Natural Gas Hydrates A Guide For Engineers 4Th Edition John Carroll Download PDF Chapter
Natural Gas Hydrates A Guide For Engineers 4Th Edition John Carroll Download PDF Chapter
Natural Gas Hydrates A Guide For Engineers 4Th Edition John Carroll Download PDF Chapter
JOHN CARROLL
Gas Liquids Engineering, Calgary, Canada
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Notices
Knowledge and best practice in this field are constantly changing. As new research and
experience broaden our understanding, changes in research methods, professional
practices, or medical treatment may become necessary.
Practitioners and researchers must always rely on their own experience and knowledge in
evaluating and using any information, methods, compounds, or experiments described
herein. In using such information or methods they should be mindful of their own safety
and the safety of others, including parties for whom they have a professional responsibility.
To the fullest extent of the law, neither the Publisher nor the authors, contributors, or
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matter of products liability, negligence or otherwise, or from any use or operation of any
methods, products, instructions, or ideas contained in the material herein.
ISBN: 978-0-12-821771-9
xi
Preface to the third edition
The objective of the third edition is the same as the first twodto give
engineers in the field the concepts to understand hydrates. From this
understanding they should be able to implement strategies to prevent them
from forming and to combat them when they form. Gas hydrates continue
to be a significant concern in the natural gas business. Companies spend
millions of dollars attempting to mitigate problems that arise from these
ice-like solid materials.
With each new edition there are new discoveries to explore; new
concepts to examine. Although the chapter structure remains unchanged
from the Second Edition, there are several new topics included in almost
every chapter. Most of these ideas come from people who have attended
my one-day course on hydrates.
For the author, hydrates remain a continuing interest because of their
unusual properties and new discoveries. This makes them an engaging
research topic. But as a process engineer, they remain a concern in my daily
work as they are for many other engineers.
Although the book is intended for engineers, others who have to deal
with hydrates will find some value in the material presented.
xiii
Preface to the second edition
The goal of the second edition is the same as the firstdto provide prac-
ticing engineers the tools to deal with hydrates.
One of the reasons that the author finds hydrates so interesting is their
unusual properties. Since the time of the first edition several new properties
have come to light and are discussed in the second edition. These include
the type of hydrate formed from mixtures of methane and ethane, hydrates
of hydrogen, the role of isopropanol in hydrate formation, etc. All of these
topics will be discussed.
Another addition to the book is discussion of a few other hydrate
formers. Notably, the hydrates of ethylene and propylene are included.
More examples are taken from the literature and additional comparisons
are made. A new section on the prediction of hydrate formation in sour gas
is also included.
xv
Preface to the first edition
Gas hydrates are of particular interest to those working in the natural gas
industry. Thus the main audience for this book is the engineers and
scientists who work in this field. Provided in this book are the tools for
predicting hydrate formation and details on how to combat them.
The reason for the genesis of this book was a one-day course presented
to engineers who work in the natural gas business. In particular, these
companies produce, process, and transport natural gas. The book has been
expanded from the original set of class notes. Much of the new material
came from feedback from attendees.
Many people outside the field of natural gas have also attended the
course and found some value in the material. These include oceanographers
studying the hydrate deposits on the seabeds throughout the world.
Astronomers investigating the possibility of hydrates on the planets of the
solar system as well as other celestial bodies may also find some of the
material in this book of some use. And those who are simply curious about
these interesting compounds will find this book to be useful.
The structure of the book is a little unusual. The chapters are meant to
be approximately independent; however, they do follow from the more
simple introductory topics to the more advanced applications. Occasionally
it is necessary to take a concept from a subsequent chapter in order to make
a point in the current chapter. This is unfortunate, but it is also necessary.
The purpose of this book is to explain exactly what gas hydrates are,
under what conditions they form, and what can be done to combat their
formation. Another purpose of this book is to explore some of the myths
associated with gas hydrates. The material is organized and presented in
such a way that the average engineer can use the information in their
day-to-day work.
In some sections of the book, especially those dealing with dehydration,
pipeline heat loss calculations, and lineheater design, the reader would
benefit greatly if they have the ability to calculate the physical properties of
natural gas. The properties of natural gas are not covered in this book.
xvii
Acknowledgments
There are many people whom I must thank. Without their help and
support, this book would not have been possible.
