Synthesis of Tribological WS 2 Powder from WO 3 Prepared by Ultrasonic Spray Pyrolysis ( USP )

This paper describes the synthesis of tungsten disulfide (WS2) powder by the sulfurization of tungsten trioxide (WO3) particles in the presence of additive potassium carbonate (K2CO3) in nitrogen (N2) atmosphere, first at lower temperature (200 ◦C) and followed by reduction at higher temperature (900 ◦C). In addition, the ultrasonic spray pyrolysis of ammonium meta-tungstate hydrate (AMT) was used for the production of WO3 particles at 650 ◦C in air. The HSC Chemistry® software package 9.0 was used for the analysis of chemistry and thermodynamic parameters of the processes for WS2 powder synthesis. The crystalline structure and phase composition of all synthesized powders were analyzed by X-ray diffraction (XRD) measurements. The morphology and chemical composition of these samples were examined by scanning electron microscopy (SEM) combined with energy dispersive X-ray analysis (EDX).


Introduction
According to current studies, nearly one-quarter of the world's total energy consumption originates from tribological contacts [1].By improving the performance of current tribological materials, energy losses due to friction and wear could potentially be reduced by 40% in the long term (15 years) and by 18% in the short term (8 years) [1].Hence, in the face of increasing global requirements for saving energy, there is no doubt that the search for efficient tribological materials with improved performances will continue in the coming years because the application conditions of future tribomechanical systems will undoubtedly be much more demanding than the current ones [2].Today's market of tribological materials has unique requirements for the release of harmful substances (Cd, Pb, Cr, etc.) and the prevention of their migration into the environment during their use [3].It is generally considered that these elements and their compounds, which can be introduced into food or water, are difficult to eliminate from the body and according to current studies can have carcinogenic effects [4].For all of the above reasons, despite their excellent performances, tribological materials must also be acceptable from economic and ecological points of view.Among the various tribological materials, WS 2 has attracted a large amount of attention from researchers for its specific properties and extensive promising applications [5].Even in small quantities, WS 2 contributes to the high performance of tribological Metals 2019, 9, 277 2 of 15 materials and their specific properties (chemical stability in a wide temperature range, the possibility of revitalizing the surface that they protect, they are corrosion-resistant, inert, non-toxic, non-magnetic, and have lamellar structure, low shear strength, high oxidation and thermal degradation resistance, and so forth), which are of particular importance for the functioning of modern tribomechanical systems.WS 2 is applicable in various types of industries, such as automotive, aerospace, military, medical, and so forth.
WS 2 crystals have a hexagonal structure composed of a layer of tungsten atoms packed in between two layers of sulfur atoms, as shown in Figure 1a.The bonding between W-S layers is very strong and covalent, but layers of S atoms are loosely bound through weak van der Waals forces.This structure is responsible for the interlayer mechanical weakness with low shear strength, which results in a macroscopic lubricating effect.Figure 1b shows the lubrication mechanism of WS 2 single sheets.So far, various methods of producing WS 2 of different size and morphology using WO 3 as precursor have been established, such as: gas-solid phase reaction [6][7][8], chemical vapor deposition (CVD) [9][10][11], hydrothermal method [12][13][14], mechanochemical activation method [15], and solid-solid phase reaction [16][17][18].
Gas-solid reactions present a very simple approach to generating WS 2 .In most cases, WO 3 is reacted with a sulfur-containing compound for extended periods of time at high temperatures.For example, WS 2 has been synthesized in a tubular furnace through gas phase reactions between WO 3 particles and H 2 /H 2 S gases at a temperature of 840 • C for 30 min in Ar gas flow [6], by sulfidation of hexagonal WO 3 with H 2 S/H 2 (15% H 2 S) at different temperatures: 400, 500, and 800 • C for 4 h [7], and by sulfurization of WO 3 nanostructured thin film in a mixture of H 2 S and Ar gas (10:90) at different partial pressure values [8].However, this method involves exposure to extremely toxic and harmful H 2 S at elevated temperatures.WS 2 flakes have been synthesized successfully on SiO 2 /Si substrate by the sulfurization of WO 3 powder at high temperatures by the CVD method [9][10][11].Furthermore, there was no poisonous H 2 S gas released during these experiments and WS 2 of a high purity was obtained.Although this method has many advantages, it is very demanding to coordinate the complicated relations among many process parameters.
Using the hydrothermal method [12][13][14], WS 2 has been synthesized by autoclaving a mixture of WO 3 and sulfur precursor, followed by washing and drying of the resulting product.Although various inexpensive precursors can be used for this method, the productivity of this process is low and additional thermal treatment is necessary because the obtained WS 2 has an amorphous structure.
Wu Z. et al. [15] have synthesized WS 2 nanosheets by novel mechanochemical activation methods in which a ball-milled mixture of WO 3 and S powder was annealed at 600 • C for 2 h in an atmosphere of Ar gas.This method seems to be environmentally advantageous and may be an alternative to the traditional route of synthesis, but it is a very complex process and a robust method for the production of particles with small dimension.Another difficulty arises from the fact that there is still a lack of clear interpretation of the exact reaction and activation mechanism.
Regarding solid-solid phase reaction, the synthesis of WS 2 powder was carried out by sulfurization of the WO 3 powder with thiourea in a N 2 atmosphere at 850 • C for 1 h in a horizontal tube furnace [16][17][18].
In this investigation the sulfurization of the WO 3 particles with S powder in the presence of additive K 2 CO 3 in a nitrogen atmosphere was studied.In order to obtain an adequate precursor for synthesis, this research involved the production of WO 3 particles using an ultrasonic spray pyrolysis method.It is a simple and low-cost method, which in continuous operation can generate spherical, non-agglomerated submicron particles by using commercially available (inexpensive) precursors [19].The as-prepared WO 3 particles were used for WS 2 synthesis without any post processing because they were free of impurities.

