Carbon Dioxide Properties and the Role of Impurities in the Subsurface
J P Martin Trusler
Department of Chemical Engineering &
Qatar Carbonates and Carbon Storage Research Centre Imperial College London, U.K.
UKCCS Research Centre, Biannual Meeting, Cardiff, 10 September 2014
CCS, CO2 Properties, Mixtures and Impurities
• Fluid properties are fundamental to all aspects of CCS • But it’s not just CO2 – many complex mixtures involved:
– Fuels and combustion gases from which CO2 is captured – Mixtures formed with inevitable impurities – Mixtures formed with brine and/or hydrocarbons when the injected
into a geological storage sink
• Hence there are huge variety of complex mixtures involved • Also a very wide range of conditions in CCS from low
pressures to 100 MPa, cryogenic temperatures to 1000°C • And a need to understand physical and chemical properties
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CCS Landscape, Properties, Mixtures and Impurities
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0.1
1
10
100
200 250 300 350 400
p/M
Pa
T/K
Gas
Liquid
Solid Super-Critical Fluid
Pipeline Storage
Capture & Compression
Mixtures and Impurities • Diluents:
• N2 • O2 • H2
• Acid Gases: • H2S • SO2
• Aqueous species: • H2O • Salts
• Hydrocarbons: • Gas • Condensates • Oils
• Others: • NOx • Trace elements
• Phase behaviour • Density • Viscosity • Diffusion coefficients
• Interfacial tension • Contact angle • pH • Reactivity w/ minerals
Properties
Storage
• Focus on deep saline aquifers and depleted oil fields • Need to consider the mixtures formed when CO2 contacts
the reservoir fluid: brines and hydrocarbons • … and allow for impurities present in the CO2 stream • Would like to predict:
– rate of dissolution of CO2 and impurities – buoyancy and convective flow of the resulting solutions – reactivity towards reservoir minerals
• Controlling physical/chemical properties: – solubility, diffusion coefficients – density, viscosity – pH, rate constants
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Role of Impurities in the Subsurface
• Diluents – much less soluble in brine than CO2
– raise interfacial tension against brine – may build up in mixing/dissolution zones
• Other acid gases – more soluble than CO2
– lower interfacial tension against brine – reactive towards carbonate minerals
• Hydrocarbons – very low solubility in brine – unknown influence on CO2 storage in saline aquifers
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QCCSRC Research Programme
• Wide ranging programme aimed at understanding CO2 storage in carbonate reservoirs – Geology, geochemistry, geophysics – Multiphase reactive flow in porous media – Thermophysical properties – Reservoir modelling
• Thermophysical properties work packages – Phase I: CO2/brines/hydrocarbon systems - Completed – Phase II: Effects of impurities in the CO2 stream - Active – Both involving experimental measurements and modelling
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QCCSRC Thermophysics Workflow
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Water
CO2
Impurities
Hydrocarbons
Minerals
pVT:Analytical VLESynthetic VLE
Density
Mol
ecul
ar M
odel
ling
Interfacial Properties:
IFTContact angle
Chemical Properties:
KineticspH
Salts
Oil - CO2Systems
Brine - CO2Systems
Brine - CO2 -MineralSystems
Components Mixtures Properties Outputs
Data
Needs
Data
Needs
Data
Needs
Experiment design
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Interfacial Tension of CO2 + Brines at Reservoir Conditions
Significance: Interfacial tension γ and contact angle θc determine the capillary entry pressure pc for a pore of radius r, and thus the over pressure needed to displace brine by CO2 during an injection process Young-Laplace equation: pc = (2γ/r) cosθc
Pendant-Drop Apparatus for Interfacial Tension
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P
DE DE
R0 θ
x θ
y
DS
O
Hastelloy and titanium cells rated for p = 50 MPa at T = 473 K.
Vent
P4
P2
P3
P1
Magnetic Stirrer Bar
V2
V1
N2
N1
Vent
V3
V4
V5
V6
Inlet 1
Inlet 2
Inlet 3
Inlet 4
C1
T
P
V7
βρΔgRγ /20=
IFT of (0.864 NaCl + 0.136 KCl) (aq) at m = 3 mol·kg-1
10
25
35
45
55
65
75
0 10 20 30 40 50
γ/(m
N/m
)
p/MPa
323.15 K
423.15 K
T = 298.15 K
25
35
45
55
65
75
0 10 20 30 40 50
γ/(m
N/m
)
p/MPa
Liquid-Liquid
Gas-Liquid
Pure water Pure brine
T > Tc
Li et al. J. Chem. Eng. Data. DOI: 10.1021/je201062r (2012).
