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Opening new doors with Chemistry
THINK SIMULATION!
Advances in Thermophysical Property Prediction
24th Conference October 23-24, 2007
Peiming WangRonald SpringerMargaret Lencka
Robert YoungJerzy Kosinski
Andre Anderko
Scope
• OLI’s two thermodynamic models: aqueous and MSE
• Outline of the mixed-solvent electrolyte (MSE) thermodynamic model
• Application highlights• Summary of MSE databanks• Predictive character of the model• Modeling transport properties
• New model for thermal conductivity
• Model and databank development plans
Structure of OLI thermodynamic models (both aqueous and MSE)
• Definition of species that may exist in the liquid, vapor, and solid phases
• Excess Gibbs energy model for solution nonideality
• Calculation of standard-state properties• Helgeson-Kirkham-Flowers-Tanger equation for
ionic and neutral aqueous species• Standard thermochemistry for solid and gas
species
• Algorithm for solving phase and chemical equilibria
OLI Thermodynamic Models:Aqueous and MSE
• The difference between the models lies in• Solution nonideality model• Methodology for defining and regressing parameters
• Aqueous model• Solution nonideality model suitable for solutions with ionic
strength below ~30 molal and nonelectrolyte mole fraction below ~0.3
• Extensive track record and large databank
• MSE model• Solution nonideality model eliminates composition limitations• Development started in 2000 and model became commercial
in early 2006• Smaller, but rapidly growing databank• Includes many important systems not covered by the
aqueous model
MSE Framework
• Thermophysical framework to calculate• Phase equilibria and other properties in
aqueous and mixed-solvent electrolyte systems
Electrolytes from infinite dilution to the fused-salt limit
Aqueous, non-aqueous and mixed solvents Temperatures up to 0.9 critical temperature
of the system• Chemical equilibria
Speciation of ionic solutions Reactions in solid-liquid systems
Outline of the MSE model:Solution nonideality
RT
G
RT
G
RT
G
RT
G exII
exLC
exLR
ex
LR Debye-Hückel theory for long-range electrostatic interactions
LC Local composition model (UNIQUAC) for neutral molecule interactions
II Ionic interaction term for specific ion-ion and ion- molecule interactions
Excess Gibbs energy
i jxijji
ii
exII IBxxnRT
G
MSE thermodynamic model:Application highlights
• Predicting deliquescence of Na – K – Mg – Ca – Cl – NO3 brines
• Challenge: Simultaneous representation of water activity and solubility for concentrated multicomponent solutions based on parameters determined from binary and selected ternary data
• Phase behavior of borate systems• Challenge: Complexity of SLE patterns; multiple
phases
• Properties of transition metal systems• Challenge: Interplay between speciation and
phase behavior
Na – K – Mg – Ca – Cl – NO3
system
• Step 1: Binary systems – solubility of solids
• The model is valid for systems ranging from dilute to the fused salt limit
0
10
20
30
40
50
60
70
80
90
100
-20 0 20 40 60 80 100 120 140 160 180 200 220 240 260 280 300 320