Materials and Methods
The raw materials used for the experimental test performed in this work were: WO 3 obtained by ultrasonic spray pyrolysis (USP), commercial WO 3 (Chemapol, Prague, Czech Republic), sulfur (Solvay & CPC Barium Strontium GmbH & Co, Hannover, Germany, powder with characteristic size <45 µm, purity 99.95%), and K 2 CO 3 (Zorka, Šabac, Serbia).Commercially available WS 2 powder (SpeedUP INTERNATIONAL, Belgrade, Serbia, with a minimum 99.4% WS 2 and WO 3 ) was used for comparative analysis.The production of precursor, WO 3 powder, as well as the synthesis of WS 2 powders were carried out in a rotary tilting tube furnace (ST-1200RGV).
The HSC Chemistry ® software package 9.0 was used for the analysis of the chemistry and thermodynamic parameters of the processes for the synthesis of WS 2 powder [20].The determination of appropriate conditions for WS 2 synthesis was crucial for this analysis.Therefore, the Gibbs free energy of theoretically suspected chemical reactions during the WS 2 synthesis process, the phase stability diagram for the W-O-S system, and the equilibrium composition of the species in the WO 3 -S-K 2 CO 3 system were calculated using HSC Chemistry software.
All obtained powders, as well as the commercial WS 2 powder, were subjected to analysis on a scanning electron microscope (SEM) equipped with energy dispersive X-ray analysis (EDX), a MIRA FE-SEM, from TESCAN Inc.In SEM images of the WO 3 powder, well-dispersed powder without any agglomerates was clearly seen and the determination of particle size distribution for the WO 3 powder was done using the Image Pro Plus Software.However, the particle size of the WS 2 powder was not identifiable using image analysis due to the poor dispersion of samples.Size measurements of the obtained WS 2 powders were thus performed using a laser particle size analyzer (Malvern Instruments, Malvern, UK).In addition, all samples were subjected to X-ray diffraction analyses using a Philips PW 1710, X-Pert Pro diffractometer (Co Kα radiation, generated at 40 kV and 30 mA).Measurements were carried out at an angle interval 10 • < 2θ < 119 • with step 0.017 • .XRD results were analyzed by employing the Rietveld method with the help of PowderCell Software and the RIFRANE ® programme.

Synthesis of WO 3 Powder
The apparatus for WO 3 synthesis consisted of an aerosol generator ("Profi Sonic", Prizma, Kragujevac), a horizontal reactor with a quartz glass tube (0.5 m diameter and 1.2 m length), a vacuum pump (VP125), and powder collectors (Figure 2).Firstly, the ammonium meta-tungstate hydrate (AMT-H26N6O41W12•aq) diluted in distilled water was put into the particle nebulizer to generate an aerosol.The concentration of AMT solution was 10 mmol/L.For this ultrasonic nebulizer system, the resonance frequency was set to 1.7 MHz.A vacuum pump and air with a flow rate of 5 L/min was used to introduce the generated aerosol droplets into the tubular reactor.Prior to the introduction, the temperature of the reactor was raised to 650 °C.The pressure of the system was adjusted using the reactor pressure controller.The calculated retention time of droplets in the reaction zone was estimated to be about one second.After thermal decomposition of the transported aerosol in the furnace, the formed WO3 was partially collected in the bottles with water and alcohol.During the spray pyrolysis process, the evaporation of water from aerosol droplets increases the concentration of AMT in the droplets.Finally, AMT is thermally decomposed according to Equation (1): 2 H26N6O41W12→24 WO3 + 12 NH3↑+ 8 H2O↑+ O2↑. ( As shown in Figure 3, the mechanism of WO3 particle formation proposed by Arutanti et al. [21] is comprised of different steps starting from an initial solution of AMT.