First, I would like to thank my employer Gas Liquids Engineering Ltd.,
Calgary, Alberta, Canada, and in particular the principals of the company
Douglas MacKenzie and James Maddocks. They allowed me the time to
build the hydrates course upon which this book is based and provided me
the time to write the manuscript. I would also like to thank them for the
other resources they provided. This book would have been impossible
without them. I would also like to thank my colleague Peter Griffin, also
from Gas Liquids Engineering, for his encouragement. With his help I have
been able to present this material throughout the world.
Words cannot express my thanks to Alan E. Mather of the University of
Alberta, Edmonton, Alberta, Canada. He was my patient supervisor during
my time as a graduate student, and he continues to be my mentor. The core
of my knowledge of thermodynamics, and in particular how it relates to
phase equilibrium, is a result of his teaching. Over the years we have
collaborated on many interesting projects. In addition, he proofread early
versions of the manuscript, which was enormously valuable.
The book is the result of a one-day course on gas hydrates that I
conducted. I have received positive feedback from many of those who
attended. Some of their ideas have been added to the book. Thus, I thank
all of those who attended the course. Many of the additions to the book are
a direct result of feedback from attendees.
I would be amiss if I did not also thank my loving wife, Ying Wu, for
her endless support, encouragement, and love.
I would like to express my gratitude to the Gas Processors Association
(GPA) and the Gas Processors Suppliers Association (GPSA), both of Tulsa,
Oklahoma, for permission to reproduce several figures from the GPSA
Engineering Data Book (11th ed.). Furthermore, over the years these associ-
ations have sponsored a significant amount of research into gas hydrates. This
research has been valuable both to the author of this book and others
working in the field.
The author would also like to thank the Center for Hydrates Research
at the Colorado School of Mines in Golden, Colorado and its Director
Dr. Carolyn Koh and Director Emeritus Dr. E. Dendy Sloan. The Center is
xix
xx Acknowledgments
Introduction
temperatures greater than the freezing point of water and (2) that the solid
was composed of more than just water. When melted, the hydrate of
chlorine released chlorine gas.
Davy’s equally famous assistant, Michael Faraday, also studied the hy-
drate of chlorine. In 1823, Faraday reported the composition of the
chlorine hydrate. Although his result was inaccurate, it was the first time the
composition of a hydrate was measured.
Throughout the 19th century, hydrates remained basically an intellec-
tual curiosity. Early efforts focused on finding which compounds formed
hydrates and under what temperatures and pressures they would form.
Many of the important hydrate formers were discovered during this era.
Among the 19th-century, hydrate researches who deserve mention are
the French chemists Villard and de Forcrand. They measured the hydrate
conditions for a wide range of substances, including hydrogen sulfide.
The first crystallographic studies of gas hydrates were published by von
Stackelberg from the University of Bonn in Germany in the 1940s and 50s.
Von Stackelberg and his group established that there were two distinct
types of hydrate crystal structures. We will discuss these hydrate types in
Chapter 2.
However, it would not be until the 20th century that the industrial
importance of gas hydrates would be established, especially for the natural
gas industry (Hammerschmidt, 1934).
Over the years, there have been many, many experimental studies of
hydrate formation. These include the hydrates for single components,
binary mixtures, and multicomponent mixtures. Some of these studies are
discussed in the chapters that follow. If the reader has doubts about methods
used in the work, they should consult the literature. They may not find the
exact data for their situation, but they may find data which are useful for
testing the models they chose to employ.
per standard cubic meter (0.16 g/Sm3) or 160 milligrams per standard cubic
meter (160 mg/Sm3). More discussion of units and standard conditions is
presented later in this chapter.
There are several other restrictions on the composition of sales gas. For
example, there is a limit on the amount of hydrogen sulfide present
(typically on the order of about 10 parts per million or 10 ppm) and the
amount of carbon dioxide (typically around 2 mole percent). These too
vary from jurisdiction to jurisdiction, contract to contract.
