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Transcript of Theoretical analysis for the heterogeneous decomposition of hydrogen sulfide to hydrogen on an...
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Applied Surface Science 253 (2006) 2327–2335
Theoretical analysis for the heterogeneous decomposition of
hydrogen sulfide to hydrogen on an iron-metallic plate in
a laminar stagnation-point flow
J.C. Martınez a, F. Mendez b,*, C. Trevino c
a Facultad de Ingenierıa, Universidad Autonoma de Campeche, 24030 Campeche, Mexicob Facultad de Ingenierıa, Universidad Nacional Autonoma de Mexico, 04510 Mexico DF, Mexicoc Facultad de Ciencias, Universidad Nacional Autonoma de Mexico, 04510 Mexico DF, Mexico
Received 4 August 2005; received in revised form 11 January 2006; accepted 21 April 2006
Available online 8 June 2006
Abstract
In this work, we have theoretically analyzed the conversion process of hydrogen sulfide, H2S, to atomic hydrogen, H0, in a planar stagnation-
point flow over an iron-metallic surface. We assume that a binary mixture of hydrogen sulfide and methane composes the laminar stagnation flow.
In order to characterize this complex phenomenon with very specific chemical activities on the surface of the metallic plate, we propose a
heterogeneous reaction scheme based on four reactions: two electrochemical, one adsorption and an additional exothermic reaction needed to
complete the direct conversion of hydrogen sulfide to hydrogen on the surface of the iron. The nondimensional governing equations, which include
the mass species and momentum conservation of the mixture and the molecular diffusion of hydrogen into the iron plate, are numerically solved by
conventional finite-difference methods. The numerical results show the critical conditions of the H2S decomposition as functions of the involved
nondimensional parameters of the present model. In particular, we show parametrically the influence that has the initial concentration of H2S on the
surface coverage of the chemical products HS� H+ and H0 derived from the chemical and electrochemical reactions.
# 2006 Elsevier B.V. All rights reserved.
PACS: 82.30.Lp; 82.40.-g
Keywords: Hydrogen sulfide; Stagnation flow; Heterogeneous reactions; Iron plate; Hydrogen diffusion
1. Introduction
Nowadays, the analysis of hydrogen sulfide decomposition
is a multidisciplinary field of fundamental importance due to
that numerous examples and applications can modify severely
the operation and performance of different industrial devices.
For instance, in the petroleum industry, the so-called sour
corrosion originated by the presence of hydrogen sulfide in oil–
gas mixtures, can either accelerate or inhibit corrosion of iron
tubes under different conditions. In these chemical and physical
interactions between sour mixtures and metallic surfaces, the
component H2S generates atomic hydrogen, H0, at the iron
surface and this chemical specie penetrates into the metallic
body, which yields cracking and multiple fractures as a clear
* Corresponding author. Tel.: +52 55 56228103; fax: +52 55 56228106.
E-mail address: [email protected] (F. Mendez).
0169-4332/$ – see front matter # 2006 Elsevier B.V. All rights reserved.
doi:10.1016/j.apsusc.2006.04.044
evidence of the corrosive process. In fact, the hydrogen in the
form of proton, H+, behaves as an ultra-fast diffuser in many
metals and alloys and different effects like electrolysis,
electroplating, aqueous corrosion, welding, etc. have a
profound influence to control the above diffusive process.
Therefore, the simultaneous presence of these combined effects
affects drastically the mechanical properties of metals and
alloys, reducing the average lifetime of metallic or dilute binary
alloy structures. A basic discussion of the above and related
aspects can be found in Glicksman [1]. The specialized
literature offers abundant experimental evidence to show this
corrosion type, including also sour solutions with the presence
of carbon dioxide CO2. In this direction, the recent work of Ren
et al. [2] clarifies as the simultaneous influence of H2S and CO2
can accelerate or inhibit the corrosion mechanism in circular
steel tubes. Similar experimental studies were reported by
Garcıa et al. [3] and Houyi et al. [4], showing the corrosive
effects caused by the decomposition of H2S. In general, the
J.C. Martınez et al. / Applied Surface Science 253 (2006) 2327–23352328
most popular experimental techniques traditionally used to
explore the corrosion process in metallic bodies are based on
electrochemical, X-ray diffraction method and the above works
offer useful information about the use of these techniques.
