# Investigation of Mild Steel Corrosion in the Cement Production Associated with the Usage of Secondary Fuels

Authors: Michael Thieme; Ute Bergmann; Anja Kiesewetter; Tobias Wehry; Kay Potzger; Arkadiusz Zarzycki; Marta Marszalek; Hartmut Worch
Journal: International Journal of Corrosion
 (2020)

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## Abstract

The present work deals with the corrosion of mild steel (1.0037) used as the outer construction material of the preheater of a modern industrial cement production facility. The facility uses secondary fuels, which introduce considerable amounts of corrosive species. The situation at the examination sites in the preheater zone is tracked over a period of two years including operation and shut-down periods. The investigation is focused on (i) the acquisition of the underlying physicochemical conditions, such as moisture, temperature, and contamination data at the examination site of the preheater, (ii) the multianalytical identification of the formed corrosion products using scanning electron microscopy combined with energy-dispersive X-ray analysis, infrared spectrometry, Raman spectrometry, X-ray diffractometry, and Möβbauer spectrometry, and (iii) voltammetric and EIS laboratory investigations using model solutions. It was evidenced that corrosion takes place at a temperature level of about 100°C in the presence of moisture and oxygen as well as chloride ion as a consequence of the usage of secondary fuels. Typical hot-gas corrosion could be excluded under the current conditions. Appearance, structure, and nature of the corrosion products were found to be not mainly dependent on the varied length of exposure, but on the conditions of the hosting preheater intake. In addition to different FeOOH phases and hematite, magnetite was found, dependent on the oxygen concentration in the process gas. The decisive role of oxygen as key factor for the corrosion rate was electrochemically confirmed.


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## Body

## 1. Introduction

The cement production is inevitably connected with two critical phenomena, which shall be addressed at first: energy and fuel consumption and the release of carbon dioxide as one of the green-house gases. As for the latter, the production of one ton of clinker from appropriate amounts of lime, sand, clay, and iron-containing material causes the emission of 0.65-0.90 t of carbon dioxide due to fuel combustion and the primary decomposition of lime CaCO3 into quick lime CaO. Correspondingly, the cement industry accounts for about 7% of the total global CO2 emission [1, 2].In terms of the consumption of energy and fuels, alternative energy sources, the so-called secondary fuels (SFs), have been increasingly deployed worldwide for about three decades in order to save fossil fuels, to diminish the green-house gas emission, and, at the same time, to manage waste problems [3]. A detailed report of the German Umweltbundesamt sums up a substituted energy equivalent of 40 PJ alone for the German cement industry in the year 2004 [4]. This corresponds to a fraction of more than 42% of the total thermal energy consumption in the cement production sector. No doubt, these figures will have considerably increased during the recent years. A Chinese paper stresses that even 91% of coal could be replaced by cofiring oil sludge [5]. Altogether, 16 different types of industrial, agricultural, and urban refuse-derived SFs are discerned by ref. [4], representing different consistency and degree of preprocessing. Old tires, waste plastics, and animal waste products amount to the largest fractions [6].The distinctly deviating chemical composition of the SFs in comparison to traditional fuels introduces a diversity of critical chemical elements, such as alkalis, chlorine, and sulphur, into the cement production facility. These elevated concentration levels may affect the cement product quality, environmental pollution [7], and, last not least, the corrosion behaviour of the incorporated construction materials, i.e., in the interior of the rotary kiln [8]. As for the mechanism, the high-contamination conditions will lead to the formation of volatile alkali compounds, mixed oxides, and metal chlorides, which spread throughout the total system [8–10]. As one of the possible pathways, these salts may undergo desublimation on sufficiently colder (metal) surfaces. Consequently, melts and substances with hygroscopic and deliquescent properties are formed and a high corrosion potential arises. All in all, the situation will be similar as described for other high-contamination, high-temperature facilities, and technologies [11–15].For the production of clinker, it should be taken into account that corrosion of the steel mantle can principally occur under the regular operation conditions, dependent on the actual position in the facility, as well as during the planned shut-down period in wintertime, when dew-point undershooting for water may happen at the cold steel cladding [8].This paper focuses on the aspects of corrosion and, hence, lifetime of unalloyed steel components in the region of the preheater, which is run on a considerably lower temperature level than in the rotary kiln. As for its function, the milled raw materials are stepwise heated up by the process gases in counter current, before they will reach the rotary kiln with its special pyroprocessing. The specific examination sites within the preheater are marked in Figure1. Both preheater branches, the so-called intakes, were considered. The steel is shielded against the hot process atmosphere by a two-layered build-up of refractory consisting of 115 mm thick bricks (fireclay, 30% Al2O3+65% SiO2) on the gas side and, on the metal side, a ceramic thermoinsulation of calcium silicates having a high porosity and a thickness of 115 mm.Figure 1
View of the two units of preheater (two intakes each) and the rotary kiln; location of the examination sites marked.Not only the metallic construction materials are subject to corrosion, but also the ceramic materials which provide both for heat insulation and for mechanical protection are increasingly attacked by the conditions exacerbated by the usage of secondary fuels. The development of materials with a high resistance to alkali-based corrosion was, therefore, in the focus of recent investigations [16].To the best of our knowledge, the specific corrosion processes of mild steel in the preheater region of the cement production facility has not closely investigated hitherto. In this investigation, we aimed in contributing to a detailed characterisation of the occurring physicochemical conditions and the corrosion phenomena at the inner surface of the mild steel preheater cladding. Basically, the decision was supposed to be taken, whether high-temperature corrosion types would be active under operation conditions, similar to the situation in the rotary kiln [8]. Alternatively, the “normal” corrosion type comes into consideration, where (thin) liquid-water films are active associated with an electrochemical mechanism. Further, the role of aggressive chloride contamination was to be cleared up. To achieve this, five experimental approaches were designed:
(i)
Exposure of prepared steel sheet samples at the examination sites of both intakes as a new manner of approach (“in-plant exposure”). These samples previously cut-out from the preheater cladding were given special pretreatments and inserted back into the corresponding cladding openings. The exposure periods amounted up to 24 months. Part of the steel surface kept uncoated, whilst the surface of the remaining area was coated for corrosion protection. These coatings were designed for hot corrosion and for aqueous electrochemical corrosion conditions, respectively. This issue will be treated separately(ii)
Collection of temperature and humidity data at the inner wall of the cladding at the examination sites of both intakes (“in situ logging”). The humidity, i.e., the presence of vaporous water, is the consequence of the combustion in the rotary kiln and, to less than 10%, of the release by the raw products. These measurements aimed at gaining basic information about the conditions prevailing at the inner steel surface in the preheaters(iii)
Visual evaluation of the observed corrosion phenomena on the uncoated steel as well as analysis of the formed solid corrosion products focusing on morphology, composition, and phase identification (“multianalytical investigation”). This approach was followed in order to deduce the effective corrosion mechanism. Different methods were used, such as scanning electron microscopy combined with energy-dispersive X-ray analysis, infrared spectroscopy, Raman spectroscopy, X-ray diffraction, and Möβbauer spectroscopy(iv)
Determination of extractable species (“chemical contamination”). This was done using ion-coupled plasma optical emission spectrometry and ion chromatography(v)
Electrochemical laboratory measurements in selected chloride-containing model electrolyte solutions under varied aeration. This approach was employed by means of linear polarisation and electrochemical impedance spectroscopy in order to elucidate further characteristic features of the steel corrosion.


## 2. Material and Methods

### 2.1. In Situ Data Logging

For in situ data logging at the inner wall of the steel cladding, two sensor types were mounted in set-in nozzles. Hereby, the sensors were positioned in such a manner that the sought parameters could be recorded just at that place where the corrosion proceeds.(i)
Humidity sensor HC2-IE105 (Rotronic, Germany): based on a capacitive principle and additionally contains a temperature sensor (Figure2(a))(ii)
Conductivity sensor: two custom-made types produced by Sensortechnik Meinsberg, Germany, detecting the presence of conductive liquids. The first had two platinum rings mounted on a glass cylinder, whereas the second contained two platinum wires fused in a shallow dimple, which forms a reservoir for condensed liquid (Figure2(b)).Figure 2
(a) Humidity sensor HC2-IE105 with its sensing elements after removal of the outer filter hull. (b) Custom-made conductivity sensor (second type).
(a)(b)In addition to these measurements, cubical test samples of calcium silicate (Calsitherm Silikatbaustoffe GmbH, Paderborn, Germany) were used for weighing experiments under defined temperature and humidity in a climate chamber (SH-242, Espec Europe GmbH, Germany).


### 2.2. Steel Samples, Pretreatment, and Exposure under In-Plant Conditions

The in-plant exposure was done using four mild steel plates of300mm×150mm×6mm in size, which had been previously cut out from the designed places of the preheater cladding using an angle grinder. The inner surfaces of the plates were blasted using chilled iron grit (size 0.6-1.0 mm), which gave a roughness of about Rz=80μm. The areas to be exposed were divided into four stripe-like partial areas of 75 mm width each (Figure 3(a)). Herewith, not only the behaviour of bare mild steel was followed up, but also corrosion protection measures were supposed to be considered.Figure 3
(a) Top view of one of the four steel plates as prepared for in-plant exposure; description of the stripes (top–down): Hempadur epoxy coating; no coating, surface blasted only; Galvosil coating; and Galvosil binder coating without zinc powder, manual painting. (b) Two plates after fixture in the cladding of intake 1 (six months after exposure start).
(a)(b)After being transported in a desiccator, the pretreated plates were mounted two by two into the corresponding cladding openings of both intakes (Figure3(b)). The edges of the inserted samples were sealed against the penetration of rain and dust. The in-plant exposure periods were 6 and 12 months for the two plates exposed in intake 2 (designation M6/2 and M12/2, respectively), 18 and 24 months in intake 1 (M18/1, M24/1, respectively).The secondary-fuel regime with burning tires, fluff, and liquid waste fuels was kept vastly constant within that two-year period.


### 2.3. Multianalytical Post-Exposure Investigations

At first, the dismounted plates were visually inspected and photographically documented. To assess the corrosion rate, the material thinning was determined microscopically. Samples of the size20mm×20mm were carefully cut out from the exposed large-area sheets using a band-saw in such a manner that both the corroded surface and the adjacent epoxy-coated, unattacked part (reference) were accounted for. The embedded cross-section was metallographically polished down to 3 μm diamond and carefully etched (3% ethanolic HNO3). In order to reduce the influence of the indigenous surface roughness, a high number of equidistant measuring lines (every 250 μm) was overlaid to the primary images, which were taken by a VHX-1000 digital Keyence microscope. The physicochemical analysis of solid corrosion products (CP) originated in the kiln was performed on compact steel-based samples and on loose CP powder materials after manually milling using an agate mortar. Loose corrosion product layers could be easily collected, and adhering parts were carefully scratched off from the base metal. Typical areas were selected, where the size was in the magnitude of 1-2 cm2.
(i)
Scanning electron microscopy (SEM): following a thin carbon coating, the images of compact CP were taken on a DSM 982 Gemini (Zeiss, Germany) provided with a field emission cathode, with an acceleration voltage of 2-15 keV. Energy-dispersive X-ray spectroscopy (EDX) for elemental analyses were done using a Voyager 3000 spectrometer (Noran, USA) provided with a Si(Li) detector(ii)
Infrared spectroscopy (IR): the usual transmission technique with KBr pellets was applied, where the fraction of the powdered substance to be analysed was 2-3%. The spectra were recorded down to 370 cm-1 averaging 5 single spectra using a Spectrum 2000 (PerkinElmer, Germany)(iii)
Raman spectroscopy (RS): the analyses were run on a RFS 100/S instrument (Bruker, Germany) combined with a Nd-YAG 1024 nm laser generator (Coherent, USA). The wavelength range was generally 500-3000 cm-1 with the beam energy as low as possible to avoid radiation damage(iv)
Differential scanning calorimetry (DSC): a DSC 404 instrument (Netzsch, Germany) was used for a few powdered FeOOH and CP samples (10 K/min).(v)
X-ray diffraction (XRD): diffractograms of powdered CPs were recorded using an RD7 instrument (Seifert-FPM, Germany) provided with an iron tube (FeKα1 0.1936087 nm, FeKα2 0.1940025 nm; 30 kV, 28 mA). The stepscan covered 0-100° (2θ) with a rate of 0.02°/4 s. These measurements were performed at the University of Applied Sciences Dresden(vi)
Möβbauer spectroscopy (MS): measurements were performed in transmission geometry using powdered samples. In a first approach, a Wissel system at HZDR was used. Further measurements were performed at IFJ PAN using a home-built setup provided with a 57Co source in rhodium matrix. The samples were sandwiched between thin mica slices. All experiments were performed at ambient temperature. The obtained Mößbauer spectra were fitted with a Voigt-based fitting routine [17] that allows to determine the distribution of hyperfine fields under the assumption of linear relationships between the width of magnetic hyperfine field and the width of other hyperfine interaction parameters, such as quadrupole and isomer shifts. Since it does not influence the main information, which is the identification of phases and its concentration, it was decided not to include these data into the paper. All spectra were fitted consecutively, starting with the most relevant components with well-defined parameters. Then, the parameters of other phases were gradually introduced.For the identification of the in-plant formed CP phases, as described above, several commercial substances were utilised:(i)
Goethite,α-FeOOH (Bayferrox 910; Lanxess, Germany)(ii)
Lepidocrocite,γ-FeOOH (Bayferrox 943)(iii)
Magnetite, Fe3O4 (98%+, <50 nm, #637106-25G, Sigma-Aldrich, Germany)(iv)
Hematite,α-Fe2O3 (z.A., Ferak, Germany).In addition to these powder materials, Akaganeit,β-FeOOH, was produced in laboratory following slightly different recipes [18]. The mostly utilised product was generated by dissolution of 27 g FeCl3.6H2O in 1 L deionised water, then warmed up to 40°C and stirred for 48 hours. The precipitated product was filtered off, gently rinsed, and dried at ambient temperature.Besides the CPs, the thin coverings that had been formed on the conductivity sensors were analysed in terms of chemical contaminants usingion-coupled plasma optical emission spectrometry (ICP-OES) (Optima 4300 DV; PerkinElmer, Germany), three single determinations each, and ion chromatography (IC) (ICS 900; DIONEX, Germany). The preceding extraction was accomplished by storing for four weeks in deionised water followed by filling up to 10 mL.