Synthesis of WS2 Powder
A schematic illustration of the WS2 synthesis process is shown in Figure 4. Firstly, the ammonium meta-tungstate hydrate (AMT-H 26 N 6 O 41 W 12 •aq) diluted in distilled water was put into the particle nebulizer to generate an aerosol.The concentration of AMT solution was 10 mmol/L.For this ultrasonic nebulizer system, the resonance frequency was set to 1.7 MHz.A vacuum pump and air with a flow rate of 5 L/min was used to introduce the generated aerosol droplets into the tubular reactor.Prior to the introduction, the temperature of the reactor was raised to 650 • C. The pressure of the system was adjusted using the reactor pressure controller.The calculated retention time of droplets in the reaction zone was estimated to be about one second.After thermal decomposition of the transported aerosol in the furnace, the formed WO 3 was partially collected in the bottles with water and alcohol.During the spray pyrolysis process, the evaporation of water from aerosol droplets increases the concentration of AMT in the droplets.Finally, AMT is thermally decomposed according to Equation (1): As shown in Figure 3, the mechanism of WO Firstly, the ammonium meta-tungstate hydrate (AMT-H26N6O41W12•aq) diluted in distilled water was put into the particle nebulizer to generate an aerosol.The concentration of AMT solution was 10 mmol/L.For this ultrasonic nebulizer system, the resonance frequency was set to 1.7 MHz.A vacuum pump and air with a flow rate of 5 L/min was used to introduce the generated aerosol droplets into the tubular reactor.Prior to the introduction, the temperature of the reactor was raised to 650 °C.The pressure of the system was adjusted using the reactor pressure controller.The calculated retention time of droplets in the reaction zone was estimated to be about one second.After thermal decomposition of the transported aerosol in the furnace, the formed WO3 was partially collected in the bottles with water and alcohol.During the spray pyrolysis process, the evaporation of water from aerosol droplets increases the concentration of AMT in the droplets.Finally, AMT is thermally decomposed according to Equation (1): 2 H26N6O41W12→24 WO3 + 12 NH3↑+ 8 H2O↑+ O2↑. ( As shown in Figure 3, the mechanism of WO3 particle formation proposed by Arutanti et al. [21] is comprised of different steps starting from an initial solution of AMT.

Synthesis of WS2 Powder
A schematic illustration of the WS2 synthesis process is shown in Figure 4.

Synthesis of WS 2 Powder
A schematic illustration of the WS 2 synthesis process is shown in Figure 4.  K2CO3 powder (5wt.%) was added to the WO3 and S powder mixture with a weight ratio of 60:40.The powders were mixed and ground for 15 min in the mixer.Then, the as-prepared mixture was transferred to a covered ceramic boat.The boat was placed in the center of the quartz tube and into the furnace.High-purity nitrogen gas was introduced through one side of the furnace, whilst the other side of the quartz tube was connected to a cooling system and outlet gas washing system.The total flow rate of the N2 gas was fixed at 200 cm 3 •min −1 for all experimental conditions.Prior to heating the furnace, nitrogen gas was flushed constantly for about 30 minutes to remove residual air in the furnace.First, the furnace with the sample was heated at a lower temperature (200 °C) at a rate of 10 °C/min and maintained under these conditions for 2 h.Then, it was further heated at a rate of 5 °C/min followed by reduction at a higher temperature (900 °C).After 2 h, the furnace was turned off and allowed to cool down to room temperature.Nitrogen gas flow was stopped and the WS2 powder was collected from the boat.

Thermodynamic Analysis
Results of the thermodynamic analysis of the process of WS2 powder synthesis are discussed below.Using the assumption of raw materials for the composition of the synthesis process, the following chemical reactions (Equations ( 2)-( 4)) were considered: Figure 5 shows the calculated results of the Gibbs energy of reactions versus temperature from the reaction of Equations ( 2)-( 4).The temperature range that was considered was up to 1000 °C.K 2 CO 3 powder (5 wt.%) was added to the WO 3 and S powder mixture with a weight ratio of 60:40.The powders were mixed and ground for 15 min in the mixer.Then, the as-prepared mixture was transferred to a covered ceramic boat.The boat was placed in the center of the quartz tube and into the furnace.High-purity nitrogen gas was introduced through one side of the furnace, whilst the other side of the quartz tube was connected to a cooling system and outlet gas washing system.The total flow rate of the N 2 gas was fixed at 200 cm 3 •min −1 for all experimental conditions.Prior to heating the furnace, nitrogen gas was flushed constantly for about 30 minutes to remove residual air in the furnace.First, the furnace with the sample was heated at a lower temperature (200 • C) at a rate of 10 • C/min and maintained under these conditions for 2 h.Then, it was further heated at a rate of 5 • C/min followed by reduction at a higher temperature (900 • C).After 2 h, the furnace was turned off and allowed to cool down to room temperature.Nitrogen gas flow was stopped and the WS 2 powder was collected from the boat.

