-
Society of Economic Geologists Special Publication 10, 2003, p.
6174
Chapter 6
Geochemistry of Light Hydrocarbons in Subduction-Related
Volcanic and Hydrothermal Fluids
YURI A. TARAN,
Institute of Geophysics, Universidad Nacional Autnoma de Mxico
04510, Mexico
AND WERNER F. GIGGENBACH*
Institute of Geological and Nuclear Sciences, P.O. Box 31312,
Lower Hutt, New Zealand
Abstract
During the last 20 years of his outstanding career, Werner
Giggenbach collected and analyzed hundreds of samples of volcanic
and hydrothermal gases from White Island volcano and geothermal
systems in New Zealand, as well as many volcanoes and geothermal
systems over the world. Hundreds of samples were ana- lyzed for
C1-C6 hydrocarbons, including benzene. On the basis of the data set
obtained for the White Island volcano, together with other
available data, several general trends in the behavior of CH4,
C2-C4 hydrocar- bons, and benzene are apparent, based on
application of techniques developed by W. Giggenbach for the
interpretation of crustal fluid composition in a high-temperature
environment. The trends can be divided into two main types
involving temperature-dependent equilibrium and mixing of carbon
from magmatic and sedimentary sources.
The common statement that the CH4 concentration in volcanic
gases decreases with increasing temper- ature is not true, as there
are no temperature-dependent trends in the CH4/CO2 behavior until
magmatic temperatures are reached. The concentrations of methane in
hydrothermal fluids are controlled mainly by the source output,
comprising organic matter buried with sedimentary rocks. Thermal
decomposition of this organic matter at upper crust levels produces
CH4 and light hydrocarbons as well as nitrogen accom- panied by a
very high N2/Ar ratio. Therefore, the CH4-rich end member of
hydrothermal fluids tends to have a high N2/Ar ratio. By contrast,
subduction-related magmatic fluids have almost no methane despite
having a high N2/Ar ratio due to degradation of subducted
organic-rich oceanic sediments. Hence, vol- canic gases and
hydrothermal fluids are characterized by two different
relationships between CH4 concen- tration and N2/Ar ratio.
Two systems show a good correlation with sampling temperature in
volcanic gases: alkane-alkene pairs with the same number of carbon
atoms and ethene-benzene. Their concentration ratios (C2H6/C2H4,
C3H8/C3H6, C4H10/C4H8, C2H4/C6H6) in volcanic gases are strongly
dependent on the temperature of the fumarole, and these ratios
change with temperature along metastable equilibrium paths. This
means that the chemical redox reactions alkane + H2 = alkane and
C6H6 + 3H2 = 3C2H4 are fast but kinetically con- trolled, probably
through catalysis by oxides and sulfur species. Variations in
alkane-alkane ratios in terms of the 2Cn = Cn 1 + Cn + 1
equilibrium, either for volcanic gases or for hydrothermal fluids,
show no sys- tematic trends, and even at magmatic temperatures
(>800C), the observed Cn/Cn 1 ratios often corre- spond to
negative equilibrium temperatures.
The reaction CO2 + 4H2 = CH4 + 2H2O, mistakenly called the
Fischer-Tropsch reaction by some geo- chemists, is unlikely to
apply under redox and temperature conditions in the hydrothermal
and magmatic environment. The only natural inorganic process in
which reduction of CO2 (and carbon) could be pos- sible is the
serpentinization of Mg-rich mafic rocks. Under conditions
prevailing in the crust, the only process that results in
equilibration within the CH4-CO2 system is the oxidation of
methane. This can be facilitated by natural catalysts, which are
usually oxides, but not native metals as in the case of the reduc-
tion of CO2.
Introduction
WERNER GIGGENBACH collected and analyzed an enormous number of
gas samples from volcanoes and geothermal sys- tems from New
Zealand and the rest of the world. At the
Corresponding author: e-mail, [email protected]
*Deceased
center of his research was the study of gases from the White
Island volcano. Apart from the major components (e.g., CO2, H2S,
SO2, N2, Ar, CH4, H2), Giggenbach also analyzed a large set of
light gaseous hydrocarbons starting with methane up to the light
aromaticsbenzene and toluene. Only some of the hydrocarbon data for
geothermal systems of New Zealand and other locations have been
published (Giggenbach et al., 1990, 1992, Giggenbach and
Corrales,
1
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2 TARAN AND GIGGENBACH
1992; Giggenbach, 1995), whereas none of the hydrocar- bon data
on volcanic samples are published. The first detailed thermodynamic
and kinetic analysis of processes controlling the content of
hydrocarbons higher than CH4 in hydrothermal fluids was presented
in Giggenbach (1997a). The following review is based mainly on this
paper as it discusses the essential problems of the geochemistry of
carbon species in the high-temperature hydrothermal envi-
ronment.
There are two main approaches to the description of hydrothermal
hydrocarbon geochemistry. The first one deals with the so-called
Fischer-Tropsch process, which at least theoretically in nature and
practically in industry allows synthesis or reequilibration of
hydrocarbons in a C- O-H system and assumes both reversible
reduction of CO2 and oxidation of CH4 and hydrocarbons (Robinson,
1963; Kiyosu et al., 1992; Kiyosu and Asada, 1995). The second one
is based on numerous observations, which show that the nature and
distribution of hydrocarbon species in hydrothermal vapors is more
consistent with the thermal degradation of kerogen rather than
inorganic production and was first proposed by Gunter (1978).
Nehring and Truesdell (1981) showed that hydrocarbons are a common
constituent of geothermal vapor discharges. Des Marais et al.
(1981) experimentally confirmed that thermal decom- position of
organic matter is the most important source of hydrocarbons in
subaerial geothermal systems. Thermody- namic calculations
suggested that the proportions of higher hydrocarbons forming in
equilibrium under natural conditions are extremely low (e.g.,
Taran, 1984; Takachi et al., 1987). Kiyosu and Asada (1995) and
Capaccioni et al. (1993, 1995, 2001) have presented a large data
set on hydrothermal hydrocarbons with some analyses from high-
temperature magmatic fumaroles. Capaccioni et al (1995, 2001)
ascribed formation of alkanes, alkenes, and aromat- ics in volcanic
and hydrothermal gases mainly to cracking and reforming
processes.