### 2.4. Electrochemical Investigations

Electrochemical laboratory investigations were carried out using a special three-electrode cell in combination with a CompactStat.e 10800 instrument (Ivium, Netherlands). Rolled mild steel sheet (1.0037, thickness 2 mm) was utilised as working electrode with sample sizes of26mm×38mm. The surface was degreased with acetone or, in a few cases, wet-ground (P800). The cell consisted of two polymethylmethacrylate blocks (base area 70mm×70mm), which were screwed together clamping the samples in between. The upper cell part contained a tightening O-ring (inner diam. 5 mm, exposed area 0.2 cm2) and a glued-in plastic tube for the solution (30 mL), whilst the lower part provided for the electric connection. The cell was completed by a platinum sheet counter electrode and a type Ag/AgCl, KCl sat. reference electrode (Sensortechnik Meinsberg, Germany), the potential of which against the standard hydrogen electrode is EH=0.20V, slightly depending on temperature [19]. A Faraday cage served for shielding against disturbing electromagnetic fields.The model electrolytes 1 M KCl, 0.1 M KCl, and 0.1 M K2SO4 were applied. The measurements were performed in (i) unstirred solutions under air access, (ii) under forced aeration, and (iii) under deaeration, which was put into practice by gentle pressurised–air purge and pure-nitrogen gas bubbling, respectively, at ambient temperature. Part of the measurements was done at 40°C.Linear polarisation experiments were performed after giving the system an ample time of 10 min for developing a stable stationary state (open circuit potential ocp). Mainly, the polarisation was run from the cathodic region into the anodic direction using a rate of 1 mV/s, at least in duplicate using fresh specimens. The polarisation resistanceRp was determined according to the Stern-Geary method using the routine implemented in IviumSoft. The respective Tafel slopes bc,a were utilised for calculating the corrosion density jcorr according to the well-known Stern-Geary equation [20].
(1)jcorr=bc·ba2.3·bc+ba·Rp.Impedance spectroscopy (EIS) was performed at ocp in the frequency range of 50 kHz down to 0.5 mHz with 10 frequency points per decade and an amplitude (peak-to-zero) of 20 mV. The reference electrode was provided with a capacitive bridge (1μF) to avoid disturbances in the high-frequency region [21]. Usually, serial scans were recorded at defined time up to five weeks of immersion in order to follow the effect of increasing corrosion. Again, at least two parallel series were measured. The evaluation in this presentation refers to spectra recorded for immersion periods of 3 h. For modelling, the data were exported into the ZView software (Scribner) and analysed based on different equivalent circuits.


## 2.1. In Situ Data Logging

For in situ data logging at the inner wall of the steel cladding, two sensor types were mounted in set-in nozzles. Hereby, the sensors were positioned in such a manner that the sought parameters could be recorded just at that place where the corrosion proceeds.(i)
Humidity sensor HC2-IE105 (Rotronic, Germany): based on a capacitive principle and additionally contains a temperature sensor (Figure2(a))(ii)
Conductivity sensor: two custom-made types produced by Sensortechnik Meinsberg, Germany, detecting the presence of conductive liquids. The first had two platinum rings mounted on a glass cylinder, whereas the second contained two platinum wires fused in a shallow dimple, which forms a reservoir for condensed liquid (Figure2(b)).Figure 2
(a) Humidity sensor HC2-IE105 with its sensing elements after removal of the outer filter hull. (b) Custom-made conductivity sensor (second type).
(a)(b)In addition to these measurements, cubical test samples of calcium silicate (Calsitherm Silikatbaustoffe GmbH, Paderborn, Germany) were used for weighing experiments under defined temperature and humidity in a climate chamber (SH-242, Espec Europe GmbH, Germany).


## 2.2. Steel Samples, Pretreatment, and Exposure under In-Plant Conditions

The in-plant exposure was done using four mild steel plates of300mm×150mm×6mm in size, which had been previously cut out from the designed places of the preheater cladding using an angle grinder. The inner surfaces of the plates were blasted using chilled iron grit (size 0.6-1.0 mm), which gave a roughness of about Rz=80μm. The areas to be exposed were divided into four stripe-like partial areas of 75 mm width each (Figure 3(a)). Herewith, not only the behaviour of bare mild steel was followed up, but also corrosion protection measures were supposed to be considered.Figure 3
(a) Top view of one of the four steel plates as prepared for in-plant exposure; description of the stripes (top–down): Hempadur epoxy coating; no coating, surface blasted only; Galvosil coating; and Galvosil binder coating without zinc powder, manual painting. (b) Two plates after fixture in the cladding of intake 1 (six months after exposure start).
(a)(b)After being transported in a desiccator, the pretreated plates were mounted two by two into the corresponding cladding openings of both intakes (Figure3(b)). The edges of the inserted samples were sealed against the penetration of rain and dust. The in-plant exposure periods were 6 and 12 months for the two plates exposed in intake 2 (designation M6/2 and M12/2, respectively), 18 and 24 months in intake 1 (M18/1, M24/1, respectively).The secondary-fuel regime with burning tires, fluff, and liquid waste fuels was kept vastly constant within that two-year period.


## 2.3. Multianalytical Post-Exposure Investigations

At first, the dismounted plates were visually inspected and photographically documented. To assess the corrosion rate, the material thinning was determined microscopically. Samples of the size20mm×20mm were carefully cut out from the exposed large-area sheets using a band-saw in such a manner that both the corroded surface and the adjacent epoxy-coated, unattacked part (reference) were accounted for. The embedded cross-section was metallographically polished down to 3 μm diamond and carefully etched (3% ethanolic HNO3). In order to reduce the influence of the indigenous surface roughness, a high number of equidistant measuring lines (every 250 μm) was overlaid to the primary images, which were taken by a VHX-1000 digital Keyence microscope. The physicochemical analysis of solid corrosion products (CP) originated in the kiln was performed on compact steel-based samples and on loose CP powder materials after manually milling using an agate mortar. Loose corrosion product layers could be easily collected, and adhering parts were carefully scratched off from the base metal. Typical areas were selected, where the size was in the magnitude of 1-2 cm2.
(i)
Scanning electron microscopy (SEM): following a thin carbon coating, the images of compact CP were taken on a DSM 982 Gemini (Zeiss, Germany) provided with a field emission cathode, with an acceleration voltage of 2-15 keV. Energy-dispersive X-ray spectroscopy (EDX) for elemental analyses were done using a Voyager 3000 spectrometer (Noran, USA) provided with a Si(Li) detector(ii)
Infrared spectroscopy (IR): the usual transmission technique with KBr pellets was applied, where the fraction of the powdered substance to be analysed was 2-3%. The spectra were recorded down to 370 cm-1 averaging 5 single spectra using a Spectrum 2000 (PerkinElmer, Germany)(iii)
Raman spectroscopy (RS): the analyses were run on a RFS 100/S instrument (Bruker, Germany) combined with a Nd-YAG 1024 nm laser generator (Coherent, USA). The wavelength range was generally 500-3000 cm-1 with the beam energy as low as possible to avoid radiation damage(iv)
Differential scanning calorimetry (DSC): a DSC 404 instrument (Netzsch, Germany) was used for a few powdered FeOOH and CP samples (10 K/min).(v)
X-ray diffraction (XRD): diffractograms of powdered CPs were recorded using an RD7 instrument (Seifert-FPM, Germany) provided with an iron tube (FeKα1 0.1936087 nm, FeKα2 0.1940025 nm; 30 kV, 28 mA). The stepscan covered 0-100° (2θ) with a rate of 0.02°/4 s. These measurements were performed at the University of Applied Sciences Dresden(vi)
Möβbauer spectroscopy (MS): measurements were performed in transmission geometry using powdered samples. In a first approach, a Wissel system at HZDR was used. Further measurements were performed at IFJ PAN using a home-built setup provided with a 57Co source in rhodium matrix. The samples were sandwiched between thin mica slices. All experiments were performed at ambient temperature. The obtained Mößbauer spectra were fitted with a Voigt-based fitting routine [17] that allows to determine the distribution of hyperfine fields under the assumption of linear relationships between the width of magnetic hyperfine field and the width of other hyperfine interaction parameters, such as quadrupole and isomer shifts. Since it does not influence the main information, which is the identification of phases and its concentration, it was decided not to include these data into the paper. All spectra were fitted consecutively, starting with the most relevant components with well-defined parameters. Then, the parameters of other phases were gradually introduced.For the identification of the in-plant formed CP phases, as described above, several commercial substances were utilised:(i)
Goethite,α-FeOOH (Bayferrox 910; Lanxess, Germany)(ii)
Lepidocrocite,γ-FeOOH (Bayferrox 943)(iii)
Magnetite, Fe3O4 (98%+, <50 nm, #637106-25G, Sigma-Aldrich, Germany)(iv)
Hematite,α-Fe2O3 (z.A., Ferak, Germany).In addition to these powder materials, Akaganeit,β-FeOOH, was produced in laboratory following slightly different recipes [18]. The mostly utilised product was generated by dissolution of 27 g FeCl3.6H2O in 1 L deionised water, then warmed up to 40°C and stirred for 48 hours. The precipitated product was filtered off, gently rinsed, and dried at ambient temperature.Besides the CPs, the thin coverings that had been formed on the conductivity sensors were analysed in terms of chemical contaminants usingion-coupled plasma optical emission spectrometry (ICP-OES) (Optima 4300 DV; PerkinElmer, Germany), three single determinations each, and ion chromatography (IC) (ICS 900; DIONEX, Germany). The preceding extraction was accomplished by storing for four weeks in deionised water followed by filling up to 10 mL.


## 2.4. Electrochemical Investigations

Electrochemical laboratory investigations were carried out using a special three-electrode cell in combination with a CompactStat.e 10800 instrument (Ivium, Netherlands). Rolled mild steel sheet (1.0037, thickness 2 mm) was utilised as working electrode with sample sizes of26mm×38mm. The surface was degreased with acetone or, in a few cases, wet-ground (P800). The cell consisted of two polymethylmethacrylate blocks (base area 70mm×70mm), which were screwed together clamping the samples in between. The upper cell part contained a tightening O-ring (inner diam. 5 mm, exposed area 0.2 cm2) and a glued-in plastic tube for the solution (30 mL), whilst the lower part provided for the electric connection. The cell was completed by a platinum sheet counter electrode and a type Ag/AgCl, KCl sat. reference electrode (Sensortechnik Meinsberg, Germany), the potential of which against the standard hydrogen electrode is EH=0.20V, slightly depending on temperature [19]. A Faraday cage served for shielding against disturbing electromagnetic fields.The model electrolytes 1 M KCl, 0.1 M KCl, and 0.1 M K2SO4 were applied. The measurements were performed in (i) unstirred solutions under air access, (ii) under forced aeration, and (iii) under deaeration, which was put into practice by gentle pressurised–air purge and pure-nitrogen gas bubbling, respectively, at ambient temperature. Part of the measurements was done at 40°C.Linear polarisation experiments were performed after giving the system an ample time of 10 min for developing a stable stationary state (open circuit potential ocp). Mainly, the polarisation was run from the cathodic region into the anodic direction using a rate of 1 mV/s, at least in duplicate using fresh specimens. The polarisation resistanceRp was determined according to the Stern-Geary method using the routine implemented in IviumSoft. The respective Tafel slopes bc,a were utilised for calculating the corrosion density jcorr according to the well-known Stern-Geary equation [20].
(1)jcorr=bc·ba2.3·bc+ba·Rp.Impedance spectroscopy (EIS) was performed at ocp in the frequency range of 50 kHz down to 0.5 mHz with 10 frequency points per decade and an amplitude (peak-to-zero) of 20 mV. The reference electrode was provided with a capacitive bridge (1μF) to avoid disturbances in the high-frequency region [21]. Usually, serial scans were recorded at defined time up to five weeks of immersion in order to follow the effect of increasing corrosion. Again, at least two parallel series were measured. The evaluation in this presentation refers to spectra recorded for immersion periods of 3 h. For modelling, the data were exported into the ZView software (Scribner) and analysed based on different equivalent circuits.