Thermodynamic Analysis
Results of the thermodynamic analysis of the process of WS 2 powder synthesis are discussed below.Using the assumption of raw materials for the composition of the synthesis process, the following chemical reactions (Equations ( 2)-( 4)) were considered: Figure 5 shows the calculated results of the Gibbs energy of reactions versus temperature from the reaction of Equations ( 2)-( 4).The temperature range that was considered was up to 1000 • C. As shown in Figure 5, it can be clearly seen that the ΔG of all reactions has a negative value at temperatures higher than 300 °C, which means that all of the reactions are theoretically possible from the thermodynamic point of view.However, among them, the changes of the Gibbs energy of reaction presented with Equation ( 2) has a more negative value relative to Equation (3) and Equation (4) (i.e., Equation ( 2) is dominant).
The equilibrium composition of the WO3-K2CO3-S system at different temperatures was calculated using the HSC computer program based on the Gibbs energy minimization method, and the results are shown in Figure 6.The highest stability of WS2 was achieved at approximately 800 °C when the stability of the reactants were decreasing.K2O•WO3 and WO2 phases also became stable at the same temperature.The main gaseous products of this reaction were gaseous SO2 and CO2.
In the analyzed system, the main products of the reactions at a temperature of 900 °C were WS2, K2O•WO3, WO2, CO2, and SO2.These results were only qualitative.
By using thermodynamic software, a phase stability diagram for the W-O-S system for constant partial pressure of oxygen was constructed (Figure 7).As shown in Figure 5, it can be clearly seen that the ∆G of all reactions has a negative value at temperatures higher than 300 • C, which means that all of the reactions are theoretically possible from the thermodynamic point of view.However, among them, the changes of the Gibbs energy of reaction presented with Equation (2) has a more negative value relative to Equations ( 3) and (4) (i.e., Equation ( 2) is dominant).
The equilibrium composition of the WO 3 -K 2 CO 3 -S system at different temperatures was calculated using the HSC computer program based on the Gibbs energy minimization method, and the results are shown in Figure 6.As shown in Figure 5, it can be clearly seen that the ΔG of all reactions has a negative value at temperatures higher than 300 °C, which means that all of the reactions are theoretically possible from the thermodynamic point of view.However, among them, the changes of the Gibbs energy of reaction presented with Equation (2) has a more negative value relative to Equation (3) and Equation (4) (i.e., Equation ( 2) is dominant).
The equilibrium composition of the WO3-K2CO3-S system at different temperatures was calculated using the HSC computer program based on the Gibbs energy minimization method, and the results are shown in Figure 6.The highest stability of WS2 was achieved at approximately 800 °C when the stability of the reactants were decreasing.K2O•WO3 and WO2 phases also became stable at the same temperature.The main gaseous products of this reaction were gaseous SO2 and CO2.
In the analyzed system, the main products of the reactions at a temperature of 900 °C were WS2, K2O•WO3, WO2, CO2, and SO2.These results were only qualitative.
By using thermodynamic software, a phase stability diagram for the W-O-S system for constant partial pressure of oxygen was constructed (Figure 7).The highest stability of WS 2 was achieved at approximately 800 • C when the stability of the reactants were decreasing.K 2 O•WO 3 and WO 2 phases also became stable at the same temperature.The main gaseous products of this reaction were gaseous SO 2 and CO 2 .
In the analyzed system, the main products of the reactions at a temperature of 900 • C were WS 2 , K 2 O•WO 3 , WO 2 , CO 2 , and SO 2 .These results were only qualitative.
By using thermodynamic software, a phase stability diagram for the W-O-S system for constant partial pressure of oxygen was constructed (Figure 7).Considering the logarithmic sulfur vapor pressure of 1 atm [22] and experimental temperature of 900 °C, it was found that the predominant stability area was of WS2.At these temperatures, the vapor pressure of sulfur is such that it led to the saturation of the atmosphere with the sulfur vapor in the furnace.This meant that the amount of sulfur gas phase necessary to react with the WO3 was sufficient to establish contact between the mentioned phases.Further, the diffusion of sulfur into WO3 was enabled to form WS2 powder.
The synthesis of WS2 was performed in two stages: i) initiation of synthesis at a low temperature (200 °C) followed by ii) high-temperature (900 °C) reduction.The temperature of the first stage was selected to prolong the contact time of sulfur and WO3 in the starting powder mixture, before sulfur self-ignition (232 °C) which promotes the transformation of sulfur to a gas phase and the evaporation of a large amount of S and/or SO2.This loss of sulfur obstructs its diffusion into WO3 and consequently obstructs the synthesis of WS2.Thermodynamic analysis of the second stage indicated that the optimal temperature of the synthesis was above 800 °C.However, at lower temperatures oxides were formed and the chemical composition of the mixture was changed, and a lower level of crystallization occurred.
For that reason, the second stage of synthesis was carried out at 900 °C to prevent oxide formation and to increase the degree of crystallinity in the final WS2 product.

