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Article

High-Temperature Corrosion Behavior of Al-Coated Ni-Base Alloys in Lithium Molten Salt for Electroreduction

by
Wan-Bae Kim
1,
Woo-Seok Choi
1,
Kyu-Seok Lim
1,
Soo-Haeng Cho
2 and
Jong-Hyeon Lee
1,2,3,*
1
Department of Materials Science and Engineering, Chungnam National University, Daejeon 34134, Korea
2
Rapidly Solidified Materials Research Center (RASOM), Chungnam National University, Daejeon 34134, Korea
3
Graduate School of Energy Science and Technology, Chungnam National University, Daejeon 34134, Korea
*
Author to whom correspondence should be addressed.
Coatings 2021, 11(3), 328; https://doi.org/10.3390/coatings11030328
Submission received: 29 January 2021 / Revised: 5 March 2021 / Accepted: 8 March 2021 / Published: 13 March 2021
(This article belongs to the Special Issue Development and Characterization of Coatings and Surface Treatments for Corrosion, Wear, and Tribocorrosion Protection of Materials in Hostile Environments)
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Abstract

:
The electrolytic reduction of a spent oxide fuel involves the liberation of oxygen in a molten salt LiCl–Li2O electrolyte, which creates a corrosive environment for typical structural materials. In this study, the corrosion behaviors of Al–Y-coated specimens in a Li molten salt kept under an oxidizing atmosphere at 650 °C for 72 and 168 h were investigated. The weight loss fraction of the coated specimen to bare specimen was approximately 60% for 3% Li2O and 54% for 8% Li2O at 72 h, and approximately 38% for 3% Li2O and 30% for 8% Li2O at 168 h. Corrosion was induced in the LiCl–Li2O molten salt by the basic oxide ion O2− via the basic flux mechanism, and the corrosion product was found to be dependent on the activity of the O2− ion. The increase in weight loss may have been caused by the increase in the O2− concentration due to the increase in the Li2O concentration rather than being because of the increased reaction time. The Al–Y coating was found to be beneficial for hot corrosion resistance, which can be useful for handling high-temperature lithium molten salt under an oxidizing atmosphere.

1. Introduction

Molten salts are used in various industries due to their high electrical conductivity, high-density processing, and fluid properties. Recently, they have been attracting increasing attention for applications in jet engines [1,2,3,4,5], fuel cells [6,7,8], energy storage [9,10,11], and metal purifications [12,13,14]. However, molten salts corrode container materials and various components of electrolysis equipment. Hence, numerous studies have been conducted to understand the corrosion of the structural materials used for handling high-temperature molten salts, such as sulfates [15,16], carbonates [17,18], fluoride [19,20,21], and chloride systems [22,23]. Superalloys have been developed as a structural material for devices using high-temperature molten salts, and studies on their high-temperature corrosion characteristics are being continuously conducted [24,25,26,27,28,29,30,31]. However, according to previous studies, this type of alloy may not be able to simultaneously fulfil the criteria of high-temperature strength and corrosion resistance when placed in a high-temperature electrolyte containing oxygen and a strongly corrosive lithium molten salt [12,31]. Therefore, employing a coating that provides a thermal barrier has been found to be the most effective and economical method for enhancing the corrosion resistance. Coating technologies improve the surface characteristics of the base material with respect to its environment, and the use of these technologies has expanded with the improvement of coating material properties, such as high-temperature corrosion resistance [32,33,34,35,36,37], abrasion resistance [38,39], and electromagnetic properties [40,41]. Such surface-coating technologies offer the advantage of improving the high-temperature corrosion resistance of the base material without significantly affecting its mechanical properties. In general, Al-based oxides formed on the surface are stable at high temperatures, have a relatively slow growth rate, and improve corrosion resistance due to the dense structure. Therefore, research is being conducted to improve corrosion resistance at high temperatures by adding Al to the base metal or coating the surface. Recent reports have confirmed that Fe [42] and Ni alloys [43,44] can be used as inert anode materials in a high-temperature electrolyte by reacting the electrolyte with Al2O3 to form an Al2O3-based composite oxide passive film, thus securing long-term durability [45]. Furthermore, in some studies, Al has been supplied either as an alloying element or from an electrolyte to form an Al2O3 composite oxide layer. Therefore, in the absence of an Al source in the electrolyte or alloy, the possible applications of general-purpose commercial alloys, for example, in high-temperature molten carbonate fuel cells (MCFCs), waste incineration systems, and molten salt electrolysis systems, can be greatly expanded if similar corrosion resistance is achieved by supplying Al through the surface treatment of the structural material.
The electrochemical reduction of spent oxide nuclear fuel is carried out in a high-temperature LiCl–Li2O molten salt system, where the fuel reduces to U metal at the cathode, and O is generated at the anode. This electrolytic reduction process is carried out in a highly corrosive molten salt system at 650 °C or higher. Due to the oxidizing atmosphere formed by the generated O, the molten salt-handling device is in a severely corrosive environment. Thus, a device material suitable for handling the molten salt, namely, an ordinary corrosion-resistant structural material, must be developed for implementation in this electrochemical reduction technology. However, only a few studies have reported the corrosion resistance of Al-coated structural materials used in devices that handle high-temperature lithium molten salts, which is the subject of this study.
In this study, Haynes 263, which has an excellent strength, ductility, and weldability at high temperatures, was used as the Ni-based superalloy. The high-temperature corrosion behaviors of the Haynes 263 specimen coated with Al and Y were investigated using magnetron sputtering and electron beam physical vapor deposition (EB-PVD) in an oxygen-generating high-temperature Li molten salt system under simulated electrolytic reduction conditions.