Even in the case of the completely thermogenic origin of CH4 and
higher hydrocarbons one can expect that under
hydrothermal and magmatic conditions, the reequilibra- tion in a
natural C-H-O system may occur due to increasing rates of reactions
at elevated temperatures and possible catalysis by minerals.
Darling (1998) has proposed a C2H6/CH4 geothermometer based on a
data set for hydrothermal hydrocarbons. Sugisaki and Nagamine
(1995) took advantage of the following simple reaction:
CH4 + C3H8 = 2C2H6. (1)
This reaction allows the pressure-independent internal
equilibrium to be expressed in terms of the CH4/C2H6 and C2H6/C3H8
ratios. Giggenbach (1987, 1997a) demon- strated with many examples
that the redox potential in hydrothermal systems is controlled by
interaction with diva- lent and trivalent Fe in the rock contacted
by the fluids, and in turn, the CH4/CO2 ratio in hydrothermal
fluids is appar- ently close to equilibrium if the hydrogen
fugacity is gov- erned by the Fe system of the hydrothermally
altered rock.
Taran (1986, 1988) and Chiodini and Marini (1998), using large
data sets from many hydrothermal systems, showed that CH4 is not in
chemical equilibrium under natural hydrothermal conditions or that
a heterogeneity exists in redox conditions of geothermal
reservoirs.
High-temperature volcanic gases originate essentially from
shallow magma degassing, and at the surface they rep- resent a
mixture of magmatic, hydrothermal, and atmos- pheric end members.
Their redox potential (hydrogen fugacity) is controlled by water
vapor and oxidized and reduced volatile sulfur species, such as SO2
and H2S
(Giggenbach, 1987; Giggenbach et al., 1987). Even very high
temperature (>600C) volcanic gases contain
detectable amounts of methane and higher hydrocarbons
(Capaccioni et al., 1995; Kiyosu and Asada, 1995). Until now a
detailed analysis of the sources and reactions of hydrocarbons in
volcanic gases has been difficult because of the few data
available. In this work, discussion of the sources, equilibria, and
chemical kinetics of hydrothermal hydrocarbons, based on a large
analytical data set obtained by W. Giggenbach in New Zealand and
other geothermal regions, is presented. Some new data on the
Kamchatkan volcanoes are also presented, and these are discussed
along with published analyses, mainly from Japan and Italy. One of
the main goals of this work is to constrain important aspects of
the hydrocarbon geochemistry of hydrothermal and volcanic fluids,
using simple thermodynamic calcula- tions and mixing relationships
but without application of isotopic data. The importance of the
so-called Fischer- Tropsch synthesis for geochemistry is discussed,
using a standard approach for interpreting the distribution of
reac- tion products in the context of catalytic chemistry.
Analytical Results
This study is based on detailed analyses of >200 gas sam-
ples from high-temperature fumaroles, most of them from White
Island and geothermal wells in New Zealand and other geothermal
areas. A selection was made of partial analyses from White Island
and other volcanoes contain- ing hydrocarbon abundances data in
addition to informa- tion on the total gas content, N2/Ar ratios,
and CO2 and H2 concentrations. Volcanic and hydrothermal gases were
collected in preevacuated bottles containing 40 ml of a 5N NaOH
solution for the absorption of acid gases such as CO2, H2S, SO2,
HCl, and HF. The samples were analyzed
by well-established techniques, as described by Giggen- bach
(1975).
Table 1 shows representative data for hydrocarbon abun- dances,
total gas content, CO2, H2, and composition from
fumaroles of the White Island volcano, in order of increas- ing
sampling temperature. The whole data set contains more than 90
analyses of hydrocarbons in dry gas. These data are not presented
here but are used for diagrams where only the ratios among
hydrocarbon concentrations are needed. The available analyses of
hydrocarbons together with the total gas contents, CO2, H2, and
N2/Ar from other volcanoes are shown in Table 2. Unfortunately the
data set for hydrocarbons and the data set for major gas
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3 GEOCHEMISTRY OF LIGHT HYDROCARBONS
TABLE 1. Hydrocarbons in Fumarolic Gases of White Island
Year ST Xg CO2 H2 CH4 C2H4 C2H6 C3H6 C3H8 C4 C6H6
1985 103 21 873 0.15 6.5 0.003 2.7 0.25 0.06 1.04 1984 106 49
911 0.4 1.3 0.13 2.6 0.26 1.9 1983 109 55 907 2.1 1.4 0.07 2.9 0.95
0.68 2.9 1979 110 22 790 0.31 4.3 0.01 2.3 0.18 0.04 1.7 1979 119
12 740 0.74 11 2.0 0.17 0.044 1.0 1978 120 26 877 0.7 5.7 0.001 1.9
0.004 0.11 0.021 1.5 1983 182 13 661 5.0 6.2 0.08 2.6 0.003 0.28
0.038 0.4 1983 182 13 665 4.8 3 0.06 2.5 0.003 0.16 0.5 1984 191 89
841 2.1 2.5 0.05 2.2 0.16 1.6 1984 193 11 489 1.9 5.2 0.07 2.2 0.11
1.3 1983 198 10 557 10 7.4 0.06 2.4 0.10 1.0 1979 208 25 241 9.7
2.7 0.06 1.5 0.003 0.08 0.03 1.6 1978 281 76 648 0.5 0.003 26 79 24
28 8 21 1979 295 71 683 1.1 0.02 0.12 1.2 2.5 1979 327 114 783 12.1
0.07 0.12 1.2 0.02 1.6 4.1 1.8 1983 370 79 579 1.6 0.02 4.2 2.2 0.5
0.5 1.0 1.8 1984 394 72 170 7.7 0.1 1.2 2.4 0.5 0.6 1.2 1983 416 99
600 3.1 0.01 1.1 2.0 1984 426 49 539 4.6 0.18 2.9 4.5 2.6 1.7 7.3
3.3 1983 430 52 558 35.8 0.26 2.3 3.3 3.1 1.5 7.0 0.9 1983 440 69
517 4.5 0.02 1.2 1.4 2.5 1.2 9.7 1.5 1984 457 59 493 9.2 0.05 3.3
3.6 1984 509 700 206 7.9 0.13 2.3 5 0.7 0.9 0.23 2 1979 510 52 331
14.2 0.94 0.41 0.9 0.007 0.003 0.002 1.1 1979 512 426 862 2.1 0.006
1.4 2.1 9.2 1978 520 301 805 12.5 0.009 7.1 2.3 2.0 1978 540 119
824 20 0.03 5.3 3.8 17 1978 540 120 786 18 0.018 5.8 2.3 20 7 27
0.8 1983 590 166 776 5.1 0.012 2.9 2.2 1983 611 177 720 26.1 0.04
5.6 7.3 3.0 1.4 1983 630 114 748 18.7 0.13 3.4 2.6 5.7 2.4 7.3 2.7
1983 655 133 754 17.2 0.10 2.7 2.8 0.7 0.9 1984 664 808 147 22.8
0.16 1.3 1.6 0.16 1983 685 253 831 9.4 0.02 5.8 7.7 9.2 1984 694 59
748 25.8 0.14 9.8 4.8 3.4 1.7 0.8 2.6 1983 745 120 719 15.6 0.01
10.9 8.8 1984 760 73 724 41.4 0.14 8.6 5.2 1984 772 56 684 41.6
0.22 3.1 2.6 3.8 1.8
Notes: ST = sampling temperature (C); Xg (mmol/mol) = the total
gas content (mmol gas/(mol gas + mol H2O); CO2, H2, and CH4
(mmol/mol) = dry gas content; C4 = all butanes and butenes; all
hydrocarbons (mmol/mol) normalized to CH4
components in White Island fumaroles were decoupled. Table 3
therefore shows the available data on CH4 concen-
trations in the total discharge and the N2/Ar ratios for White
Island fumaroles separately from the hydrocarbons data. Most of the
gas analyses containing hydrocarbons in hydrothermal fluids from
New Zealand were published in Giggenbach (1995). The hydrocarbon
concentrations in Kamchatkan hydrothermal fluids were published in
Taran (1984, 1988). However, analytical data with concentrations of
CH4 in samples from hydrothermal wells together with the N2/Ar
ratio for different hydrothermal systems are dis- tributed in the
literature. Table 4 is a compilation of these analyses.