Characterization of Synthesized WO3 Powder
Figure 8a,b shows the SEM images of the synthesized WO3 powder by USP method under different magnifications.The result of EDX analyses from the presented scanning surface is given in Figure 8c, which reveals that the sample consisted of the elements tungsten and oxygen, and no other elements were observed.Considering the logarithmic sulfur vapor pressure of 1 atm [22] and experimental temperature of 900 • C, it was found that the predominant stability area was of WS 2 .At these temperatures, the vapor pressure of sulfur is such that it led to the saturation of the atmosphere with the sulfur vapor in the furnace.This meant that the amount of sulfur gas phase necessary to react with the WO 3 was sufficient to establish contact between the mentioned phases.Further, the diffusion of sulfur into WO 3 was enabled to form WS 2 powder.
The synthesis of WS 2 was performed in two stages: (i) initiation of synthesis at a low temperature (200 • C) followed by (ii) high-temperature (900 • C) reduction.The temperature of the first stage was selected to prolong the contact time of sulfur and WO 3 in the starting powder mixture, before sulfur self-ignition (232 • C) which promotes the transformation of sulfur to a gas phase and the evaporation of a large amount of S and/or SO 2 .This loss of sulfur obstructs its diffusion into WO 3 and consequently obstructs the synthesis of WS 2 .Thermodynamic analysis of the second stage indicated that the optimal temperature of the synthesis was above 800 • C.However, at lower temperatures oxides were formed and the chemical composition of the mixture was changed, and a lower level of crystallization occurred.
For that reason, the second stage of synthesis was carried out at 900 • C to prevent oxide formation and to increase the degree of crystallinity in the final WS 2 product.

Characterization of Synthesized WO 3 Powder
Figure 8a,b shows the SEM images of the synthesized WO 3 powder by USP method under different magnifications.The result of EDX analyses from the presented scanning surface is given in Figure 8c, which reveals that the sample consisted of the elements tungsten and oxygen, and no other elements were observed.Considering the logarithmic sulfur vapor pressure of 1 atm [22] and experimental temperature of 900 °C, it was found that the predominant stability area was of WS2.At these temperatures, the vapor pressure of sulfur is such that it led to the saturation of the atmosphere with the sulfur vapor in the furnace.This meant that the amount of sulfur gas phase necessary to react with the WO3 was sufficient to establish contact between the mentioned phases.Further, the diffusion of sulfur into WO3 was enabled to form WS2 powder.
The synthesis of WS2 was performed in two stages: i) initiation of synthesis at a low temperature (200 °C) followed by ii) high-temperature (900 °C) reduction.The temperature of the first stage was selected to prolong the contact time of sulfur and WO3 in the starting powder mixture, before sulfur self-ignition (232 °C) which promotes the transformation of sulfur to a gas phase and the evaporation of a large amount of S and/or SO2.This loss of sulfur obstructs its diffusion into WO3 and consequently obstructs the synthesis of WS2.Thermodynamic analysis of the second stage indicated that the optimal temperature of the synthesis was above 800 °C.However, at lower temperatures oxides were formed and the chemical composition of the mixture was changed, and a lower level of crystallization occurred.
For that reason, the second stage of synthesis was carried out at 900 °C to prevent oxide formation and to increase the degree of crystallinity in the final WS2 product.The XRD pattern of the prepared WO 3 particles is shown in Figure 9.It is evident from the pattern that no diffraction peaks from other elements of compounds were found in the samples.Therefore, it is obvious that the as-prepared samples were composed of WO 3 .The XRD pattern suggested that the prepared particles had two types of crystal structures: hexagonal and monoclinic.The XRD pattern of the prepared WO3 particles is shown in Figure 9.It is evident from the pattern that no diffraction peaks from other elements of compounds were found in the samples.Therefore, it is obvious that the as-prepared samples were composed of WO3.The XRD pattern suggested that the prepared particles had two types of crystal structures: hexagonal and monoclinic.The particle size distribution determination for the WO3 powder prepared by USP is presented in Figure 10.The particle size distribution determination for the WO 3 powder prepared by USP is presented in Figure 10.The XRD pattern of the prepared WO3 particles is shown in Figure 9.It is evident from the pattern that no diffraction peaks from other elements of compounds were found in the samples.Therefore, it is obvious that the as-prepared samples were composed of WO3.The XRD pattern suggested that the prepared particles had two types of crystal structures: hexagonal and monoclinic.The particle size distribution determination for the WO3 powder prepared by USP is presented in Figure 10.

