chapter 5 single phase systems. introduction before carrying out a complete material balance, we...
TRANSCRIPT
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Chapter 5
Single Phase Systems
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Introduction
Before carrying out a complete material balance, we usually need to determine various physical properties of materials in order to derive additional relationship among the system variables.
As an example we need the density to relate the volumetric flow rate to mass flow rate or vice versa.
3 ways to obtain the values of physical properties (such as density, vapor pressure, solubility, heat capacity, etc)1. Handbook or database
- Perry’s Chemical Handbook, CRC Handbook of Chemistry & Physics, TRC Database in Chemistry & Engineering, etc
2. Estimation using empirical correlations3. Experimental work
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Density of Liquid and Solid
Temperature dependence: modest but sometimes important (liquid and solid expanded during heating and density decrease)
Pressure dependence: usually negligible (solid and liquid are incompressible with pressure).
2 methods to estimate the density of mixture which consist n liquid (n is number of different type of liquid) Method 1: Volume Additivity
Works best for mixture of liquid species with similar molecular structure
Method 2: Average Pure Component Densities
n
i i
ix
1
1
n
iiix
1
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Ideal Gases
Equation of state Relates the molar quantity and volume of a gas to temperature and
pressure. Ideal gas equation of state
Simplest and most widely used Used for gas at low pressure and high temperature Derived from the kinetic theory of gases by assuming gas molecules
1. have a negligible volume;2. Exert no forces on one another;3. Collide elastically with the wall of container
or
The use of this equation does not require to know the gas species:1 mol of an ideal gas at 0˚C and 1 atm occupies 22.415 liters, whether the gas is argon, nitrogen, mixture of propane and air, or any other single species or mixture of gases
nRTPV RTnVP
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Ideal Gas Equation of State
P = absolute pressureV = volume of the gasn = number of moles of gasR = gas constant which the unit depend on unit of P, V, n, TT = absolute temperature
Ideal gas equation of state can also be written as Which ; specific molar volume of gas.
Unit for gas constant, R
or
nRTPV
RTVP ˆnVV /ˆ
etemperaturmole
volumepressureRfor Unit
etemperaturmole
energyRfor Unit
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Ideal Gas Equation of State Density of ideal gas (M is average molecular weight-refer back previous
chapter Eq. 3.3-7)
Rule of thumb for when it is reasonable to assume ideal gas behavior. Let Xideal be a quantity calculated using ideal gas equation of state (X can be
pressure, volume, temperature or mole). Error is estimated value is ε
Let’s say quantity to be calculate is ideal specific molar volume,
If error calculated satisfies this criterion, the ideal gas equation of state should yield an error less than 1%
RT
MP
V
M
ˆ
%100
true
trueideal
X
XX
V̂
gasesother mole)-lb/ ft (320 L/mol 20
gasesdiatomicmole)lb/ ft (80L/mol 5ˆ%13
3
idealVif
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Class Discussion
Example 5.2-1
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Standard Temperature and Pressure (STP)
A way to avoid the use of gas constant, R when using ideal gas equation For ideal gas at arbitrary temperature, T and pressure, P
For the same ideal gas at standard reference temperature, Ts and standard reference pressure, Ps (refer to STP).
Divide eq. 1 to eq. 2
Value of standard conditions (Ps, Ts, Vs) are known, above equation can be used to determine V for a given n or vice versa
Standard cubic meters (SCM) : m3 (STP) Standard cubic feet (SCF) : ft3 (STP) Let say 18 SCMH mean 18 m3 (STP)/h
nRTPV
sss RTVP ˆ
sssT
Tn
VP
PV
ˆ
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Standard Conditions for Gases
System Ts Ps Vs ns VsSI 273K 1atm 0.022415 m3 1 mol 22.4 m3/kmolcgs 273K 1atm 22.415 L 1 mol 22.4 L/molEnglish 492˚R 1atm 359.05ft3 1 lb-mole 359.05 ft3/lb-mole
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“ Saya pasti akan berjaya kerana saya telah
kehabisan benda-benda yang tidak berjaya”
Thomas Edison
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Class Discussion
Example 5.2-2
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Class Discussion
Example 5.2-3
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Class Discussion
Example 5.2-4
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Ideal Gas Mixture
Suppose nA moles of species A, nB moles of species B, nc moles of species C and so on, contained in a volume, V at temperature, T and pressure, P Partial pressure, pA
The pressure that would be exerted by nA moles of species A alone in the same total volume, V at the same temperature, T of the mixture.