## 3. Results and Discussion

### 3.1. In Situ Logging of Temperature and Humidity

The temporal course of the temperature and the relative humidity is displayed in Figure4. The diagram makes clear that the regular operation of the facility is accompanied with a temperature level of 100-110°C at the inner surface of the steel mantle, just there, where the corrosion investigations were carried out. This relatively low temperature level presupposes, of course, the presence of the adjacent ceramics, which act as effective thermal insulation against the interior of the preheater with process temperatures of about 800°C. Thus, it can be derived from the temperature findings that typical hot-gas corrosion phenomena are definitely excluded for the examination sites. Rather, the type of corrosion is designated as “aqueous corrosion” with an electrochemical mechanism under elevated temperatures.Figure 4
Courses of temperature (intake 1) and relative humidity (intake 2) in the period Jan–Jun 2016. Both quantities refer to different intakes due to limited on-site wiring. The humidity excursion in the beginning of March 2016 is due to testing the sensor at free atmosphere.Figure4 addresses a second point of interest, namely the relation between temperature and humidity, as determined by the special sensor(s) set in the preheater mantle. On the very left-hand side of the diagram, the high temperature signalises the last phase of the operating state in January 2016 before the onset of shut-down, which is usually planned for wintertime. It may be seen that along with the decrease of temperature also the humidity decreases. Correspondingly, the temperature movements after onset of operation in the beginning of April 2016—three raises and three short-time interruptions—are associated with in-phase movements of the relative humidity, i.e., a maximum of the relative humidity occurred when a temperature maximum was observed and vice versa. After some time, the humidity changes diminish in their amplitudes, although temperature minima keep linked with those of the relative humidity until the end of the records.However, it was expected that shut-down and cooling-down would lead to an increase of the relative humidity with the consequence that the vaporous water condenses on the relatively cooler kiln cladding. To explain the contrary findings, a set of laboratory measurements was designed to follow up the weight changes of a sample of the practically established calcium silicate. Starting from 20°C and 50% relative humidity, the cube specimens were kept for 18 h under the designed conditions and weighted directly afterwards. As seen in Figure5, the ceramic releases humidity for temperatures higher than 40°C. Accordingly, a higher humidity will be present in the gap between ceramics and steel cladding under conditions of temperature increase and vice versa. Obviously, these in-phase changes of relative humidity and temperature occur, although the solubility of the gas for vaporous water enhances with increasing temperature.Figure 5
Water sorption/desorption properties of cubical calcium silicate samples (50×50×50mm3) determined by storage under defined temperature and humidity conditions followed by instantaneous weighing. The mass at 20°C and 50% relative humidity was arbitrarily set as starting point and reference state.The conductivity sensors were to collect aqueous solution as a consequence of potential condensation, which was thought to happen at the kiln mantle as the relative coldest part of the system. However, the recorded conductivity data, covering a period of 20 months, were typically at the lower limit and not quantitatively assessable in the intended manner. Correspondingly, no liquid could be detected, when the sensors were inspected after shut-down. All in all, these findings agree with those of the humidity measurements and the explanation derived.


### 3.2. Appearance of the Steel Plates following the In-Plant Exposure in the Preheater Zone

After in-plant exposure of 6 to 24 months, the uncoated steel areas were covered with thick rust layers. The images of Figure6 give an idea of their appearance. Comparing their structure and compactness, differences can be seen at a glance. The plates M6/2 and M12/2 show CP layers that consist two portions, an upper fraction with more or less spalling character and a lower fraction that is well adherent to the metallic substrate. This feature is clearly seen in Figure 6(b) for the state M12/2. Contrarily, the plates M18/1 and M24/1 embody a less degradation, where spalling phenomena of the CP are much less present. That means that the general degradation has proceeded in a different manner, which does not mainly correspond to the varied length of exposure, as was initially assumed. Instead, there is, obviously, a greater influence of the special location of the exposure of the plates. This statement will be discussed later on.Figure 6
Macroimages of the uncoated areas after exposure. Small light regions on most of the plates (white arrows) are spalled particles from other regions of the plates or ceramic material of the thermal insulation due to direct contact.
(a)(b)(c)(d)


### 3.3. Corrosion Rate

The amount of the wall thickness reduction per specimen during exposure was estimated metallographically (Figure7) as described in the Materials and Methods. The respective mean values of at least 50 material thickness data xi were subtracted from each other and compiled in Table 1 together with their standard errors SE according to equation (2) [22]: s: standard deviation, n: sample size.
(2)SE=sn=∑i=1nxi−x¯2nn−1.Figure 7
Cross-section of a sample from exposed plate M12/2 provided with an overlaid metallographic measurement grid. Two selected lines demonstrate the principle of determining the corrosion attack.Table 1
Amount of corrosion attack according to metallographic measurements on one cross-section of each plate. Differences of the respective thickness mean values provided with their standard errors (cf. Figure7, equation (2)).
SampleThickness loss (μm)M6/2(158±9)M12/2(113±8)M18/1(46±7)M24/1(36±7)The data of Table1 make clear that, in accordance with the heterogeneous images of the corroded surfaces (Figure 6), a relative high degree of scattering has to be supposed for the local corrosion rates. Obviously, the four prepared samples reveal an incorrect relation for increasing exposure time by chance, because the overall thickness loss will undoubtedly grow with increasing time under the respective surrounding conditions. Nevertheless, it must be stated that the intake proves again to be an initially not expected dominant influence factor on the corrosion rate: The absolute corrosion attack in case of the plates exposed in intake 2 is clearly higher, although the exposure time was lower compared to intake 1. Therefore, the corrosion rates in both intakes differ very much.


### 3.4. Multianalytical Investigations of the Corrosion Products

These investigations aim at gaining information about the micromorphological features of the different CPs as well as about their element status and phase composition.


#### 3.4.1. Scanning Electron Microscopy and Local Element Analysis

Generally, the outer surfaces of the four samples are characterised by a markedly heterogeneous appearance in SEM, similarly as stated in [23]. Highly crystalline areas alternate with compact gel-like areas. The crystals encountered show quite different forms, such as platelets, leaf-like crystals, columnar and needle-like structures, and cubes. It could be often observed that zooming-in gives evidence of finer substructures.The first group of results as displayed in Figure8 relates to the sample M6/2, which had undergone a six-month operation regime without wintertime interruption. Figure 8(a) depicts an area on the outer surface of the loose CP layer with differently compact/crystalline regions. The corresponding elemental analyses revealed pronounced peaks of iron, oxygen, and chlorine, with the Cl concentrations ranking EDX2 > EDX1 > EDX3 (Figures 8(a)–8(c)). As for the lower, adherent layer (Figure 8(d)), both investigated sites were found to have relatively high Cl contents in spite of their different morphological shapes (Figures 8(e) and 8(f)). All in all, both parts of the CP layers stemming from intake 2 showed a variety of crystalline shapes, ranging from flimsy platelets over rods to feather-like forms, mostly grown together.Figure 8
SEM images and corresponding EDX spectra; (a–c) referring to the outer surface of the upper, loose CP layer of sample M6/2 (spectrum of EDX1 not shown), (d–f) referring to the lower, adherent CP layer of sample M6/2, and (g–h) referring to the integral layer of M18/1. Spectra regions beyond 10 keV (right edge of the diagram) were free of any signals and, hence, cut off.
(a)(b)(c)(d)(e)(f)(g)(h)Samples M18/1 and M24/1 from intake 1 were characterised by a higher noncrystalline fraction on the outer surface associated with minute Cl contents smaller than that for samples from intake 2 (Figures8(g) and 8(h)). This agrees with the contamination results shown in Figure 9.Figure 9
Concentrations (logarithmic plot) for selected chemical species determined in aqueous extraction solutions from the conductivity sensors; metal ion species according to ICP-OES, and anion concentrations according to IC.


#### 3.4.2. Infrared and Raman Spectroscopy

The IR spectroscopic results obtained for the five utilised reference materials in transmission geometry show a generally very good agreement of the band positions with literature data, based both on synthesised compounds [18, 24–26] and on CPs and others [27, 28]. As Table 2 indicates, the bands of the FeOOH modifications differ from each other in a sufficient manner, whereas the spectra of Fe3O4 and α-Fe2O3 are somewhat similar in the region of 500–600 cm-1. Interestingly, the magnetite spectrum is partly missing in compilations [18]. It appears to be somewhat critical in its IR signature. As for β-FeOOH, the comparison with the full spectrum displayed in ref. [18] evidences the presence of the rod-like crystallised form.Table 2
Transmission minima of the IR bands determined for reference compounds.
PhaseBand position (cm-1)α-FeOOH798, 899β-FeOOH660-670, 846γ-FeOOH748, 1024Fe3O4558, 620 (shoulder)α-Fe2O3459, 535, 600 (shoulder)The results for the CPs are shown in Figure10. For the CPs of samples M6/2 and M12/2, considerable amounts of hematite (α-Fe2O3) are found. Hematite is present in both fractions of the CPs (upper/loose and lower/adherent fractions). On sample M6/2, both fractions contain additionally akaganeite (β-FeOOH). Contrarily, the upper, loose CP fraction of M12/2 reveals no sure indication of any FeOOH, whereas the adherent fraction appears to contain α- and γ-FeOOH. Certain differences in the phase state may be present between M6/2 and M12/2, because the former had undergone an exposure under sole operation conditions in contrast to the latter that was subjected also to a two-month shut-down period.Figure 10
IR spectra (cut-out) for powdered CPs. –upp: upper CP fraction; -low: lower CP fraction; -int: integral fraction. Experimental band positions for the reference materials are marked by dashed lines (cf. Table2).On the contrary, the CPs of the samples M18/1 and M24/1 have a quite deviating composition in that hematite appears to be vastly or completely substituted by magnetite, as it is attested by the missing band at 460 cm-1 and, macroscopically, by magnetic properties of the powdered CP. This fact is not explainable by the higher exposure times. Instead, it points to differing operating conditions in the plant. This detail will be discussed later. Moreover, goethite (α-FeOOH) and lepidocrocite (γ-FeOOH) are present.Raman spectroscopic data are shown in Figure11, again focused on the most relevant wavenumber region. As for the positions of the reference compounds, the major peaks agree with literature data [18, 26, 29–31]. Interestingly, magnetite (Fe3O4) was characterised as a weak Raman scatterer [26]. Moreover, it is easily subject to laser-based in situ oxidation. The spectra recorded confirm the presence of α-Fe2O3 in the cases of M6/2 and M12/2 very clearly. Astonishingly, the indication of FeOOH phases as minor components in the CPs by this technique proves to be difficult. The measurements of the pure reference materials suggest that the sensitivity for hematite is perceptibly higher than in the case of the FeOOH compounds. It appears that the acquisition time would have to be considerably higher.Figure 11
Raman spectrometric results for powdered CPs and reference substances; designations like for Figure10. Experimental peak positions for reference materials are marked by dashed lines; for Fe3O4 at ca. 660 cm-1 taken from reference [26, 27].The CP composition of M18/1 was quite different from those with M6/2 and M12/2. Hematite is missing, whereas magnetite is indicated. This confirms the finding obtained with the infrared measurements.