Characterization of WS 2 Powder
Figure 11a demonstrates an SEM image of powder obtained using the WO 3 precursor powder prepared by the USP method.The sample was composed of a large number of ultrathin WS 2 flakes.Furthermore, WO 2 , WO 3 , and K 2 O•WO 3 phases with larger dimensions of particles were noticeable.The structure of the ultrathin flakes from the marked locations is presented more clearly in Figure 11b.The results demonstrate the presence of flower-shaped WS 2 particles composed of nanoflakes of 200-500 nm in length and 50 nm in mean thickness.A further EDX analysis of the sample presented in Figure 11c reveals that the product was composed of W, S, O, and K, which suggests that the powder was composed of mainly WS 2 (Spectrum 1) and WO 2 , WO 3 , and K 2 O•WO 3 (Spectrum 2) phases, in accordance with the results presented in Figure 6.

Characterization of WS2 Powder
Figure 11a demonstrates an SEM image of powder obtained using the WO3 precursor powder prepared by the USP method.The sample was composed of a large number of ultrathin WS2 flakes.Furthermore, WO2, WO3, and K2O•WO3 phases with larger dimensions of particles were noticeable.The structure of the ultrathin flakes from the marked locations is presented more clearly in Figure 11b.The results demonstrate the presence of flower-shaped WS2 particles composed of nanoflakes of 200-500 nm in length and 50 nm in mean thickness.A further EDX analysis of the sample presented in Figure 11c reveals that the product was composed of W, S, O, and K, which suggests that the powder was composed of mainly WS2 (Spectrum 1) and WO2, WO3, and K2O•WO3 (Spectrum 2) phases, in accordance with the results presented in Figure 6.The results of the XRD analysis employing the Rietveld method are shown in Figure 12.These results revealed that WS2 phase was predominant (present in two crystalized forms: hexagonal and rhombohedral) and was accompanied by the presence of WO2 (9.80%), WO3 (3.04%), and K2O•WO3 (1.56%) phases.The results of the XRD analysis employing the Rietveld method are shown in Figure 12.These results revealed that WS 2 phase was predominant (present in two crystalized forms: hexagonal and rhombohedral) and was accompanied by the presence of WO 2 (9.80%),WO 3 (3.04%),and K 2 O•WO 3 (1.56%)phases.
The obtained WS 2 particles were tested for their size and size distribution and the mean particle size was found to be around 950 nm (Figure 13).
WS 2 powder synthesized using WO 3 prepared by USP as precursor was selected as a lubrication additive in SF SAE 15W-40 motor oil.WS 2 powder was ultrasonically dispersed into the base oil for 10 min.In addition, a base oil without any additive was also prepared.Wear tests were conducted using a ball-on-disc configuration on a Bruker UMT-3 tribometer (Bruker, Billerica, MA, USA).This test method involves a ball-shaped upper specimen that slides against a rotating disk as a lower specimen under a prescribed set of conditions.Both the ball and the steel disc were cleaned with acetone and dried with a normal stream of air before the test.A normal load of 50 N and a linear sliding speed of 0.1 m/s were used for the experiments, for a sliding distance of 500 m.The results of base oil with additive showed that the average value of the friction coefficient was µ ~0.1.It was concluded that the friction coefficient of the base oil (µ ~0.16) was improved by adding WS 2 .The mass ratio of WS 2 /base oil in samples was 1.0 wt.%.
The generated WS 2 powder had plate-like particles, which were oriented differently when the starting material was commercial WO 3 powder (Figure 14a).It can also be clearly seen from Figure 14b that WS 2 particles were clustered together and exhibited evident agglomeration of up to 1 µm in size.The thickness of the WS 2 plate-like particles was approximately 100 nm and their lengths varied from 500 nm to 1 µm.Results of EDX analyses from marked locations showed the presence of W and S elements and a certain content of O and K elements which indicated the presence of WS 2 (Spectrum 2) and WO 2 , WO 3 , and K 2 O•WO 3 (Spectrum 1) phases (Figure 14c).The obtained WS2 particles were tested for their size and size distribution and the mean particle size was found to be around 950 nm (Figure 13).The obtained WS2 particles were tested for their size and size distribution and the mean particle size was found to be around 950 nm (Figure 13).starting material was commercial WO3 powder (Figure 14a).It can also be clearly seen from Figure 14b that WS2 particles were clustered together and exhibited evident agglomeration of up to 1 µm in size.The thickness of the WS2 plate-like particles was approximately 100 nm and their lengths varied from 500 nm to 1 µm.Results of EDX analyses from marked locations showed the presence of W and S elements and a certain content of O and K elements which indicated the presence of WS2 (Spectrum 2) and WO2, WO3, and K2O•WO3 (Spectrum 1) phases (Figure 14c).The sample of WS2 powder synthesized using commercial WO3 as precursor was analyzed by XRD (Figure 15).Results showed the predominance of the WS2 phase, present in two crystalized forms: hexagonal and rhombohedral.WO3, WO2, K2O•WO3, and S phases were also identified, of which WO3 was hexagonal and monoclinic.The strong and sharp diffraction peaks in the pattern indicated that the product