2. Materials and Methods

2.1. Preparation of Specimen

The Ni-based superalloy Haynes 263 (Ni: 51.35, Cr: 20.0, Fe: 0.50, C: 0.05, Si: 0.13, Mn: 0.10, Mo: 5.80, Al: 0.45, Co: 19.20, and Ti: 2.39 wt.%) was used as the base material. The specimen was heated and then water-cooled at 1050 °C for 1 h to remove internal defects and decompose carbides. A specimen 70 mm in length, 15 mm in width, and 70 mm thick was prepared and then heat-treated at 950 °C for 1 h for stabilization treatment. Before the corrosion test, the specimen was polished in one direction with 1200-grit SiC paper and then degreased with distilled water and acetone. Magnetron sputtering was performed to deposit a uniform Al–Y coating layer because it has high sputtering efficiency, reduces collisions with the specimens and thin films by the vortex motion of electrons, and has a constant deposition rate and uniform thickness at a given input power [39]. In addition, unlike in the conventional diffusion coating process, the microstructures of the deposited ceramics can be varied in EB-PVD by adjusting the deposition process parameters, such as the deposition rate, obtaining a coating layer with a uniform surface and good adhesion. Due to these features, magnetic sputtering and EB-PVD processes were used in this experiment.

2.2. Coating Formulation

A preliminary experiment using magnetron sputtering was conducted for the conditions where the Al coating exhibits optimal adhesion to the specimen. The initial vacuum degree was 133.322 × 10−6 Pa, the specimen temperature was 250 °C, the electron beam power was 4 kW, and the deposition rate was approximately 0.3 μm/min. The thickness of the coating layer deposited by controlling the deposition time (35 min) was 10 μm. The EB-PVD coating conditions for the optimal adhesion of an Y coating on the deposited Al were also evaluated. The initial vacuum was 133.322 × 10−5 Pa, the electron beam power was 8 kV (100–110 mA), the specimen temperature was 400 °C, and the deposition rate was approximately 1 nm/s. The thickness of the coating layer deposited by controlling the deposition time was 0.3 μm.