Other interesting application directly related with the
petroleum industry is the use of metal oxides in reactors. In
these systems, we find that the metal oxides can operate as non-
catalyst and catalyst substrates for the processes of desulfur-
ization and denitrogenation of oil–gas mixtures with high
content of H2S. For instance, Wu et al. [5] studied
experimentally the adsorption and desorption mechanisms of
H2S on a polycrystalline UO2 catalytic sample, operating under
non-isothermal conditions. They used an ultrahigh vacuum X-
ray chamber containing instrumentation to collect experimental
data with photoelectron spectroscopy, low energy ion scattering
and temperature programmed desorption techniques. The
experimental results obtained for different temperatures of
the catalyst show the dissociative character of the component
H2S. Other experimental studies have also been performed with
different metal oxides and similar results were reported by
Reshetenko et al. [6]. They investigated experimentally the
reaction of heterogeneous decomposition of the hydrogen
sulfide on bulk oxides g-A12O3, a-Fe2O3 and V2O5 in the
interval of temperature 500–900 8C. In these studies, the main
objective is focused on the design of membrane reactors, which
offer evident advantages for the hydrogen production by means
of the direct decomposition of H2S. Chan et al. [7] used a
catalytic-membrane reactor containing a packed bed of Ru-Mo
sulfide catalyst to investigate the H2S decomposition. In order
to validate their experimental results, they developed also a
one-dimensional analytical model under non-isothermal con-
ditions, examining in detail the effect of some hydrodynamic
and transport properties on the decomposition of H2S to H0.
They showed that the nondimensional Reynolds and Peclet
numbers (which define the hydrodynamic and transport
conditions of the acid mixtures), affect dramatically the
conversion of H2S. A practical advantage of this type of
catalytic reactors, among others, is that the recovery of H0 from
H2S is a plausible economical alternative to the conventional
Claus process widely used in petroleum and minerals
processing industries, Chan et al. (op. cit.).
Recognizing that the study of the H2S conversion is very vast
and complex, we have included some additional references [8–
13] that offer sufficient details to appreciate correctly the
fundamental and practical importance of these processes.
However, apart from the work of Chan et al., the majority of
the above works together with the references [2–6] only give
experimental evidence of this decomposition for different
applications. To our knowledge, new theoretical methodologies
and predictions in the specialized literature are missing. There-
fore, in the present work we study theoretically the conversion
process of hydrogen sulfide into atomic hydrogen, using a simple
analytical model that takes into account the following fact:
In order to accelerate the corrosive process under laboratory
conditions is indispensable to elevate gradually the temperature
of the catalytic surface to control, among other factors, the
simultaneous adsorption–desorption reactions. However, the
corrosion in typical cases, particularly in petroleum industry is
not manifested immediately. Therefore, it should be accepted
that at room temperature (as normally are operating some
equipments of the petroleum industry), the chemical and
electrochemical interactions between oil–gas mixtures (with a
given percentage of H2S) and metallic structures are, in general,
very slow processes, and in a first approximation, the desorption
reactions are negligible. Then, we have not considered necessary
the use of a catalytic surface to accelerate the conversion of H2S.
Instead; we choose a simple iron plate immersed in a sour
environment composed by a binary mixture of methane and
hydrogen sulfide. The mixture as well as the iron plate is found at
room temperature. In this sense, the present physical config-
uration is in accordance with real prototypes frequently used in
laboratory conditions. In fact, in the previously cited works non-
isothermal catalytic surfaces or electrochemical cells are
exposed to very strong acid ambient to promote rapidly the
corrosive effect. Therefore, the present physical model is
visualized as an isothermal mixture of methane and hydrogen
sulfide flowing perpendicularly to an iron horizontal plate. In the
following sections, we derive the mathematical model and
showing the corresponding numerical results that are obtained
with conventional finite-difference methods. However, we
anticipate that the mass transport of hydrogen sulfide from the
mixture to the iron plate, the heterogeneous conversion of H2S to
H0 on the surface of the metal and the diffusive transport of it
through the iron plate, represents a conjugate mass transfer
problem, because the corresponding mathematical formulation
reflects just this simultaneous mixture-metallic surface interac-
tion. Therefore, the present work is organized following this
structure: first, we derive theoretically the conjugate mass
transfer-conversion problem, which is required to solve the
heterogeneous decomposition of hydrogen sulfide on an iron-
metallic plate in a laminar stagnation-point flow and second, we
include other sections to show specifically numerical results,
discussion and conclusions.