was very highly crystallized.The sample of WS 2 powder synthesized using commercial WO 3 as precursor was analyzed by XRD (Figure 15).Results showed the predominance of the WS 2 phase, present in two crystalized forms: hexagonal and rhombohedral.WO 3 , WO 2 , K 2 O•WO 3 , and S phases were also identified, of which WO 3 was hexagonal and monoclinic.The strong and sharp diffraction peaks in the pattern indicated that the product was very highly crystallized.The obtained WS2 particles were tested for their size and size distribution and the mean particle size was found to be around 500 nm (Figure 16).The obtained WS 2 particles were tested for their size and size distribution and the mean particle size was found to be around 500 nm (Figure 16).The obtained WS2 particles were tested for their size and size distribution and the mean particle size was found to be around 500 nm (Figure 16).Commercial WS 2 powder as evidenced by SEM images consisted of nanoparticles with the presence of large agglomerates (Figure 17a).The uniform shape of particles can be seen in Figure 17b.On the basis of the EDX analysis as well as the high content of W and S, the presence of O was also confirmed (Figure 17c).Commercial WS2 powder as evidenced by SEM images consisted of nanoparticles with the presence of large agglomerates (Figures 17a).The uniform shape of particles can be seen in Figure 17b.On the basis of the EDX analysis as well as the high content of W and S, the presence of O was also confirmed (Figure 17c).The XRD analysis of the commercial WS2 powder indicated that there were major WS2 and WO3 phases and a minor WO3•0.33H2Ophase, with low levels of crystallinity (Figure 18c).The presence of the amorphous phase was dominant, although the crystalline phase was also present.The XRD analysis of the commercial WS 2 powder indicated that there were major WS 2 and WO 3 phases and a minor WO 3 •0.33H 2 O phase, with low levels of crystallinity (Figure 18c).The presence of the amorphous phase was dominant, although the crystalline phase was also present.The XRD analysis of the commercial WS2 powder indicated that there were major WS2 and WO3 phases and a minor WO3•0.33H2Ophase, with low levels of crystallinity (Figure 18c).The presence of the Comparative analysis of the obtained powders with commercial WS2 powder showed differences in particle size and agglomerates.The commercial WS2 powder had the smallest particle size, but had more agglomerates compared to synthesized powders.Agglomerated powders are not good for tribological properties [23].
Particles of the synthesized WS2 powders ranged from submicrometers to micrometers in size.The mixture of these two powders should provide better friction and wear performance between contacting surfaces, according to N. Wu et al [24].Comparative analysis of the obtained powders with commercial WS 2 powder showed differences in particle size and agglomerates.The commercial WS 2 powder had the smallest particle size, but had more agglomerates compared to synthesized powders.Agglomerated powders are not good for tribological properties [23].
Particles of the synthesized WS 2 powders ranged from submicrometers to micrometers in size.The mixture of these two powders should provide better friction and wear performance between contacting surfaces, according to N. Wu et al [24].
Apart from the presence of sulfide as the main product, commercial WS 2 powders had a WO 3 (8.70%)phase, whereas synthesized WS 2 powders had K 2 O•WO 3 (1.52-1.56%),WO 2 (9.80-10.34%),and WO 3 (2.04-3.04%)phases.In order to obtain WS 2 powders that will provide low and stable friction coefficients, the presence of WO 3 should be avoided [25].In synthesized powders, the WO 3 phase was less abundant relative to the levels found in commercial WS 2 powders.Both tungsten dioxides and tungsten disulfides exhibited similar lubrication performances [26].The materials with low oxygen content were more resistant to wear [27].In this respect, WO 2 in synthesized WS 2 powders led to a lower friction coefficient.In addition, the K 2 O•WO 3 phase in synthesized powders improved the thermal stability of obtained WS 2 powders [28].

Conclusions
In response to the requirements for improving performances of currently available tribological materials, this work demonstrated the synthesis of WS 2 powder using ultrafine WO 3 powder prepared by USP method.In addition, we synthesized WS 2 powder using commercial WO 3 powder as precursor.
The synthesis of WS 2 powder with the addition of K 2 CO 3 as a fluxing agent reduced the WO 3 precursor and protected the sample against oxidation, which is one of the advantages of the applied method.
Further, the results of the XRD analysis of synthesized powders were in accordance with thermodynamic predictions.In the synthesized WS 2 powders, K 2 O•WO 3 and WO 2 phases were present in addition to the WS 2 phase.These phases are useful from the aspect of thermal stability and friction coefficient control of the powders.
As a result of this investigation, two sizes of WS 2 particles ranging from submicrometers to micrometers were obtained.Hence, future efforts are planned to investigate mixed micro/submicron lubrication systems composed of the synthesized WS 2 powders.
In summary, tribological WS 2 powder was successfully prepared by a and environmentfriendly method.

