water-hydrocarbon phase behavior...
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Water Content of Sweet and Sour Natural Gas
Water-Hydrocarbon Phase Behavior
Learning Objectives
By the end of this lesson, you will be able to:
Estimate the water content of sweet and sour natural gas.
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By the end of this lesson, you will be able to:
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Operational Concerns
• Liquid water aides in corrosion.
• Liquid water may cause hydrates to form at room temperature (hydrates can be thought of as dirty ice that burns).
• Liquid water can freeze to ice at cold temperatures.
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Water in natural gas is a concern because:
Water Content of Sweet Natural Gas
• Chart accuracy is between 6% and 10%, which is probably more accurate than the underlying data used to develop the correlation
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The saturated water content of natural gas depends on temperature (T), pressure (P) and composition.
Generalized pressure-temperature correlations can be used for sweet, lean natural gas.
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Water Content of Sweet, Lean Natural Gas (SI Units)
Constant Pressure Curves
Water Content
Is water content more sensitive to changes in temperature or pressure? Let’s work this together by filling in the following Table in SI units:
5 MPa (725 psia)
10 MPa(1450 psia)
30 C (86 F)
40 C (104 F)
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5 MPa (725 psia)
10 MPa(1450 psia)
30 C (86 F)
40 C (104 F)
Water Content
Water content is very sensitive to temperature
The effect of pressure on water is much less
800 500
1300 840
What Are Hydrates and How They Are Formed
Water/Hydrocarbon Phase Behavior Core
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Learning Objectives
By the end of this lesson, you will be able to:
Describe what are hydrates and how they are formed. System temperature
System pressure
The presence of water-saturated gas The composition of the gas stream
By the end of this lesson, you will be able to:
Hydrate Formation
Hydrates are composed of light hydrocarbon molecules (plus CO2, H2S and N2) and water.
Hydrates can form at temperatures well above the freezing point of water.
Hydrate formation temperature depends on the gas composition and pressure.
Hydrates typically form when liquid water is present in the system however this is not a requirement.
The gas must be water saturated to form hydrates.
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Hydrate Formation
Hydrates consists of a lattice that traps molecules.
The lattice is formed by water molecules, which are connected by hydrogen bonds.
The molecules that build the lattice are called “host” molecules.
The cage structures in the lattice are occupied or filled by “guest” molecules.
The molecules that fill the lattice are primarily light hydrocarbons.
Hydrates can form at temperatures well above the freezing point of water and can block the flow through pipelines and process equipment.
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Schematic of Natural Gas Hydrate Lattices
Structure IRadius ≈ 4.3 Å
Structure HRadius ≈ 5.7 Å
Structure IIRadius ≈ 4.7 Å
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Schematic of Natural Gas Hydrate Lattices
Structure IRadius ≈ 4.3 Å
Structure HRadius ≈ 5.7 Å
Structure IIRadius ≈ 4.7 Å
Stabilized by:• Methane• Ethane• Carbon dioxide• Hydrogen sulfide
Schematic of Natural Gas Hydrate Lattices
Structure IRadius ≈ 4.3 Å
Structure HRadius ≈ 5.7 Å
Structure IIRadius ≈ 4.7 Å
Stabilized by:• Methane• Hydrogen sulfide• Propane• Iso-butane
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Schematic of Natural Gas Hydrate Lattices
Structure IRadius ≈ 4.3 Å
Structure HRadius ≈ 5.7 Å
Structure IIRadius ≈ 4.7 Å
Stabilized by:• Methane• Hydrogen sulfide• Neohexane• Cyclohexane• Cycloheptane
Gas Hydrates
• Pipelines / Flowlines
• Wellbores
• Process piping
• Heat exchangers
• Expansion devices – Valves, expanders
• Separator internals
Potential Hydrate Deposition Locations
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Hydrate Forming Conditions for Natural Gas Components
i-Butane
n-Butane
Phase Behavior of Propane Water System
1.00.90.80.7
0.6
0.5
0.4
0.3
0.2
0.10.090.080.07
0.06
0.05-20 -15 -10 -5 0 5 10
Temperature, °C
78910
20
30
40
50
60
708090100
14550403020100
Temperature, °F
Propane Vapor + Water
Liquid Propane + WaterLiquid Propane
+ Ice + Hydrate
Propane Vapor + Hydrate + Ice
Propane Vapor + Ice
Propane Vapor + Hydrate
Liquid Propane +
Hydrate
Quadruple point
Hydrates
Ice
NoHydrates
Propane = liquid
Propane = vapor
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General Hydrate Formation Characteristics of a Gas Mixture
T
P Hydrocarbon Bubble Point Line
Hydrate Curve
WaterDewpoint Line
CG
H
E
FHydrocarbon
Dewpoint Line
1234
hydrocarbon vaporhydrocarbon liquid
liquid waterhydrates
Hydrate Formation Temperature
Water/Hydrocarbon Phase Behavior Core
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Learning Objectives
By the end of this lesson, you will be able to:
Estimate the hydrate formation temperature of a natural gas stream.
