chapter 3 (1) (volumetric properties)
TRANSCRIPT
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Chapter 3
Volumetric Properties
of Pure Fluids
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Objectives of Chapter 3
To apply the energy balance to a system of interest
requires knowledge of the properties of the system and
how the properties are related.
The objective of Chapter 3 is to introduce property relations
relevant to engineering thermodynamics.
We will focus on the use of the closed system energy
balance introduced in Chapter 2, together with the property
relations considered in this chapter.
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Outline of chapter 3
PVT Behaviour
Equation of state
1. Ideal gas equations
2. Virial equations
3. Cubic equation of state
- van der Waals equation
- modified van der Waals equations
Generalised correlation
1. gas
2. liquid
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PVT Behaviour
PVT relationship is between three important properties of pure substances: pressure, specific volume, and temperature.
Generally is given in the form of a phase diagram, in which the different regions of phase state (solid, liquid, and vapor and their combinations) are shown.
Understanding of such diagrams is essential to thermodynamics because there will be many occasions in which you will have to refer to a phase diagram in order to obtain needed property information.
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PVT - 3D diagram
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PVT Diagrams
Red lines: isobars
Blue lines: isotherms
Green areas: two-phase regions
Yellow areas: single phase
regions
isochoric
Isothermal
Isobaric
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P-T diagram
Fusion curve = melting curve
isochoric
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Supercritical fluid region
When T > Tc and P > Pc
Properties are combination of liquid and gas
fluid
Density is close to liquid density but with higher
diffusivity and lower viscosity
Attractive in extraction as it evaporates easily
without leaving much residue
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P-V Diagram
Isothermal
Saturation curve
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T-V Diagram
Isobaric C = Saturated liquid E = Saturated vapour Tc = boiling point
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T-V Diagram
Red : saturated liquid curve Green: saturated vapour curve Meeting point = critical point
Subcooled region
Superheated region (between boiling point and supercritical region) Eg: wet steam and super- heated steam
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Eg: specific volume
specific volume v - it could be any number between vf and vg In the two phase region, the liquid phase is always saturated liquid and the vapor phase is always saturated vapor. The two phase mixture is simply a mixture of saturated liquid and saturated vapor.
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Quality
liquidvapor
vapor
total
vapor
mm
m
m
mx
Quality is the fraction of the total mass in a vapor-liquid system that is in the vapor phase.
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Quality - derivation
The total mass M of material in the vessel: (1) M = ML + MV Total volume V of the vessel (2) V = VL + VV
Relation between specific volume v and total volume V (3) V = vM Now consider the liquid phase. (4) VL = vfML By the same argument, we can write for the vapor phase: (5) VV = vgMV Substituting (3), (4) and (5) into (2) and (1) yields: (6) v = {MV/(MV + ML)}vg + {ML/(MV + ML)}vf At this point the quality x is defined as (7) x = MV/(MV + ML)
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Equation of state (EOS)
PVT data can be measured using Beattle’s
apparatus
PVT data can be fitted to algebraic equations called
“equation of state”.
Equations are mostly obtained empirically and very
few from molecular theory
Advantage of EOS: data reduction during
calculations
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Equation of state
Relates PVT of pure homogeneous fluid in equilibrium state
Previously - Boyle Law
- Charles Law
- Dalton’s Law
- Van der Waals
- Ideal Gas Law
In the gas region, when pressure is decreased and temperature is increased Ideal Gas behaviour can be considered
As behaviour moves away from ideal gas, various EOS are derived depending on properties
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1) The Ideal Gas – constant volume
Definition for ideal gas: simplified model of real gas behaviour
1) PV=RT
2) U = f (T) only (if no intermolecular force exist)
Constant volume (Isochoric)
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The Ideal Gas – constant pressure
Constant pressure (Isobaric)
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The Ideal Gas – constant temperature
Constant temperature (Isothermal)
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The Ideal Gas – constant heat
Adiabatic
Continued…
No heat transfer between
system and its surroundings
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The Ideal Gas – 3 adiabatic relationships
T and V
T and P
P and V
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Polytrophic process
Polytropic processes are internally reversible. Useful in Carnot cycle calculations where ideal gas is assumed.
Some examples are vapors and perfect gases in many non-flow processes. The polytrophic obeys:
PVd = constant
d=0 P=constant isobaric process.
d=infinity v=constant isochoric process.
d=1 Pv=constant isothermal process for an ideal gas.
d= g reversible adiabatic process for an ideal gas.