Temperature, C
NaN
O3,
wei
ght
%
NaNO3
H2O(s)
Cal, NaNO3
Cal, H2O(s)
0
10
20
30
40
50
60
70
80
90
100
-40 -20 0 20 40 60 80 100 120 140 160 180 200
Temperature, C
Mg(
NO
3)2,
wei
ght
%
H2O(s)Mg(NO3)2.9H2OMg(NO3)2.6H2OMg(NO3)2.2H2OMg(NO3)2Cal, H2O(s)Cal, Mg(NO3)2.9H2OCal, Mg(NO3)2.6H2OCal, Mg(NO3)2.2H2OCal, Mg(NO3)2
NaNO3 – H2O
Mg(NO3)2 – H2O
Na – K – Mg – Ca – Cl – NO3
system: Step 1: Binary systems – water activity
• Deliquescence experiments
• Water activity decreases with salt concentration until the solution becomes saturated with a solid phase (which corresponds to the deliquescence point)
0
0.1
0.2
0.3
0.4
0.5
0.6
0.7
0.8
0.9
1
0 0.05 0.1 0.15 0.2 0.25 0.3 0.35 0.4 0.45 0.5 0.55 0.6 0.65
Total apparent salt, mole fraction
Wat
er a
ctiv
ity 1 - NaCl
6 - LiCl
11 - CaCl2
3 - Mg(NO3)2
12 - Ca(NO3)2Ca(NO3)2
LiCl
Mg(NO3)2
CaCl2.2H2O
NaCl
Step 2: Ternary systems• Solubility in the
system NaNO3 – KNO3 – H2O at various temperatures
• Activity of water over saturated NaNO3 – KNO3 solutions at 90 C: Strong depression at the eutectic point
0.35
0.4
0.45
0.5
0.55
0.6
0.65
0.7
0.75
0 0.1 0.2 0.3 0.4 0.5 0.6 0.7 0.8 0.9 1
NaNO3, mole fraction (water free)
Wat
er A
ctiv
ity KNO3
NaNO3+KNO3
NaNO3
0
10
20
30
40
50
60
70
80
90
0 5 10 15 20 25 30 35 40 45 50 55 60 65 70 75 80 85 90 95
KNO3, weight %
NaN
O3,
wei
ght
%
0C 10C20C 25C30C 40C50C 75C100C 125C150C 175C200C
NaNO3(s)
KNO3(s)
NaNO3.KNO3(s)
Step 3: Verification of predictions for multicomponent systems
• Deliquescence data simultaneously reflect solid solubilities and water activities
• Break points reflect solid-liquid transitions
0
0.1
0.2
0.3
0.4
0.5
0.6
0.7
0.8
0.9
1
0 0.1 0.2 0.3 0.4 0.5 0.6 0.7 0.8 0.9 1
Total apparent salt, mole fraction
Wat
er a
ctiv
ity
10 - NaNO3+KNO3
4 - NaNO3+KNO3+Ca(NO3)2+Mg(NO3)2
NaNO3
NaNO3+NaNO3.KNO3
NaNO3
NaNO3+Ca(NO3)2
Mixed nitrate systems at 140 C
Borate chemistry:Complexity due to multiple competing solid phases
Na – B(III) – H – OH system
t=94C0
5
10
15
20
25
30
35
0 1 2 3 4 5
m0.5 Na2O
m B
2O3
H3BO3Na2O.5B2O3.10H2O2Na2O.5.1B2O3.7H2ONa2O.2B2O3.4H2O2Na2O.5B2O3.5H2ONa2O.B2O3.4H2ONa2O.B2O3.H2O
t=60C
0
2
4
6
8
10
12
14
0 1 2 3 4 5
m0.5 Na2O
m B
2O3
H3BO3
Na2O.5B2O3.10H2O
2Na2O.5.1B2O3.7H2O
Na2O.2B2O3.5H2O
Na2O.2B2O3.4H2O
Na2O.2B2O3.10H2O
Na2O.B2O3.4H2O
Na2O.B2O3.H2O
Na2O.B2O3.H2O
NAOH.1H2O
Borate chemistry:Complexity due to multiple competing solid phases
Ca – B(III) – H – OH
0
0.1
0.2
0.3
0.4
0.5
0.6
0.7
0.8
0.9
1
0 0.01 0.02 0.03 0.04 0.05m CaO
m B
2O3
Rza-Zade (1964) - Ca(OH)2
Rza-Zade (1964) - 1:1:4
Rza-Zade (1964) - 2:3:9
Rza-Zade (1964) - 1:3:4
Rza-Zade (1964) - BH
Ca(OH)2PPT
H3BO3PPT
CaB2O4.4H2O
CaB6O10.4H2O
CaB6O10.4H2O
Ca2B6O11.9H2O
Ca2B6O11.9H2O
Mg – B(III) – H – OH
00.10.2
0.30.40.50.60.7
0.80.9
1
0 0.01 0.02 0.03 0.04 0.05 0.06 0.07 0.08m MgO
m B
2O3
1 - MH 4 - MH 5 - MH2 - MH 1 - 2:3:15 4 - 2:3:152 - 2:3:15 5 - 2:3:15 1 - 1:2:94 - 1:2:9 5 - 1:3:7.5-metast. 5 - 1:3:7.51 - 1:3:7.5 4 - 1:3:7.5 2 -1:3:7.52 - BH 1 - BH 4 - BH25C - MH - calc. 25C - 2:3:15 - calc. 25C - 1:3:7.5 - calc.25C - B(OH)3 - calc.
