thermodynamics. in physical world outside and inside the living body. important factor for heat and energy for the living. different forms of energy, kinetic energy and pottential energy. different forms of system, open and closed. laws of thermodynamics and gibbs free energy. entrophy and enthalphy

1. Thermodynamics..
Shlok Pushpesh Mathur
Nayan Biswas

2. Introduction ..
 All organisms require energy to stay alive
 Orgamisms are energy transformer
 Organisms take energy and transduce it to new forms
 All chemicals reaction in cells involve energy transformations
 For example green plants transform radient energy into chemical energy.

3. Forms of energy ..
Energy
Kinetic energy
Energy in motion
Light, heat, electric power
Potential energy
Stored energy
Dam, battery wood, fossil
fuels

4. Kinnetic energy..
It is the energy of motion
observable as a movement of a
partial, or set of particles.

5. Potential Energy..
Is the Energy by virtual of
an objects position
related to other object .

6. What is system ?
 An assemblage of matter, which can interact with energy is called a system
 A system is separated from its surroundings by a boundary.
1. An open system
2. A closed system
3. An isolated system

7. Open System..
 An open system exchanges matter and energy
with its environment
 Biological system are open E.g. living cells,
living things
 Earth is an open system.

8. Closed system..
 A closed system exchanges only energy with
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 isotheral system.

9. Isolated system..
 An isolated system exchanges neither matter or
nor energy with its environment
 An isolated system has boundary which is
impermeable to both and all forms of energy.

10. The First Law of Thermodynaics..
 Law of conservation of energy – Robert Mayer
 “The first law states that the total energy of 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.”

11. Gibbs Free Energy..
 The driving forces 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.
 V 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.
 If ∆ G=0= the reaction is at equilibrium
Joseph Willard Gibbs

12. 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”.

13. Concept of entropy (∆S)..
 The word entropy (from 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.

14. The Third law of thermodynamics ..
 The entropy of a system approaches a
constant value as the temperature
approaches absolute zero.
 At zero temperature the system must be in a
state with the minimum thermal energy. This
statement holds true if the perfect crystal has
only one state with minimum energy energy.

15. Concept of enthalpy (∆h) ..
 Enthalpy is defined as a change in heat content or heat or 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 system
W= work done by the system

16. Two types of biochemical reactions..
Exergonic reactions (catabolic)
 ΔG is negative
 ΔH is less than zero
 Increase in stability
 Spontaneous movement towards equilibrium
 Coupled to ATP formation
 catabolism
Enderogenic reaction (anabolic)
 ΔG is Positive
 ΔH is greater than zero
 Decrease in stability
 Non spontaneous
 Movement away from Equilibrium
 Coupled to ATP utilization
 Anabolism

17. Thank You..
Doubt ??