2.3. High-Temperature Corrosion Tests

The experimental apparatus consisted of a reactor and a mixed gas supply, as shown in Figure 1. A LiCl (Rare Metallic Co., Ltd., Tokyo, Japan, 99.9%) and Li2O (Cerac, WI, USA, −100 mesh, 99.5%) powder mixture and a thermocouple shielded with an Al2O3 tube were introduced into a high-density MgO crucible and then heated at 300 °C for 3 h in an Ar atmosphere to remove any moisture picked up. Subsequently, the specimens and Al2O3 tube were immersed into the molten salt, and mixed gas (Ar–10%O2) was supplied through an Al2O3 tube. Two MgO crucibles were used in the apparatus, as shown in Figure 1, and each crucible held one specimen. The corrosion test was conducted for the bare and coated specimens. For the bare specimens, the corrosion environment temperature was 650 °C, the corrosion time was 24–168 h, and the Li2O concentration was 1–5 wt.%. For the coated specimens, the corrosion environment temperature was 650 °C, the corrosion times were 72 and 168 h, and the Li2O concentrations were 3 and 8 wt.%. Following the corrosion tests, the specimens were separated from the molten salt and cooled to room temperature (15–20 °C) in an Ar atmosphere.

2.4. Characterization

The reactor was opened, and the specimens were removed for a visual examination. The specimens were then cleaned ultrasonically in distilled water to remove the molten salt and dried for more than 24 h in a drying furnace at 80 °C. The initial and final weights of the tested specimens were then recorded to assess the extent of corrosion using an analytical balance (Sartorius QUINTIX224-1S, Goettingen, Germany). The corroded specimens were then cut using a diamond cutter and ultrasonically cleaned in acetone for characterization. Some of the specimens were then prepared for metallographic examination via cold mounting, grinding, and polishing. The microstructure, morphology, chemical composition, and elemental distribution of the corrosion layer and substrate were examined using a microscope for field emission-scanning electron microscopy (FE-SEM, JEOL, JSM-7000F, Tokyo, Japan) with apparatus equipped with a spectrometer for energy dispersive X-ray spectroscopy (EDS, JEOL, Tokyo, Japan) [46]. X-ray powder diffraction (XRD, D/MAX-2200 Ultima/PC, Rigaku, Tokyo, Japan) analysis was used to determine the structure of the hot corrosion products using the standard method [47]. The following conditions were applied in the analyses: the FE-SEM/EDS applied voltage and vacuum pressure were 15 kV and 7.04 × 10−4 Pa, respectively; the XRD scan rate, step, and half-width range (2θ) were 3.5°/min, 0.05°, and 15–100°, respectively.

3. Results and Discussion

3.1. Corrosion Kinetics

The weight loss of the bare (closed legends) and Al-coated (open legends) Haynes 263 specimens after the corrosion tests in the LiCl–(1, 3, 5, and 8 wt.%) Li2O molten salt as a function of time is shown in Figure 2. The bare specimens lost weight as the Li2O concentration increased, and the weight loss increased linearly with time, which suggests that the corrosion product formed a porous, nonprotective film. The formation of the porous film in the molten salt LiCl–Li2O may have resulted from the basic fluxing mechanism owing to the increased oxide ion O2− (Li2O) concentration [47,48]. Through the basic fluxing mechanism, in a molten salt with a high concentration of O2−, O2− reacts with the oxide formed at the beginning of oxidation, and the oxide is dissolved in the molten salt and then reprecipitates as crystal grains of the oxide on the alloy surface [49]. As this phenomenon repeats itself, the porous film grows inside. In the case of a porous film, molten salt easily moves to the corrosion layer/alloy interface through the pores, and the corrosion layer grows from the interface toward the alloy as a product of the reaction with the alloy [50]. In the case where the Al-coated specimens were in the molten salt LiCl–(3 and 8 wt.%) Li2O for 72 and 168 h, the fraction of the weight loss of the coated specimen to the bare specimen was approximately 60% for 3 wt.% Li2O and 54% for 8 wt.% Li2O at 72 h, and approximately 38% for 3 wt.% Li2O and 30% for 8 wt.% Li2O at 168 h. When the Li2O concentration was low, the fraction of the weight loss of the coated specimen to the bare specimen may have decreased owing to the protective film of the Al-based oxide formed on the surface of the coated specimen. However, as the Li2O concentration and the corrosion reaction time increased, the coating effect decreased. Considering that the oxide ion O2− in the basic fluxing mechanism significantly participated in the corrosion reaction in the high-temperature molten salt, the increase in weight loss may have resulted from the increase in the oxide ion O2− concentration due to the increased Li2O concentration, rather than the effect of the coating.