Pure component volume, vA
The volume would be occupied by nA moles of A alone at the same total pressure, P and temperature, T of the mixture.
Ideal gas mixture Each of the individual species component and the mixture as whole
behave in an ideal manner
Pyp AA
Vyv AA
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Ideal Gas Mixture
Dalton’s Law The summation of partial pressure of the component of an
ideal gas mixture is equal to total pressure
Amagat’s Law
Volume fraction = vA/V; percentage by volume (%v/v)= (vA/V )x 100%
For an ideal gas mixture, the volume fraction is equal to the mole fraction of the substance:
70% v/v C2H6 = 70 mole% C2H6
PPyyyppp CBACBA ....)(.....
VVyyyvvv CBACBA ....)(.....
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Class Discussion
Example 5.2-5
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Equation of State for Nonideal Gases
Critical temperature (Tc)- the highest temperature at which a species can exist in two phases (liquid and vapor), and the corresponding pressure is critical pressure (Pc)
Other definition: highest temperature at which isothermal compression of the species vapor results in the formation of a separate liquid phase.
Critical state- a substance at their critical temperature and critical pressure.
Species below Pc: Species above Tc- gas Species below Tc- vapor
Species above Pc and above Tc- supercritical fluids
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Virial Equation of State Virial equation of state
B,C,D- second, third, fourth virial coefficient respectively
Truncated virial equation
Tr=T/Tc ω – acentric factor from Table 5.3-1
Tc,Pc from Table B.1
....ˆˆˆ
1ˆ
32
V
D
V
C
V
B
RT
VP
V
B
RT
VPˆ
1ˆ
6.102.4110
422.0083.0;
172.0139.0);(
rrc
c
TB
TBBB
P
RTB
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Class Discussion
Example 5.3-1
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Kebebasan tanpa tanggungjawab membawa
kehancuran
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Cubic Equations of State
Refer as cubic equation because when the equation is expanded, it becomes third order equation for the specific volume
To evaluate volume for a given temperature and pressure using cubic equation of state, we need to do trial and error procedure.
Two famous cubic equation of statea) Van der Waals equation of stateb) Soave-Redlich-Kwong (SRK) equation of state
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Van der Waals Equation of State
(a/V2) - account for attractive force between moleculesb - correction accounting for the volume occupied by the
molecules themselves
2ˆˆ V
a
bV
RTP
c
c
c
c
P
RTb
P
TRa
864
27 22
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Soave-Redlich-Kwong (SRK) equation of state
)ˆ(ˆˆ bVV
a
bV
RTP
2
2
2
1561.055171.148508.0
)]1(1[/
08664.0)(
42747.0
m
TmTTT
P
RTb
P
RTa
rcr
c
c
c
c
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Class Discussion
Example 5.3-2
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Compressibility Factor Equation of State
or
If z=0, equation become ideal gas equation of state
Value of z is given in Perry’s Chemical Engineering Handbook pg. 2.140- 2.150.
Alternatively; can use generalized compressibility chart Figure 5.4-1 – generalized compressibility chart Fig. 5.4-2 to Fig. 5.4-4 – expansion on various region in Fig.
5.4-1
zRTVP ˆRT
VPz
ˆ
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Step to Read Compressibility Factor
1. Find Tc and Pc2. If gas is either Hydrogen or Helium, determine adjusted critical
temperature and pressure from Newton’s correction equation
3. Calculate reduce pressure and reduce temperature of the two known variables
4. Read off the compressibility factor from the chart
c
cidealr RT
VPV
Pc
P
Tc
TTr
ˆ;Pr;
atmPPKTT cacc
ac 88
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Class Discussion
Example 5.4-2
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Nonideal Gas Mixtures
Kay’s Rule: estimation of pseudocritical properties of mixture as simple average of pure a component critical constants
Pseudocritical temperature (Tc’)
Tc’= yATcA + yBTcB +……
Pseudocritical pressure (Pc’)
Pc’= yAPcA + yBPcB +……
Pseudocritical reduced temperature (Tr’)
Tr’= T/Tc’
Pseudocritical reduce pressure (Pr’)
Pr’= P/Pc’
Compressibility factor for gas mixture, Zm P
RTzV mˆ
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Class Discussion
Example 5.4-3
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ANY QUESTION?