Methane in Volcanic and Hydrothermal Gases
From the very beginning of the geochemical exploration of
geothermal fields, methane was always used as one of the principal
gas species for the estimation of reservoir tem- perature by using
the so-called Fischer-Tropsch geother- mometer based in the
following equilibrium (Gunter and
Musgrave, 1971; Ellis and Mahon, 1977; DAmore and Panichi, 1980;
Giggenbach, 1980):
CO2 + 4H2 = CH4 + 2H2O. (2)
Giggenbach (1980) developed a technique that takes into account
the distribution of gases between saturated vapor and liquid water,
which became a common geo- chemical tool (DAmore and Celati, 1983;
DAmore and Truesdell, 1984; Taran, 1986). For liquid-dominated
reser- voirs in subaerial geothermal systems the direct use of this
geothermometer (comparing values of the quotient and the
equilibrium constant) gives equilibration temperatures that
generally matched measured ones. In combination with another gas
reaction (e.g., 2NH3 = N2 + 3H2), one can
use a grid discriminating temperature and the steam frac- tion
dependences (DAmore and Celati, 1983). This approach assumes the
attainment of full chemical equilib- rium between CO2, H2, CH4, and
H2O, and a good agree-
ment between measured and calculated temperatures can
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4 TARAN AND GIGGENBACH
TABLE 2. Hydrocarbons in Gases from Subduction-Related
Volcanoes
Codes
(see
T
CO2
H2
CH4
Fig. 4) Volcano (C) (mol%) (mol %) (ppm) C2H4 C2H6 C3H6 C3H8 C4
C6H6 N2/Ar Ref.
v Vulcano 313 11.0 0.04 0.10 0.13 0.17 0.4 0.30 818 1 v Vulcano
329 9.32 0.003 0.30 505 2 v Vulcano 604 12.1 0.20 0.11 975 2 g
Galeras 642 2.73 0.11 11 0.15 0.21 0.31 0.31 0.20 47 1,3 sw
Showashinzan 750 0.47 0.18 60 200 4 sw Showashinzan 637 0.02 0.06
0.9 15 5.8 1.7 5.1 5 sw Showashinzan 617 0.27 0.21 0.4 39 1.1 3.3
6.7 5 k Kuju 350 0.29 0.005 0.3 0.67 0.60 0.24 0.24 6 k Kuju 143
5.36 0.001 2.5 65 7 m Merapi 803 2.60 0.24 21 16 5.3 21 13 4.3 54 8
m Merapi 575 3.79 0.16 2.2 55 33 12 12 29 80 8 p Papandayan 356
2.20 0.008 0.3 5.9 4.2 1.2 2.2 0.7 907 8 kr Koryak 220 4.97 0.07
600 6.7 40 8.3 88 8 a Avacha 473 2.26 0.05 3 15 7.1 5.5 2.3 0.5 275
8
ch Chornyi 344 0.88 0.08 0.3 19 15 5.6 3.1 1.2 826 8 gr Groznyi
174 0.72 0.001 20 2.6 8.1 1.8 3.0 4.9 200 8 ku Kudryavy 825 1.81
1.2 10 2.4 0.5 1.2 0.2 0.8 280 8 ku Kudryavy 705 2.11 0.24 6.3 11
7.5 4.3 5.2 198 8 md Mendeleev 114 0.57 0.0001 150 7.0 140 0.6 2.1
0.15 8 e Ebeko 144 1.13 0.00001 10 32 1.0 16 21 180 8,9
mt Mutnovsky 360 0.51 0.02 13 12 8 0.3 1.0 1.0 115 8,10 ki Kawah
Ijen 187 11.4 0.002 0.1 331 11 ki Kawah Ijen 169 9.41 0.002 0.19
370 11 si S-Iwojima 870 0.34 0.54 5.0 275 12 ng Ngauruhoe 640 1.61
0.26 0.3 810 13 sh Mt. St Helens 540 0.91 0.24 0.2 618 13
Notes: Hydrocarbon concentrations (mmol/mol) are normalized to
methane; the concentrations of CO2, H2, and CH4 in the total
discharge (H2O + gases) and N2/Ar ratios are also presented
References: 1 = Capaccioni et al. (1995), 2 = Giggenbach and
Matsuo (1991), 3 = Fischer et al. (1997), 4 = Mizutani and Sugiura,
1982, 5 = Kiyosu and Asada (1995), 6 = Mizutani et al. (1986), 7 =
Saito et al. (2001), 8 = this work, 9 = Menyailov et al. (1986), 10
= Taran et al. (1992), 11 = Delmelle et al. (2000), 12 = Shinohara
et al. (1993), 13 = Giggenbach et al. (1990)
TABLE 3. Methane Mole Fraction and N2/Ar Mole Ratio
ST XCH4 10
6 N2/Ar
100 230 156 101 110 30 104 79 471 106 430 213 107 500 87 110 94
411 110 82 34 120 150 190 120 76 38 139 62 110 156 96 251 229 110
47 327 120 306 350 26 633 355 66 37 356 4.9 630 365 27 122 365 42
397 396 19 164 513 33 91 515 14 970 520 2.7 1,220 540 2.2 530 540
3.3 920 550 2.3 650
ST = sampling temperature (C)
be considered as reasonable experimental proof for such
equilibrium. However, if equilibrium is attained, and if the redox
conditions are controlled in a uniform way, the equi- librium
fugacity ratios CH4/CO2 should have monotonic temperature
dependence along an appropriate buffer line. For geothermal
systems, redox conditions of fluids, as shown by DAmore and