Lead chemistry
• Solubility patterns are strongly influenced by speciation (Pb-Cl and Pb-SO4 complexation)
0.001
0.01
0.1
1
0.001 0.01 0.1 1 10 100HCl, molal
Pb
Cl 2
, mol
al
0C 25C 50C 80C 100C
0.000001
0.00001
0.0001
0.001
0.01
0.1
1
10
0.0001 0.001 0.01 0.1 1 10 100 1000
SO3, molal
Pb
SO
4, m
olal
0C
18C
25C
35C
50C
60C
127C
149C
166C
PbCl2 + HCl
PbSO4 + H2SO4
Lead chemistry
• With speciation and ionic interactions correctly accounted for, mixed sulfate – chloride systems are accurately predicted
0
0.001
0.002
0.003
0.004
0.005
0.006
0.007
0.008
0.009
0 0.2 0.4 0.6 0.8 1 1.2 1.4 1.6
HCl, molal
Pb
SO
4, m
olal
18C
25C
30C
37C
0.0001
0.001
0.01
0.1
0.001 0.01 0.1 1 10
NaCl, molal
Pb
SO
4, m
olal
18C
25C
30C
50C
70C
PbSO4 + HCl
PbSO4 + NaCl
Transition metal systems
• Specific effects of anions on the solubility of oxides
• Prediction of pH – accounting for hydrolysis of cations
0.0
0.5
1.0
1.5
2.0
2.5
3.0
3.5
0.0 1.0 2.0 3.0 4.0 5.0
molality
pH
CrCl3
Cr2(SO4)3 pH of Cr salts
0.000001
0.00001
0.0001
0.001
0.01
0.1
1
0.0001 0.001 0.01 0.1 1 10 100
concentration of ACID, mol/kg H2O
so
lub
ility
of
H2W
O4,
mo
l/kg
H2O
HNO3-20C
HNO3-20C-EXP
HNO3-50C
HNO3-50C-EXP
HNO3-100C
HNO3-100C-EXP
HCl-20C
HCl-20C-EXP
HCl-50C
HCl-50C-EXP
HCl-70C
HCl-70C-EXP
cc
Solubility of WO3 in acidicCl- and NO3
- environments
Mixed organic – inorganic systems
• Solubility of oxalic acid in mineral acid systems
0
10
20
30
40
50
60
70
80
90
100
0 10 20 30 40 50 60 70 80 90 100
w% H2SO4
w%
(C
OO
H)2
Hill et al. 1946, t=25CHill et al. 1946, t=60CWirth 1908, t=25CMSE, t=25CMSE, t=60C
0
10
20
30
40
50
60
70
80
90
100
0 10 20 30 40 50 60 70 80 90 100
w% HNO3
w%
(C
OO
H)2
Masson 1912, t=30CMSE, t=30C
0
10
20
30
40
50
60
70
80
90
100
0 10 20 30 40 50 60 70 80 90 100w% HCl
w%
(C
OO
H)2
Masson 1912, t=30CChapin and Bell 1931, t=0CChapin and Bell 1931, t=50CChapin and Bell 1931, t=80CMSE, t=0CMSE, t=30CMSE, t=50CMSE, t=80C
HNO3
H2SO4
HCl
Chemistry Coverage in the MSEPUB Databank (1)
• Binary and principal ternary systems composed of the following primary ions and their hydrolyzed forms • Cations: Na+, K+, Mg2+, Ca2+, Al3+, NH4
+
• Anions: Cl-, F-, NO3-, CO3
2-, SO42-, PO4
3-, OH- • Aqueous acids, associated acid oxides and acid-containing mixtures
• H2SO4 – SO3
• HNO3 – N2O5
• H3PO4 – H4P2O7 – H5P3O10 – P2O5
• H3PO2
• H3PO3
• HF• HCl• HBr• HI
•H3BO3
•CH3SO3H•NH2SO3H•HFSO3 – HF – H2SO4
•HI – I2 – H2SO4
•HNO3 – H2SO4 – SO3 •H3PO4 with calcium phosphates•H – Na – Cl – NO3•H – Na – Cl – F•H – Na – PO4 - OH
• Inorganic gases in aqueous systems • CO2 + NH3 + H2S• SO2 + H2SO4
• N2
• O2
• H2 • Borate chemistry
• H+ - Li+ - Na+ - Mg2+ - Ca2+ - BO2- - OH-
• H+ - Li+ - Na+ - BO2- - HCOO- - CH3COO- - Cl- - OH-
• Silica chemistry• Si(IV) – H+ - O - Na+
• Hydrogen peroxide chemistry • H2O2 – H2O – H - Na – OH – SO4 – NO3
Chemistry Coverage in the MSEPUB Databank (2)
• Transition metal aqueous systems • Fe(III) – H+ – O – Cl-, SO4
2-, NO3-
• Fe(II) – H+ – O – Cl-, SO42-, NO3