#### 3.4.3. X-Ray Diffraction

Diffraction recordings were taken from CPs of M6/2-upp, M12/2-upp, M18/1-int, M24/1-upp, and M24/1-low.Whilst a mixture of a ferric oxide hydroxide (to be specified asβ-FeOOH referring to the original literature [32, 33]) and hematite (α-Fe2O3) was found for the CP samples from intake 2 (Figure 12(a)), the diffraction pattern of the samples from intake 1 proved to be substantially different. Here, a mix of FeOOH phases and magnetite (Fe3O4) was present (Figure 12(b)).Figure 12
X-ray diffractograms of powdered CPs of M12/2, upper fraction (a), and M18/1, integral fraction (b); reference lines augmented for the sake of perceptibility.
(a)(b)


#### 3.4.4. Mößbauer Spectroscopy

The results shown here were obtained at IFJ PAN as described in the Multianalytical Investigations. Fit-relevant data were additionally taken from references [34–37]. The discussion focuses on one sample of each intake. Figures 13(a) and 13(b) display results for the different CP fractions of M12/2.Figure 13
Mößbauer spectra for powdered CPs of M12/2, upper (a) and lower (b) fractions, and M18/1, integral fraction (c), along with the fitting results.
(a)(b)(c)The spectrum for the upper, loose CP fraction is dominated by the sextet of hematite (α-Fe2O3), which exhibits hyperfine parameter values close to those observed in reference [37]. The quantification gives 95% of the iron compounds (Table 3), i.e., the overwhelming portion. A residue of about 5% is ascribed to akaganeite (β-FeOOH) or lepidocrocite (γ-FeOOH). Due to the peak broadening, the two phases cannot be distinguished, since they have very close hyperfine parameters at room temperature. This uncertainty holds also for more or less large portions of the other selected CP samples.Table 3
Compiled results for Möβbauer-derived phase compositions of the samples M12/2, upper and lower fractions, and M18/1, integral fraction, along with the fit-based quantification. δ: isomer shift; ΔEQ: electric quadrupole split; Bhf: magnetic hyperfine field.
SampleComponentδ (mm/s)ΔEQ (mm/s)Bhf (T)PhaseFraction (%)M12/2 upper CP fractionDoublet I0.390.69β- or γ-FeOOH5Doublet II1.102.98Mica2Sextet I0.37-0.1151α-Fe2O393M12/2 lower CP fractionDoublet I0.390.69β- or γ-FeOOH23Doublet II1.102.98Mica2.5Sextet I0.39-0.1151Fe2O320Sextet II0.2649Fe3O418.5Sextet III0.6645.5Sextet IV0.38-0.1338α-FeOOH36M18/1 integrated fractionDoublet I0.390.59β- or γ-FeOOH10Doublet II1.102.98Mica3Sextet I0.2649.5Fe3O447Sextet II0.6746.0Sextet III0.38-0.1338α-FeOOH40.5The lower, adherent part of M12/2 shows a markedly deviating spectrum (Figure13(b), Table 3). In particular, magnetite (Fe3O4) was identified in addition to hematite. The spectrum of magnetite is characterised by two sextets based on the simultaneous presence of ferrous and ferric ions in the inverse spinel lattice. From the thermodynamical point of view, the presence of magnetite in the neighbourhood of the metal substrate is a necessary issue; this will be discussed in the next section. In addition to the mentioned phases, the lower CP fraction of M12/2 contains a rest that was fitted assuming the presence of goethite (α-FeOOH) (Table 3). However, the fitting process suggested a modification of the original sextet. Literature indicates that dispersion of particle sizes, imperfect crystallinity, and/or deviations from stoichiometry may lead to distorted sextets and hyperfine field distribution, especially at room temperature [28, 38, 39]. Further, the clusters of goethite can be influenced from surrounding clusters of material with different symmetry and magnetic properties (i.e., different phases present in the sample) affecting the hyperfine parameters and widening the distribution of the magnetic hyperfine field. In order to take these factors into account, the fitting of the presumably existing goethite component was performed here in a manner described in the Materials and Methods with the assumption of a Gaussian distribution of hyperfine fields Bhf being not larger than 15 T. As Figure 13(b) makes clear, this resulted in markedly broadened linewidths, whereby the external lines of the sextet merge with the middle ones.For the integral CP of M18/1, as displayed in Figure13(c) and Table 3, a high portion of magnetite was found. Thus, this result addresses the aspect of an intake influence again. Further, a ferromagnetic fraction likely originates from goethite with a broad linewidth, as it was discussed above.


#### 3.4.5. Summarising Considerations of Phase Analyses

The analytical findings for the CPs studied are compiled in Table4. Summarising, there is a good agreement of the four analytical techniques applied. Incomplete agreements, e.g., in view of the presence of the single oxide hydroxides, may be tolerable because of the probable lateral heterogeneity in context with punctual sampling. After all, Fe(III) oxide hydroxide phases appear to play an important role in the composition of the formed CPs. Thermodynamically, it can be easily shown that the formation of α-FeOOH from metallic iron and water is possible under aerobic conditions. From the tabulated data [40], a Gibbs free energy of reaction ΔrGo of -357 kJ/mol is calculated for 373 K, the measured temperature level for the investigation sites in the preheater. The formation of β- and γ-FeOOH needs the presence of chloride as a necessary or favourable prerequisite [18], which is fulfilled under the current conditions. In view of the thermal stability of goethite and the other FeOOH modifications, another thermodynamic calculation shows that the decomposition to the water-free oxide α-Fe2O3 under release of water proves to be principally possible (ΔrGo=−3.5kJ/mol for 373 K). In reality, the FeOOH compounds are, however, sufficiently stable on the temperature level of about 100°C.Table 4
Compiled analytical results for the CPs (goe.: goethiteα-FeOOH; aka.: akaganeite β-FeOOH; lep.; lepidocrocite γ-FeOOH; mag.: magnetite Fe3O4; hem.: hematite α-Fe2O3).
SampleIR spectroscopyRaman spectroscopyXRDMößbauer spectroscopyM6/2-uppM6/2-lowhem. + aka.hem. + aka.hem. + lep.hem. + lep.hem. + aka.--hem. + aka./lep.hem. + mag. + aka./lep.M12/2-uppM12/2-lowhem.hem. + goe. + lep.hem.(hem.)hem. + aka.--hem. + aka./lep.hem. + mag. + goe. + aka./lep.M18/1-intmag. + goe. + lep.mag.mag. + goe. + lep. + aka.mag. + goe. + aka./lep.M24/1-uppM24/1-lowmag. + goe. + lep.mag. + goe. + lep.mag. + goe. + lep.mag. + goe. + lep. + aka.This matter of fact could be unequivocally stated by DSC experiments with goethite and lepidocrocite, where the decomposition occurred indeed well beyond 250°C (Figure14 for goethite). This observation is in agreement with literature data of Weckler and Lutz [24]. They stated a much faster decomposition rate of akaganeite than those of the other polymorphs, obviously due to the Cl− ion impurities present in this compound.Figure 14
DSC tracks for goethite with decomposition to hematite, which was confirmed by the Raman spectroscopy. In case of lepidocrocite as starting product, maghemite (γ-Fe2O3) was primarily formed.Thus, it can be emphasised for a relatively wide temperature range that the FeOOH species are metastable compounds whose decomposition is, obviously, kinetically hampered. This in turn can be considered a verification of our experimental findings that the FeOOH species represent significant components of the corrosion products formed under the relevant preheater conditions.Further, it should be noted that thermodynamics claim for the presence of metallic iron as substrate that magnetite Fe3O4 containing Fe(II) aside from Fe(III) must be present in the contact zone to the metal, because α-Fe2O3 will be reduced to Fe3O4 (ΔrGo=−25.3kJ/mol Fe3O4, 373 K). Indeed, this phase was preferentially found for the low-oxygen conditions of intake 1 according to the infrared and Raman spectroscopy, XRD, and MS (Figures 10, 11, 12(b), and 13(c), Tables 2 and 3). Moreover, the evidence of magnetite was suggested by Möβbauer spectroscopy also for the lower, adherent fraction of CP layers formed under the conditions of intake 2 (Figure 13(b), Tables 2 and 3).


### 3.5. Chemical Contamination

Information on the occurrence of chemical species, which will influence the corrosion phenomena at the examination site, was gained from the water-based extraction of the coverings on the glassy conductivity sensors after an exposure period of 11 months.Figure9 shows analytical data for selected metal ion and anionic species determined for the inner surfaces of the both intakes. It is seen at a glance that there is a marked difference between the concentrations of corrosion relevant anionic species for both intakes. This means in view of the halogenides that especially intake 2 is characterised not only by a higher degree of “contamination,” but also by more serious corrosive conditions. The findings may be interpreted by an unequal distribution of the chemical freights, which are transported in the mass streams from the rotary kiln into the both intakes including the chemically multifaceted input from the secondary fuel (Figure 15). Intake 2 is located on that side of the rotary kiln, where the upward motion takes places, so that a greater part of dusty particles are forwarded into this branch. Contrarily, intake 1 is fed with the greater portion of combustion gases, among those also carbon monoxide CO. Gas analyses carried out separately make clear that intake 2 has a higher oxygen concentration than intake 1 with a typical oxygen difference of 2-3%. These facts are responsible that also the corrosion phenomena, as discussed above, are substantially different, with the mild steel exposed in intake 2 undergoing a markedly higher corrosion rate and a more distinct CP formation.Figure 15
Different mass transport in both intakes of the preheater.