Gianelli (1984) and Giggenbach (1980, 1987), are governed by the
interaction of aqueous fluids with rock containing di- and
trivalent Fe. Redox potential in terms of RH = log (H2/H2O) can be
calculated by use of fayalite and hematite as thermodynamic proxies
for mineral phases containing iron in these two oxidation states
(Giggenbach, 1987). In this case the H2/H2O ratio remains
practically constant with temperature, and a value RH = 2.8 can be
taken to adequately describe the equilib- rium redox potential over
a hydrothermal range of tem- perature, up to ~400C, buffered by
typical altered volcanic host rocks. Another important assumption
is that the fugac- ity of water vapor in volcanic hydrothermal
systems is con- trolled by an NaCl brine. In this case, log H2O =
4.9 1,820/T, and hence, using other thermodynamic data (e.g., Stull
et al., 1969; Barin and Knake, 1973): log (CH4/CO2) log (PCH4/PCO2)
=
log (XCH4/XCO2)v = log Kc + 4RH + 2log H2O = (3) 5,280/T
11.12.
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5 GEOCHEMISTRY OF LIGHT HYDROCARBONS
TABLE 4. Methane Mole Fraction and N2/Ar Mole Ratio in Gases
from Wells and Steam Vents in Some Geothermal Fields
(2003). The Taran (1988) line represents the function (eq
Codes Geothermal
XCH4 fluids from wells at various aquifer temperatures (from
(see Fig. 3) system 106 N2/Ar Ref.
ru El Ruiz 1,680 295 1 ru El Ruiz 1.6 86 1 cf Campi Flegrei 33
738 1 kr Krafla 1.9 69 1 mt Mutnovsky 90 220 2 pz Pauzhetka 150 260
2 su Sumikawa 2 73 3 ni Nigorikawa 70 155 3 ni Nigorikawa 80 200 3
kw Kaverau 29 135 4 kw Kaverau 28 107 4 mo Mokai 18 68 4 mo Mokai 8
65 4 mo Mokai 2 70 4 br Broadlands 24 416 4 br Broadlands 26 429 4
br Broadlands 56 428 4 br Broadlands 15 192 4 br Broadlands 100 454
4 ro Rotorua 110 140 4 ro Rotorua 51 429 4 wr Wairakei 0.2 48 4 wr
Wairakei 2.7 48 4 wr Wairakei 0.04 79 4 ld Larderello 230 632 5 ld
Larderello 300 527 5 ld Larderello 960 913 5 G1 The Geysers 45 165
6 ge The Geysers 3,700 597 6 ge The Geysers 2.7 44 6
Taran, 1984, 1988), geothermal systems of New Zealand
(Giggenbach, 1997a), and volcanic gases including White Island data
from Tables 1 and 2. Two clusters of data points can be seen: one
below 300C, which can be called hydrothermal, with the average
CH4/CO2 ratio close to 102, and another >300C, which can be
called volcanic, with the average CH4/CO2 near 10
4. The scattering of data
points is of three to four orders of magnitude for the same
temperature, and there are no trends along any buffer, though the
data for high-temperature ( 300C) hydrother- mal fluids are close
to the intersection between the FeO- FeO1.5 and the Taran (1988)
buffer lines. This may indicate a partial equilibration of CO2 and
CH4 under hydrother- mal conditions, and the scatter of data points
can be attrib- uted to the redistribution of CO2 and CH4 between
steam
and water, resulting from their different solubilities
(Giggenbach, 1980, 1987; Taran, 1986; Chiodini and Marini, 1998).
However, large deviations of data from the buffer lines of more
than 1.5 log units, or 100C, pre- cludes the use of CH4/CO2 ratios
as a geothermometer, as discussed by Chiodini and Marini
(1998).
The main reason for the apparent success of the Fischer- Tropsch
geothermometer is the temperature dependence of the hydrogen
partial pressure, which for liquid-domi- nated aquifers is very
steep (Taran, 1986; Giggenbach,
1991). For volcanic gases, as shown by Giggenbach (1987), 1
Average for The Geysers References: 1 = Giggenbach et al. (1990), 2
= this work, 3 = Chiba
Lowenstern et al. (1999)
For hydrothermal fluids, H2O is controlled by coexisting steam
and water and can be expressed as log H2O = log PH2O = 5.51 2,048/T
(Giggenbach, 1980). In this case:
log (CH4/CO2) log (PCH4/PCO2) =
log (XCH4/XCO2)v = log Kc + 4RH + 2log PH2O = (3a) 4,625/T
10.4,
where P and X are partial pressures and mole fractions,
respectively; subscript (v) stands for the vapor phase; Kc is
the equilibrium constant for reaction (2), and T is Kelvin.