1.2.2 Hydrates
In combination with water, many of the components commonly found in
natural gas form hydrates. One of the problems in the production, pro-
cessing, and transportation of natural gas and liquids derived from natural
gas is the formation of hydrates. Hydrates cost the natural gas industry
millions of dollars annually. In fact, individual incidents can cost $1,000,000
or more depending upon the damage inflicted. There is also a human price
to be paid because of hydrates. Sadly, there have been deaths either directly
or indirectly associated with hydrate and their mishandling.
However, the importance of natural gas hydrates was not apparent in
the early era of the gas business. In the early era of the natural gas business,
gas was produced and delivered at relatively low pressure. Thus, hydrates
were never encountered. In the 20th century, with the expansion of the
natural gas industry, the production, processing, and distribution of gas
became high-pressure operations. Under pressure, it was discovered that
pipelines and processing equipment were becoming plugged with what
appeared to be ice, except the conditions were too warm for ice to form. It
was not until the 1930s that Hammerschmidt (1934) clearly demonstrated
that the “ice” was actually gas hydrates. And that the hydrates were a
mixture of water and the components of natural gas.
In the petroleum industry, the term “hydrate” is reserved for substances
that are usually gaseous at room temperature. These include methane,
ethane, carbon dioxide, and hydrogen sulfide. This leads to the term “gas
hydrates” and also leads to one of the popular misconceptions regarding
these compounds. It is commonly believed that nonaqueous liquids do not
form hydrates. However, liquids may also form hydrates. An example of a
compound that is liquid at room conditions, yet forms a hydrate, is
dichlorodifluoromethane (Freon 12). But we are getting ahead of ourselves.
6 Natural Gas Hydrates
Figure 1.1 Iconic “Ice on Fire” picture showing a methane hydrate burning. (Credit: J.
Pinkston and L. Stern (USGS), USGS. Public domain.)
Introduction 7
hydrogen telluride
-10
-20
Normal Boiling Point (°C)
-30
-40
hydrogen selenide
-50
-60
hydrogen sulfide
-70
water?
-80
10 20 30 40 50 60 70 80 90 100 110 120 130 140 150
Molar Mass (kg/kmol)
Figure 1.2 The normal boiling points of hydrogen compounds.
8 Natural Gas Hydrates
shows a plot of the normal boiling points for these three compounds. Note
that as the size of the molecule increases, so does the normal boiling point.
Although it is not exactly linear, we can use a linear approximation to
estimate the boiling point of water. This extrapolation yields an estimated
boiling point of 74 C! As the boiling point of water is 100 C, this is
clearly a very poor estimation. There is probably something unusual about
water.
It is worth noting that a similar plot could be constructed showing the
melting points for these compounds. Again the predicted melting point of
water, based on the other substances, is much too low.
As a second example, consider the homologous series of normal alco-
hols. Fig. 1.3 shows a plot of the normal boiling points of the alcohols as a
function of their molar mass (molecular weight). In this case, the relation is
nearly linear. Assume that water is the smallest member of this group of
compounds, and extrapolate the correlation to estimate the boiling point.
This yields 43 C for the boiling point, which is significantly lower than the
actual value.
140
n-pentanol
130
120
n-butanol
110
Normal Boiling Point (°C)
100
water
n-propanol
90
80
ethanol
70
60 methanol
50
40
10 20 30 40 50 60 70 80 90 100
Molar Mass (kg/kmol)
Figure 1.3 The normal boiling points of alcohols.
Introduction 9
Table 1.1 The enthalpy of vaporization of several substances at their normal boiling
point.
Compound Nature Enthalpy of vaporization (kJ/kg)
Water Polar 2257
Methanol Polar 1100
Ethanol Polar 855
Acetone Polar 521
Ethylene glycol Polar 800
Ammonia Polar 1369
Methane Nonpolar 510
n-pentane Nonpolar 357
n-octane Nonpolar 306
Benzene Nonpolar 394
o-xylene Nonpolar 347
Cyclohexane Nonpolar 358
Data taken from Dean, J.A. (ed.), 1973. Lange’s Handbook of Chemistry, eleventh ed. McGraw-Hill,
New York, NY, pp. 9e85 to 9e95.