3.2. Phase of Corrosion Products

Figure 3 shows the XRD patterns of the corrosion products of the bare specimen corroded at 650 °C for 72 h in a molten salt of LiCl–(1, 3, and 5 wt.%) Li2O. The corrosion products were Cr2O3, NiO, and NiCr2O4 for 1 wt.% Li2O (Figure 3a); Li(Ni,Co)O2 and Li(Cr,Al)TiO4 for 3% Li2O (Figure 3b); and Li(Ni,Co)O2 and LiFeO2 for 5% Li2O (Figure 3c). Because Li2O is a strong basic oxide with properties similar to those of Na2O, the phenomenon where corrosion is accelerated by Li2O can be explained by the basic fluxing mechanism suggested by Goebel et al. [48]. Cr2O3 and NiO were formed on the specimen surface at the beginning of the corrosion by the dissolved O present in the molten salt. The Cr2O3 and NiO reacted with the oxide ion O2− (Li2O) to form CrO42− (Li2CrO4) and NiO22− (Li2NiO2) and dissolved into the molten salt, which diffused outward and reprecipitated as Cr2O3 and NiO particles at the molten salt/atmosphere interface. For the reprecipitation of oxides suggested by Goebel et al. [48], a reduction in oxide ion O2− activity from the specimen surface to the molten salt/atmosphere, i.e., a negative gradient of oxide solubility in the molten salt, is a prerequisite. Therefore, in the case of the 1 wt.% Li2O, the corrosion products were Cr2O3, NiO, and NiCr2O4. Spinel-type NiCr2O4 was formed by a solid-state reaction with the corresponding oxides (NiO and Cr2O3) [51]. For Li2O concentrations of 3 wt.% or more, the absence of the reprecipitation of Cr2O3 and NiO may have occurred, resulting from a positive gradient of oxide solubility in the molten salt. Moreover, a corrosion product was formed by a basic fluxing reaction, in contrast to that observed in 1 wt.% Li2O. The physical properties of Co, such as its crystal structure at a high temperature, atomic diameter, density, and melting point, are very similar to those of Ni. Therefore, Co and Ni show similar diffusion behaviors, resulting in their coexistence on the surface oxide layer. The Ti content in the bare specimen was approximately 2.4%, and the external diffusion rate of the more oxidative Ti at a high temperature was faster than that of Cr [52]. Thus, Ti diffused through the oxide and existed in the surface oxide layer. As the metal ions in the oxide can be ranked by their diffusion coefficients as Fe3+ > Fe2+ > Ti3+ > Ni2+ > Cr3+ [51], the Fe ion diffused through the initially formed Cr–oxide layer to form the corresponding oxide. Li(Ni,Co)O2, LiFeO2, and Li(Cr,Al)TiO4 were formed by the basic fluxing reaction. The examination of the formation process for these corrosion products revealed that the mechanism of formation differed depending on the concentration of Li2O.
Figure 4 shows the XRD patterns of the corrosion products of the coated specimen corroded at 650 °C for 72 and 168 h in a molten salt of LiCl–(3 and 8 wt.%) Li2O. The corrosion products of the coated specimen were LiAlO2, LiFeO2, and Li(Ni,Co)O2 for 72 h (Figure 4a) and Li(Ni,Co)O2, LiAlO2, LiTiO2, and LiFeO2 for 168 h (Figure 4b) in a molten salt of LiCl–(3 wt.%) Li2O, and LiAlO2 and LiFeO2 for 72 h (Figure 4c) and Li(Ni,Co)O2 and LiFeO2 for 168 h (Figure 4d) in a molten salt of LiCl–(8 wt.%) Li2O. As shown in Figure 4, the protective role of the LiAlO2 generated by the basic fluxing reaction of Al oxide in the coating layer may have inhibited the external diffusion of elements of the base metal, thereby affecting the corrosion rate. However, as shown in Figure 2, it is believed that the increase in the corrosion rate was greatly influenced by the decrease in the protective role due to the dissolution of the Al oxide layer, which was caused by the increase in Li2O concentration and corrosion time. According to a report that discussed the change in the solubility of Al2O3 according to the Na2O concentration in a Na2SO4 electrolyte at 1200 K, the solubility gradually decreases as the Na2O concentration increases, and the solubility increases rapidly after passing the critical point [49]. Based on this result, it is believed that an excessive increase in Li2O concentration in this study caused an increase in the solubility of Al2O3 due to a basic dissolution mechanism, leading to the destruction of the protective layer.

