# Size Control of Iron Oxide Nanoparticles Using Reverse Microemulsion Method: Morphology, Reduction, and Catalytic Activity in CO Hydrogenation

Authors: Mohammad Reza Housaindokht; Ali Nakhaei Pour
Journal: Journal of Chemistry
 (2013)

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## Abstract

Iron oxide nanoparticles were prepared by microemulsion method and evaluated in Fischer-Tropsch synthesis. The precipitation process was performed in a single-phase microemulsion operating region. Different HLB values of surfactant were prepared by mixing of sodium dodecyl sulfate (SDS) and Triton X-100. Transmission electron microscopy (TEM), surface area, pore volume, average pore diameter, pore size distribution, and XRD patterns were used to analyze size distribution, shape, and structure of precipitated hematite nanoparticles. Furthermore, temperature programmed reduction (TPR) and catalytic activity in CO hydrogenation were implemented to assess the performance of the samples. It was found that methane and CO2 selectivity and also the syngas conversion increased as the HLB value of surfactant decreased. In addition, the selectivity to heavy hydrocarbons and chain growth probability (α) decreased by decreasing the catalyst crystal size.


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## Body

## 1. Introduction

Nanoscale materials exhibited novel properties including quantum size effect on photochemistry, nonlinear optical properties of semiconductor and new catalytic properties of metallic nanoparticles [1]. Therefore, synthesis of nanoparticles is of a great interest field during the past few years. As compared to their bulk counterparts, nanoparticles often have superior or even new catalytic properties following from their nanometer size [2]. Hence, the size of the nanoparticles is pivotal in determining the catalytic properties and understanding how size may affect the catalytic properties remains a central goal in nanocatalysis research [3].Many methods have been reported for preparation of nanoparticles [2, 3]. Preparation of metallic nanoparticles using microemulsion has been well established [4–7]. Due to the specific structure of the microemulsion system, it was expected as a suitable environment for producing small metal nanoparticles with narrow size distribution. A microemulsion is defined as a system of water, oil, and amphiphile (surfactant) [4–7]. In some respects, microemulsions can be considered as small-scale versions of emulsions, that is, droplet type dispersions either of oil-in-water (o/w) or of water-in-oil (w/o), with a size range in the order of 5−50 nm in drop radius. In the hydrophilic interior of these droplets, a certain amount of water-soluble material can be dissolved, for example, transition metal salts that then serve as precursor(s) for the final metal particles. As for simple aqueous systems, microemulsion formation is dependent on surfactant type and structure. A surfactant substance reduces the surface tension of a liquid in which it is dissolved [4–7]. Hydrophilic-lipophilic balance (HLB) is an important concept which relates the molecular structure to the interfacial packing and film curvature. It is generally expressed as an empirical equation based on the relative proportions of hydrophobic and hydrophilic groups within the molecule. If the structure of the surfactant molecule is designed precisely, the surfactant film may spontaneously adopt a natural radius of curvature of the interface, which has a direction and magnitude without any need for an energy input [4–7].Recent studies revealed structure sensitive properties of many catalytic reactions like CO hydrogenation process in Fischer-Tropsch synthesis (FTS) [8–12]. Murzin reported that FTS reactions on the supported cobalt based catalysts show many sensitivities to the catalyst particle size [13, 14]. Moreover, many new results showed that nanosized iron particles play an essential role to achieve high FTS activity [8–12]. Iron-based catalysts are preferred for utilizing synthesis gas derived from coal or biomass because of the excellent activity for the water-gas-shift reaction, which allows using a synthesis gas with a low H2/CO ratio directly without an upstream shift-step [15, 16]. In our previous works, we tried to show structure sensitivity of unsupported iron catalysts [10, 11, 17].In this the present work, feasibility of iron nanoparticle formation in the microemulsion systems with different HLB values was investigated. Moreover, effects of HLB values on the particle size were investigated. Then, catalyst characterization and catalytic FTS reaction are examined at different particle sizes.