However, we must emphasize that the present theoretical
predictions must be completed and compared with experimental
results. To our knowledge, this particular mechanism of
heterogeneous decomposition of the specie H2S in a sour-gas
mixture on a iron-metallic plate subject to a laminar stagnation
flow has still not been previously treated with some measurement
techniques in order to show experimental evidence. In this
direction, we consider that novel techniques like cross-sectional
scanning electron microscopy (SEM) images and scanning
electrochemical microscope (SECM) used to estimate the
surface coverage of metallic vapor deposition and catalytic
activity on surfaces can be preliminarily used to obtain
experimental data.
2. Theoretical formulation
2.1. Governing equations for the gas-phase mixture and for
the iron plate
In Fig. 1, we show the physical model, coordinate system
and a sketch of the stagnation-point flow configuration.
J.C. Martınez et al. / Applied Surface Science 253 (2006) 2327–2335 2329
Fig. 1. Schematic diagram of the physical model.
The system of coordinates is located on the vertical axis of
symmetry of the plate. Also in this figure, x and y denote the
horizontal and vertical axis, respectively. A binary mixture of
methane and hydrogen sulfide with mass concentrations
denoted by YCH4and YH2S, respectively, flows permanently
with a gradient velocity a and ambient temperature T1,
perpendicular to the iron horizontal plate of finite thickness h.
We assume that the iron plate is found also at ambient
temperature T1 and in the lower surface of the plate, the
presence of hydrogen is absent. Due to heterogeneous
electrochemical and chemical reactions on the surface of the
iron plate (the detailed reaction mechanism will be providing in
the following subsection), continuously is carried out the
decomposition of H2S to H0. Therefore, for the binary mixture
zone (we assume that in this region, no exist homogeneous
reactions of any type), the stagnation-point boundary layer
governing equations are the following: mass and momentum
equations,
@u
@xþ @v
@y¼ 0; (1)
ru@u
@xþ rv
@u
@y¼ m
@2u
@y2þ ra2x; (2)
the term—ra2x represents the pressure gradient that is easily
obtained by using the boundary layer theory, Schlichting [14].
Here, u and v are the longitudinal and transversal components
of the velocity vector and a is a constant related with the
velocity. r and m represent the density and dynamic viscosity of
the mixture, respectively. During the decomposition process of
H2S to H0, we assume uniform values for the properties of the
mixture. On the other hand, the mass conservation equation by
specie can be written as,
u@Yi
@xþ v
@Yi
@y¼ Di
@2Yi
@y2(3)
where i = CH4 or H2S and Di is the molecular diffusion coeffi-
cient of the specie i. Furthermore, we accept a global mass
conservation between both species, given by the relationshipPYi ¼ 1. Therefore, we require only considering the mass
conservation equation of the hydrogen sulfide H2S. In addition,
in order to solve the system of Eqs. (1)–(3); we need appropriate
boundary conditions. Far from the iron plate, we have that,
y!1 : u ¼ ax; YH2S ¼ YH2S1 ; (4)
where YH2S1 and u represent the mass concentration of H2S and
the longitudinal component of the velocity u = ax evaluated
both at infinity, respectively. This last condition is easily
derived from the potential theory of a stagnation laminar flow.
Other relevant boundary conditions are directly related to the
heterogeneous reactions at the upper surface of the iron. At
room temperature, the methane gas is inert and therefore cannot
react with the iron surface. However, due to the presence of H2S
into the mixture, the contact of this specie with the metal can
induce a dissociative adsorption. Nelen et al. [11] and Lai et al.
[15] have supported spectroscopic experimental evidence of
this chemical dissociation, using metals in contact with a sour
ambient composed basically by H2S and operating at room
temperature or lower than it. In addition, Wilhelm and Abayar-
athna [16] using electrochemical cells showed that the hydro-
gen permeation could be utilized to investigate hydrogen
sulfide adsorption in refinery environments. In the past, the
concept of dissociative adsorption has been widely studied and
we suggest the work of Somorjai [17] to see details that are
more specific. Therefore, we accept the existence of this
molecular dissociation (together with the chemical kinetic
given in the next section), destroys the hydrogen sulfide and
inversely, atomic hydrogen is created at the surface of the iron.