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Note:
The methods discussed in this lesson are based on the measurement of the hydrate melting point.
The hydrate melting point is also called the hydrate dissociation point.
The actual hydrate formation temperature will be lower than the hydrate dissociation temperature.
The accuracy of all these correlations, including computer simulations, is at best +/- 1°C (2°F).
By the end of this lesson, you will be able to:
Estimating the Hydrate Formation Temperature
Hydrate Formation Temperature (HFT) as a function of pressure and relative density.
Empirical Correlations (developed based on empirical data).
• Katz Method• Trekell-Campbell
Method• The McLeod-
Campbell Method
Equation of State (EOS) correlations.
The Baille and WichertMethod.
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Pre
ssu
re,
Mp
a(a
bs)
Pre
ssu
re,
psi
a
Temperature, °C
Temperature, °F
Conditions for Formation of Natural Gas Hydrates
Methane
Relative Density 0.6
Relative Density 0.7
Relative Density 0.8
• Work the exercise in SI or FPS units
Guided Exercise
Estimate the hydrate formation temperature of a sweet, lean natural gas with a relative density of 0.7 at 6.9 Mpa (1000 psia).
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Temperature, °F
Temperature, °C
Pre
ssu
re, p
sia
Pre
ssu
re, M
pa
(ab
s)
Solution (In SI Units)
18
Conditions for Formation of Natural Gas Hydrates
ROT: The HFT of a typical natural gas stream at 69 bar [1000 psia] is 18 °C [65 °F]
Solution (In FPS Units)
65ROT: The HFT of a typical natural gas stream at 69 bar [1000 psia] is 18oC [65oF]
Conditions for Formation of Natural Gas Hydrates
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The Impact of N2, Acid Gases and Light Hydrocarbons on the Sweet Gas Hydrate Formation Curve
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Component N2 CO2 H2S CH4 C2H6 C3H8 iC4 nC4 iC5 nC5 C6 C7 H2O Total
Mol % 0.031 0.000 0.000 85.620 7.886 3.758 0.595 0.785 0.372 0.220 0.127 0.486 0.121 100.0
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Temperature, °C
Pre
ssu
re,
kPa
Pre
ssu
re,
Psi
a
Temperature, °F
1800
1600
1400
1200
1000
800
600
400
200
0
32 42 52 62 72 82
0
1000
2000
3000
4000
5000
6000
7000
8000
9000
10000
11000
12000
332822171160
Preventing Hydrate Formation
Water/Hydrocarbon Phase Behavior Core
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Learning Objectives
By the end of this lesson, you will be able to:
Describe methods to prevent hydrate formation.
By the end of this lesson, you will be able to:
Hydrates can only form when the gas is saturated with water
Injecting chemicals can inhibit hydrate formation Chemical inhibitors:
− Thermodynamic inhibitors− Low Dosage Hydrate Inhibitors (LDHI)
Dehydrate the gas.
Maintain gas temperature above the hydrate formation temperature.
Maintain the gas pressure below the hydrate formation pressure.