3.3. Corrosion Behavior

Figure 5 shows the cross-sectional SEM image and elemental distribution of the bare specimen corroded at 650 °C for 72 h in a molten salt of LiCl–(1, 3, and 5 wt.%) Li2O. In the case of the LiCl–1% Li2O salt, the corrosion layer was continuous, dense, and adherent, as shown in Figure 5a. The corresponding SEM image and elemental distribution show that the corrosion layer was mainly composed of Cr2O3, NiO, and small amounts of Al, Fe, and Ti oxides. An intermediate layer rich in Ni-oxide scale formed close to the base metal. The oxygen active elements, such as Al and Ti, were preferentially oxidized and participated in the corrosion layer [53]. Ni is an element that inhibits the internal diffusion of an oxygen ion by its accumulation at the oxide/oxide interface or beneath the oxide layers [54]. In this study, the enrichment of Ni in an internal corrosion layer was observed, and Ni was considered as a useful element for the enhancement of the corrosion resistance in an oxidative molten salt. As shown in Figure 2, the abovementioned features are considered to influence the corrosion rate. For LiCl–3% Li2O, as shown in Figure 5b, the corrosion layer consisted of Cr, Al, Ti-based oxides, and an Ni–Co-based complex oxide. The corrosion layer was continuous and dense. However, part of the corrosion layer peeled off, which may have resulted from damage during the polishing process, and a crack appeared between the corrosion layer and the substrate. As shown in Figure 2, molten salt easily diffused through the peeled parts and cracks, which may have affected the corrosion rate. In the case of LiCl–5% Li2O, the corrosion layer consisted of an Fe-based oxide and a Ni–Co-based complex oxide, as shown in Figure 5c. The corrosion layers and cracks appeared larger than those in Figure 5b, which had a significant influence on the corrosion rate, as shown in Figure 2.
Figure 6 shows the cross-sectional SEM image and EDS analysis results for the coated specimen corroded at 650 °C for 72 h in molten salts of LiCl–3 (a) and 8 wt.% Li2O (b). As shown in Figure 6a, the corrosion layer formed of Al oxide, Fe oxide, and Ni–Co oxide appeared to be rough, while that composed of Fe-based and Ni–Co-based oxide is believed to have formed due to the diffusion coefficients of these elements being greater than those of the other elements; for example, Fe3+ > Ni2+(Co2+) > Cr3+ [51]. Y is an element that promotes the oxidation of Al deposited on a base metal, densifies the Al-based oxide film, and improves adhesion; however, in this experiment, the Y deposited on the surface with a thickness of 0.3 μm may have peeled off during the formation of the oxide layer or been removed during the dissolution of the formed oxide in the molten salt. Thus, the deposited Y did not significantly contribute to the corrosion inhibition during the corrosion test. In addition, the internal corrosion layer appeared to be thin, which is thought to be due to the corrosion layer containing the Al-based oxide acting as a protective film inhibiting internal corrosion. Furthermore, there was a close correlation between the thin internal corrosion layer and the decrease in the corrosion rate, as shown in Figure 2 (open legends). In the case of LiCl–8 wt.% Li2O, as shown in Figure 6b, the corrosion layer was composed of Al-based oxide and Fe-based oxide, and the Fe-based oxide may have formed by the diffusion of Fe, which has a higher diffusion coefficient than the other elements present in the base metal. In addition, the thickness of the corrosion layer shown in Figure 6b was less than that shown in Figure 6a; the large number of pores and cracks in the corrosion layer or the corrosion layer/substrate interface caused the large internal corrosion. These results are considered to have had a great influence on the corrosion rate, as shown in Figure 2.
Figure 7 shows the cross-sectional SEM images and elemental distribution of the coated specimen corroded at 650 °C for 168 h in molten salts of LiCl–3 wt.% (a) and 8 wt.% Li2O (b). As shown in Figure 7a, the corrosion layer was formed of Ni, Co, Cr, Ti, and Fe-based oxides in addition to Al-based oxides, which are believed to have been generated due to the external diffusion of these elements in the base metal. Unlike that observed in Figure 6a, internal corrosion largely formed beneath the corrosion layer due to cracks generated at the corrosion layer/substrate interface. Moreover, considering the results of Figure 2 (open legends), as the reaction time increased, the weight loss increased due to the decrease in the protective role of the corrosion layer, including the Al-based oxide. In the case of 8 wt.% Li2O, as shown in Figure 7b, the corrosion layer was composed of Ni–Co-based oxide and Fe-based oxide, and Al-based oxide was not observed, as shown in the results of Figure 4d. When the Li2O concentration was high and the reaction time increased, the corrosion layer composed of Ni–Co-based oxide and Fe-based oxide peeled and cracked, and internal corrosion proceeded greatly due to the deterioration of the protective performance of the corrosion layer. The peeling of the corrosion layer was caused by the internal stress and the difference in the thermal expansion coefficients of the oxides generated by the external diffusion of the internal elements of the base metal [55,56].