Hence, we propose the following mass-transfer boundary con-
ditions, together with the classical hydrodynamic conditions for
the velocity’s components,
y ¼ 0 :@YH2S
@y� v9GWH2S
rDH2S
¼ @YH0
@y� v11G
DH0
¼ 0 and
u ¼ v ¼ 0:
(5)
Here, WH2S is the molecular weight of specie H2S. v9 and v11
are the surface reaction rates in units of mol of H2S and H0
destructed and created by unit time and unit surface of the plate,
respectively. The parameter G and appropriate laws for the
reaction rates vj (here j denotes the equation number corre-
sponding to the heterogeneous reaction model defined by
Eqs. (8)–(11), given lines below), are defined in the following
section. The above mass transportation boundary conditions
represent the compatibility conditions needed to solve the
conjugate mass transfer problem. Because the mass concentra-
tion YH2S and molar concentration YH0 at the upper surface of
the iron metal are unknowns, we need additional information
provided by the molecular diffusion of the hydrogen into the
iron metal. In the present work, we adopt a simple model for the
molecular diffusion of hydrogen, taking into account the crea-
tion of this specie at the iron surface. However, it is important to
mention that in the present model, we avoid to consider
sophisticated diffusion models, which take into account unsa-
turable traps. Physically, the appearance of these traps is similar
J.C. Martınez et al. / Applied Surface Science 253 (2006) 2327–23352330
to fissures or voids where hydrogen as proton, H+, remains
trapped into the metals in large concentrations causing poten-
tially the corrosion phenomenon [1]. Considering stationary
conditions, we propose
@2YH0
@y2¼ 0; (6)
together with,
y ¼ �h : YH0 ¼ 0; (7)
2.2. Heterogeneous reaction model
We assume a surface reaction model to describe the
simultaneous reactions of the dissociative adsorption of H2S
and the oxidation of iron metal. In general, Nelen et al. [11] and
Lai et al. [15] showed that this dissociative adsorption is
selective, depending strongly on surface and temperature
conditions. On the other hand, the first step to yield corrosion in
metals comes from the anodic reaction of the metal with the
sour environment. This result has been widely confirmed
experimentally in the above works [11,15,16]. In this
electrochemical reaction, there is an electronic interchange
between the sour ambient and the iron metal, which easily
conducts to the formation of Fe2+. Thus, we follow the above
works together with recent experimental evidence of Cabrera
et al. [18] to propose the following reaction model:
Fe ! Fe2þ þ 2e�; (8)
H2S ! HS� þHþ; (9)
Fe2þ þHS� ! FeS þ Hþ; (10)
Hþ þ e� ! H0; (11)
thus, electrochemically, when the iron metal is in contact with
the sour mixture, the HS� ion is reduced to hydrogen atomic
H0, reacting with Fe2+ and in this form, ferrous sulfide, FeS, is
formed at the metal surface. However, it is very important to
note that this mechanism does not contain the adsorption–
desorption of the film product FeS, as well as the adsorption
of methane gas CH4. Surface films of FeS can retard the
corrosion process. However, we assume moderate generation
rates for this component. In this reactive scheme, we have
assumed that the specie HS� reacts necessarily with Fe2+;
otherwise, the generation of ions H+ would be drastically
reduced. On the other hand, the adsorption kinetic is given
by a sticking probability, Si or accommodation coefficient,
which represents the portion of the collisions with the surface
that successfully leads to adsorption, [17]. Since we have only
one adsorption reaction given by Eq. (9), in the following lines
we denote this coefficient as Si = k9. In addition, the rate of
collisions, Zw, can be computed by using the classical kinetic
theory and the specie concentrations at the surface can be
represented by the surface coverages ui. This is defined as
the ratio of the number of sites occupied by surface species i to
the total number of available sites. Considering the stationary
case, then the steady-state governing equations can be written
as
uv þ uHS� þ uHþ þ uH0 ¼ 1; (12)
duHS�
dt¼ v9 � v10 ¼ 0; (13)
duHþ
dt¼ v9 þ v10 � v11 ¼ 0 (14)
and since the mechanism of surface coverage of the hydrogen is
affected by the presence of diffusion of this specie into the
metal; then the corresponding reaction rate can be written as
duH0
dt¼ v11 �
DH0
G
���� @CH0
@y
����y¼0
¼ 0: (15)
In the above relationships, uv denotes the surface coverage of
empty sites. All the reaction rates, vj, in above equations are in
s�1 units and are defined by,
v9 ¼ k9u2v; v10 ¼ k10uvuHS� ; v11 ¼ k11uHþ (16)
and the kinetic factors kj as
k9 ¼S2
0PM
G ð2pWH2SRTÞ1=2exp
�� DE9
RT
�; (17)
k10 ¼ A10exp
�DE10
RT
�; (18)
k11 ¼kBT
hP
exp
�� ne11FDV11
RT
�: (19)
In the above relationships, S20 is the pre-exponential factor of the
sticking coefficient between the hydrogen sulfide and the iron
and is of order of 0.02, [19]. The superscript ‘‘2’’ on S20
represents the dissociative character of this reaction.