(Giggenbach, 1987). The calculated PCH4/PCO2 ratio is very
sensitive to redox control because of the high weighting of the RH
in equation (3). For example, if RH is controlled by
the function proposed by DAmore and Panichi (1980):
log PCH4/PCO2 = 0.30 853/T (3b)
(Taran, 1988; Chiodini and Marini, 1998). The redox dia- gram in
Figure 1 is similar to that used by Giggenbach (1987, 1997a). Lines
represent RH control by rock buffers involving the minerals
fayalite, magnetite, hematite, and quartz, and the SO2/H2S gas
buffer. For details see Giggen- bach (1987), and more recent
discussion by Einaudi et al.
hydrogen partial pressure (concentration) is controlled by the
so-called gas buffer redox reactions between reduced and oxidized
sulfur species with H2S and SO2 as proxies (Fig. 2A). The XCH4/XCO2
ratio shows no obvious trend with temperature (Fig. 2B), but if
log(XCH4/XCO2) 4RH is plotted versus temperature, as it is done in
Figure 2C, a good correlation can be seen, with the trend close to
the calculated equilibrium with the gas buffer. Such a correla-
tion means that concentrations of CH4 in volcanic gases are
strongly controlled by the discharge temperature or that
chemical reactions with CH4 are very fast. But this does not make
sense. Methane cannot be easily produced from CO2 or oxidized to
CO2. However, equilibrium hydrogen con- centrations controlled by
the gas buffer attain equilibrium very fast and vary in the range
of 100 to 800C by more than eight orders of magnitude. Therefore,
the trend in Figure 2C is a consequence of the fast response of the
water thermal dissociation to temperature variations.
If there is no tendency to equilibrate, what is the reason of
the large variations of the CH4 concentrations in
hydrothermal and volcanic fluids? To answer this we can start by
assuming that most of the methane comes from organic-rich
sediments. One of the important signatures of natural gases
produced by the degradation of organic-rich sediments is their high
to very high N2/Ar ratio, because the degradation of organics
produces N2 but not Ar. This was shown by Jenden et al. (1988) and
Motyka et al. (1989) for natural gases from California and Alaska
and used by Giggenbach (1992, 1997b) to develop the triangular plot
of
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6 TARAN AND GIGGENBACH
FeO
log
PC
H4
/PC
O 2
logX
CH
4 /
XC
O2
4R
H
logX
CH
4 /
XC
O2
RH
= logX
H2 /
XH
2O
B
3
2
1
0
-1
-2
-3
-4
-5
-6
-7
-8
-9
-10
White Island
Other volcanoes
NZ hydrothermal systems
Other hydrothermal systems
200 400 600 800
Temperature C
A -1
-2
-3
-4
-5
-6
-2
-3
-4
FeO
1.5
FIG. 1. Variations in observed values of log XCH4/XCO2 in
hydrothermal fluids and volcanic gases (Tables 1 and 2) as a
function of sampling tem- perature. Solid lines = redox control by
potential mineral buffers involving fayalite-magnetite-quartz, the
FeO-FeO1.5 (fayalite-hematite-quartz) buffer of Gigenbach (1987),
magnetite-hematite, and the H2S/SO2 gas buffer at the brine H2O.
The Taran 1988 line = empirical (average) buffer of H2, according
to Taran (1988).
relative concentrations of N2, Ar, and He. If the main
source of methane in hydrothermal fluids is organic-rich
sediments, a correlation should exist between the CH4 con-
centration in the total discharge and the N2/Ar ratio. A high
proportion of magmatic fluids released from subduc- tion-related
volcanoes comes from the subducted oceanic sediments, rich in
organics. High N2/Ar ratios in volcanic
gases of subduction zones have been observed at many vol-
canoes, and this characteristic was interpreted as an indica- tor
of the subduction-type magmatic fluid (Giggenbach, 1992, 1997b).
However, in contrast to hydrothermal fluids circulating in the
upper crust, magmatic fluids, if contain- ing detectable amounts of
methane, should at the surface be characterized by CH4/CO2
ratios
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7 GEOCHEMISTRY OF LIGHT HYDROCARBONS X
CH
4 m
ole
fra
ction
XC
H4 m
ole
fra
ctio
n
XC
H4 m
ole
fra
ction
G
1E-4
1E-5
1E-6
ru
ro
pz
ni ni
ge
ld
ld ld
ro br
rates are high enough to equilibrate the C-H-O system by oxi-
dation of the excess methane. Even so, the equilibrium con-
centrations of the resulting CH4 are extremely low.
Giggenbach (1997a), using a selected set of gas analyses,
demonstrated an apparent equilibrium trend in CH4/CO2 ratios for a
set of samples starting from low-temperature,
1E-7
1E-8
mt br kw kw br cf
mo br
mo su br
ge kr ru
wr
CH4-rich natural gases, through medium CH4, CO2-
enriched natural gases from the high-heat flow gas deposits in
Thailand and ending with the high-temperature
hydrothermal systems in New Zealand. The apparent equi- librium
trend has little to do with the equilibration by chem-
wr
1E-9 wr
10 100 1000
N2/Ar
FIG. 3. The observed correlation between the concentration of
CH4
and the N2/Ar ratio in the fluids from geothermal wells and
steam vents listed in Table 4.
These data correspond to low-temperature fumaroles and most
probably are the result of a shallow subsurface boiling of a
condensed mixture between magmatic brine and mete- oric water
(Taran et al., 1997). A negative N2/Ar-CH4 cor- relation is clearly
expressed in both plots.
In summary, the concentrations of methane in subduction- related
hydrothermal and volcanic gases in general are not controlled by
temperature-dependent chemical reactions, and instead probably
depend on the mixing proportions from magmatic and sedimentary
sources. The exception for typical magmatic redox conditions may
exist at very high tem- peratures, near to magmatic environment,
where reaction
ical reactions involving CH4. Rather, the decrease in the
CH4/CO2 ratio is caused by the temperature-dependent CO2 production
from dissolution of reservoir carbonates and oxidation of organic
matter and, so, the observed trend reflects the admixture of CO2
from sedimentary sources.
Distribution of Higher Alkanes in Volcanic and Hydrothermal
Fluids
Equilibrium distribution of Cn (n > 1) hydrocarbons in
an aqueous fluid is always monotonic and depends on the redox
conditions, but for typical rock buffer systems and
pressures below 10 kbars, C1 > C2 >> Cn > Cn + 1...
For more oxidized conditions, the Cn/Cn 1 ratios are lower than for
reduced conditions, which can be seen from equa-
tions for subreactions controlling ratios Cn/Cn 1 of satu- rated
hydrocarbon chains:
CnH2n + 2 + 2H2O = Cn 1H2n + CO2 + 3H2. (4)
This is an expression of the so-called hydrolytic dispropor-
tionation of alkanes (Helgeson et al., 1993; Price and DeWitt,
2001), which skips the CH4 production step. Such a
presentation is convenient because it includes the redox term
H2. The equilibrium Cn/Cn 1 ratio can be found from the following
equation:
1E-3
A 1E-3 kr B
1E-4 1E-4
sw m
gr
1E-5
shallow boiling?