Inject chemical inhibitors.• Thermodynamic (equilibrium) inhibitors
– Monoethylene glycol (MEG)
– Methanol (MeOH)• Low Dosage Hydrate Inhibitors (LDHIs)
– Kinetic
– Anti-agglomerate
Hydrate Prevention Options
Lower hydrate formation temperature
Does not lower hydrate formation temperature
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J
I
Thermodynamic Inhibitors in Pipelines
Tcold
Pop
I
IJJ
HydrocarbonBubble Point Line
Hydrocarbon Dewpoint Line
H
G
E
C
F
Water DewpointLine
HydrateCurve
J
I
Water DewpointLine
General Hydrate Formation Characteristics of a Gas Mixture
Tcold
Pop
HydrocarbonBubble Point Line
Hydrocarbon Dewpoint Line
H
G
E
C
F
Water DewpointLine
HydrateCurve
D
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Hydrate Depression vs. Inhibitor Concentration in Mol%, Comparison of Correlation and Data
HammerschmidtKi = 1297 (2335)
Nielsen & Bucklin
d, °
C
d, °
F
25 wt% MEG RR -92
50 wt% MEG RR -92
25 wt% MeOH RR -9250 wt% MeOH RR -92
50 wt% MeOH RR -10670 wt% MEG RR -205
60 wt% MeOH RR -106
73.7 wt% MeOH RR -106
85 wt% MeOHRR -106
Inhibitor Concentration, mol%
Pipelines typically have hydrate depression points at or below 20°C or 36°F
The hydrate depression in a gas processing facility is often higher
The Neilsen-Bucklin equation would provide more accurate results for hydrate depressions greater than 20°C or 36°F
10 20 30 40 50 60 70 80 90
mi mW
XRXL XR
Lean Inhibitor Concentration in Weight Percent
Rich Inhibitor Concentration in Weight Percent
This equation allows us to calculate the mass flow of inhibitor solution mi
• The mass of lean liquid inhibitor available to combine with the free water in the system
It does not account for losses due to vaporization or solubility in liquid hydrocarbons
Mass Flow of Inhibitor Solution
Lean Inhibitor Concentration in Weight Percent
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Methanol Losses to Hydrocarbon Vapor Phase
Methanol partitions to vapor phase because of its high vapor pressure compared to water
Thermodynamic inhibitors must be in the liquid phase to depress the hydrate point
Vapor Pressure at 20 °C, kPa
Vapor Pressure at 68 °F, psia
MeOH 12.8 1.876
Water 2.3 0.33
MEG 0.0075 0.0011MEG 0.0075 0.0011
Summary of Results Lean and Rich Inhibitor Concentrations
XL, wt% XR, wt% mI, kg/d
MeOH 100 23 51.4
MEG 80 39 164
XL, wt% XR,wt% mI, lbm/day
MeOH 100 23 108
MEG 80 39 343
SI
FPS
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FPS
SI
Summary of Results when Vapor Losses are Accounted for
XL, wt% XR, wt% mI, kg/d Vapor Losseskg/d
Total Inj. RateKg/d m3/d
MeOH 100 23 51.4 98.6 148.2 0.19
MEG 80 39 164 Nil 164 0.15
XL, wt% XR,wt% mI, lbm/day
Vapor Losses lbm/day
Total Inj. Ratelbm/day gpm
MeOH 100 23 108 212.8 320.8 0.034
MEG 80 39 343 Nil 343 0.026
Density of MEG = 1100 kg/m3 (9.19 lbm/US gal)Density of MeOH = 800 kg/m3 (6.64 lbm/US gal)
Liquid-Liquid Distribution Ratios for Methanol and Hydrocarbons
No Toluene
28 – 33 Mol% Toluene
50 – 70 Mol% Toluene
70 – 80 Mol% Toluene
Distribution of methanol between aqueous and hydrocarbon phases, data from various sources. Hydrocarbon phases includes various alkane and cycloalkane compounds. Data shows the variation of distribution with changes in the amount of toluene in the hydrocarbon phase.
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wt% MEG in Aqueous Solution
Tem
per
atu
re, °
C
Tem
per
atu
re, °
F
Freezing Points of MEG-Water Solutions
= RR -205(Ref. 6.54) Experimental DataNote: Shaded region represents range of experimental data where freezing may have been observed.
Methanol or MEG?
Applications that require continuous injection typically use MEG. MEG can easily be regenerated but will only inhibit down to - 40 C (- 40 F). Per unit volume, it is relatively expensive compared to methanol.