-, Br-
• Sn(II, IV) – H+ – O – CH3SO3-
• Zn(II) – H+ – Cl-, SO42-, NO3
-
• Zn(II) – Li+ - Cl-
• Cu(II) – H+ – SO42-, NO3
- • Ni(II) – H+ – Cl-, SO4
2-, NO3-
• Ni(II) – Fe(II) – H+ - O – BO2-
• Cr(III) – H+ - O – Cl-, SO42-, NO3
-
• Cr(VI) – H+ - O – NO3-
• Ti(IV) – H+ – O – Ba2+ – Cl-, OH-, BuO-
• Pb(II) – H+ - O – Na+ - Cl-, SO42-
•Mo(VI) – H+ – O – Cl-, SO42-,
NO3-
•Mo(IV) – H+ - O•Mo(III) – H+ - O•W(VI) – H+ - O – Na+ – Cl-, NO3
-
•W(IV) – H+ - O
Chemistry Coverage in the MSEPUB Databank (3)
• Miscellaneous inorganic systems in water • NH2OH
• NH4HS + H2S + NH3
• Li+ - K+ - Mg2+ - Ca2+ - Cl-
• Na2S2O3
• Na+ - BH4- – OH-
• Na+ - SO32- - SO2
- OH-
• BaCl2
• Most elements from the periodic table in their elemental form
• Base ions and hydrolyzed forms for the majority of elements from the periodic table
Chemistry Coverage in the MSEPUB Databank (4)
• Organic acids/salts in water and alcohols • Formic
H+ - Li+ - Na+ - Formate - OH-
Formic acid – MeOH - EtOH• Acetic
H+ - Li+ - Na+ - K+ - Ba2+ - Acetate - OH-
Acetic acid – MeOH – EtOH – CO2
• Citric H+ - Na+ - Citrate - OH-
• Oxalic H+ - Oxalate – Cl- - SO4
2-, NO3-,
MeOH, EtOH, 1-PrOH• Malic• Glycolic
•Adipic H+ - Na+ - AdipateAdipic acid – MeOH, EtOH
•NicotinicH+ - Na+ - NicotinateNicotinic acid - EtOH
•Terephthalic H+ - Na+ - TerephthalateTerephthalic acid – MeOH, EtOH
•IsophthalicIsophthalic acid - EtOH
•TrimelliticTrimellitic acid - EtOH
Chemistry Coverage in the MSEPUB Databank (5)
• Hydrocarbon systems • Hydrocarbon + H2O systems
Straight chain alkanes: C1 through C30 Isomeric alkanes: isobutane, isopentane, neopentane Alkenes: ethene, propene, 1-butene, 2-butene, 2-
methylpropene Aromatics: benzene, toluene, o-, m-, p-xylenes,
ethylbenzene, cumene, naphthalene, anthracene, phenantrene
Cyclohexane
• Hydrocarbon + salt generalized parameters H+, NH4
+, Li+, Na+, K+, Mg2+, Ca2+, Cl-, OH-, HCO3-, CO3
2- NO3-,
SO42-
Chemistry Coverage in the MSEPUB Databank (6)
• Organic solvents and their mixtures with water • Alcohols
Methanol, ethanol, 1-propanol, 2-propanol, 1-butanol, cyclohexanol
• Glycols Mono, di- and triethylene glycols, propylene glycol,
polyethylene glycols• Phenols
Phenol, catechol• Ketones
Acetone, methylisobutyl ketone • Aldehydes
Butylaldehyde• Carbonates
Diethylcarbonate, propylene carbonate
Chemistry Coverage in the MSEPUB Databank (7)
• Organic solvents and their mixtures with water • Amines
Tri-N-octylamine, triethylamine, methyldiethanolamine
• Nitriles Acetonitrile
• Amides Dimethylacetamide, dimethylformamide
• Halogen derivatives Chloroform, carbon tetrachloride
• Aminoacids Methionine
• Heterocyclic components N-methylpyrrolidone, 2,6-dimethylmorpholine
Chemistry Coverage in the MSEPUB Databank (8)
• Polyelectrolytes• Polyacrylic acid
Complexes with Cu, Zn, Ca, Fe(II), Fe(III)
• Mixed-solvent inorganic/organic system • Mono, di- and triethylene glycols - H – Na – Ca – Cl – CO3 – HCO3 - CO2 – H2S