1E-5
1E-6
g mt e ku ku si
k m a
ch
n p
1E-6
White Island
1E-7 1E-8
ki sh
ki v
v v
100 1000 10 100 1000
N2/Ar N2/Ar
FIG. 4. Variations in the CH4 concentration in volcanic gases as
a function of their N2/Ar ratio. A. White Island fumaroles. B.
Other volcanoes. For codes see Table 2.
-
8 TARAN AND GIGGENBACH
log C
2H
6/C
3H
8
log C
H4/C
2H
6
log (XCn/XCn 1) =
3RH + log H2O + log CO2 log K4, (5) A 6
and the equilibrium constant for n = 2, 3, and 4 can be
approximated by the following:
log K4 = 10.5 (5,150 + 310n)/T (6)
(Taran, 1984). These hydrolytic disproportionation reac- tions
involve the stepwise breakage of a C-C bond of a higher carbon
number alkane. They represent a final stage of oxidation of one
link of the C chain to CO2, and the
reduction of the rest to the more positive nominal oxida- tion
state of carbon, in the terminology proposed by Helge-
son et al. (1993). They suggested that a set of these irre-
versible hydrolysis reactions at the oil-water interface produces
light gaseous hydrocarbons.
It follows from equation (6) that for hydrothermal temper-
atures of 250 to 300C, log K4 is close to zero, and the equi-
librium Cn/Cn 1 ratio can be calculated from the value of RH and
the total fluid pressure, if Ptotal = PH2O + PCO2 is assumed. The
RH values for hydrothermal conditions are always nega- tive, close
to 2.8, accepting the FeO-FeO1.5 buffer control. Thus, for
hydrothermal fluids where total pressure is 1 kbar) conditions. The
temperature relationships between temperature and CH4/C2H6 and
C2H6/C3H8 ratios in vol-
canic and hydrothermal fluids are shown in Figure 5 together
with equilibrium lines of redox buffers.
The fully empirical CH4/C2H6 geothermometer proposed
by Darling (1998) for geothermal systems is based on an
assumption that there are temperature-controlled reactions
5
4
3
2
1
0
B 2.5
2.0
1.5
1.0
0.5
0.0
-0.5
200 400 600800
Temperature C
consuming ethane and/or producing methane as tempera- ture
increases. We can suggest that this is the previously men- tioned
irreversible hydrolysis of ethane, facilitated at higher
temperatures. At close to magmatic temperatures one could expect
that the CH4/C2H6 ratio in hot volcanic gases should show a clear
temperature dependence compared to cooler hydrothermal fluids. The
data plotted in Figure 5A show that this is not the case. By
contrast, the CH4/C2H6 ratios in
White Island fumarolic gases (100800C) show no temper- ature
dependence or correlation with redox buffers or the geothermometer
line of Darling (1998). There is no indica- tion of temperature
correlation with the C2H6/C3H8 ratios,
which similarly remain almost constant over the whole tem-
perature range (Fig. 5B).
Following Sugisaki and Nagamine (1995), we plot analyt- ical
data and calculated equilibrium lines on the CH4/C2H6 vs. C2H6/C3H8
diagram (Fig. 6A) using the pressure-independent equilibrium, as
follows:
2C2H6 = CH4 + C3H8. (7)
The idea of metastable chemical equilibrium between adja-
FIG. 5. Variations in log CH4/C2H6 (A) and log C2H6/C3H8 (B)
values in White Island fumaroles as a function of sampling
temperature. For log CH4/C2H6 in (A) redox buffers are shown, as
well as the empirical CH4/C2H6 geothermometer line proposed by
Darling (1998). cent alkanes with a low carbon number (n 200C.
-
9 GEOCHEMISTRY OF LIGHT HYDROCARBONS
log C
2H
6/C
3H
8
log C
H4/C
2H
6
log C
H4/C
2H
6
A
4
3
B 2
4
1
3
0 2
-1 0 1 2 3 1
log C2H6/C3H8
0
Geothermal systems of
New Zealand
Dry pyrolysis of kerogen
2 -1
-1 0 1
2 3 4
1 log C2H6/C3H8
0
-1
-2
-1.5 -1.0 -0.5 0.0 0.5 1.0 1.5
log C3H8/C4H10
FIG. 6. A. Variations in log CH4/C2H6 vs. log C2H6/C3H8 and log
C2H6/C3H8 vs. log C3H8/C4H10 values in White Island fumaroles
(Table 1). The lines represent expected ratios for equilibrium at
100, 400, and 1,000C. B. Variations of log CH4/C2H6 vs. log
C2H6/C3H8 in hydrother- mal fluids of New Zealand (data from
Giggenbach, 1995) and in the prod- ucts of the dry pyrolysis of
kerogen (Tannenbaum and Kaplan, 1986).
In other words, there are some reaction pathways with fast
kinetics for the reversible breaking and forming of the C-C bonds.
Giggenbach (1997a) showed that this is only a coinci- dence and
that the irreversible thermodegradation of long carbon chains gives
the apparent equilibrium Cn/Cn 1 con- centration ratios due to
random breakage of C-C bonds. Fig- ure 6 demonstrates that, in
general, most of the data points for volcanic and hydrothermal
alkanes lie far from the equi- librium lines, and thus there are no
metastable equilibria among light alkanes under hydrothermal and
shallow mag- matic conditions. It should be noted that the CH4/C2H6
ratios for hydrothermal fluids vary 3 log units and that the
C2H6/C3/H8 ratio, in general, varies within 1 log unit (Fig. 6B).
Dry pyrolysis of kerogen and bitumen in the presence of clay
minerals at 200 to 300C as shown in Figure 6B gives
products with a much lower CH4/C2H6 ratio (Tannenbaum and
Kaplan, 1985).