G = (NV)/(NA) � 3 � 10�27 mol/cm2 is the surface molar con-
centration and corresponds to the surface site density divided by
the Avogadro’s number. Here, NV ¼ Naexpð�Qv=kBTÞ (in
units of sites/cm2) and represents the total number of vacancies
formed by thermal agitation per unit surface; Na is the total
number of atoms in the solid, is the energy required to form a
vacancy, which Qv depends on the material and is of order of
�1.08 eV (see references [20,21] for more details) and NA is the
Avogadro’s number (=6.0225 � 1023 molecules/mol). R is the
universal gas constant (=8.3143 J/K mol), ne11 = 1 and repre-
sents, in general, the number of participating electrons in the
electrochemical reaction [Eq. (11)], F is the constant of Fara-
day (=9.6487 � 104C/mol), kB is the Boltzmann’s constant
(=1.3805 � 10�23 J/K) and hP is the constant of Planck
(=6.6256 � 10�34 J s). Furthermore, T is the temperature in
Kelvin and PM is the pressure of the mixture of H2S and CH4;
we assume in the numerical calculations that both are fixed
parameters, which means that the mixture during the stationary
reactive process is subject to isobaric and isothermal condi-
tions. The reactant concentrations, YH2Sw, YH0w
, etc. are the
surface concentrations and are obtained after solving the
YH2Swcoupled gas-phase equations with the governing
J.C. Martınez et al. / Applied Surface Science 253 (2006) 2327–2335 2331
equations for the surface coverage of the adsorbed species,
together with hydrogen diffusion into the metal. We can
anticipate that at room temperature conditions, the surface
coverages corresponding to the species HS� and H0 are pre-
dominant, indicating a rich generation of hydrogen.
It is important to mention that the contact of the metal with
the sour mixture yields spontaneously a cell-electrochemical
potential of magnitude DV8. Because at room conditions this
electrochemical potential is of order of 0.44 V [22], with the aid
of the Faraday’s law, the corresponding electrochemical energy
associated with this reaction is DE8 = ne8FDV8 with ne8 = 2
(reciprocally, the electrochemical energy associated with
reaction (11) is zero, because DV11 = 0). Therefore, we assume
that this electrochemical energy is used to initiate the
adsorption reaction, Eq. (11), which is equivalent to write
DE8 = ne8FDV8 � DE9. Finally, the stationary condition is used
in Eqs. (12)–(16) to derive, after some simple algebraic
manipulations, that surface coverage of the products are
directly related to uV by means of the following relationships,
uHS� ¼k9
k10
uv; uHþ ¼2k9
k11
u2v and
uH0 ¼ 1� uv �k9
k10
uv �2k9
k11
u2v;
(20)
3. Nondimensional governing equations
The set of coupled governing Eqs. (1)–(20) can considerably
simplify by introducing appropriate nondimensional variables.
The main advantage is to reduce the number of involved
physical parameters. In particular, for the gas phase we
introduce a stream function c to satisfy the global mass
conservation, Eq. (1): u = @c/@y and v ¼ �@c=@x. In this case,
the governing equations for the gas-mixture region have a
similarity solution. Therefore, we define the following
nondimensional variables
h ¼ y
d¼�
ra
m
�1=2
y; j ¼ � y
h; f ¼ c
xðam=rÞ1=2;
YH2S ¼YH2S
YH2S1
and CH0 ¼ YH0
ðYH2S1Þm:
(21)
In the above change of variables, we use (YH2S1 )m to denote
molar concentration of H2S at infinity. The resulting nondimen-
sional governing equations now take the form
d3 f
dh3þ f
d2 f
dh2��
d f
dh
�2
þ 1 ¼ 0; (22)
d2YH2S
dh2þ ScH2S f
dYH2S
dh¼ 0; (23)
where ScH2S is the Schmidt number of H2S, given by
ScH2S ¼ m=ðrDH2SÞ. The nondimensional boundary conditions
are then given by
h!1 :d f
dh� 1 ¼ YH2S � 1 ¼ 0; (24)
h ¼ 0 : f ¼ d f
dh¼ 0; (25)
and the compatibility conditions at the upper surface of the iron
plate as
dYH2S
dh
����h¼0
¼�
n1a
�1=2k9GWH2S
rDH2SYH2S1
u2v;
@CH0
@j
����j¼0
¼ � hk9GWH2S
rDH0 YH2S1
u2v;
(26)
which can be combined in only one relationship,
� bdYH2S
dh
����h¼0
¼ @CH0
@j
����j¼0
; (27)
where the nondimensional parameter b is defined as
b ¼ DH2S=ðm=raÞ1=2
DH0=h; (28)
and represents the competition between the rate of molecular
diffusion of hydrogen sulfide into the momentum boundary
layer thickness of the mixture zone to the rate of hydrogen
diffusion along the thickness of the iron metal. In fact, an order
of magnitude analysis reveals that the momentum and mass
transfer boundary layers at the mixture zone are given by
d � (m/ra)1/2 and dDeðDH2S=aÞ1=2; respectively. Therefore,
the ratio of both thicknesses is related to the Schmidt number
through the relationship d=dD ¼ Sc1=2H2S. In addition, we use the
coordinate h defined in relationships (21) in order to avoid that
the momentum boundary layer, Eq. (22), depends on any
nondimensional parameter. This is an advantage from the
numerical point of view, because the numerical solution of
Eq. (22) will be universal and can be found elsewhere, [14].