IFT for the (CO2 + N2 + H2O) System
11
15
25
35
45
55
65
75
0 10 20 30 40
Υ/m
N∙m
-1
p/MPa
15
25
35
45
55
65
75
0 10 20 30 40Υ
/mN
∙m-1
p/MPa
15
25
35
45
55
65
75
0 10 20 30 40
Υ/m
N∙m
-1
p/MPa
15
25
35
45
55
65
75
0 10 20 30 40
Υ/m
N∙m
-1
p/MPa
298 K 323 K
373 K 448 K
N2 + H2O correlation
CO2 + H2O correlation
(0.5CO2 + 0.5N2) + H2O data
Mole-fraction-weighted average
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Phase Behaviour of CO2 with Brines at Reservoir Conditions
Measurements with: • Static-Analytic Apparatus for Coexisting Water- and CO2-Rich Phases • Static-Synthetic Apparatus for CO2 Solubility in Brines
Static-Analytic Apparatus (298 to 450) K @ p ≤ 50 MPa
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`
30.000 C
Temperature Readout
Gas Chromatography
1320
Pressure Transducer
Brine
Hydrocarbon
CO2 Magnetic Pump
Equilibrium Cell
Thermometer Probe
Rolsi Valve
Filter
Vindum Valve
Cross
Reducer
Tee
Vaccum Pump
Drain
Safety Head
Needle Valve
Check Valve
Tube Heater
Results for CO2 + NaCl(aq)
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T = 323.15 K • Measurements from 298 K to 443 K with pressures to 18 MPa
• Modelling with asymmetric approach:
• eNRTL for the aqueous phase
• Peng-Robinson EoS for the gas phase
• Good account of CO2 solubility in the liquid phase
• Imperfect description of the gas phase
Hou et al. J. Chem. Eng. Data. DOI: 10.1016/j.supflu.2013.03.022 (2013).
T = 423.15 K
Static-Synthetic Apparatus (298 to 473) K @ p ≤ 50 MPa
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Vacuum
P
SP
C1
V2 V1
T
V3 Drain
V4
PG
• Little CO2 solubility data have been reported for complex brines under reservoir conditions
• Interest in mixed brines, including bivalent cations such as Ca2+, Mg2+
• pH is also of special interest
Solubility of CO2 in MgCl2(aq)
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, T = 309 K; , T = 345 K; , T = 375 K; , T = 424 K
• Experimental measurements from 309 K to 424 K with pressures up to 35 MPa • CaCl2(aq) also studied • Modelling with Krichevsky-Kasarnovski model:
RTppVHxf /)(ln)/ln( ref11211 −+= ∞
m = 1 mol/kg m = 3 mol/kg m = 5 mol/kg
Tong et al. J. Chem. Eng. Data. DOI: 10.1021/je400396s (2013).
Other QCCSRC Thermophysics Research
Completed: • Viscosity of CO2-saturated water/brine • Diffusion coefficients of CO2 and N2 in water/brine • Kinetics of carbonate dissolution in CO2-saturated water • pH of CO2 saturated water/brine • Phase behaviour studies of CO2-hydrocarbon mixtures In progress: • Coexisting phase densities of CO2 + water • Solubility of H2S and SO2 in water and brine at HTHP • More phase behaviour studies of CO2-hydrocarbon mixtures • Effect of impurities on CO2-water IFT • Solubility of light hydrocarbons in water/brine
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Research Team: • John Crawshaw • Shuxin Hou • Saif Al Ghafri • Yolanda Sanchez • Mihaela Stevar • David Vega • Chidi Efika • Shane Cadogan • Xuesong Li • Cheng Peng
• Mark McBride-Wright
• Benaiah Anabaraonye
• Claudio Calabrese
• Florence Chow • Rayane Hoballah • Ruien Hu
Acknowledgements
Co-Investigators • Geoff Maitland • Edo Boek Collaborators • Amparo Galindo • George Jackson • Andrew Haslam • Velisa Vesovic
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We gratefully acknowledge funding from QCCSRC, provided jointly by Qatar Petroleum, Shell, and Qatar Science & Technology Park