### 3.6. Electrochemical Lab Investigations

The following electrochemical investigations were done to clear up the importance of oxygen and chloride content in the exhaust air of the two intakes. Therefore, the parameters for the model electrolyte solutions were varied correspondingly. Open circuit potentials (Table5) are given for different aeration and temperature conditions based on measurements in 1 M KCl solution. Parallel measurements showed ocp differences of a few mV only; also, the temporal movements over 10 min were small. The ocp for enhanced temperature under aerated, but unstirred conditions, occupies the most negative position. The considerable positive ocp shift under forced aeration through pressurised air is in accordance with the mixed potential theory. Similar findings in view of aeration/deaeration were gained, e.g., for carbon steel in a near-neutral mixed carbonate-chloride-sulphate salt medium under consecutively varied gas purging regimes [41, 42].Table 5
Open circuit potentials (mean values at 200 s after immersion start of three measurements each) for 1 M KCl electrolyte solution.
Conditionocp (mV)Ambient temp., aerated, unstirred-61040 °C, aerated, unstirred-637Ambient temp., pressurised-air purge-530Ambient temp., N2 purge-599Figure16 depicts the influence of different aeration on the course of voltammetric measurements and the Stern-Geary corrosion data as well. Under pressurised-air purging, the ocp is shifted in the positive direction, and the cathodic currents are favoured in accordance with the mixed potential theory. The control of the corrosion rate at ocp is more on the side of the cathodic partial reaction, because the oxygen reduction takes place under a high degree of transport control, where the diffusion layer thickness is substantially decreased for the vigorously moved electrolyte solution. It is easily conceivable that the corresponding curves are subject of higher scattering due to the less controlled air purging. The outlined situation is reflected also by the mean values of the polarisation resistance Rp and the corrosion current density jcorr, which surpass for pressurised-air conditions those for the unstirred state by a factor of about 40 (Figure 16, inserts).Figure 16
Single polarisation measurements under varied aeration conditions at ambient temperature recorded after 0.5-1 h of immersion in 0.1 M KCl electrolyte solution from cathodic (ocp−0.3V) to anodic with 1 mV/s; inserts: corresponding Stern-Geary corrosion data (mean values).After all, the major role of oxygen/cathodic partial reaction for the corrosion process is emphasised, thus confirming the derived statements for the real corrosion phenomena encountered at the examination site of the preheater.A recalculation of the corrosion current densityjcorr into a corrosion rate based on the thickness loss of steel kd gives, according to Equation (3), a corrosion rate of kd=58μm/a (jcorr=5μA/cm2). This roughly conforms to the order of magnitude of the values of Table 1, which was measured for the preheater-exposed steel plates. MFe: atomic mass of Fe (55.85 g/mol); z: charge-transfer number for the dissolution reaction (2); F: Faraday’s number (9.65×104 As/mol); ρFe: density (7.85 g/cm3).
(3)kd=jcorr·MFez·F·ρFe.In addition to the dc measurements, ac perturbation was applied to gain a deeper insight into mechanistic issues. The Bode diagram of Figure17 illustrates the impedance behaviour in 1 M KCl solutions in terms of the influence of aeration, deaeration through simultaneous N2 purging, and temperature enhancement to 40°C. The depicted curves, chosen from a series of consecutive EIS measurements over 5 d each, refer to a resting time of 3 h in order to provide for approximate stationarity during the longer-lasting EIS measurement. On the other hand, significant covering by corrosion products, i.e., the development of an inhomogeneous surface, which had been previously taken into account by different authors [43, 44], should be avoided. Here, the thickness of the formed CP layer could be estimated to 5×10−8m for unstirred conditions, based on the corrosion current density of 5μA/cm2 (cf. Figure 16).Figure 17
EIS measurements (Bode plot) under varied aeration/deaeration and temperature conditions recorded after 3 h of immersion in 1 M KCl electrolyte solution at ocp.Irrespective of quantitative differences between the three curve pairs for aerated, aerated/40°C, and deaerated conditions, they show a nonidentical shape. The curves are characterised by a number of features: (i) the asymmetric shape of the phase angle bumps at medium frequencies, (ii) the flattening slope oflog∣Z∣ in the direction of decreasing frequency, and (iii) the low-frequency (LF) plateau of about 2 kΩ cm2. It is somewhat surprising that the LF log∣Z∣ values for these condition sets differ only negligibly. As for the enhanced temperature, it may be argued that the expected reactivity increase will be counteracted by the decreased oxygen solubility. The curves for simultaneous air purging show, notwithstanding the scatter, a more symmetric shape of the phase angle course associated with a considerably decreased LF log∣Z∣ plateau of about 0.15kΩcm2. This is a further evidence for the decisive role of oxygen for the corrosion. Finally, the LF plateau levels confirm the behaviour at dc (Figure 16) very well.The high-frequency (HF) plateau oflog∣Z∣ at the right-hand side of the spectra allows reading the electrolyte resistance Re, which is, of course, dependent both on the electrolyte concentration and on the temperature. Indeed, three of the condition sets show completely coinciding electrolyte resistances of about 4 Ω cm2, whilst Re (40°C) is somewhat lower in accordance with theory.Modelling of the measured curves was best performed using a modified Randles equivalent circuit (Figure18(a)). It contains two features: (i) a constant phase element (CPE) with the parameters TCPE and PCPE instead of the pure double layer capacity and (ii) an element Ws designed for a finite diffusion length d, which is characterised by a finite limiting value of its real part for f=0, instead of the original Warburg diffusion impedance [45]. The corresponding impedance equation for Ws is inserted in Figure 18(b). It can be shown that the ZView-based parameter RWs is equal to the limiting value mentioned above. Parameter TWs stands for d2/D, where D is the diffusion coefficient for dissolved oxygen (2.1×10−5cm2/s at 298 K) and d is the diffusion length. Finally, parameter PWs is nearby 0.5.Figure 18
(a) Randles-based equivalent circuit.Re: electrolytic resistance; Rct: charge-transfer resistance; CPE: constant phase element; Ws: modified Warburg impedance with finite diffusion length. (b) Impedance equation for Ws provided with the parameters RWs, TWs, and PWs acc. to ZView; i: imaginary unit; ω: angular frequency. (c) Measured and fitted curves for 1 M KCl, ambient temperature, aerated, and unstirred conditions. The lowest frequency points were omitted due to scattering. (d) Corresponding fitted parameters.
(a)(b)(c)(d)The selected measurement for aerated, unstirred conditions documents the high goodness of fitting (Figure18(c)). As the figures of the table in Figure 18(d) point out, the diffusion-related resistance RWs is determined to be more than one order larger than the interface-related resistance Rct. That means diffusion plays a significant role within the total process and forms the rate-determining step. Thus, diffusion control is active both for the cathodic reduction (as was evidenced by dc measurements, cf. Figure 16) and for normal corrosion at ocp.Turning to air purging, the parameterRWs is dramatically reduced down to 0.15-0.2 kΩ cm2 in agreement with the decreased level of the measured LF log∣Z∣ plateau in Figure 17. It appears now that the inverse relation RWs<Rct holds, which conforms to the improved diffusion under convective conditions.A second impedance diagram (Figure19) addresses different solution compositions. These curves provide evidence that a concentration modification from 1 to 0.1 mol/L KCl does not give significant change in the LF log∣Z∣ plateau. A similar result, within the normal scatter, is gained, when the chloride is completely removed using the sulphate salt of the same molar concentration. This means that the overall corrosion rate will not be essentially influenced by the actual concentration or even by the absence of chloride anions. The negligible chloride influence may be regarded as unexpected, because it is well known that the chloride ion is involved in the anodic dissolution mechanism [46]. However, earlier experiments using AISI 4340 low-alloyed steel in neutral sulphate and chloride solutions [47] gave similar results. Further, a relatively low concentration dependence of corrosion current densities was observed in polarisation measurements on SAE 1010 carbon steel in aerated 0.02-1 M NaCl solutions [44, 48]. This was explained by the fact that both partial reactions—the cathodic partial reaction with mixed control of charge-transfer and mass transport and the anodic subprocess with pure charge-transfer control—undergo a concentration influence.Figure 19
EIS measurements (Bode plot) recorded after 3 h of immersion in different electrolyte solutions at ocp under ambient temperature and aeration without stirring; comparative application of wet-ground surface.As for the electrolyte resistance, the ratios of theRe values for Re0.1MKCl/Re1MKCl=8.3 and for Re0.1MKCl/Re0.1MK2SO4=1.58 reflect the specific effects of the involved ions quite regularly. Theory states that the electrolytic conductivity and, hence, the reciprocal of the electrolyte resistance are determined by the product of ionic charge, ionic concentration, and ionic mobility [49].Finally, a few EIS measurements referred to the influence of the surface pretreatment. As the forth curve pair in Figure19 evidences, wet-grinding, i.e., removing the rolling skin, led practically to no differing results.


## 3.1. In Situ Logging of Temperature and Humidity

The temporal course of the temperature and the relative humidity is displayed in Figure4. The diagram makes clear that the regular operation of the facility is accompanied with a temperature level of 100-110°C at the inner surface of the steel mantle, just there, where the corrosion investigations were carried out. This relatively low temperature level presupposes, of course, the presence of the adjacent ceramics, which act as effective thermal insulation against the interior of the preheater with process temperatures of about 800°C. Thus, it can be derived from the temperature findings that typical hot-gas corrosion phenomena are definitely excluded for the examination sites. Rather, the type of corrosion is designated as “aqueous corrosion” with an electrochemical mechanism under elevated temperatures.Figure 4
Courses of temperature (intake 1) and relative humidity (intake 2) in the period Jan–Jun 2016. Both quantities refer to different intakes due to limited on-site wiring. The humidity excursion in the beginning of March 2016 is due to testing the sensor at free atmosphere.Figure4 addresses a second point of interest, namely the relation between temperature and humidity, as determined by the special sensor(s) set in the preheater mantle. On the very left-hand side of the diagram, the high temperature signalises the last phase of the operating state in January 2016 before the onset of shut-down, which is usually planned for wintertime. It may be seen that along with the decrease of temperature also the humidity decreases. Correspondingly, the temperature movements after onset of operation in the beginning of April 2016—three raises and three short-time interruptions—are associated with in-phase movements of the relative humidity, i.e., a maximum of the relative humidity occurred when a temperature maximum was observed and vice versa. After some time, the humidity changes diminish in their amplitudes, although temperature minima keep linked with those of the relative humidity until the end of the records.However, it was expected that shut-down and cooling-down would lead to an increase of the relative humidity with the consequence that the vaporous water condenses on the relatively cooler kiln cladding. To explain the contrary findings, a set of laboratory measurements was designed to follow up the weight changes of a sample of the practically established calcium silicate. Starting from 20°C and 50% relative humidity, the cube specimens were kept for 18 h under the designed conditions and weighted directly afterwards. As seen in Figure5, the ceramic releases humidity for temperatures higher than 40°C. Accordingly, a higher humidity will be present in the gap between ceramics and steel cladding under conditions of temperature increase and vice versa. Obviously, these in-phase changes of relative humidity and temperature occur, although the solubility of the gas for vaporous water enhances with increasing temperature.Figure 5
Water sorption/desorption properties of cubical calcium silicate samples (50×50×50mm3) determined by storage under defined temperature and humidity conditions followed by instantaneous weighing. The mass at 20°C and 50% relative humidity was arbitrarily set as starting point and reference state.The conductivity sensors were to collect aqueous solution as a consequence of potential condensation, which was thought to happen at the kiln mantle as the relative coldest part of the system. However, the recorded conductivity data, covering a period of 20 months, were typically at the lower limit and not quantitatively assessable in the intended manner. Correspondingly, no liquid could be detected, when the sensors were inspected after shut-down. All in all, these findings agree with those of the humidity measurements and the explanation derived.


## 3.2. Appearance of the Steel Plates following the In-Plant Exposure in the Preheater Zone

After in-plant exposure of 6 to 24 months, the uncoated steel areas were covered with thick rust layers. The images of Figure6 give an idea of their appearance. Comparing their structure and compactness, differences can be seen at a glance. The plates M6/2 and M12/2 show CP layers that consist two portions, an upper fraction with more or less spalling character and a lower fraction that is well adherent to the metallic substrate. This feature is clearly seen in Figure 6(b) for the state M12/2. Contrarily, the plates M18/1 and M24/1 embody a less degradation, where spalling phenomena of the CP are much less present. That means that the general degradation has proceeded in a different manner, which does not mainly correspond to the varied length of exposure, as was initially assumed. Instead, there is, obviously, a greater influence of the special location of the exposure of the plates. This statement will be discussed later on.Figure 6
Macroimages of the uncoated areas after exposure. Small light regions on most of the plates (white arrows) are spalled particles from other regions of the plates or ceramic material of the thermal insulation due to direct contact.
(a)(b)(c)(d)


## 3.3. Corrosion Rate

The amount of the wall thickness reduction per specimen during exposure was estimated metallographically (Figure7) as described in the Materials and Methods. The respective mean values of at least 50 material thickness data xi were subtracted from each other and compiled in Table 1 together with their standard errors SE according to equation (2) [22]: s: standard deviation, n: sample size.
(2)SE=sn=∑i=1nxi−x¯2nn−1.Figure 7
Cross-section of a sample from exposed plate M12/2 provided with an overlaid metallographic measurement grid. Two selected lines demonstrate the principle of determining the corrosion attack.Table 1
Amount of corrosion attack according to metallographic measurements on one cross-section of each plate. Differences of the respective thickness mean values provided with their standard errors (cf. Figure7, equation (2)).
SampleThickness loss (μm)M6/2(158±9)M12/2(113±8)M18/1(46±7)M24/1(36±7)The data of Table1 make clear that, in accordance with the heterogeneous images of the corroded surfaces (Figure 6), a relative high degree of scattering has to be supposed for the local corrosion rates. Obviously, the four prepared samples reveal an incorrect relation for increasing exposure time by chance, because the overall thickness loss will undoubtedly grow with increasing time under the respective surrounding conditions. Nevertheless, it must be stated that the intake proves again to be an initially not expected dominant influence factor on the corrosion rate: The absolute corrosion attack in case of the plates exposed in intake 2 is clearly higher, although the exposure time was lower compared to intake 1. Therefore, the corrosion rates in both intakes differ very much.


## 3.4. Multianalytical Investigations of the Corrosion Products

These investigations aim at gaining information about the micromorphological features of the different CPs as well as about their element status and phase composition.


### 3.4.1. Scanning Electron Microscopy and Local Element Analysis

Generally, the outer surfaces of the four samples are characterised by a markedly heterogeneous appearance in SEM, similarly as stated in [23]. Highly crystalline areas alternate with compact gel-like areas. The crystals encountered show quite different forms, such as platelets, leaf-like crystals, columnar and needle-like structures, and cubes. It could be often observed that zooming-in gives evidence of finer substructures.The first group of results as displayed in Figure8 relates to the sample M6/2, which had undergone a six-month operation regime without wintertime interruption. Figure 8(a) depicts an area on the outer surface of the loose CP layer with differently compact/crystalline regions. The corresponding elemental analyses revealed pronounced peaks of iron, oxygen, and chlorine, with the Cl concentrations ranking EDX2 > EDX1 > EDX3 (Figures 8(a)–8(c)). As for the lower, adherent layer (Figure 8(d)), both investigated sites were found to have relatively high Cl contents in spite of their different morphological shapes (Figures 8(e) and 8(f)). All in all, both parts of the CP layers stemming from intake 2 showed a variety of crystalline shapes, ranging from flimsy platelets over rods to feather-like forms, mostly grown together.Figure 8
SEM images and corresponding EDX spectra; (a–c) referring to the outer surface of the upper, loose CP layer of sample M6/2 (spectrum of EDX1 not shown), (d–f) referring to the lower, adherent CP layer of sample M6/2, and (g–h) referring to the integral layer of M18/1. Spectra regions beyond 10 keV (right edge of the diagram) were free of any signals and, hence, cut off.
(a)(b)(c)(d)(e)(f)(g)(h)Samples M18/1 and M24/1 from intake 1 were characterised by a higher noncrystalline fraction on the outer surface associated with minute Cl contents smaller than that for samples from intake 2 (Figures8(g) and 8(h)). This agrees with the contamination results shown in Figure 9.Figure 9
Concentrations (logarithmic plot) for selected chemical species determined in aqueous extraction solutions from the conductivity sensors; metal ion species according to ICP-OES, and anion concentrations according to IC.