However, our numerical calculations included the numerical
solution of this equation in order to solve necessarily Eq. (23).
The details are given in the next section.
On the other hand, the molecular diffusion of hydrogen into
the iron is governed by the following equation,
@2CH0
@j2¼ 0; (29)
and at j = 1 we have imposed for simplicity that,
CH0 ¼ 0: (30)
3.1. Numerical procedure
In this section, we describe briefly the iterative scheme to
solve the set of Eqs. (22)–(30), together with the surface
coverage relationships (20). The procedure is the following:
we assume an arbitrary or initial value for the nondimen-
sional concentration of hydrogen at the surface of the iron
J.C. Martınez et al. / Applied Surface Science 253 (2006) 2327–23352332
Fig. 3. Surface coverage of the product H+, uHþ , as a function of the non-
dimensional parameter k9/k10 and different values of the nondimensional
concentration YH2S1 .
metal, ðCH0Þi, in order to know the right-hand side of
boundary condition (27). Thus, assuming a given value of the
nondimensional parameter b, we obtain the concentration
gradient of H2S at the surface of the iron plate and therefore,
the governing Eqs. (22)–(25) for the region of binary mixture
can be solved in a closed form. However, this initial value of
ðCH0Þi is not sufficient to guarantee that the boundary
condition (24), h!1: Y! 1 is fulfilled. Therefore, we
develop a simple iterative scheme on ðCH0Þi in order to satisfy
this condition. Hence, we solve the ordinary differential
Eqs. (22)–(25) with the Runge-Kutta’s technique of fourth-
order, together with an appropriate shooting method to obtain
the optimal number of iterations that guarantee the
satisfaction of the above boundary condition at infinity.
Once that we have correctly found the right-hand side of the
Eq. (27); we replace the concentration gradient of H2S into
Eq. (26) to estimate uv. The other surface coverages of the
products HS�, H+ and H0 are evaluated with the aid of the
relationship (20). In addition, the solution of the binary
mixture governing equations permits to know, among other
results, the value of the nondimensional concentration of H2S
at the surface.
4. Results
In this section, we show the numerical results obtained by
solving numerically the system of Eqs. (22)–(30), together with
the stationary coverage relationships (20). All numerical
calculations were performed with the following data: Schmidt
number ScH2S ¼ 1:8, b = 4.9922 � 10�2 and Figs. 2–11 were
plotted with a room temperature of T1 = 300 K, except Fig. 12,
for which we have analyzed the influence of the parameter G on
the nondimensional surface concentration of the hydrogen, CH0 ,
in the temperature interval 300 K < T < 500 K. Under these
conditions, k9 = 2.85 � 104 s�1 and k11 = 6.25 � 1012 s�1; how-
ever, we have not sufficient data to estimate k10. Therefore, we
Fig. 2. Surface coverage of the product HS�, uHS� ; as a function of the
nondimensional parameter k9/k10 and different values of the nondimensional
concentration YH2S1 .
assign arbitrary values to this parameter. In this sense, we present
the numerical predictions by using the nondimensional ratio k9/
k10 as a relevant parameter to understand the decomposition
process. In Figs. 2–5 we have plotted the surface coverages of the
product species HS�, H+, H0 and the vacancy surface coverage uv
as functions of the nondimensional parameter k9/k10 with four
different values of the hydrogen sulfide mass concentration at
infinity, YH2S1 ; respectively. Hence, in Fig. 2 we can appreciate
the surface coverage of HS�, uHS� as a function of the parameter
k9/k10. Here, the influence of this parameter is clear because for
increasing values of k9/k10, the surface coverage is also increased
and this behavior is amplified for increasing values of the initial
concentration of H2S. In the approximated interval 0.03 9 k9/
k10 9 70, we obtain the major sensitivity to this parameter. For
Fig. 4. Surface coverage of the product H0, uH0 , as a function of the non-
dimensional parameter k9/k10 and different values of the nondimensional
concentration YH2S1 .