– H2O • Methanol - H2O + NaCl, HCl• Ethanol – LiCl - H2O• Phenol - acetone - SO2 - HFo - HCl – H2O• n-Butylaldehyde – NaCl - H2O • LiPF6 – diethylcarbonate – propylene carbonate
• Mixed-solvent organic systems • HAc – tri-N-octylamine – toluene – H2O• HAc – tri-N-octylamine – methylisobutylketone – H2O • Dimethylformamide – HFo – H2O• MEG – EtOH – H2O
Chemistry Coverage in the MSEPUB Databank (9)
• GEMSE databank• MSE counterpart of the GEOCHEM databank
Minerals that form on an extended time scale• Contains all species from GEOCHEM• 7 additional silicates and aluminosilicates have been
included
• CRMSE databank• MSE counterpart of the CORROSION databank
Various oxides and other salts that may form as passive films but are unlikely to form in process environments
Chemistry Coverage in the MSEPUB Databank (10)
Predictive character of the model
• Levels of prediction• Prediction of the properties of multicomponent
systems based on parameters determined from simpler (especially binary) subsystems
Extensively validated for salts and organics Subject to limitations due to chemistry changes (e.g.
double salts)
• Prediction of certain properties based on parameters determined from other properties
Extensively validated (e.g.,speciation or caloric property predictions)
Predictive character of the model
• Levels of prediction - continued• Prediction of properties without any knowledge of
properties of binary systems Standard-state properties: Correlations to predict the
parameters of the HKF equation Ensures predictive character for dilute solutions
Properties of solids: Correlations based on family analysis
Parameters for nonelectrolyte subsystems Group contributions: UNIFAC estimation Quantum chemistry + solvation: CosmoTherm estimation
Also has limited applicability to electrolytes as long as dissociation/chemical equilibria can be independently calculated
Determining MSE parameters based on COSMOtherm predictions
• Solid-liquid-liquid equilibria in the triphenylphosphate-H2O system
• Only two data points are available: melting point and solubility at room T
• Predictions from COSMOtherm are consistent with the two points and fill the gaps in experimental data
0
50
100
150
200
250
300
1E-05 1E-04 0.001 0.01 0.1 1 10 100
%w TPP
t/C
Saeger, Hicks et al. 1979
Merck
NIST
COSMOtherm
COSMOtherm 2nd phase
MSE LLE
MSE LLE 2nd phase
MSE SLE
Determining MSE parameters based on COSMOtherm predictions
• Solid-liquid-liquid equilibria in the P-H2O system
• Predictions from COSMOtherm are shown for comparison
0
50
100
150
200
250
300
0.0001 0.001 0.01 0.1 1 10 100
%w P4
t/C
Stich 1953 SLEMerck SLEMSE SLEMSE SLE extrapolatedMSE LLEMSE LLE 2nd liquidCOSMOtherm LLECOSMOtherm LLE 2nd liquid
Transport properties in the OLI software
• Available transport properties:• Diffusivity• Viscosity• Electrical conductivity
• These models were developed first in conjunction with the aqueous model and then extended to mixed-solvent systems