### 3.4.2. Infrared and Raman Spectroscopy

The IR spectroscopic results obtained for the five utilised reference materials in transmission geometry show a generally very good agreement of the band positions with literature data, based both on synthesised compounds [18, 24–26] and on CPs and others [27, 28]. As Table 2 indicates, the bands of the FeOOH modifications differ from each other in a sufficient manner, whereas the spectra of Fe3O4 and α-Fe2O3 are somewhat similar in the region of 500–600 cm-1. Interestingly, the magnetite spectrum is partly missing in compilations [18]. It appears to be somewhat critical in its IR signature. As for β-FeOOH, the comparison with the full spectrum displayed in ref. [18] evidences the presence of the rod-like crystallised form.Table 2
Transmission minima of the IR bands determined for reference compounds.
PhaseBand position (cm-1)α-FeOOH798, 899β-FeOOH660-670, 846γ-FeOOH748, 1024Fe3O4558, 620 (shoulder)α-Fe2O3459, 535, 600 (shoulder)The results for the CPs are shown in Figure10. For the CPs of samples M6/2 and M12/2, considerable amounts of hematite (α-Fe2O3) are found. Hematite is present in both fractions of the CPs (upper/loose and lower/adherent fractions). On sample M6/2, both fractions contain additionally akaganeite (β-FeOOH). Contrarily, the upper, loose CP fraction of M12/2 reveals no sure indication of any FeOOH, whereas the adherent fraction appears to contain α- and γ-FeOOH. Certain differences in the phase state may be present between M6/2 and M12/2, because the former had undergone an exposure under sole operation conditions in contrast to the latter that was subjected also to a two-month shut-down period.Figure 10
IR spectra (cut-out) for powdered CPs. –upp: upper CP fraction; -low: lower CP fraction; -int: integral fraction. Experimental band positions for the reference materials are marked by dashed lines (cf. Table2).On the contrary, the CPs of the samples M18/1 and M24/1 have a quite deviating composition in that hematite appears to be vastly or completely substituted by magnetite, as it is attested by the missing band at 460 cm-1 and, macroscopically, by magnetic properties of the powdered CP. This fact is not explainable by the higher exposure times. Instead, it points to differing operating conditions in the plant. This detail will be discussed later. Moreover, goethite (α-FeOOH) and lepidocrocite (γ-FeOOH) are present.Raman spectroscopic data are shown in Figure11, again focused on the most relevant wavenumber region. As for the positions of the reference compounds, the major peaks agree with literature data [18, 26, 29–31]. Interestingly, magnetite (Fe3O4) was characterised as a weak Raman scatterer [26]. Moreover, it is easily subject to laser-based in situ oxidation. The spectra recorded confirm the presence of α-Fe2O3 in the cases of M6/2 and M12/2 very clearly. Astonishingly, the indication of FeOOH phases as minor components in the CPs by this technique proves to be difficult. The measurements of the pure reference materials suggest that the sensitivity for hematite is perceptibly higher than in the case of the FeOOH compounds. It appears that the acquisition time would have to be considerably higher.Figure 11
Raman spectrometric results for powdered CPs and reference substances; designations like for Figure10. Experimental peak positions for reference materials are marked by dashed lines; for Fe3O4 at ca. 660 cm-1 taken from reference [26, 27].The CP composition of M18/1 was quite different from those with M6/2 and M12/2. Hematite is missing, whereas magnetite is indicated. This confirms the finding obtained with the infrared measurements.


### 3.4.3. X-Ray Diffraction

Diffraction recordings were taken from CPs of M6/2-upp, M12/2-upp, M18/1-int, M24/1-upp, and M24/1-low.Whilst a mixture of a ferric oxide hydroxide (to be specified asβ-FeOOH referring to the original literature [32, 33]) and hematite (α-Fe2O3) was found for the CP samples from intake 2 (Figure 12(a)), the diffraction pattern of the samples from intake 1 proved to be substantially different. Here, a mix of FeOOH phases and magnetite (Fe3O4) was present (Figure 12(b)).Figure 12
X-ray diffractograms of powdered CPs of M12/2, upper fraction (a), and M18/1, integral fraction (b); reference lines augmented for the sake of perceptibility.
(a)(b)


### 3.4.4. Mößbauer Spectroscopy

The results shown here were obtained at IFJ PAN as described in the Multianalytical Investigations. Fit-relevant data were additionally taken from references [34–37]. The discussion focuses on one sample of each intake. Figures 13(a) and 13(b) display results for the different CP fractions of M12/2.Figure 13
Mößbauer spectra for powdered CPs of M12/2, upper (a) and lower (b) fractions, and M18/1, integral fraction (c), along with the fitting results.
(a)(b)(c)The spectrum for the upper, loose CP fraction is dominated by the sextet of hematite (α-Fe2O3), which exhibits hyperfine parameter values close to those observed in reference [37]. The quantification gives 95% of the iron compounds (Table 3), i.e., the overwhelming portion. A residue of about 5% is ascribed to akaganeite (β-FeOOH) or lepidocrocite (γ-FeOOH). Due to the peak broadening, the two phases cannot be distinguished, since they have very close hyperfine parameters at room temperature. This uncertainty holds also for more or less large portions of the other selected CP samples.Table 3
Compiled results for Möβbauer-derived phase compositions of the samples M12/2, upper and lower fractions, and M18/1, integral fraction, along with the fit-based quantification. δ: isomer shift; ΔEQ: electric quadrupole split; Bhf: magnetic hyperfine field.
SampleComponentδ (mm/s)ΔEQ (mm/s)Bhf (T)PhaseFraction (%)M12/2 upper CP fractionDoublet I0.390.69β- or γ-FeOOH5Doublet II1.102.98Mica2Sextet I0.37-0.1151α-Fe2O393M12/2 lower CP fractionDoublet I0.390.69β- or γ-FeOOH23Doublet II1.102.98Mica2.5Sextet I0.39-0.1151Fe2O320Sextet II0.2649Fe3O418.5Sextet III0.6645.5Sextet IV0.38-0.1338α-FeOOH36M18/1 integrated fractionDoublet I0.390.59β- or γ-FeOOH10Doublet II1.102.98Mica3Sextet I0.2649.5Fe3O447Sextet II0.6746.0Sextet III0.38-0.1338α-FeOOH40.5The lower, adherent part of M12/2 shows a markedly deviating spectrum (Figure13(b), Table 3). In particular, magnetite (Fe3O4) was identified in addition to hematite. The spectrum of magnetite is characterised by two sextets based on the simultaneous presence of ferrous and ferric ions in the inverse spinel lattice. From the thermodynamical point of view, the presence of magnetite in the neighbourhood of the metal substrate is a necessary issue; this will be discussed in the next section. In addition to the mentioned phases, the lower CP fraction of M12/2 contains a rest that was fitted assuming the presence of goethite (α-FeOOH) (Table 3). However, the fitting process suggested a modification of the original sextet. Literature indicates that dispersion of particle sizes, imperfect crystallinity, and/or deviations from stoichiometry may lead to distorted sextets and hyperfine field distribution, especially at room temperature [28, 38, 39]. Further, the clusters of goethite can be influenced from surrounding clusters of material with different symmetry and magnetic properties (i.e., different phases present in the sample) affecting the hyperfine parameters and widening the distribution of the magnetic hyperfine field. In order to take these factors into account, the fitting of the presumably existing goethite component was performed here in a manner described in the Materials and Methods with the assumption of a Gaussian distribution of hyperfine fields Bhf being not larger than 15 T. As Figure 13(b) makes clear, this resulted in markedly broadened linewidths, whereby the external lines of the sextet merge with the middle ones.For the integral CP of M18/1, as displayed in Figure13(c) and Table 3, a high portion of magnetite was found. Thus, this result addresses the aspect of an intake influence again. Further, a ferromagnetic fraction likely originates from goethite with a broad linewidth, as it was discussed above.


### 3.4.5. Summarising Considerations of Phase Analyses

The analytical findings for the CPs studied are compiled in Table4. Summarising, there is a good agreement of the four analytical techniques applied. Incomplete agreements, e.g., in view of the presence of the single oxide hydroxides, may be tolerable because of the probable lateral heterogeneity in context with punctual sampling. After all, Fe(III) oxide hydroxide phases appear to play an important role in the composition of the formed CPs. Thermodynamically, it can be easily shown that the formation of α-FeOOH from metallic iron and water is possible under aerobic conditions. From the tabulated data [40], a Gibbs free energy of reaction ΔrGo of -357 kJ/mol is calculated for 373 K, the measured temperature level for the investigation sites in the preheater. The formation of β- and γ-FeOOH needs the presence of chloride as a necessary or favourable prerequisite [18], which is fulfilled under the current conditions. In view of the thermal stability of goethite and the other FeOOH modifications, another thermodynamic calculation shows that the decomposition to the water-free oxide α-Fe2O3 under release of water proves to be principally possible (ΔrGo=−3.5kJ/mol for 373 K). In reality, the FeOOH compounds are, however, sufficiently stable on the temperature level of about 100°C.Table 4
Compiled analytical results for the CPs (goe.: goethiteα-FeOOH; aka.: akaganeite β-FeOOH; lep.; lepidocrocite γ-FeOOH; mag.: magnetite Fe3O4; hem.: hematite α-Fe2O3).
SampleIR spectroscopyRaman spectroscopyXRDMößbauer spectroscopyM6/2-uppM6/2-lowhem. + aka.hem. + aka.hem. + lep.hem. + lep.hem. + aka.--hem. + aka./lep.hem. + mag. + aka./lep.M12/2-uppM12/2-lowhem.hem. + goe. + lep.hem.(hem.)hem. + aka.--hem. + aka./lep.hem. + mag. + goe. + aka./lep.M18/1-intmag. + goe. + lep.mag.mag. + goe. + lep. + aka.mag. + goe. + aka./lep.M24/1-uppM24/1-lowmag. + goe. + lep.mag. + goe. + lep.mag. + goe. + lep.mag. + goe. + lep. + aka.This matter of fact could be unequivocally stated by DSC experiments with goethite and lepidocrocite, where the decomposition occurred indeed well beyond 250°C (Figure14 for goethite). This observation is in agreement with literature data of Weckler and Lutz [24]. They stated a much faster decomposition rate of akaganeite than those of the other polymorphs, obviously due to the Cl− ion impurities present in this compound.Figure 14
DSC tracks for goethite with decomposition to hematite, which was confirmed by the Raman spectroscopy. In case of lepidocrocite as starting product, maghemite (γ-Fe2O3) was primarily formed.Thus, it can be emphasised for a relatively wide temperature range that the FeOOH species are metastable compounds whose decomposition is, obviously, kinetically hampered. This in turn can be considered a verification of our experimental findings that the FeOOH species represent significant components of the corrosion products formed under the relevant preheater conditions.Further, it should be noted that thermodynamics claim for the presence of metallic iron as substrate that magnetite Fe3O4 containing Fe(II) aside from Fe(III) must be present in the contact zone to the metal, because α-Fe2O3 will be reduced to Fe3O4 (ΔrGo=−25.3kJ/mol Fe3O4, 373 K). Indeed, this phase was preferentially found for the low-oxygen conditions of intake 1 according to the infrared and Raman spectroscopy, XRD, and MS (Figures 10, 11, 12(b), and 13(c), Tables 2 and 3). Moreover, the evidence of magnetite was suggested by Möβbauer spectroscopy also for the lower, adherent fraction of CP layers formed under the conditions of intake 2 (Figure 13(b), Tables 2 and 3).


## 3.4.1. Scanning Electron Microscopy and Local Element Analysis

Generally, the outer surfaces of the four samples are characterised by a markedly heterogeneous appearance in SEM, similarly as stated in [23]. Highly crystalline areas alternate with compact gel-like areas. The crystals encountered show quite different forms, such as platelets, leaf-like crystals, columnar and needle-like structures, and cubes. It could be often observed that zooming-in gives evidence of finer substructures.The first group of results as displayed in Figure8 relates to the sample M6/2, which had undergone a six-month operation regime without wintertime interruption. Figure 8(a) depicts an area on the outer surface of the loose CP layer with differently compact/crystalline regions. The corresponding elemental analyses revealed pronounced peaks of iron, oxygen, and chlorine, with the Cl concentrations ranking EDX2 > EDX1 > EDX3 (Figures 8(a)–8(c)). As for the lower, adherent layer (Figure 8(d)), both investigated sites were found to have relatively high Cl contents in spite of their different morphological shapes (Figures 8(e) and 8(f)). All in all, both parts of the CP layers stemming from intake 2 showed a variety of crystalline shapes, ranging from flimsy platelets over rods to feather-like forms, mostly grown together.Figure 8
SEM images and corresponding EDX spectra; (a–c) referring to the outer surface of the upper, loose CP layer of sample M6/2 (spectrum of EDX1 not shown), (d–f) referring to the lower, adherent CP layer of sample M6/2, and (g–h) referring to the integral layer of M18/1. Spectra regions beyond 10 keV (right edge of the diagram) were free of any signals and, hence, cut off.
(a)(b)(c)(d)(e)(f)(g)(h)Samples M18/1 and M24/1 from intake 1 were characterised by a higher noncrystalline fraction on the outer surface associated with minute Cl contents smaller than that for samples from intake 2 (Figures8(g) and 8(h)). This agrees with the contamination results shown in Figure 9.Figure 9
Concentrations (logarithmic plot) for selected chemical species determined in aqueous extraction solutions from the conductivity sensors; metal ion species according to ICP-OES, and anion concentrations according to IC.