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Polytrophic process
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The Ideal Gas – polytrophic process
Polytropic process – adiabatic reversible process
More polytropic equations: textbook pg 78-79 – add into your notes!!!
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Ideal gas: example
An ideal gas undergoes following reversible processes in a closed system:
(a) From 70oC and 1 bar, it is compressed adiabatically to 150oC.
(b) The gas is cooled from 150oC to 70oC at constant pressure.
(c) The gas is expanded isothermally to its original state.
Calculate W, Q, DU and DH for each of the processes and for the entire cycle.Take Cv = 3/2 R
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Ideal gas: solution
Adiabatic, Q = 0
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Ideal gas: solution
For ideal gas
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Ideal gas: solution DU = CvdT DH = CpdT
Both are zero as the start and end point is the same. Q = -W
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Ideal gas: irreversible
Repeat calculations for the same state changes but accomplished
irreversibly. Assume that the efficiency of each process is 80% compared
with the equivalent reversible operation.
Solution: The property changes for the steps will be the same (i.e. DU and
DH are the same as for reversible). However Q and W are not
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Irreversible: solution
Work done on system
Work done by system
Why not divide? because the work should be less
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Compare reversible and irreversible
What is observed? Even though irreversible step has 80% efficiency, Total work (883/167 = 5.2) is five times more!
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2) Virial equations
The virial equation is important because it can be derived directly from statistical mechanics.
Virial equation is expressed as a dimensionless
ratio, called compressibility factor, Z Z= pV/RT as a power series in density (reciprocal
volume)
Extended parameters – B and C are called 2nd and 3rd virial coefficients (functions of T) and increases accuracy
Used mostly for low to moderate pressures
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Virial equations
Virial Equation is used when:
1) Series converges rapidly - not more than 2 or 3 terms are used
eg: during low pressure
2) Used for VLE correlations and predictions
Where B, C, D are virial coefficients
For Ideal Gas, Z = 1, as PV = RT
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Virial equations – applications
For cases when convergence is rapid, simplification is carried out
P 0, tangent line can be applied,
2
0
11
'1
'
V
C
V
B
RT
BP
RT
PVZ
PBZ
BP
Z
P
d
d
Validity: 1) Vapours at subcrticial temperatures up to their saturation pressures 2) Gases with low pressure (several bars)
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3) Cubic* equation of state
1) Van der Waals equation
a = Attractive forces between molecules
b = Correction for volume occupied by the molecules
*Cubic refers to the volume
Validity: For T>Tc the van der Waals equation is an improvement of the ideal gas law. For lower temperatures the equation is reasonable for the two phase state at low pressure
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2) Modified van der Waals equation
Van der Waals: rough approximate of the two phase region
Starting point for the development of many equations representing PVT data in this region
Some modifications:
a) Redlich-Kwong
b) RK-Soave
c) Peng-Robinson
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2. (a) Redlich and Kwong Equation
Validity:
Adequate for calculation of gas phase properties
when the ratio of the Pr< 0.5 Tr or
*Note Pr = P/Pc and Tr = T/Tc
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(b) Redlich-Kwong-Soave Equation
The a function was devised to fit the vapor pressure data of hydrocarbons and the equation does fairly well for these materials.
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(c) Peng-Robinson Equation
• The equation provides reasonable accuracy near the critical point, particularly for calculations of compressibility factor and liquid density • The equation performance is similar to the Soave equation, although it is generally superior in predicting the liquid densities of many materials, especially nonpolar ones • The equation should be applicable to all calculations of all fluid properties in natural gas processes
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Acentric Factor
• Van der Waals and Redlich-Kwong: two parameters Tr and Pr • Soave-RK and Peng Robinson: three parameters Tr, Pr and acentric factors a (Tr, w) • The acentric factor, w is defined as the difference evaluated at Tr=0.7 :
•Further numerical assignments for parameters: Table 3.1 pg 98
Values for w, Tc, Pc, Vc, etc can be obtained from App. B
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Generalized Correlation
Equations where Z (dimensionless, reduced quantity) is expressed as reduced temperature (Tr) and reduced pressure (Pr) generalised correlations
Why? Because of general application to all liquid and gas:
“ All fluids, when compared at the same Tr and Pr have approximately the same compressibility factor, and all deviate from the ideal gas behaviour to about the same degree.”