J.C. Martınez et al. / Applied Surface Science 253 (2006) 2327–2335 2333
Fig. 5. Surface coverage of the vacancy sites, uv, as a function of the non-
dimensional parameter k9/k10 and different values of the nondimensional
concentration YH2S1 .
Fig. 7. Surface coverage of the product HS�, uHS� , as a function of the
nondimensional concentration YH2S1 and different values of the nondimen-
sional parameter k9/k10.
instance, for k9/k10 = 1, the increments in uHS� are very
pronounced and just for this value of the parameter k9/k10, the
surface coverage uHS� reaches maximum values. In Fig. 3, we
show similar results for the surface coverage of H+, uHþ . In this
case, we obtain the opposite behavior: for increasing values of the
parameter k9/k10, the surface coverage uHþ , decreases. However,
this effect is attenuated if the initial concentration of H2S is
increasing. This result is interesting because the presence in the
mixture of this specie reflects the incipient activity of the
heterogeneous surface reactions in order to yield this specie. In
the limit of small values of the nondimensional parameter k9/k10,
we found that for values of k9/k10 � 0.04 practically the surface
coverage uHþ has been stabilized in an asymptotic value, which
Fig. 6. All surface coverages, u, as functions of the nondimensional parameter
k9/k10 and YH2S1 ¼ 0:1.
depends on the assumed initial values of the H2S concentration.
In the opposite case of k9/k10� 1, the corresponding surface
coverage practically disappears for values of k9/k10 � 10.
Therefore, the approximate interval 0.04 9 k9/k10 9 10 defines
the major sensitivity of the reaction to this parameter. In Fig. 4,
the production of H0 diminishes rapidly for increasing values of
the parameter k9/k10 and is very sensible to the assumed values of
the initial concentration of H2S. In this case, the critical interval
corresponds to 0.01 9 k9/k10 9 100. In order to complete the
results related with the prediction of surface coverage, in Fig. 5
we also show the surface coverage of the vacancy sites, uv as a
function of the same parameter k9/k10 and different values of the
nondimensional concentration YH2S1 . Here, we obtain qualita-
Fig. 8. Surface coverage of the product H0, uH0 , as a function of the non-
dimensional concentration YH2S1 and different values of the nondimensional
parameter k9/k10.
J.C. Martınez et al. / Applied Surface Science 253 (2006) 2327–23352334
Fig. 9. All surface coverages, u, as functions of the nondimensional concen-
tration YH2S1 and k9/k10 = 0.1.Fig. 11. Nondimensional hydrogen distribution, CH0 , as a function of the
nondimensional coordinate j, YH2S1 ¼ 0:1 and different values of the non-
dimensional parameter k9/k10.
tively the same results that those obtained by the surface coverage
of H+; in addition, the interval is practically the same. Also, in
Fig. 6 we have plotted together (for a representative value of
YH2S1 ¼ 0:1), the different surface coverage as functions of the
nondimensional parameter k9/k10. Complementary, in Figs. 7 and
8 we show only the surface coverage of the products HS� and H0
as functions of the nondimensional concentration YH2S1 . In
Fig. 7, the HS� surface coverage increases for increasing values
of YH2S1 and this increment is very sensible to increasing values
of the parameter k9/k10. Similarly in Fig. 8, the presence of a
major quantity of hydrogen sulfide in the mixture reflects a drop
of the surface coverage of H0, reaching smaller values if the ratio
k9/k10 is increased. This result confirms some experimental
predictions of that those mixtures with high content of hydrogen
sulfide can inhibit the corrosion effect.
Fig. 10. Nondimensional hydrogen distribution, CH0 , as a function of the
nondimensional coordinate j, k9/k10 = 0.1 and different values of the nondi-
mensional parameter YH2S1.