Unsaturated Hydrocarbons in Volcanic Fluids
As was shown by Seewald (1994, 2001) in a series of labo- ratory
experiments at 300 to 350C and 350 bars pressure, low molecular
weight aqueous hydrocarbons interact with water and Fe-bearing
mineral assemblages under controlled redox conditions. The
stability of aqueous hydrocarbons at elevated temperature and
pressure reactions was found to be a function of time and
temperature but depended also on the oxidation state and the
presence of catalytically active aqueous sulfur species. However,
the main mechanisms of this interaction are the stepwise oxidation
and decomposi- tion of low molecular weight hydrocarbons and the
produc-
-
10 TARAN AND GIGGENBACH
log
C3H
8/C
3H
6
log
C2H
6/C
2H
4
tion of CO2-rich and methane-enriched gas. An important finding
from these experiments is that the alkane-alkene
4
pair and some other reduced-oxidized pairs with the same carbon
number attained metastable thermodynamic equi-
3
librium states. They react reversibly according to a general
simple redox reaction, as follows: 2
CnH2n + H2 = CnH2n + 2. (8)
The equilibrium constants of reaction (eq 8) for ethene- ethane
and propene-propane pairs can be approximated as follows:
log K (n = 2) = 6.82 + 7,337/T, (9)
log K (n = 3) = 6.32 + 5,676/T + 222,490/T2. (10)
For the dehydrogenation (oxidation) of alkanes and the formation
of alkenes more oxidized conditions, higher temperatures and lower
pressures are preferable. We sug- gest that under appropriate
geochemical conditions, this type of temperature-controlled
reaction can be found in nature. Unsaturated hydrocarbons are very
rare in hydrothermal fluids in detectable amounts, but they are
always present in volcanic gases (Tables 1 and 2). From Fig- ure 7,
where the ratios C2H6/C2H4 and C3H8/C3H6 are
plotted versus sampling temperature, the relative amount of
light saturated and unsaturated hydrocarbons with the
same carbon number is apparently controlled by the tem- perature
of a fumarolic vent. In other words, reaction (eq 8) in volcanic
gases seems to be very fast, similar to the ther- mal decomposition
of water that controls the H2/H2O ratio. In contrast to the
experimental conditions (Seewald, 2001) where hydrocarbons
interacted in the over pressured
1
0
A -1 4
3
2
1
0
-1 B
White Island Other volcanoes
200 400 600 800
Temperature C
and heterogeneous mixtures of water and mineral phases under
static conditions, reactions in volcanic gases are thought to take
place as the gas (vapor) phase flows through altered volcanic
rocks. The mass action equation for the reaction (eq 8) can be
written in the following form:
log (XCnH2n + 2/XCnH2n) = log K + RH + log H2O, (11)
where RH = log H2/H2O and K is one of the equilibrium constants
(eqs 9, 10). If, following Giggenbach (1987), it is assumed that
the fugacity of water vapor beneath the White Island crater is
controlled by vapor saturated brine (log H2O = 4.9 1,820/T for
-
11 GEOCHEMISTRY OF LIGHT HYDROCARBONS
C2H4
C2H4
canic gases are too high and very far from equilibrium even at a
high temperature. This may indicate that the source of hydrocarbons
in volcanic gases is buried organic matter of varying maturity.
Thermal degradation of these organics, probably by stepwise
hydrolytic disproportionation or by some other mechanism of
high-temperature thermal destruction, produces light hydrocarbons
with concentra- tions much higher than at equilibrium. However,
under high-temperature magmatic-hydrothermal conditions, light
alkanes are reversibly disproportionate to alkenes and hydrogen but
without breakage and rearrangement of the C-C bonds. Any reactions
involving the breakage of C-C bonds may be fast enough to produce
lower carbon num- ber hydrocarbons and eventually CH4, H2, and CO2;
how- ever, within the dynamic fluid flow system of a volcano, this
seems to be unlikely. The formation of new C-C bonds requires very
specific conditions and catalysts, and in the natural
high-temperature, magmatic-hydrothermal envi- ronment can be
practically excluded.
Benzene in Volcanic Gases
Benzene and more complicated volatile aromatics like toluene and
ethylbenzene were analyzed in volcanic and hydrothermal gases on
the parts per million and parts per billion level in dry gas
(Giggenbach and Corales, 1992; Capaccioni et al., 1995; Giggenbach,
1995; Darling, 1998). Aromatics are an important part of oil and
sedimentary organic material, and the aromatic ring itself
(benzene) is stable at a high temperature even under highly
oxidizing conditions. It may be that there is geochemical
importance in the fact that benzene can be synthesized in an empty
(catalyst-free) reactor at 950C from a CH4 air mixture with a yield
of 2.5 percent (York et al., 1996). This so-called oxidative
aromatization of methane is the subject of many studies in the
catalytic chemistry of hydrocarbons. Methane can be converted to
benzene in the presence of oxides like MoO3 or WO3, and the
mechanism of the aromatization
includes formation of ethane and ethene as intermediate
reactants (Arutunov and Krylov, 1998, and references therein). We
suggest that the presence of CH4 and unsatu-
rated hydrocarbons in volcanic gases could possibly control the
concentration of benzene. The thermodynamic con- straints can be
obtained from the following reaction:
3C2H4 = C6H6 + 3H2. (12)
The equilibrium constant can be approximated as log K12 = 1.36 +
3,446/T. Equilibrium (eq 12) is pressure dependent, and taking into
account that the total pressure in volcanic gases is controlled
mainly by the water vapor and log H2 = RH + log H2O:
ence of the saline brine or at 1 bar total pressure. In Figure
8A the data for White Island fumaroles lie between the FeO-FeO1.5
and gas buffer lines and also show a correlation
with temperature. At high temperatures, the data cluster near
the gas buffer lines. In Figure 8B and C, C6H6 and C2H4 trends
broadly correlate with temperature, despite considerable scatter.
These trends suggest that some fast reactions occur involving
unsaturated and aromatic hydro- carbons in volcanic gases. However,
these reactions cannot fully equilibrate benzene as well as alkanes
and alkenes. Their concentrations in volcanic (and hydrothermal,
see Giggenbach et al., 1990; Darling, 1998) fluids are many orders
of magnitude higher than expected for full equilib- rium. A
decrease in the C6H6 concentration with an
increasing temperature suggests that benzene is irreversibly
consumed (reduced?), partially converting to alkenes, and that new
C-C bonds do not form under high-temperature volcanic-hydrothermal
conditions. In other words, oxida- tive or reductive degradation
are the only mechanisms of equilibration for hydrocarbons and CH4
in the high-tem- perature crustal environment. Relationships
between con- centrations of alkanes and alkenes with the same
carbon number, or between ethane and benzene, showing close to
equilibrium ratios of concentrations, most probably corre- spond to
metastable equilibrium; without forming or rear- ranging C-C bonds,
the kinetic barriers of reactions ("waves in the metastability
pond; Giggenbach, 1997a) are much lower than for the full
disproportionation of hydrocarbons to CO2, H2, and H2O.