Figure 1 .
Figure 1.(a) Hexagonal structure of WS 2 (top view); (b) The relative sliding between two single layers of WS 2 (slide view).

Figure 2 .
Figure 2. Schematic illustration of experimental setup for the ultrasonic spray pyrolysis (USP) synthesis of WO3.

Figure 3 .
Figure 3.The mechanism of the formation of WO3 particles in the spray pyrolysis method.

Figure 2 .
Figure 2. Schematic illustration of experimental setup for the ultrasonic spray pyrolysis (USP) synthesis of WO 3 .

15 Figure 2 .
Figure 2. Schematic illustration of experimental setup for the ultrasonic spray pyrolysis (USP) synthesis of WO3.

Figure 3 .
Figure 3.The mechanism of the formation of WO3 particles in the spray pyrolysis method.

Figure 3 .
Figure 3.The mechanism of the formation of WO 3 particles in the spray pyrolysis method.

Figure 4 .
Figure 4. Schematic illustration of the experimental setup for the synthesis of WS2 powder.

Figure 4 .
Figure 4. Schematic illustration of the experimental setup for the synthesis of WS 2 powder.

Figure 5 .
Figure 5.The change in Gibbs free energy (ΔG) versus temperature for the different possible reactions that take place during the WS2 synthesis.

Figure 5 .
Figure 5.The change in Gibbs free energy (∆G) versus temperature for the different possible reactions that take place during the WS 2 synthesis.

Metals 2019, 9 , x 6 of 15 Figure 5 .
Figure 5.The change in Gibbs free energy (ΔG) versus temperature for the different possible reactions that take place during the WS2 synthesis.

Figure 7 .
Figure 7. Temperature-partial pressures (Tpp) phase stability diagram for the W-O-S system at constant oxygen partial pressure.

Figure 7 .
Figure 7. Temperature-partial pressures (Tpp) phase stability diagram for the W-O-S system at constant oxygen partial pressure.

Metals 2019, 9 , x 7 of 15 Figure 7 .
Figure 7. Temperature-partial pressures (Tpp) phase stability diagram for the W-O-S system at constant oxygen partial pressure.

FigureFigure 8 .
Figure8a,b shows the SEM images of the synthesized WO3 powder by USP method under different magnifications.The result of EDX analyses from the presented scanning surface is given in Figure8c, which reveals that the sample consisted of the elements tungsten and oxygen, and no other elements were observed.

Figure 8 .
Figure 8. (a,b) SEM images and (c) EDX spectrum of WO3 powder synthesized by USP.

Figure 9 .
Figure 9. XRD pattern of WO3 powder prepared by USP method.

Figure 9 .
Figure 9. XRD pattern of WO 3 powder prepared by USP method.

Figure 9 .
Figure 9. XRD pattern of WO3 powder prepared by USP method.

Figure 10 .
Figure 10.Particle size distribution for WO 3 powder prepared by USP method.

Figure 11 .
Figure 11.(a,b) SEM images and (c) EDX spectrum for WS2 synthesized using WO3 prepared by USP as precursor.

Figure 11 .
Figure 11.(a,b) SEM images and (c) EDX spectrum for WS 2 synthesized using WO 3 prepared by USP as precursor.

Figure 12 .
Figure 12.XRD pattern of WS2 synthesized using WO3 prepared by USP as precursor.

Figure 13 .
Figure 13.Particle size distribution by intensity of WS2 particles synthesized using WO3 prepared by USP as precursor.

Figure 13 .
Figure 13.Particle size distribution by intensity of WS2 particles synthesized using WO3 prepared by USP as precursor.

Figure 13 .
Figure 13.Particle size distribution by intensity of WS 2 particles synthesized using WO 3 prepared by USP as precursor.

Figure 14 .
Figure 14.(a,b) SEM images and (c) EDX spectrum for WS2 synthesized using commercial WO3 as precursor.

Figure 14 .
Figure 14.(a,b) SEM images and (c) EDX spectrum for WS 2 synthesized using commercial WO 3 as precursor.

Figure 15 .
Figure 15.XRD pattern of WS 2 synthesized using commercial WO 3 as precursor.

Figure 16 .
Figure 16.Particle size distribution by intensity of WS2 particles synthesized using commercial WO3 powder as precursor.

Figure 16 .
Figure 16.Particle size distribution by intensity of WS 2 particles synthesized using commercial WO 3 powder as precursor.