slides on entropy fr subject engineering thermodynamics(ET)

1. -:Entropy:-
Submitted to:- Mr. Mitesh Gohil
By:-Harsh Parmar(PG-18)
Akash Parikh(PG-02)
Devarsh Jadavanee(PG-22)
Moyun Sherasiya(PG-43)
Smith Parekh (PG-34)
Vivekkumar Boda (FOE-23
Yug TripathiI (FOE-21)
Harsh Dalsania(PG-11)

2. Entropy:- The Entropy is a thermodynamic property of a working
substance and serves as a valuable tool in the second law
analysis of engineering devices.
• Entropy is afunction of a quantity of heat which shows the
possibility of conversoin of that into work.
• Entropy is a thermodynamic property; it can be viewed as a
measure of disorder i.e. More disorganized a system the higher
its entropy.

5. Clausius Theorem

6. • Entropy is a thermodynamic property; it can be viewed as a
measure of disorder. i.e. More disorganized a system the
higher its entropy. Defined using Clausius inequality
• where Q is the differential heat transfer & T is the absolute
• temperature at the boundary where the heat transfer occurs
0 





revT
Q

7. th, from Carnot efficiceny 1 1 ,
Q Q
Therefore, 0 for a reversible Carnot cycle 0
T T
H L L L L L
H L H H H H
rev
Q Q Q Q T Q T
T T T Q T Q T


 
      
 
  
 

 
Ñ
Ñ Ñ
• Clausius inequality is valid for all cycles,
reversible and irreversible.
• Consider a reversible Carnot cycle:

8. • Since entropy is a thermodynamic property, it has
fixed values at a fixed thermodynamic states.
Hence, the change, S, is determined by the initial
and final state. BUT..
• The change is = only for a Reversible Process 





T
Q

10. Consider a cycle, where Process 2-1 is reversible and 1-2 may
or may not be reversible
2 1
1 2
2 2 2
2 1
1 1 1
2 1
2 1
1 2
0
From entropy definition
Q Q
dS= , 0
Therefore,
rev
rev rev revrev
rev
Q Q Q
T T T
Q Q
dS
T T T T
Q Q
dS S S S
T T
Q
S S S
T
  
   
 

   
     
   
       
          
       
   
        
   
 
     
 
  
   
  
Ñ
Ñ Ñ
2
1
, This is valid for all processes
Q Q
, since = ,
T Trev irrev
Q
dS dS dS
T
     
    
   

1
2
reversible
process
any
process
T
S

12. Entropy change for Open System

13. Processes can be discussed profitably using the entropy concept.
For a reversible process:

B
A
AB
T
Q
SSS

• If the reversible process is isothermal:
STQ
T
Q
Q
T
SSS
B
A
AB  
1
S increases if the system absorbs heat, otherwise S decreases
00   S
T
Q
SSS
B
A
AB

Reversible isothermal processes are isentropic
But in irreversible ones the entropy may change
• If the reversible process is adiabatic:

14. Increase of Entropy Principle
2
2 1 gen
1
2 2
2 1
1 1
, define entropy generation S
where 0. If the system is isolated and "no" heat transfer
The entropy will still increase or stay
system gen
gen
Q
S S S
T
Q Q
S S S S
T T
S

 
 
     
 
   
        
   


 
the same but never decrease
0, entropy increase principlesystem genS S  
Entropy change
Entropy Transfer
(due to heat transfer)
Entropy Generation
The principle states that for an isolated Or a closed adiabatic Or
System + Surroundings.A process can only take place such that Sgen 0
where Sge = 0 for a reversible process only
And Sge can never be les than zero.
Increase of Entropy Principle

15. • Entropy, unlike energy, is non-conservative since it is always
increasing.
• The entropy of the universe is continuously increasing, in
other words, it is becoming disorganized and is
approaching chaotic.
• The entropy generation is due to the presence of
irreversibilities. Therefore, the higher the entropy generation
the higher the irreversibilities and, accordingly, the lower the
efficiency of a device since a reversible system is the most
efficient system.
• The above is another statement of the second law

16. Third law of Thermodynamics
• The Third Law of Thermodynamics was first
formulated by German chemist and physicist
Walther Nernst.
• The Third Law states, “The entropy of a
perfect crystal is zero when the temperature of
the crystal is equal to absolute zero (0 K).”

17. Applications of Third law of
Thermodynamics
• Provides an absolute reference point for the
determination of entropy.
• Explaining the behavior of solids at very low
temprature.
• Measurement of action of chemical forces of the
reacting substances.
• Analysing the chemical and Phase Equilibrium.