10 Natural Gas Hydrates
The simple reason for this expansion is that the water atoms arrange
themselves in an ordered fashion and the molecules in the crystal occupy
more space than those in the liquid water. The reason for this behavior is
also because of the shape of the water molecule and something called the
hydrogen bond.
The molecules in solid water form a hexagonal crystal. This is most
obvious in snow with its characteristic pattern structures (see for example
Fig. 1.4).
Figure 1.5 The shape of the water molecule. (A) Stick representation showing induced
charges, which result in hydrogen bonding, and (B) ball model showing the angle
between the hydrogen molecules.
12 Natural Gas Hydrates
1.4 Hydrates
It is a result of the hydrogen bond that water can form hydrates. The
hydrogen bond causes the water molecules to align in regular orientations.
The presence of certain compounds causes the aligned molecules to stabilize
and a solid mixture precipitates.
The water molecules are referred to as the “host” molecules and the
other compounds, which stabilize the crystal, are called the “guest” mol-
ecules. In this book the guest molecules are more often referred to as
Figure 1.7 Simplified diagram of the three criteria for hydrate formation.
14 Natural Gas Hydrates
Although this figure gives a quick visual image, it lacks the detail provided
by the discussion presented earlier. However, it provides a useful visual.
These three points will be examined in some detail in subsequent
chapters, but they deserve a few comments at this point. As was noted, low
temperature and high pressure favor hydrate formation. The exact tem-
perature and pressure depends upon the composition of the gas. However,
hydrates form at temperatures greater than 0 C (32 F), the freezing point of
water. The nature of hydrate formers is discussed in detail in Chapter 2.
To prevent hydrate formation, one merely has to eliminate one of the
three conditions stated above. Typically we cannot remove the hydrate
formers from the mixture. In the case of natural gas, it is the hydrate formers
that are the desired product. So we attack hydrates by addressing the other
two considerations.
Other phenomena that enhance hydrate formation include the
following:
1. Turbulence
a. High velocity
Hydrate formation is favored in regions where the fluid velocity
is high. This makes choke valves particularly susceptible to hydrate
formation. First, there is usually a significant temperature drop
when natural gas is choked through a valve due to the Joulee
Thomson effect. Second, the velocity is high through the narrowing
in the valve.
b. Agitation
Mixing in a pipeline, process vessel, heat exchanger, etc., en-
hances hydrate formation. The mixing may not be due to an actual
mixer but perhaps a tortuous routing of the line.
2. Nucleation sites
In general terms, a nucleation site is a point where a phase transition
is favored, and in this case the formation of a solid from a fluid phase. An
example of nucleation is the deep fryer used to make French fries in fast-
food restaurants throughout the world. In the fryer the oil is very hot
but it does not undergo the full rolling boil because there are no suitable
nucleation sites. However, when the potatoes are placed into the oil, it
vigorously boils. The French fries provide an excellent nucleation site.
Good nucleation sites for hydrate formation include an imperfection
in the pipeline, a weld spot, or a pipeline fitting (elbow, tee, valve, etc.).
Corrosion by-products, silt, scale, dirt, and sand all make good nucle-
ation sites as well.
Introduction 15
3. Free water
No, this is not a contradiction to earlier statements. Free water is not
necessary for hydrate formation, but the presence of free water certainly
enhances hydrate formation.
The presence of free water also assures that there is plenty of water
present, which is more likely to form a plug.
In addition, the wateregas or the watereoil interface is a good
nucleation site for hydrate formation.
The items in the above list enhance the formation of a hydrate, but are
not necessary. Only the three conditions given earlier are necessary for
hydrate formation.
Another important aspect of hydrate formation is the accumulation of
the solid. The hydrate does not necessarily agglomerate in the same location
as it is formed. In a pipeline, the hydrate can flow with the fluid phase,
especially the liquid. It would tend to accumulate in the same location as
the liquid does. Usually it is the accumulations of the hydrates that cause the
problems. In a multiphase pipeline, it is the accumulations that block line
and plug and damage equipment.
Often pigging is sufficient to remove the hydrate from the pipeline.
Pigging is the process of inserting a tool (called a “pig”) into the line.