In order to complete the numerical results related with the
diffusive process of hydrogen; in Fig. 10, we show the hydrogen
distribution into the iron metal as a function of the
nondimensional transversal coordinate j, different values of
the concentration YH2S1 and k9/k10 = 0.1. Following this
numerical prediction for the hydrogen profile, we can see that
an increment of the H2S fraction in the mixture yields a minor
fraction of the hydrogen specie at the surface, inhibiting the
diffusive process. Reciprocally, in Fig. 11, we can appreciate
the same hydrogen distribution into the metal as a function of
the nondimensional transversal coordinate j, YH2S1 ¼ 0:1 and
different values of k9/k10. The sensitivity of the reactions, which
is measured through the values of the parameter k9/k10, shows
that the diffusive process of the atomic hydrogen H0 can be
accelerated or inhibited for moderate or high values of this
Fig. 12. Nondimensional hydrogen concentration at the surface (j = 0), CH0 , as
a function of the parameter G and YH2S1 ¼ k9=k10 ¼ 0:1.
J.C. Martınez et al. / Applied Surface Science 253 (2006) 2327–2335 2335
parameter, respectively. Finally, in Fig. 12, we have plotted the
surface concentration of hydrogen as a function of the
parameter G and YH2S1 ¼ k9=k10 ¼ 0:1. Here, the hydrogen
concentration increases very sensibly to increasing values of G.
We anticipate in Section 2.2 to G as an exponential function of
the temperature; then for increasing values of the room
temperature, the hydrogen concentration also increases.
However, for large increments of the temperature we can
active the desorption reactions at the upper surface of the iron
metal. Therefore, the present results must take with care: in
order to analyze the physical influence of temperature effects
with large deviations of the room temperature, it is
indispensable to include the energy equations for the mixture
and for the iron metal. Hence, this last figure shows that for
moderate deviations of the room temperature, we can obtain a
more vigorous hydrogen generation at the metal surface.
5. Conclusions
In the present work, we have developed an analytical model
to understand the mechanism of adsorption and decomposition
of hydrogen sulfide to hydrogen into an iron–metal plate. The
physical model used is very simple: a binary mixture of
methane and hydrogen sulfide, flows perpendicularly to an iron
horizontal plate. At room temperature the metal reacts easily
with this sour mixture, yielding Fe2+, which is recombined with
HS� to conduct the process of generation of atomic hydrogen
H0. The specie HS� comes directly from the dissociative
adsorption of H2S and operates as a control to drive the reaction
Fe2+ + HS� ! FeS + H+. We follow the well-known sticking
surface coverage concept to predict as the available sites of the
surface metal are occupied with the different products, due to
the proposed heterogeneous kinetic mechanism. Since a finite
fraction of the generated hydrogen is conducted to the metal,
we have included a simple process of diffusion of this specie. In
this sense, the mathematical model is based on a conjugate
mass transfer analysis, where the simultaneous interaction
between the stagnation-point flow and the iron metal
determines the heterogeneous surface reactions of the iron.
The numerical results of the present work determine clearly
the surface coverage of the involved products. However, we
have not found directly in the specialized literature, experi-
mental data to support these theoretical predictions. Probably,
the main reason is due to that the sour corrosion in metallic
pieces under laboratory conditions, always is carried out in
short times, by increasing the temperature of the system. On the
other hand, in the Section 1 we cited the references
[3,4,9,11,15,18] where indirectly the theoretical predictions
of the present work are confirmed. For instance, it is well known
and documented in some of these references that a major
content of hydrogen sulfide in the mixture yields a drop of the
surface coverage of H0. This result was showed in Fig. 8, which
predicts theoretically that those mixtures with high content of
hydrogen sulfide can inhibit the corrosion effect.
On the other hand, the numerical predictions show that the
electrochemical reactions (8) and (11) are, in general faster than
other reactions (9) and (10), because the surface coverage of the
transition specie H+ is smaller than the surface coverage of the
other products. This result can be well appreciated in Fig. 6.
Finally, it is important to note that the present model which is
evaluated at room temperature only explains the decomposition
of the specie H2S and the corresponding generation and
molecular diffusion of atomic hydrogen H0 into the metal. The
trapping and cracking mechanisms that spread hydrogen in the
form of protons, H+, through the surrounding lattice of the
metal, accumulating internally H0 molecules in specific voids
or traps to conduct the sour corrosion is outside of the main
objectives of the present work.
Acknowledgements
This work has been supported by a research grant no. 43010-
Y of Consejo Nacional de Ciencia y Tecnologıa at Mexico.
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