HIDRATOS DE GAS

GAS HYDRATES AND THEIR PREVENTION

Gas hydrates are representatives of a class of compounds known as clathrates or inclusion compounds.

Natural gas and crude oil normally reside in reservoir in contact with connate water. Water can

combine with low-molecular weight natural gases to form a solid, hydrate, even if the temperature is

above water freezing point.

Hydrates are considered as nuisance because they block transmission lines, plug blowout preventers,

jeopardize the foundation of deepwater platforms and pipelines, cause tubing and casing collapses, and

foul process heat exchangers, valves, and expanders.

Hydrates act to concentrate hydrocarbons; 1 cuft of hydrates may contain as much as 180 SCF of gas.

Large natural reserves of hydrocarbons exist in hydrated form, both in deep oceans and in the

permafrost. Evaluation of these reserves is highly uncertain, yet even conservative estimates indicate

that there is perhaps twice as much energy in the hydrated form as in all other hydrocarbon sources

combined.

This chapter is intended to provide the basic information needed for engineering purposes about

hydrates.

4.1 WATER CONTENT OF NATURAL GAS

When natural gas leaves the reservoir, it flows up the wellbore, which has lower temperatures than the

reservoir, and hence the gas saturated with water will tend to yield a liquid water condensate. Pressure

drop also affects the water content, but this effect during flow up a wellbore is smaller than that of

temperature.

Figure 4.1 shows a chart giving the water content of natural gases saturated with water vapor. Plotted

on this graph is an equilibrium curve of hydrate formation, which should be a function of gas

composition.

Determination of water content by this chart produces an error not exceeding 4%, which is acceptable

for engineering purposes.

As seen in Figure 4.1, the water content of a natural gas increases with the increase in temperature and

decreases with increase in pressure. Moreover, the water content of natural gases drops with an

increase in their molecular weight and with an increase in the water salinity. The two auxiliary graphs

shown in Figure 4.1 are for finding the correction factors for the molecular weight (gas density), Cg and

water salinity (Cs).

Let us now look at analytical methods, which allow us to find the water content of natural gases in a

selected range of pressures and temperatures.

The most suitable analytical method is Bukacek's method1 permitting the determination of water

content within a pressure range from 1 to 700 kgf/cm2 and of temperature range from -40 to 230 0C.

The error by this method does not exceed 4%.

The following expression is used for finding gas water content:

25

where

A, B = coefficients, function of temperature. The values of A and B are given in Table 4.1.

P = gas pressure, kg/cm2

Table 4.1 Coefficients for Equation 4.1

In view of the fact that Equation 4.1 was obtained for natural gases with a specific gravity of 0.6 in

contact with fresh water. For finding the water content of gases with a different gravity and of gases in

contact with mineralized water, the Equation 4.1 takes the following form:

+B

P

A

W = (4.1)

+B)C C

P

A

W =( g s (4.2)

26

Cg, Cs = Correction factors for gas gravity and salinity of water.

The correction factors Cg and Cs can be obtained from the insert graphs of Figure 4.1. It is also possible

to obtain the salinity correction, Csfrom Equation 4.32.

where S is the salinity in weight percent. Figure 4.3 agrees with existing graphical correlation to within

1%.

4.2 WHAT IS A GAS HYDRATE?

Natural gas hydrates are two or multi-component non-stoichiometric crystalline compounds where one

of the components is always water. Gas hydrates exist due to the ability of water molecules to form a

lattice structure, through hydrogen bonding, stabilized by small, non-polar gas molecules. By the

inclusion of the gaseous component, the structure, which alone is thermodynamically unstable,

becomes stabilized.

Gas molecules are physically enclosed in the cavities of the water lattice, and they are released from the

cavities only under appropriate circumstances, when the water lattice breaks down. Thus, the gas

components filling the cavities are not directly bonded to the water molecules of the framework. It is

for geometrical reasons that they cannot leave the hydrogen-bonded water molecule lattice until it

collapses.

Gas hydrates

...