## 3.4.2. Infrared and Raman Spectroscopy

The IR spectroscopic results obtained for the five utilised reference materials in transmission geometry show a generally very good agreement of the band positions with literature data, based both on synthesised compounds [18, 24–26] and on CPs and others [27, 28]. As Table 2 indicates, the bands of the FeOOH modifications differ from each other in a sufficient manner, whereas the spectra of Fe3O4 and α-Fe2O3 are somewhat similar in the region of 500–600 cm-1. Interestingly, the magnetite spectrum is partly missing in compilations [18]. It appears to be somewhat critical in its IR signature. As for β-FeOOH, the comparison with the full spectrum displayed in ref. [18] evidences the presence of the rod-like crystallised form.Table 2
Transmission minima of the IR bands determined for reference compounds.
PhaseBand position (cm-1)α-FeOOH798, 899β-FeOOH660-670, 846γ-FeOOH748, 1024Fe3O4558, 620 (shoulder)α-Fe2O3459, 535, 600 (shoulder)The results for the CPs are shown in Figure10. For the CPs of samples M6/2 and M12/2, considerable amounts of hematite (α-Fe2O3) are found. Hematite is present in both fractions of the CPs (upper/loose and lower/adherent fractions). On sample M6/2, both fractions contain additionally akaganeite (β-FeOOH). Contrarily, the upper, loose CP fraction of M12/2 reveals no sure indication of any FeOOH, whereas the adherent fraction appears to contain α- and γ-FeOOH. Certain differences in the phase state may be present between M6/2 and M12/2, because the former had undergone an exposure under sole operation conditions in contrast to the latter that was subjected also to a two-month shut-down period.Figure 10
IR spectra (cut-out) for powdered CPs. –upp: upper CP fraction; -low: lower CP fraction; -int: integral fraction. Experimental band positions for the reference materials are marked by dashed lines (cf. Table2).On the contrary, the CPs of the samples M18/1 and M24/1 have a quite deviating composition in that hematite appears to be vastly or completely substituted by magnetite, as it is attested by the missing band at 460 cm-1 and, macroscopically, by magnetic properties of the powdered CP. This fact is not explainable by the higher exposure times. Instead, it points to differing operating conditions in the plant. This detail will be discussed later. Moreover, goethite (α-FeOOH) and lepidocrocite (γ-FeOOH) are present.Raman spectroscopic data are shown in Figure11, again focused on the most relevant wavenumber region. As for the positions of the reference compounds, the major peaks agree with literature data [18, 26, 29–31]. Interestingly, magnetite (Fe3O4) was characterised as a weak Raman scatterer [26]. Moreover, it is easily subject to laser-based in situ oxidation. The spectra recorded confirm the presence of α-Fe2O3 in the cases of M6/2 and M12/2 very clearly. Astonishingly, the indication of FeOOH phases as minor components in the CPs by this technique proves to be difficult. The measurements of the pure reference materials suggest that the sensitivity for hematite is perceptibly higher than in the case of the FeOOH compounds. It appears that the acquisition time would have to be considerably higher.Figure 11
Raman spectrometric results for powdered CPs and reference substances; designations like for Figure10. Experimental peak positions for reference materials are marked by dashed lines; for Fe3O4 at ca. 660 cm-1 taken from reference [26, 27].The CP composition of M18/1 was quite different from those with M6/2 and M12/2. Hematite is missing, whereas magnetite is indicated. This confirms the finding obtained with the infrared measurements.


## 3.4.3. X-Ray Diffraction

Diffraction recordings were taken from CPs of M6/2-upp, M12/2-upp, M18/1-int, M24/1-upp, and M24/1-low.Whilst a mixture of a ferric oxide hydroxide (to be specified asβ-FeOOH referring to the original literature [32, 33]) and hematite (α-Fe2O3) was found for the CP samples from intake 2 (Figure 12(a)), the diffraction pattern of the samples from intake 1 proved to be substantially different. Here, a mix of FeOOH phases and magnetite (Fe3O4) was present (Figure 12(b)).Figure 12
X-ray diffractograms of powdered CPs of M12/2, upper fraction (a), and M18/1, integral fraction (b); reference lines augmented for the sake of perceptibility.
(a)(b)


## 3.4.4. Mößbauer Spectroscopy

The results shown here were obtained at IFJ PAN as described in the Multianalytical Investigations. Fit-relevant data were additionally taken from references [34–37]. The discussion focuses on one sample of each intake. Figures 13(a) and 13(b) display results for the different CP fractions of M12/2.Figure 13
Mößbauer spectra for powdered CPs of M12/2, upper (a) and lower (b) fractions, and M18/1, integral fraction (c), along with the fitting results.
(a)(b)(c)The spectrum for the upper, loose CP fraction is dominated by the sextet of hematite (α-Fe2O3), which exhibits hyperfine parameter values close to those observed in reference [37]. The quantification gives 95% of the iron compounds (Table 3), i.e., the overwhelming portion. A residue of about 5% is ascribed to akaganeite (β-FeOOH) or lepidocrocite (γ-FeOOH). Due to the peak broadening, the two phases cannot be distinguished, since they have very close hyperfine parameters at room temperature. This uncertainty holds also for more or less large portions of the other selected CP samples.Table 3
Compiled results for Möβbauer-derived phase compositions of the samples M12/2, upper and lower fractions, and M18/1, integral fraction, along with the fit-based quantification. δ: isomer shift; ΔEQ: electric quadrupole split; Bhf: magnetic hyperfine field.
SampleComponentδ (mm/s)ΔEQ (mm/s)Bhf (T)PhaseFraction (%)M12/2 upper CP fractionDoublet I0.390.69β- or γ-FeOOH5Doublet II1.102.98Mica2Sextet I0.37-0.1151α-Fe2O393M12/2 lower CP fractionDoublet I0.390.69β- or γ-FeOOH23Doublet II1.102.98Mica2.5Sextet I0.39-0.1151Fe2O320Sextet II0.2649Fe3O418.5Sextet III0.6645.5Sextet IV0.38-0.1338α-FeOOH36M18/1 integrated fractionDoublet I0.390.59β- or γ-FeOOH10Doublet II1.102.98Mica3Sextet I0.2649.5Fe3O447Sextet II0.6746.0Sextet III0.38-0.1338α-FeOOH40.5The lower, adherent part of M12/2 shows a markedly deviating spectrum (Figure13(b), Table 3). In particular, magnetite (Fe3O4) was identified in addition to hematite. The spectrum of magnetite is characterised by two sextets based on the simultaneous presence of ferrous and ferric ions in the inverse spinel lattice. From the thermodynamical point of view, the presence of magnetite in the neighbourhood of the metal substrate is a necessary issue; this will be discussed in the next section. In addition to the mentioned phases, the lower CP fraction of M12/2 contains a rest that was fitted assuming the presence of goethite (α-FeOOH) (Table 3). However, the fitting process suggested a modification of the original sextet. Literature indicates that dispersion of particle sizes, imperfect crystallinity, and/or deviations from stoichiometry may lead to distorted sextets and hyperfine field distribution, especially at room temperature [28, 38, 39]. Further, the clusters of goethite can be influenced from surrounding clusters of material with different symmetry and magnetic properties (i.e., different phases present in the sample) affecting the hyperfine parameters and widening the distribution of the magnetic hyperfine field. In order to take these factors into account, the fitting of the presumably existing goethite component was performed here in a manner described in the Materials and Methods with the assumption of a Gaussian distribution of hyperfine fields Bhf being not larger than 15 T. As Figure 13(b) makes clear, this resulted in markedly broadened linewidths, whereby the external lines of the sextet merge with the middle ones.For the integral CP of M18/1, as displayed in Figure13(c) and Table 3, a high portion of magnetite was found. Thus, this result addresses the aspect of an intake influence again. Further, a ferromagnetic fraction likely originates from goethite with a broad linewidth, as it was discussed above.


## 3.4.5. Summarising Considerations of Phase Analyses

The analytical findings for the CPs studied are compiled in Table4. Summarising, there is a good agreement of the four analytical techniques applied. Incomplete agreements, e.g., in view of the presence of the single oxide hydroxides, may be tolerable because of the probable lateral heterogeneity in context with punctual sampling. After all, Fe(III) oxide hydroxide phases appear to play an important role in the composition of the formed CPs. Thermodynamically, it can be easily shown that the formation of α-FeOOH from metallic iron and water is possible under aerobic conditions. From the tabulated data [40], a Gibbs free energy of reaction ΔrGo of -357 kJ/mol is calculated for 373 K, the measured temperature level for the investigation sites in the preheater. The formation of β- and γ-FeOOH needs the presence of chloride as a necessary or favourable prerequisite [18], which is fulfilled under the current conditions. In view of the thermal stability of goethite and the other FeOOH modifications, another thermodynamic calculation shows that the decomposition to the water-free oxide α-Fe2O3 under release of water proves to be principally possible (ΔrGo=−3.5kJ/mol for 373 K). In reality, the FeOOH compounds are, however, sufficiently stable on the temperature level of about 100°C.Table 4
Compiled analytical results for the CPs (goe.: goethiteα-FeOOH; aka.: akaganeite β-FeOOH; lep.; lepidocrocite γ-FeOOH; mag.: magnetite Fe3O4; hem.: hematite α-Fe2O3).
SampleIR spectroscopyRaman spectroscopyXRDMößbauer spectroscopyM6/2-uppM6/2-lowhem. + aka.hem. + aka.hem. + lep.hem. + lep.hem. + aka.--hem. + aka./lep.hem. + mag. + aka./lep.M12/2-uppM12/2-lowhem.hem. + goe. + lep.hem.(hem.)hem. + aka.--hem. + aka./lep.hem. + mag. + goe. + aka./lep.M18/1-intmag. + goe. + lep.mag.mag. + goe. + lep. + aka.mag. + goe. + aka./lep.M24/1-uppM24/1-lowmag. + goe. + lep.mag. + goe. + lep.mag. + goe. + lep.mag. + goe. + lep. + aka.This matter of fact could be unequivocally stated by DSC experiments with goethite and lepidocrocite, where the decomposition occurred indeed well beyond 250°C (Figure14 for goethite). This observation is in agreement with literature data of Weckler and Lutz [24]. They stated a much faster decomposition rate of akaganeite than those of the other polymorphs, obviously due to the Cl− ion impurities present in this compound.Figure 14
DSC tracks for goethite with decomposition to hematite, which was confirmed by the Raman spectroscopy. In case of lepidocrocite as starting product, maghemite (γ-Fe2O3) was primarily formed.Thus, it can be emphasised for a relatively wide temperature range that the FeOOH species are metastable compounds whose decomposition is, obviously, kinetically hampered. This in turn can be considered a verification of our experimental findings that the FeOOH species represent significant components of the corrosion products formed under the relevant preheater conditions.Further, it should be noted that thermodynamics claim for the presence of metallic iron as substrate that magnetite Fe3O4 containing Fe(II) aside from Fe(III) must be present in the contact zone to the metal, because α-Fe2O3 will be reduced to Fe3O4 (ΔrGo=−25.3kJ/mol Fe3O4, 373 K). Indeed, this phase was preferentially found for the low-oxygen conditions of intake 1 according to the infrared and Raman spectroscopy, XRD, and MS (Figures 10, 11, 12(b), and 13(c), Tables 2 and 3). Moreover, the evidence of magnetite was suggested by Möβbauer spectroscopy also for the lower, adherent fraction of CP layers formed under the conditions of intake 2 (Figure 13(b), Tables 2 and 3).