• A new model for calculating thermal conductivity has been recently developed
,,, ,ikii'j xxf sss elec
elecms 0
ms0 ̶ thermal conductivity of the mixed
solvent
Δelec ̶ contribution of electrolyte
concentrationDerived from a local composition approach
contribution of individual ion
species-species interaction
,,,0jljjj kwqf 0
ms
Thermal Conductivity in Mixed-Solvent Electrolyte Solutions
organic + water mixtures at 20ºC
cyclohexane + CCl4 + benzene and cyclohexane + CCl4 + toluene
0.10
0.20
0.30
0.40
0.50
0.60
0.70
0.0 0.2 0.4 0.6 0.8 1.0
X-H2O
, W
.m-1
.K-1
acetone-1966RG
ethanol-1997LHLethanol-1966RG
ethanol-1938BHPmethanol-1938BHP
methanol-1966RGisopropanol-1966RG
-5.0
0.0
5.0
0.0 0.2 0.4 0.6 0.8 1.0
x-cyclohexane
10
0*(
exp-
cal)/
exp
Toluene+CCl4+cyclohexane@40C
Toluene+CCl4+cyclohexane@25C
Benzene+CCl4+cyclohexane@40C
Benzene+CCl4+cyclohexane@25C
Thermal conductivity of solvent mixtures
KNO3+water P2O5+water
0.35
0.40
0.45
0.50
0.55
0.60
0.65
0.70
0.00 0.25 0.50
x-P2O5
, W
.m-1
.K-1
0C-1999A20C-1951R20C-1999A25C-1999A25C-1971T25C-1969LW25C-DIPPR29C-1951R50C-1969LW50C-1999A50C-DIPPR75C-1969LW75C-1999A75C-DIPPR100C-1969LW100C-1999A100C-DIPPR125C-1969LW125C-DIPPR150C-1969LW150C-DIPPR
pure liquid H3PO4
0.35
0.40
0.45
0.50
0.55
0.60
0.65
0.70
0.0 0.2 0.4 0.6 0.8 1.0
(x-KNO3)1/2
, W
.m-1
.K-1 20C
60C
100C
150C
200C
338C
Aqueous Electrolytes from Dilute to Concentrated Solutions
ZnCl2+ethanol ZnCl2+ethanol+water
0.154
0.156
0.158
0.160
0.162
0.164
0.166
0.168
0.170
0.172
0.174
0.00 0.05 0.10 0.15 0.20
x-ZnCl2
, W
.m-1.K
-1
25C
40C
60C
70C0.00
0.10
0.20
0.30
0.40
0.50
0.60
0.70
0.0 0.2 0.4 0.6 0.8 1.0
X'-ETHANOL
, W
.m-1.K
-1
ZnCl2=0 (exp)ZnCl2=10 wt% (exp)ZnCl2=25 wt% (exp)ZnCl2=0ZnCl2=10wt%ZnCl2=25 wt%
0.15
0.16
0.17
0.18
0.8 0.9 1.0
X'-ETHANOL
l, W
.m-1
.K-1
Electrolytes in Non-aqueous and Mixed Solvents
Further Development of MSE
• Thermophysical property models• Implementation of thermal conductivity in OLI software• Development of a surface tension model
• Major parameter development projects• Refinery overhead consortium (in collaboration with SwRI)
Development of parameters for amines and amine hydrochlorides
• Hanford tank chemistry in MSE• Modeling hydrometallurgical systems (University of Toronto)• Transition metal chemistry including complexation• Natural water chemistry (including common scales) with
methanol and glycols • Urea chemistry• Other projects as defined by clients
Summary • OLI’s two thermophysical property packages
• Mixed-solvent electrolyte model Thermophysical engine for the future General, accurate framework for reproducing the
properties of electrolyte and nonelectrolyte systems without concentration limits over wide ranges of conditions
Parameter databanks are being rapidly expanded New thermophysical properties (thermal conductivity,
surface tension) are being added
• Aqueous model Widely used and reliable Continues to be maintained and parameters continue to
be added as requested by clients