Thermodynamics IChapter 6Entropy

Mohsin Mohd SiesFakulti Kejuruteraan Mekanikal, Universiti Teknologi Malaysia

Entropy (Motivation)

The preferred direction implied by the 2nd Law can be better understood and quantified by the concept of entropy.Entropy quantifies the 2nd Law and imposes the direction of processes.Here we will study entropy and how processes will proceed 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 cycleTQ

(a) Erev

0

0

11

rev

L

L

H

H

LL

HH

L

L

H

H

rev

TQ

TQ

TQ

QT

QT

TQ

TQ

TQ

(b) Eirrev

ΔQ+Q=QQ>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

TQ

TQ

TQ

TQ

TQ

TQ

Does not depend on path; thermodynamic property!

Let's call this property entropy, S [kJ/K]

revTQdS

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 absolute entropy

T-ds Relations

To find the relationship between Q and T so that the integration of Q/T can be performed

- From the 1st Law (neglecting KE & PE)

pdvduTdspdVdUTdSdUpdVTdS

(a)

dU=δWδQU=WQ

revrev

pdV=δWTdS=δQ

rev

rev

- From the definition of enthalpy

vdppdvdhduvdppdvdudh

pvuh

From (a)

vdpdhTdspdvvdppdvdh

pdvduTds

(b)

Tvdp

Tdhds

Tpdv

Tduds

&

vdpdhTdspdvduTds

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 other thermodynamic relationsFor 2 phase substances like water and R-134a, use property tables

S = S2 – S1

For ideal gas, from Tds relations

1

2

1

212 lnln

vvR

TTCsss

vdvR

TdTCds

vdvR

TdTCds

Tpdv

Tduds

v

v

v

vR

TpRTpv

dTCdu v

Assume Cv=constant& integrate

1

2

1

212 lnln

ppR

TTCsss

pdpR

TdTCds

pdpR

TdTCds

Tvdp

Tdhds

p

p

p

Another relation,

pR

TvRTpv

dTCdh p

Assume Cp =constant& integrate

1

2

1

212

1

2

1

212

lnln

lnln

ppR

TTCsss

vvR

TTCsss

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

vv

TT

vv

TT

vv

vv

CR

TT

vvR

TTC

vvR

TTCs

v

1

kCR

CC

k

RCC

v

v

p

vp

kk

kk

CR

p

p

pp

TT

pp

pp

pp

CR

TT

ppR

TTCs

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

kk

CR

kCC

CC

CR

RCC

p

p

v

p

p

p

vp

1

11

Combined to become

1

2

1

1

1

2

1

2

kk

k

vv

pp

TT Isentropic process

for ideal 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 for closed systems

pdvwB

Open system reversible work, from 1st Law (single inlet/outlet)

Reversible work for open system

neglecting ke & pe, & rearrange;vdpdh=δq

vdpdh=TdsTds=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 the processes is irreversible

From Clausius Inequality;

gen

irrev

irrev

S+TδQ=SS

TδQSS

TδQ>SS

TδQ<SS

2

112

2

112

2

112

2

112

Rearrange

Generalize for all processes

= when rev> when irrev< impossible

Sgen=entropy generated = 0 when rev. > 0 when irrev. < 0 impossible

genb

STQSS

2

112

Change of system entropy

Transfer of entropy (T where Q is transferred, usually at boundary

Entropy generation

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

STQ

SS

STQSS

STQSSS

112

12

12

For multiple heat transfers at different temperatures

gen

n

j j

j

gen

n

j j

j

STQ

dS

STQ

dtdS

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

SmsmsTQ

S

SSSTQ

S

1

1

genoutinj j

jCV SsmsmTQ

dtdS

1

Rate of change of system entropy

Rate of entropy transfer

Rate of entropy generation

Qin

min

sin

CV

Entropy Generation for Open Systems

Steady Flow Process

genooiij j

j

genooiij j

jCV

CV

outinCV

SsmsmTQ

SsmsmTQ

dtdS

dtdS

mmdt

dm

1

1

0

0

0

mS

Tm

Qss

SssmTQ

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 no irreversibilities and serves as the ideal

process for adiabatic devices.

The h-s diagram for the actual and isentropic processes of an adiabatic turbine.

Isentropic Efficiency of Turbines

Also known as Adiabatic Efficiency or 2nd Law Efficiency

31

Isentropic Efficiencies of Compressors and Pumps

The h-s diagram of the actual and isentropic processes of an

adiabatic compressor.

Compressors are sometimes intentionally cooled to minimize the work input.

When kinetic and potential energies are negligible

32

Isentropic Efficiency of Nozzles

The h-s diagram of the actual and

isentropic processes of an

adiabatic nozzle.

If the inlet velocity of the fluid is small relative to the exit velocity, the energy balance is

Then,

A substance leaves actual nozzles at a

higher temperature (thus a lower velocity) as a result of friction.