Compressibility factor, Z = PV/RT = Z (Tr, Pr, Zc)
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Generalised correlation - Gas
Most popular type: Pitzer correlation
Uses compressibility factor, Z and second virial coefficient, B
Values for Zo and Z1 (functions of Tr and Pr, can be referred from the
Lee Kesler Tables in App E1-E4 through interpolation)
Validity:
1) Non-polar or slightly polar gases
Example: CO2, 02, H2, N2 and hydrocarbons
2) Low to moderate pressures
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Generalised correlation - Gas
Pitzer correlation for the second virial coefficient
Objective: simplify calculations as compared to Zo and Z1
onlyToffunctionsareBandB
TBand
TBwhere
BBB
RT
BPBtcoefficienvirialondreducedthewhere
T
PBZ
r
rr
c
c
r
r
10
2.4
1
6.1
0
10
172.0139.0
422.0083.0
ˆ
ˆ,sec
ˆ1
w
For the third virial coefficient, refer to pg 103 of the textbook
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Examples: EOS problems
Problem 3.10
Determine the molar volume of n-butane at 510K and 25 bar using the following methods:
a) The ideal gas equation
b) The generalised compressibility-factor correlation
c) The generalised correlation for
B̂
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Problem 3.10 (a)
Ideal gas law: PV = RT
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Problem 3.10 (b)
Generalised compressibility factor correlation
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Problem 3.10(b)
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Problem 3.10(c)
2.4
1
6.1
0
10
172.0139.0
422.0083.0
ˆ
ˆ
ˆ1
rr
c
c
r
r
TBand
TBwhere
BBB
RT
BPBwhere
T
PBZ
w
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Examples of EOS problems
Question 3.11:
What pressure would be generated if 1 1b-mol methane were stored in a volume of 2 ft3 at 122oF.
Make use of :
(a) The ideal-gas law
(b) The Redlich-Kwong equation
(c) A generalized correlation
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3.11 (a) ideal gas law
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3.11(b) Redlich-Kwong
From Equations in pg 94 and App B1 (Tc and Pc),
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3.11(c): A generalised correlation
We have the option of compressibility factor Z method or
virial correlation B.
Which should we use? - Check pressure value – small or large? - Methane is non-polar Looking at (a) & (b) answer, P is rather high (moderate)
and the gas in non-polar, So we can use either one of the generalised correlation So let us try using Z method: P=ZRT/V
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3.11(c): A generalised correlation
As P is unknown, Pr cannot be determined but Pc can be obtained for methane in App B1
Start assuming values for Z, start with Z = 1,
Use properties of Pr and Tr based on Z=1
Compare with Z = Zo + wZ1….(Eq 3.57)
Stop when guessed Z is the same as Z in (Eq 3.57)
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3.11(c): A generalised correlation
Z = 0.89 gives the equivalent results
Discussion
1) Both Redlich Kwong and generalised correlation gave the
same results = 189 atm
2) This is similar to experimental value
3) Ideal gas equation gave a result almost 15% higher.
Optionally you can try the second virial generalised correlation
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Generalized Correlation for Liquids
Though molar volumes of liquids can be estimated by generalized cubic equations of state, result are not very accurate for saturated liquids.
Generalized equations available for estimating molar volumes of saturated liquids.
By Rackett
Only critical constant data is required
])1(1[ 7/2Tr
c
r
r ZT
PZsat
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Fig 3.16 : Generalised density correlation for liquids
Two parameter corresponding-states correlation for liquid volume estimation
Saturated
Liquid
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Example of EOS problems
Question 3.13
For ammonia at 310K, estimate the density:
(a) The saturated liquid
(b) The liquid at 100 bar
Phase: liquid/gas? Bond: polar/non-polar?
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3.13(a) saturated liquid
Data can be found in Appendix Table B.1 for Tr, Vc and Zc
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3.13(b) liquid at 100 bars
You can use two methods by using Fig 3.16
From notes, 1st option:
1)
r2
r1V1 V2
nscalculatio liquidsaturated
using
fromdatavolumeeapproximatelyalternativor
VV
r
C
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2)
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Additional notes:
Relates PVT of pure homogeneous fluid in equilibrium state
Volume expansivity, b Isothermal compressibility, K