Department of Mechanical Engineering ME 322 – Mechanical Engineering Thermodynamics Lecture 20...
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Transcript of Department of Mechanical Engineering ME 322 – Mechanical Engineering Thermodynamics Lecture 20...
Department of Mechanical Engineering
ME 322 – Mechanical Engineering Thermodynamics
Lecture 20
Entropy Balance Equation
2
The Second Law of Thermodynamics
Entropy is a balanced quantity. Therefore,
Entropy transported
into a system
Entropy transported out
of a system
Entropy produced within
a system
Entropy gained within
a system- + =
TS PS GS
T P GS S S
T P GS S S Total Entropy Form
Entropy Rate Form
Something to think about ... We have already seen that entropy production occurs due to irreversibility. But, how is entropy transported across a system boundary?
The Second Law of Thermodynamics
3
T P G T P GS S S dS dS dS
First, consider a closed system. For this system, we know that the Second Law is,
Recall that Clausius discovered entropy analyzing a Carnot cycle as a closed system. His discovery was,
E
LT
HT
rev
dQdS
T
Q W
T in this expression is the boundary temperature where Q is being transferred.
The Second Law of Thermodynamics
4
Q WFor a reversible process, we know that the entropy production is zero. Therefore, for a reversible process, the Second Law says,
T GdS dS
rev
dQdS
T
Now, consider Clausius’ discovery again,
For the closed system that we are analyzing, it is clear that heat and work cross the system boundary. Therefore, we can say that,
and T G sys
rev
dQdS dS dS
T
The Second Law of Thermodynamics
5
We have just discovered that that the entropy is transported into the system by heat, but NOT by work!
Q W
P sys
dQdS dS
T
For any closed system process, we can write,
This expression can now be integrated between any two states,
2 2 2
1 1 1P sys
dQdS dS
T
The Second Law of Thermodynamics
6
2 2 2
1 1 1P sys
dQdS dS
T
Analyzing each integral ...
2
1
k
kk
QdQ
T T
Assumption: The system boundary is isothermal.
The summation sign accounts for all heat transfer.
2
2 1 2 11
sysdS S S m s s The entropy change of the system.
2
1???PdS
This is the integral of the entropy production in an irreversible process. But ... how do we evaluate the integral???
The Second Law of Thermodynamics
7
Entropy production is caused by irreversibilities. Consider two piston-cylinder assemblies. They are identical in every way except that one of them operates reversibly and the other is irreversible.
Q
revW
Q
irrW
reversible irreversible
Questions ...
1. Which system has zero entropy production?
2. Which system delivers more work?
3. Is work a property?
4. Is entropy production a property?
The Second Law of Thermodynamics
8
Entropy production is NOT a property. It is a function of path, just like heat and work!
P sys
dQdS dS
T
2
,121
P PdS S
Now, we can integrate the entropy production term!
> 0 means that the process is irreversible= 0 means the process is reversible< 0 means the process is impossible
The Second Law of Thermodynamics
9
For a closed system, the Second Law of Thermodynamics can be written as,
,12 2 1k
Pkk
QS m s s
T T P GS S S
This can be written on a per unit mass basis by dividing both sides of the equation by the mass of the system,
,12 2 1k
Pkk
qs s s
T ,12
2 1
/ Pk
kk
SQ ms s
T m
The Second Law of Thermodynamics
10
syski i e e P
k i ek
dSQm s m s S
T dt
Incorporating the net entropy transport into the system due to the mass flows gives the complete form of the Second Law of Thermodynamics!
Notice that if the system is closed,
syskP
k k
dSQS
T dt
,12 2 1k
Pk k
QS m s s
T
11
The Laws of the Universe
2 2
2 2sysi e
i i i e e ei ec c c c
dEV Vg gQ W m h z m h z
g g g g dt
sysi e
i e
dmm m
dt
Conservation of Mass – The Continuity Equation
Conservation of Energy – The First Law of Thermodynamics
The Entropy Balance – The Second Law of Thermodynamics
syski i e e P
k i ek
dSQm s m s S
T dt
Special Application – Closed Systems
12
Consider a closed system that is reversible and adiabatic. The second law for such a system is,
,12 2 1k
Pk k
QS m s s
T
00
2 1 2 10s s s s
We have just learned that a reversible and adiabatic process for a closed system is isentropic!
Notice: Reversible does not mean isentropic Adiabatic does not mean isentropic Reversible and adiabatic means isentropic!
We have just learned that a reversible and adiabatic process for a system of this type is isentropic!
Entropy is the gate keeper of the Second Law!
Special Application – Open Systems
13
Consider an open system that is operating in steady state and is reversible and adiabatic with one flow in and one flow out. The second law for such a system is,
00
0i e i em s s s s
syski i e e P
k i ek
dSQm s m s S
T dt
0
Ideal Gases w/constant cp
14
2
1
22 1
1
lnT
vT
vdTs s c R
T v
2
1
22 1
1
lnT
pT
PdTs s c R
T P
2 22 1
1 1
ln lnp
T Ps s c R
T P
We previously derived the following expressions for an ideal gas from the Gibbs Equations,
If the gas is undergoing a process where the heat capacity can be assumed to be constant,
Consider a case where the process is also isentropic. Then,
2 2
1 1
ln ln 0p
T Pc R
T P
Ideal Gases w/constant cp
15
2 2
1 1
ln ln 0p
T Pc R
T P
Algebra time ...
2 2
1 1
ln lnp
T Pc R
T P 2 2
1 1
ln lnp
T PR
T c P
2 2
1 1
p
R
cT P
T P
Rearrange the exponent,
p v
p p
c cR
c c
/ /
/
p v v v
p v
c c c c
c c
1 p
v
ckk
k c
Ideal Gases w/constant cp
16
Substitution gives,
1
2 2
1 1
k
kT P
T P
2 22 1
1 1
0 ln lnv
T vs s c R
T v
If we consider an isentropic process with the other Ds equation,1
2 2
1 1
kT v
T v
Therefore, for an ideal gas with constant heat capacity undergoing an isentropic process,
11
2 2 2
1 1 1
kk
kT P v
T P v
Ideal Gases w/constant cp
17
But wait ... there’s more!!1
1
2 2 2
1 1 1
kk
kT P v
T P v
11
2 2
1 1
kk
kP v
P v
Rearranging ... 1 11 1
2 1 1 2
k kk kk kP v P v
1 11 1
2 2 1 1
k kk kk kP v P v
1 11 1
2 2 1 1
k kk k
k kP v Pv
2 2 1 1k kP v Pv Does this look familiar?
Polytropic Process RelationsconstantnPv
Any fluid model
Ideal Gas Model
Ideal Gas Model – Isentropicprocess, constant heat capacity
(isochoric)n
18
1 1 /
2 2 2 2
1 1 1 1
k k kT v T P
T v T P
1 1 /
2 2 2 2
1 1 1 1
n n nT v T P
T v T P
1/
2 1 2 1
1 2 1 2
n nP v v P
P v v P
/ (ideal gas with constant heat capacity - isentropic process)p vn k c c
1 (ideal gas, isothermal)n0 (isobaric)n