusvictor@gmail.com