thermodynamics i chapter 6 entropymohsin/sme1413/01.english/chap06/06... · 2013-11-25 ·...
TRANSCRIPT
Thermodynamics IChapter 6Entropy
Mohsin Mohd SiesFakulti Kejuruteraan Mekanikal, Universiti Teknologi Malaysia
Entropy (Motivation)
The preferred direction implied by the 2nd Law can bebetter understood and quantified by the concept ofentropy.Entropy quantifies the 2nd Law and imposes thedirection of processes.Here we will study entropy and how processes willproceed only in the direction of increasing entropy.
Clausius Inequality
Erev Eirrev
QH QH
QL QL,irrev
W Wirrev
TH
TL
Consider two heat engines between the same temperatures
Consider of the whole cycle
T
Q
(a) Erev
0
0
11
=
=
−=
−=
−=
∫
∫∫
∫∫∫
rev
L
L
H
H
LL
HH
L
L
H
H
rev
T
Q
T
Q
T
Q
QT
QT
T
Q
T
Q
T
Q
(b) Eirrev
ΔQ+Q=Q
Q>Q
LirrevL,
LirrevL,
Combined to be:
= 0 if reversible< 0 if irreversible> 0 impossible
ENTROPY
1
2B
A
∫
∫∫
∫∫∫
=
−=
=
+
=
2
1
1
2
2
1
1
2
2
1
0
B
BA
BArev
T
Q
T
Q
T
Q
T
Q
T
Q
T
Q
Does not depend onpath; thermodynamicproperty!
Let's call this property entropy, S[kJ/K]
revT
QdS
≡
Entropy , S = extensive property [kJ/K]
Specific entropy, s = intensive property [kJ/kg.K]
∫∫
=−=
2
112
2
1revT
QSSdS
We have actually defined entropy change
From statistical thermodynamics, entropy ~ measure of molecular disorderWork is an ordered form of energy (High quality)
No entropy transfer along with work transferHeat is a disordered form of energy (Low quality)
Entropy is transferred along with heat transfer
“Entropy = zero for pure crystal at 0 K”Third Law of Thermodynamics
Entropy with a 0 K reference is called absoluteentropy
T-ds Relations
To find the relationship between δQ and T so that theintegration of δQ/T can be performed
- From the 1st Law (neglecting KE & PE)
pdvduTds
pdVdUTdS
dUpdVTdS
+=+==−
(a)
dU=δWδQU=WQ
revrev −−
pdV=δWTdS=δQ
rev
rev
- From the definition of enthalpy
vdppdvdhdu
vdppdvdudh
pvuh
−−=++=
+=
From (a)
vdpdhTds
pdvvdppdvdh
pdvduTds
−=+−−=
+=
(b)
T
vdp
T
dhds
T
pdv
T
duds
−=
+=&
vdpdhTds
pdvduTds
−=+=
Can be used for ∆S of any process (rev. & irrev.)Can be used for open & closed system
T-ds Relations
Entropy Change of Pure Substances
Can be obtained from Tds Relations in conjunction with otherthermodynamic relationsFor 2 phase substances like water and R-134a, use property tablesS = S2 – S1
For ideal gas, from Tds relations
1
2
1
212 lnln
v
vR
T
TCsss
v
dvR
T
dTCds
v
dvR
T
dTCds
T
pdv
T
duds
v
v
v
+=−=∆
+=
+=
+=
∫∫∫
v
R
T
pRTpv
dTCdu v
=→=
=
Assume Cv=constant& integrate
1
2
1
212 lnln
p
pR
T
TCsss
p
dpR
T
dTCds
p
dpR
T
dTCds
T
vdp
T
dhds
p
p
p
−=−=∆
−=
−=
−=
∫∫∫
Another relation,
v
R
T
pRTpv
dTCdh p
=→=
=
Assume Cp =constant& integrate
1
2
1
212
1
2
1
212
lnln
lnln
p
pR
T
TCsss
v
vR
T
TCsss
p
v
−=−=∆
+=−=∆
Both equations give the same resultChoose according to available data..