Modern pigs have many functions, but the main one remains pipeline
cleaning. The pig fits tightly into the line and scraps the inside of the pipe. It
is transported along the line with the flow of the fluid and by doing so it
removes any solids (hydrate, wax, dirt, etc.) from inside the line. The
pigging can also be used to remove accumulations of liquids.
However, the pigging must be scheduled such that the accumulations of
hydrates do not become problematic. Usually pigging is not used to clean
hydrates from a line. Other measures are more commonly used to deal with
hydrates and these are detailed in subsequent chapters of this book.
Another benefit of pigging is the removal of salt, scale, etc., which is
important for the proper operation of a pipeline. It also means that potential
nucleation sites for hydrate formation are removed.
this locus. Again, without getting to far ahead of ourselves, some pre-
liminary discussion of hydrate curves is appropriate.
Fig. 1.8 shows a typical hydrate curve (labeled “hydrate curve”). The
region to the left and above this curve (high pressure, low temperature) is
where hydrates can form. In the region to the right and below the hydrate
curve, hydrates can never formdin this region, the first criterion is violated.
Therefore, if your process, pipeline, well, etc., operates in the region
labeled “no hydrates,” then hydrates are not a problem. On the other hand,
if it is in the region labeled “hydrates region,” then some remedial action is
required to avoid hydrates.
It might seem as though we can treat the temperature and pressure as
separate variables but when discussing hydrates, they are linked. For
example, you cannot say “A hydrate will not form at 10 C for the gas
mixture shown in Fig. 1.8.” You must qualify this with a pressure. So at
10 C and 5 MPa, the process is in the “hydrate region,” whereas at 10 C
and 1 MPa, the process is in the region where a hydrate will not form.
Thus, we must talk about a combination of temperature and pressure and
not each variable on its own.
14
12
10
hydrate region
Pressure (MPa)
4 hydrate curve
plus 3 Celsius
2
no hydrates
0
0 5 10 15 20 25
Temperature (°C)
Figure 1.8 Pressureetemperature diagram showing the hydrate region, the region
with no hydrates, and a safety margin.
Introduction 17
1.5.1 Free-water
There is a myth in the natural gas industry that “free water” (i.e., an
aqueous phase) must be present to form a hydrate. In subsequent sections of
this book, we will demonstrate that this is not correct. Free water certainly
increases the possibility that a hydrate will form, but it is not a necessity.
A strong argument demonstrating that free water is not necessary for
hydrate formation is presented in Chapter 9 on phase diagrams.
Another argument, the so-called “frost argument,” asks the simple
question: Is it necessary to have free water to form ice? The answer is no.
Frost forms without liquid water forming. The frost sublimes from the air
onto my car on winter nights. The water goes directly from the air to the
solid phase without a liquid being encountered. The airewater mixture is a
gas, and the water is not present in the air in a liquid form. If you have an
old-fashioned freezer, i.e., one that is not frost-free, just look inside. A layer
of frost builds without liquid water ever forming. Hydrates can “frost” via
the same mechanism.
One of the reasons why it is believed that free water is required for
hydrate formation is that hydrates formed without free water may not be
problematic. The inside of a pipe may “frost” with hydrates, but still
function properly. Or the amount of hydrate may be small and thus does
not plug lines or damage processing equipment. Such “frost” hydrates can
be easily cleaned using the pigging process discussed earlier.
The process of going directly from the gas to the solid is called subli-
mation and it is not that rare. For example, carbon dioxide sublimes at
atmospheric pressure. Solid CO2, commonly called “dry ice,” goes directly
from the solid to the vapor without forming a liquid. At atmospheric
pressure, CO2 goes directly from the solid to the vapor at a temperature of
about 78 C (108 F). Another example of a solid that sublimes at at-
mospheric pressure is naphthalene, the main component of moth balls. The
reason why you can smell moth balls is because the naphthalene goes
directly from the solid to the vapor and it is the vapor that you can smell. In
reality, all pure substances sublime at pressures below their triple point
pressure and this includes pure water. So it should come as no surprise that
hydrates, under the right set of conditions, can sublime directly from the gas
phase to the solid phase.
Introduction 19
A. Sleeping and sitting-rooms. c. Little houses for holding grain. F. House of entrance.
B. Stables. D. Houses of the slaves. 4. Places for cooking.