4. Conclusions

The following conclusions were drawn from the results of the study:
(1) The corrosion rate of the coated specimen decreased compared to that of the bare specimen. In the case of 3 wt.% Li2O, it decreased by approximately 60% at 72 h and approximately 38% at 168 h. On the other hand, for the 8 wt.% Li2O, the corrosion rate decreased by approximately 54% at 72 h and 30% at 168 h.
(2) In the molten salt of LiCl–Li2O, corrosion was carried out by the basic oxide ion O2− by the basic fluxing mechanism, and the corrosion product depended on the activity of the oxide ion O2−.
(3) The corrosion products of the bare specimens at 72 h were Cr2O3, NiO, and NiCr2O4 for 1 wt.% Li2O; Li(Ni,Co)O2 and Li(Cr,Al)TiO4 for 3 wt.% Li2O; and Li(Ni,Co)O2 and LiFeO2 for 5 wt.% Li2O. However, the corrosion products of the coated specimens for 3 wt.% Li2O showed LiAlO2, LiFeO2, and Li(Ni,Co)O2 peaks for 72 h and Li(Ni,Co)O2, LiAlO2, LiTiO2, and LiFeO2 peaks for 168 h. In the case of 8 wt.% Li2O, LiAlO2 and LiFeO2 peaks for 72 h and Li(Ni,Co)O2 and LiFeO2 peaks for 168 h were exhibited, respectively.
(4) The increase in the weight loss may have a higher dependence on the increase in the oxide ion O2− concentration owing to the increase in the Li2O concentration than the reaction time.
(5) This coating was found to significantly increase the hot corrosion resistance of the structural material, improving its ability to handle high-temperature lithium molten salt under an oxidizing atmosphere. Thus, it is expected to be applicable to other processes that involve harsh conditions such as MCFC and waste incineration systems.

Author Contributions

Conceptualization, W.-B.K., S.-H.C., and J.-H.L.; methodology, W.-B.K. and J.-H.L.; software, W.-S.C., and K.-S.L.; validation, W.-B.K. and J.-H.L.; formal analysis, W.-B.K., S.-H.C., and J.-H.L.; investigation, W.-B.K., S.-H.C., and J.-H.L.; resources, J.-H.L.; data curation, S.-H.C. and J.-H.L.; writing—original draft preparation, W.-B.K. and S.-H.C.; writing—review and editing, J.-H.L.; visualization, W.-B.K.; supervision, J.-H.L.; project administration, J.-H.L.; funding acquisition, J.-H.L. All authors have read and agreed to the published version of the manuscript.

Funding

This research was funded by Chungnam National University.

Institutional Review Board Statement

Not applicable.

Informed Consent Statement

Not applicable.

Data Availability Statement

The data are available from the corresponding author upon request.

Acknowledgments

This work was supported by the research fund of Chungnam National University.

Conflicts of Interest

The authors declare no conflict of interest.