Concluding Remarks
The application of the CO2-CH4 reaction (eq 2) as a
geothermometer for hydrothermal fluids suggests that full
equilibrium between members of the equation can be attained, or
that methane (and other hydrocarbons) can be produced from CO2
under hydrothermal conditions simi-
lar to those in industry where the Fischer-Tropsch synthesis is
the basis for the multitonnage production of various H-
O-C-chemicals (Storch et al., 1951; Anderson, 1984). The original
Fischer-Tropsch synthesis is a catalytic reaction of so-called
synthesis gas CO/H2 mixture of different pro- portions conducted on
native metal catalysts with the redox state corresponding to the
pure H2-CO mixture. These con-
ditions are not generally typical for the crust as a whole.
However, they may exist on a large scale along ocean-
spreading zones or locally within ophiolite formations where
present-day serpentinization of Mg-rich mafic rocks can produce
highly reducing conditions (Abrajano et al., 1988; Lyon and
Giggenbach, 1990; Sano et al., 1993; Taran et al., 2002).
Experiments confirm the possibility of reduc- ing CO2 to produce
CH4 during serpentinization of olivine (Berndt at al., 1996; Horita
and Berndt, 1999; McCollom
log XC6H6/X3 = log K12 3RH log H2O. (13) and Seewald, 2001).
Limited bodies of coal and oil heated to a sufficiently high
temperature by magmatic sources, as
Here Xi is concentrations in mole fraction of the total fluid.
Lines in Figure 8 represent the equilibrium XC6H6/X
3
ratios expected for the gas and rock (FeO-FeO1.5) buffers
of the hydrogen fugacity with H2O controlled by the pres-
is the case for some geothermal fields in Kamchatka (Taran,
1988), could also be important. Whatever the real environment is,
the hydrocarbons produced by the Fischer- Tropsch reaction should
have a very special distribution,
-
12 TARAN AND GIGGENBACH
work like a normal industrial Fe-Co or Fe-Ni catalyst, yield-
ing the same set of products with the same distribution, same
conversion, and same selectivity. The main feature of the alkane
distribution in the Fischer-Tropsch reaction is a maximum at a
carbon number (n) between 3 and 5, depending mainly on two kinetic
parameters, the probabil- ity of the chain growing at the end or
the chain growing at the next-to-end carbon atom (Anderson, 1984).
The distri- bution is called the Anderson-Shultz-Flory
distribution, which for long chains does not differ from the
Shultz-Flory
200
400 600 800
distribution and can be evaluated for the random chain growth or
breaking. The production of ethane in the Fis- cher-Tropsch
synthesis is always minimal for 1 < n < 6
logX
C6H
6
3lo
g X
C2H
4
log X
C2H
4
log X
C6H
6
Yie
ld,
mole
%
28 A 60
24 50
20 40
16
30
Basalt
Rhyolite
Dacite
250C, 50 atm
H2:CO = 1:1
FeCo
12
-6.0 20
B -6.5
10
-7.0
-7.5
-8.0
-8.5
0
1 2 3 4 5 6
Carbon Number (n)
-9.0
-6
-7
FIG. 9. Distribution of light alkanes in the Fischer-Tropsch
synthesis on volcanic rock catalysts (Taran et al., 1981) and the
Co-Fe industrial catalyst (one of numerous examples from Storch et
al., 1951).
C
-8
-9
-10
Temperature C
FIG. 8. Variations in the quotient log XC6H6 3logXC2H6 (A),
benzene (B), and ethene (C) concentrations in the total discharge
(mole fractions) of fumarolic gases from White Island, as a
function of the sampling tem- perature (Table 1).
quite different from those of natural CH4-rich gases or any
natural gases from the Earths crust (Anderson, 1984).
Figure 9 shows the distribution of alkanes in the Fischer-
Tropsch synthesis from a 1/1, CO/H2 mixture, at 250C
and 50-bar pressure in a flow-through reactor using basalt,
dacite, and rhyolite as catalysts (Taran, 1980; Taran et al.,
1981). The reaction has a long inductive period involving reduction
of part of the iron in the rock to the native form but mainly to
magnetite. Then, this natural catalyst starts to
because its next-to-end carbon is the end atom and ethane
becomes an actively consuming intermediate in the Fischer- Tropsch
synthesis.
It should be noted that Fischer-Tropsch distribution of the
light alkanes has never been observed in natural gases, including
volcanic and hydrothermal gases. Instead the dis- tribution of
light alkanes in terrestrial gases is very similar to those
obtained in experiments on thermal decomposi- tion (catalytic or
not) of kerogen (Tannenbaum and Kaplan., 1985) and model organic
compounds (Jackson et al., 1995) produced by the catalytic
decomposition of oil or a long linear alkane in the presence of H2
(Mango, 2000).
The main crustal process involved with the transforma- tion of
organic-rich sediments, including oil and gas, is recombination and
oxidation. Oil may dissipate probably by a stepwise hydrolytic
disproportionation mechanism
-
13 GEOCHEMISTRY OF LIGHT HYDROCARBONS
(Helgeson et al., 1993; Price and DeWitt, 2001), eventually
converting in the oil-water interface to CO2 and CH4 at ele-
vated temperatures and pressures. Methane in the presence of
oxides can participate in a number of reactions of oxida- tive
conversion (Arutunov and Krylov, 1998), producing minor amounts of
more complex hydrocarbons, oxy- genated hydrocarbons, and
eventually, CO2 and H2O. This is probably the most important
mechanism of leading to equilibration of CH4 and CO2 in
high-temperature
hydrothermal systems. Terrestrial hydrothermal systems and
volcano-hydrothermal systems do not produce methane and
higher hydrocarbons except through conversion of organic
material at a high temperature.
Acknowledgments
This work was supported by the Marsden project Under- standing
Crustal Fluids and partially by a grant from Okayama University. I
wish to thank Ian Graham for the invitation to participate in the
project and Agnes Reyes for assistance with Werners data and
archives. Many thanks to Doug Sheppard for supplying much of the
unpublished data on the gas chemistry of White Island and for his
per- mission to use them. Discussions with Jeff Hedenquist and
Minoru Kusakabe were very helpful. Marino Martini and Jeff Seewald
have provided constructive reviews. I am espe- cially grateful to
Stuart Simmons for the effort he put into the improvement of the
paper.
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