## 3.5. Chemical Contamination

Information on the occurrence of chemical species, which will influence the corrosion phenomena at the examination site, was gained from the water-based extraction of the coverings on the glassy conductivity sensors after an exposure period of 11 months.Figure9 shows analytical data for selected metal ion and anionic species determined for the inner surfaces of the both intakes. It is seen at a glance that there is a marked difference between the concentrations of corrosion relevant anionic species for both intakes. This means in view of the halogenides that especially intake 2 is characterised not only by a higher degree of “contamination,” but also by more serious corrosive conditions. The findings may be interpreted by an unequal distribution of the chemical freights, which are transported in the mass streams from the rotary kiln into the both intakes including the chemically multifaceted input from the secondary fuel (Figure 15). Intake 2 is located on that side of the rotary kiln, where the upward motion takes places, so that a greater part of dusty particles are forwarded into this branch. Contrarily, intake 1 is fed with the greater portion of combustion gases, among those also carbon monoxide CO. Gas analyses carried out separately make clear that intake 2 has a higher oxygen concentration than intake 1 with a typical oxygen difference of 2-3%. These facts are responsible that also the corrosion phenomena, as discussed above, are substantially different, with the mild steel exposed in intake 2 undergoing a markedly higher corrosion rate and a more distinct CP formation.Figure 15
Different mass transport in both intakes of the preheater.


## 3.6. Electrochemical Lab Investigations

The following electrochemical investigations were done to clear up the importance of oxygen and chloride content in the exhaust air of the two intakes. Therefore, the parameters for the model electrolyte solutions were varied correspondingly. Open circuit potentials (Table5) are given for different aeration and temperature conditions based on measurements in 1 M KCl solution. Parallel measurements showed ocp differences of a few mV only; also, the temporal movements over 10 min were small. The ocp for enhanced temperature under aerated, but unstirred conditions, occupies the most negative position. The considerable positive ocp shift under forced aeration through pressurised air is in accordance with the mixed potential theory. Similar findings in view of aeration/deaeration were gained, e.g., for carbon steel in a near-neutral mixed carbonate-chloride-sulphate salt medium under consecutively varied gas purging regimes [41, 42].Table 5
Open circuit potentials (mean values at 200 s after immersion start of three measurements each) for 1 M KCl electrolyte solution.
Conditionocp (mV)Ambient temp., aerated, unstirred-61040 °C, aerated, unstirred-637Ambient temp., pressurised-air purge-530Ambient temp., N2 purge-599Figure16 depicts the influence of different aeration on the course of voltammetric measurements and the Stern-Geary corrosion data as well. Under pressurised-air purging, the ocp is shifted in the positive direction, and the cathodic currents are favoured in accordance with the mixed potential theory. The control of the corrosion rate at ocp is more on the side of the cathodic partial reaction, because the oxygen reduction takes place under a high degree of transport control, where the diffusion layer thickness is substantially decreased for the vigorously moved electrolyte solution. It is easily conceivable that the corresponding curves are subject of higher scattering due to the less controlled air purging. The outlined situation is reflected also by the mean values of the polarisation resistance Rp and the corrosion current density jcorr, which surpass for pressurised-air conditions those for the unstirred state by a factor of about 40 (Figure 16, inserts).Figure 16
Single polarisation measurements under varied aeration conditions at ambient temperature recorded after 0.5-1 h of immersion in 0.1 M KCl electrolyte solution from cathodic (ocp−0.3V) to anodic with 1 mV/s; inserts: corresponding Stern-Geary corrosion data (mean values).After all, the major role of oxygen/cathodic partial reaction for the corrosion process is emphasised, thus confirming the derived statements for the real corrosion phenomena encountered at the examination site of the preheater.A recalculation of the corrosion current densityjcorr into a corrosion rate based on the thickness loss of steel kd gives, according to Equation (3), a corrosion rate of kd=58μm/a (jcorr=5μA/cm2). This roughly conforms to the order of magnitude of the values of Table 1, which was measured for the preheater-exposed steel plates. MFe: atomic mass of Fe (55.85 g/mol); z: charge-transfer number for the dissolution reaction (2); F: Faraday’s number (9.65×104 As/mol); ρFe: density (7.85 g/cm3).
(3)kd=jcorr·MFez·F·ρFe.In addition to the dc measurements, ac perturbation was applied to gain a deeper insight into mechanistic issues. The Bode diagram of Figure17 illustrates the impedance behaviour in 1 M KCl solutions in terms of the influence of aeration, deaeration through simultaneous N2 purging, and temperature enhancement to 40°C. The depicted curves, chosen from a series of consecutive EIS measurements over 5 d each, refer to a resting time of 3 h in order to provide for approximate stationarity during the longer-lasting EIS measurement. On the other hand, significant covering by corrosion products, i.e., the development of an inhomogeneous surface, which had been previously taken into account by different authors [43, 44], should be avoided. Here, the thickness of the formed CP layer could be estimated to 5×10−8m for unstirred conditions, based on the corrosion current density of 5μA/cm2 (cf. Figure 16).Figure 17
EIS measurements (Bode plot) under varied aeration/deaeration and temperature conditions recorded after 3 h of immersion in 1 M KCl electrolyte solution at ocp.Irrespective of quantitative differences between the three curve pairs for aerated, aerated/40°C, and deaerated conditions, they show a nonidentical shape. The curves are characterised by a number of features: (i) the asymmetric shape of the phase angle bumps at medium frequencies, (ii) the flattening slope oflog∣Z∣ in the direction of decreasing frequency, and (iii) the low-frequency (LF) plateau of about 2 kΩ cm2. It is somewhat surprising that the LF log∣Z∣ values for these condition sets differ only negligibly. As for the enhanced temperature, it may be argued that the expected reactivity increase will be counteracted by the decreased oxygen solubility. The curves for simultaneous air purging show, notwithstanding the scatter, a more symmetric shape of the phase angle course associated with a considerably decreased LF log∣Z∣ plateau of about 0.15kΩcm2. This is a further evidence for the decisive role of oxygen for the corrosion. Finally, the LF plateau levels confirm the behaviour at dc (Figure 16) very well.The high-frequency (HF) plateau oflog∣Z∣ at the right-hand side of the spectra allows reading the electrolyte resistance Re, which is, of course, dependent both on the electrolyte concentration and on the temperature. Indeed, three of the condition sets show completely coinciding electrolyte resistances of about 4 Ω cm2, whilst Re (40°C) is somewhat lower in accordance with theory.Modelling of the measured curves was best performed using a modified Randles equivalent circuit (Figure18(a)). It contains two features: (i) a constant phase element (CPE) with the parameters TCPE and PCPE instead of the pure double layer capacity and (ii) an element Ws designed for a finite diffusion length d, which is characterised by a finite limiting value of its real part for f=0, instead of the original Warburg diffusion impedance [45]. The corresponding impedance equation for Ws is inserted in Figure 18(b). It can be shown that the ZView-based parameter RWs is equal to the limiting value mentioned above. Parameter TWs stands for d2/D, where D is the diffusion coefficient for dissolved oxygen (2.1×10−5cm2/s at 298 K) and d is the diffusion length. Finally, parameter PWs is nearby 0.5.Figure 18
(a) Randles-based equivalent circuit.Re: electrolytic resistance; Rct: charge-transfer resistance; CPE: constant phase element; Ws: modified Warburg impedance with finite diffusion length. (b) Impedance equation for Ws provided with the parameters RWs, TWs, and PWs acc. to ZView; i: imaginary unit; ω: angular frequency. (c) Measured and fitted curves for 1 M KCl, ambient temperature, aerated, and unstirred conditions. The lowest frequency points were omitted due to scattering. (d) Corresponding fitted parameters.
(a)(b)(c)(d)The selected measurement for aerated, unstirred conditions documents the high goodness of fitting (Figure18(c)). As the figures of the table in Figure 18(d) point out, the diffusion-related resistance RWs is determined to be more than one order larger than the interface-related resistance Rct. That means diffusion plays a significant role within the total process and forms the rate-determining step. Thus, diffusion control is active both for the cathodic reduction (as was evidenced by dc measurements, cf. Figure 16) and for normal corrosion at ocp.Turning to air purging, the parameterRWs is dramatically reduced down to 0.15-0.2 kΩ cm2 in agreement with the decreased level of the measured LF log∣Z∣ plateau in Figure 17. It appears now that the inverse relation RWs<Rct holds, which conforms to the improved diffusion under convective conditions.A second impedance diagram (Figure19) addresses different solution compositions. These curves provide evidence that a concentration modification from 1 to 0.1 mol/L KCl does not give significant change in the LF log∣Z∣ plateau. A similar result, within the normal scatter, is gained, when the chloride is completely removed using the sulphate salt of the same molar concentration. This means that the overall corrosion rate will not be essentially influenced by the actual concentration or even by the absence of chloride anions. The negligible chloride influence may be regarded as unexpected, because it is well known that the chloride ion is involved in the anodic dissolution mechanism [46]. However, earlier experiments using AISI 4340 low-alloyed steel in neutral sulphate and chloride solutions [47] gave similar results. Further, a relatively low concentration dependence of corrosion current densities was observed in polarisation measurements on SAE 1010 carbon steel in aerated 0.02-1 M NaCl solutions [44, 48]. This was explained by the fact that both partial reactions—the cathodic partial reaction with mixed control of charge-transfer and mass transport and the anodic subprocess with pure charge-transfer control—undergo a concentration influence.Figure 19
EIS measurements (Bode plot) recorded after 3 h of immersion in different electrolyte solutions at ocp under ambient temperature and aeration without stirring; comparative application of wet-ground surface.As for the electrolyte resistance, the ratios of theRe values for Re0.1MKCl/Re1MKCl=8.3 and for Re0.1MKCl/Re0.1MK2SO4=1.58 reflect the specific effects of the involved ions quite regularly. Theory states that the electrolytic conductivity and, hence, the reciprocal of the electrolyte resistance are determined by the product of ionic charge, ionic concentration, and ionic mobility [49].Finally, a few EIS measurements referred to the influence of the surface pretreatment. As the forth curve pair in Figure19 evidences, wet-grinding, i.e., removing the rolling skin, led practically to no differing results.


## 4. Conclusions

Unlike earlier investigations that were directed to the events in the rotary kiln region, this study focused on the corrosion and the underlying conditions in the zone of the preheater of a running cement clinker production facility, more precisely at the inner surface of the mild steel preheater cladding. The following conclusions are drawn from the exposure experiments performed over a long-term period of 24 months as well as from the lab investigations:(i)
It was possible to record humidity and temperature on-line during the production process by inserting special sensors directly at the specific preheater sites that were relevant for the corrosion investigation. The temperature movements following onset and shut-down of operation were found to be associated with in-phase movements of the relative humidity. This was attributed to the participation of the built-in ceramic materials as water sorbents/desorbents. An unambiguous evidence of liquid water at the inner surface of the cladding could not be found(ii)
The corrosion phenomena at the inner surface of the preheater mantle were tracked by reexposure of four large-area, indigenous steel plate cutouts of the mantle. The two parallel intakes 1 and 2 were taken into account. Generally, the steel corrosion was affected by contaminants, originating from secondary fuels. Appearance and structure of the corrosion products were found to be not mainly dependent on the varied length of exposure, as was expected in the beginning. Instead, it became apparent that the preheater branch exerts the major influence. The plates in the preheater branch that are influenced by the higher oxygen and chloride concentrations (intake 2) show a markedly higher corrosion rate and, correspondingly, corrosion product (CP) layers of higher thickness. In addition, a distinct spalling character of the upper portions of these CPs was observed(iii)
The investigations made a contribution to a safer operation of the whole production facility as well as to the maintenance procedures(iv)
Various independent analytic methods for the identification of the present oxidic phases yielded a vast agreement. Whilst hematite proved the main component of the CPs formed in intake 2 under conditions of higher oxygen concentrations, magnetite was identified for low-oxygen conditions (intake 1). Different Fe(III)-oxyhydroxide phases were identified by the multianalytical approach. These substances play an important role in the composition of the CPs formed, though being a basically metastable compound class. For the factory-assigned position of examination in the preheater zone was stated that a corrosion process takes place under conditions of humidity, limited oxygen access, and chloride ion presence at an elevated temperature level of about 100-110°C. A typical high-temperature corrosion mechanism could be distinctly excluded(v)
The electrochemical laboratory investigations emphasised the presence of oxygen as a key factor in the occurring corrosion of the unalloyed steel. It was proved by linear polarisation and impedance measurements that diffusion control dominates both for the cathodic reduction and for normal corrosion without polarisation. A roughly coincident level of the corrosion current density was determined by the both methodical approaches (dc/ac). Further, a satisfactory agreement could be established between the electrochemical lab data for the corrosion rate and the metallographically determined data after real preheater exposure(vi)
An accelerating effect of chloride ions could not be derived for the investigated laboratory model conditions. This may be explained by the markedly simplifying conditions compared with the high in-plant complexity. Nevertheless, further need of research at temperatures close to the real data is seen.



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*Source: 7341029-2020-09-18.xml*