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Coatings 11 00328 g001 550
Figure 1. Schematic of corrosion test apparatus.
Figure 1. Schematic of corrosion test apparatus.
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Figure 2. Weight loss of the bare (closed legends) and Al-coated (open legends) Haynes 263 specimens corroded at 650 °C, as a function of time.
Figure 2. Weight loss of the bare (closed legends) and Al-coated (open legends) Haynes 263 specimens corroded at 650 °C, as a function of time.
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Figure 3. X-ray diffraction patterns of the corrosion products on bare specimens corroded in molten salt of LiCl–1 (a), 3 (b), and 5 wt.% Li2O (c) at 650 °C for 72 h.
Figure 3. X-ray diffraction patterns of the corrosion products on bare specimens corroded in molten salt of LiCl–1 (a), 3 (b), and 5 wt.% Li2O (c) at 650 °C for 72 h.
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Figure 4. X-ray diffraction patterns of the corrosion products on Al-coated specimens corroded at 650 °C in molten salt of LiCl–3 wt.% Li2O for 72 (a) and 168 h (b), and in molten salt of LiCl–8 wt.% Li2O for 72 (c) and 168 h (d).
Figure 4. X-ray diffraction patterns of the corrosion products on Al-coated specimens corroded at 650 °C in molten salt of LiCl–3 wt.% Li2O for 72 (a) and 168 h (b), and in molten salt of LiCl–8 wt.% Li2O for 72 (c) and 168 h (d).
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Figure 5. Cross-sectional SEM image and EDS elemental map of bare specimens corroded in LiCl–1 wt.% Li2O (a), LiCl–3 wt.% Li2O (b), and LiCl–5 wt.% Li2O (c) molten salt at 650 °C for 72 h.
Figure 5. Cross-sectional SEM image and EDS elemental map of bare specimens corroded in LiCl–1 wt.% Li2O (a), LiCl–3 wt.% Li2O (b), and LiCl–5 wt.% Li2O (c) molten salt at 650 °C for 72 h.
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Figure 6. Cross-sectional SEM image and EDS point analysis results for Al-coated specimen corroded in LiCl–3 wt.% Li2O (a) and LiCl–8 wt.% Li2O (b) molten salt at 650 °C for 72 h.
Figure 6. Cross-sectional SEM image and EDS point analysis results for Al-coated specimen corroded in LiCl–3 wt.% Li2O (a) and LiCl–8 wt.% Li2O (b) molten salt at 650 °C for 72 h.
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Figure 7. Cross-sectional SEM image and EDS elemental map of Al-coated specimen corroded in LiCl–3 wt.%Li2O (a) and LiCl–8 wt.% Li2O (b) molten salt at 650 °C for 168 h.
Figure 7. Cross-sectional SEM image and EDS elemental map of Al-coated specimen corroded in LiCl–3 wt.%Li2O (a) and LiCl–8 wt.% Li2O (b) molten salt at 650 °C for 168 h.
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Kim, W.-B.; Choi, W.-S.; Lim, K.-S.; Cho, S.-H.; Lee, J.-H. High-Temperature Corrosion Behavior of Al-Coated Ni-Base Alloys in Lithium Molten Salt for Electroreduction. Coatings 2021, 11, 328. https://doi.org/10.3390/coatings11030328

AMA Style

Kim W-B, Choi W-S, Lim K-S, Cho S-H, Lee J-H. High-Temperature Corrosion Behavior of Al-Coated Ni-Base Alloys in Lithium Molten Salt for Electroreduction. Coatings. 2021; 11(3):328. https://doi.org/10.3390/coatings11030328

Chicago/Turabian Style

Kim, Wan-Bae, Woo-Seok Choi, Kyu-Seok Lim, Soo-Haeng Cho, and Jong-Hyeon Lee. 2021. "High-Temperature Corrosion Behavior of Al-Coated Ni-Base Alloys in Lithium Molten Salt for Electroreduction" Coatings 11, no. 3: 328. https://doi.org/10.3390/coatings11030328

APA Style

Kim, W.-B., Choi, W.-S., Lim, K.-S., Cho, S.-H., & Lee, J.-H. (2021). High-Temperature Corrosion Behavior of Al-Coated Ni-Base Alloys in Lithium Molten Salt for Electroreduction. Coatings, 11(3), 328. https://doi.org/10.3390/coatings11030328

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