Entropy change
Isentropic Processes, S = 0
For ideal gases, with constant Cp & Cv
1
2
1
1
2
1
2
1
1
2
2
1
1
2
1
2
1
2
1
2
1
2
1
2
lnln
lnlnln
lnln
0lnln
−
−
=
=→
=−=
−=
=+=∆
k
k
CR
v
v
v
v
v
T
T
v
v
T
T
v
v
v
v
C
R
T
T
v
vR
T
TC
v
vR
T
TCs
v
1−=∴
=
=−
kC
R
C
Ck
RCC
v
v
p
vp
k
k
k
k
CR
p
p
p
p
T
T
p
p
p
p
p
p
C
R
T
T
p
pR
T
TCs
p
1
1
2
1
2
1
1
2
1
2
1
2
1
2
1
2
1
2
ln
ln
lnln
0lnln
−
−
=
=
=
=
=−=∆
Another one
k
k
C
R
kC
C
C
C
C
R
RCC
p
p
v
p
p
p
vp
1
11
−=∴
−=−=
=−
Combined to become
1
2
1
1
1
2
1
2
−−
=
=
kk
k
v
v
p
p
T
T Isentropic process forideal gas,constant Cp , Cv
( ) ( )
( ) ( )
dpv=w
vdp=δw
ped+ked+dh=δwvdpdh
ped+ked+dh=δwδq
rev
rev
rev
revrev
∫−
−
−−
−
2
1
Work for Open Systems
Reversible boundary work forclosed systems
∫= pdvwB
Open system reversible work, from 1st Law (single inlet/outlet)
Reversible work foropen system
neglecting ke & pe, & rearrange;vdpdh=δq
vdpdf=Tds
Tds=δq
rev
rev
−→−
Increase in Entropy Principle
• For reversible processes, entropy of universe (system surrounding)doesn't change, it is just transferred (along with heat transfer)
• In real processes, irreversibilities cause entropy of universe to increase• Heat reservoirs don't have irreversibility• To simplify analysis, assume irreversibilities to exist only inside the
system under study.• Inside the system, entropy transfer and generation occur.
irrev
1
2
rev
Irreversible cycle since one of theprocesses is irreversible
From Clausius Inequality;
gen
irrev
irrev
S+T
δQ=SS
T
δQSS
T
δQ>SS
T
δQ<SS
∫
∫
∫
∫
−
≥−
−
−−
2
1
12
2
1
12
2
1
12
2
1
12
Rearrange
Generalize for all processes
= when rev> when irrev< impossible
Sgen=entropy generated= 0 when rev.> 0 when irrev.< 0 impossible
genb
ST
QSS +
=− ∫
2
112
Change ofsystementropy
Transfer of entropy(T where Q istransferred, usuallyat boundary
Entropygeneration
Entropy Generation for Closed System
Sgen is the measure of irreversibilities involved during process
S surrounding or system may decrease (-ve), but S total(surrounding + system) must be > 0
Entropy of universe always increases (Entropy increase principle)
No such thing as entropy conservation principle
For a process to occur, Sgen> 0
0≥= systemgsurroundinuniversetotal,gen ΔS+ΔS=ΔSS
Entropy Generation for Closed System
gen
n
j j
j
genb
genb
ST
QSS
ST
QSS
ST
QSSS
+=−
+=−
+=−=∆
∑
∫
=112
12
12
For multiple heat transfers at different temperatures
gen
n
j j
j
gen
n
j j
j
ST
QdS
ST
Q
dt
dS
+=
+=
∑
∑
=
=
1
1
In rate form
In differential form
Sgen - depends on the process (friction, ∆T etc.)- not a property
Entropy Generation for Closed System
Entropy Generation for Open Systems
Apart from heat, mass flows also carry entropy along with them
Qin
min
sin
mout
soutCV
genoutinj j
jCV
genoutinj j
jCV
SmsmsT
QS
SSST
QS
+−+=∆
+−+=∆
∑∑∑
∑∑∑
=
=
1
1
genoutinj j
jCV SsmsmT
Q
dt
dS
+−+= ∑∑∑=1
Rate ofchange ofsystementropy
Rate of entropytransfer
Rate ofentropygeneration
Qin
min
sin
CV
Entropy Generation for Open Systems
Steady Flow Process
genooiij j
j
genooiij j
jCV
CV
outinCV
SsmsmT
Q
SsmsmT
Q
dt
dS
dt
dS
mmdt
dm
+−+=
+−+=
=
=→=
∑∑∑
∑∑∑
∑∑
=
=
1
1
0
0
0
m
S
Tm
Q
ss
SssmT
Q
gen
j jio
genoij j
j
j
+=−
+−+=
∑
∑
=
=
1
1
)(0
single inlet/outlet;
Steady Flow Process
Reversible adiabatic process = isentropic process
Isentropic is not necessarily reversible adiabatic
Reversible process Sgen = 0
Produces Wmax
Consumes Wmin
30
ISENTROPIC EFFICIENCIES OF STEADY-FLOW DEVICES
The isentropic process involves noirreversibilities and serves as the ideal
process for adiabatic devices.
The h-s diagram forthe actual andisentropic processesof an adiabaticturbine.
IsentropicEfficiencyof Turbines
Also known as Adiabatic Efficiencyor 2nd Law Efficiency
31
Isentropic Efficiencies of Compressors and Pumps
The h-s diagram of the actualand isentropic processes of an
adiabatic compressor.
Compressors aresometimesintentionallycooled tominimize thework input.
When kinetic andpotential energiesare negligible
32
Isentropic Efficiency of Nozzles
The h-s diagramof the actual and
isentropicprocesses of an
adiabatic nozzle.
If the inlet velocity of thefluid is small relative tothe exit velocity, theenergy balance is
Then,
A substance leavesactual nozzles at a
higher temperature(thus a lower velocity)as a result of friction.