Methanol is generally used in applications that have intermittent inhibition requirements, such as start-ups or shutdowns, or during periods of cold weather. It can inhibit down to - 100 C (- 148 F). Methanol contamination in both vapor and liquid hydrocarbon phases is becoming a significant issue.
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Typical Mechanical Refrigeration Plant with MEG Injection System (for Rich Wet Inlet Gas)
Low Dosage Hydrate Inhibitors vs.
Thermodynamic Inhibitors
Water/Hydrocarbon Phase Behavior Core
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Learning Objectives
By the end of this lesson, you will be able to:
Describe the differences between low dosage hydrate inhibitors (LDHI) and thermodynamic inhibitors.
By the end of this lesson, you will be able to:
Low Dosage Hydrate Inhibitors vs. Thermodynamic Inhibitors
LDHIs do not change the equilibrium hydrate formation temperature.
LDHIs require much lower concentration levels compared to thermodynamic inhibitors.
Typical concentrations for LDHIs range from 1000 to 10 000 parts per million by weight.
Thermodynamic inhibitors typically require between 200,000 and 400,000 parts per million by weight.
Compared to methanol and glycols, LDHI’s lower concentration levels often outweigh their higher unit cost.
Advantages of LDHIs include lower inhibitor losses, reduced capital and operating costs, and lower toxicity.
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Heating
Hydrate Formation
Subcooling = TE - TB
Pre
ssu
re
Temperature
A
B
CD
E
Start of Hydrate Formation
Hydrate May Form Here
Start of Dissociation
Thermodynamic Point
Kinetic Hydrate Inhibitors (KHIs)
KHIs inhibit hydrate formation by significantly reducing the rate of hydrate formation. They do not change the equilibrium hydrate formation temperature.
KHIs are currently limited to about 15.5 C (28 C) subcooling. The amount of subcooling required to form hydrates is time dependent. KHIs are most effective in systems where the fluid residence time is short.
KHIs are not effective in pipelines that are shut down if the pipeline temperature is below the hydrate formation temperature.
KHIs can be used in combination with methanol or glycol. The thermodynamic inhibitor reduces the equilibrium hydrate formation temperature and the KHI provides additional hydrate suppression by increasing the subcooling.
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Hydrate Prevention with Thermodynamic Inhibitor
With Inhibitor
Hydrates PipelineIn
Out
Thermodynamic Equilibrium Inhibitors (MEG and Methanol) lower hydrate formation temperature by freezing point depression.
Antiagglomerant Inhibitors (AAs)
Allow hydrates to form, but keep them suspended in the hydrocarbon liquid solution.
Were developed to extend the range of subcooling beyond the capabilities of KHIs.
May not be effective in systems that have high water cuts.
Can perform for longer periods of non-flowing conditions compared to KHIs.
Can achieve subcooling greater than 22 °C (40 °F).
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Hydrate Prevention with LDHIs
HydratesIn
Out
KHIsAAs Pipeline
Advantages/Disadvantages of LDHIs
Note: Table 6.5 in the PetroCore reference book, Gas Conditioning and Processing, shows a comparison of KHIs and AAs.
AD
VA
NTA
GE
SD
ISA
DV
AN
TAG
ES
• Injection of small amount of chemical compared to thermodynamic inhibitors.
• No regeneration required.
– Reduce CAPEX and OPEX, particularly on offshore installations
• Compatibility with other production chemicals could be an issue.
– Corrosion inhibitors, demulsifiers, scale inhibitors, wax inhibitors
– Must test chemical compatibility before selecting an LDHI
• High unit cost compared to thermodynamic inhibitors.
• Cannot inhibit below 0 °C (32 °F).
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PetroAcademyTM Gas Conditioning and Processing Core
Hydrocarbon Components and Physical Properties Core
Introduction to Production and Gas Processing Facilities Core
Qualitative Phase Behavior and Vapor Liquid Equilibrium Core
Water / Hydrocarbon Phase Behavior Core
Thermodynamics and Application of Energy Balances Core
Fluid Flow Core
Relief and Flare Systems Core
Separation Core
Heat Transfer Equipment Overview Core
Pumps and Compressors Overview Core
Refrigeration, NGL Extraction and Fractionation Core
Gas Dehydration Core
Contaminant Removal (Dehydration and Sweetening) Core
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