## 2. Experimental

### 2.1. Catalyst Preparation

Fe-Cu nanoparticles were prepared by coprecipitation in a water-in-oil microemulsion [11–15]. The precipitation was performed in the single-phase microemulsion operating region. For this purpose, a water solution of metal precursor, Fe(NO3)3-9H2O (Fluka puriss, p.a. ACS: 98–100%), and Cu(NO3)2-4H2O (Fluka, purum, p.a. > 97%) were added to a mixture of an oil phase (Chloroform, Aldrich, >99%) and mixed surfactants contain Triton X-100 and SDS. The HLB values of Triton X-100 and SDS are 13.4 and 40, respectively. Besides, 1-butanol as a cosurfactant was added to system in order to obtain a proper microemulsion.For preparation of various sizes of hematite nanoparticles, reverse microemulsions were prepared with different HLB values through varying the weight ratio of Triton X-100 and SDS. For a quaternary system of surfactant (S, g), oil (O, g), alcohol (A, g), and water (W, g), the following symbols were defined; α represents the mass fraction of oil in water plus oil, α=O/(W+O), β the mass ratio of surfactant in the whole system, β=S/(W+O+S+A), and ε the mass fraction of alcohol in the whole system, ε=A/(W+O+S+A) [4–7]. In the prepared microemulsion system, the parameters are, α=0.62, β=0.03, and ε=0.28. After stirring well and stabilizing for 24 h, a transparent mixture was obtained. Then, hydrazine was added to reduce metal precursor. The resulting mixture was decanted overnight. The solid was recovered by centrifuging and then washing thoroughly with distilled water and ethanol for several times. Lanthanum promoter was added by wet impregnation method with La(NO3)3 precursor on its optimal value after treatment in air as described previously [10–12, 17]. The promoted catalysts were dried at 383 K for 16 h and calcined at 723 K for 3 h in air. The catalyst compositions were designated in terms of the atomic ratios as 100Fe/5.64Cu/2La.


### 2.2. Catalyst Characterization

Elemental analysis was performed to determine the composition of the elements in the bulk of catalysts. The surface area was calculated from the Brunauer-Emmett-Teller (BET) equation and pore volume, average pore diameter, and pore size distribution of the catalysts were determined by N2 physisorption using a micromeritics ASAP 2010 automated system. A 0.5 g catalyst sample was degassed in the micromeritics ASAP 2010 at 100°C for 1 h and then at 573 K for 2 h prior to analysis. The analysis was done using N2 adsorption at 77 K. Both the pore volume and the average pore diameter were calculated by Barrett-Joyner-Hallender (BJH) method from the adsorption isotherm. Assuming that the Fe2O3 particles are spherical, the corresponding particle size (dBET) can be estimated as [18]
(1)dBET=6ρA,
where ρ is the true density of Fe2O3, that is, 5.24 g/cm3, and A is the specific surface area of samples.The XRD spectrum of the catalysts was collected by an X-ray diffractometer, Philips PW1840 X-ray diffractometer, using monochromatizedCu/Kα radiation (40 kV, 40 mA), and a step scan mode at a scan rate of 0.02° (2θ) per second from 10–80°. XRD peak identification was recognized by comparison to the JCPDS database software. The average crystallite size of samples, dXRD, can be estimated from XRD patterns by applying full-width half-maximum (FWHM) of characteristic peak (104) Fe2O3 located at 2θ=33.3° peak to Scherrer equation:
(2)dXRD=0.9λFWHMcosθ,
where λ is the X-ray wavelength (1.5406 Å in this study) and θ is the diffraction angle for the (104) plane.Temperature programmed reduction (TPR) measurements of the calcined catalysts were recorded by using a Micromeritics TPD-TPR 2900 system. The catalyst samples (50 mg) were purged with argon at 473 for 30 min and cooled to 323 K. The samples were heated from 350 to 1100 K at a rate of 10 K/min under flow of 5.1% hydrogen in argon gas mixture. The consumption of hydrogen was monitored by a thermal conductivity detector (TCD).The morphology of prepared catalysts was observed with a transmission electron microscope (TEM, LEO 912 AB, Germany). An appropriate amount of Fe2O3 suspension directly taken from the reaction solution was dropped onto the carbon-coated copper grids for TEM observation. The average particle size (dTEM) and particle size distribution were determined by TEM images considering more than 100 particles.


### 2.3. Catalytic Performance

The catalysts were tested in a fixed-bed microreactor. A detailed description of the experimental setup and procedures has been provided elsewhere [15, 16]. The catalyst samples (3.0 g catalyst diluted with 12 g quartz, 100–180 μm) were activated by a 5% (v/v) H2/N2 gas mixture with space velocity of 15.1 nl·h-1·gFe-1 at 0.1 MPa by increasing temperature from ambient to 673 K at 5 K/min, then maintained for one hour, and subsequently reduced to 543 K. The pretreatment was followed by the synthesis gas stream with H2/CO = 1 and space velocity of 3.07 nl·h-1·gFe-1 for 24 h in 0.1 Mpa and 543 K. After catalyst pretreatment, synthesis gas was feed to the reactor at 563 K, 17 bar, (H2/CO)feed=1 and a space velocity of 4.9 nl·h-1·gFe-1.The products were analyzed by means of three gas chromatographs, a Shimadzu 4C gas chromatograph equipped with two subsequent connected packed columns: Porapak Q and Molecular Sieve 5A, and a thermal conductivity detector (TCD) with Ar as carrier gas for hydrogen analyzing. A Varian CP 3800 with a chromosorb column and a thermal conductivity detector (TCD) were used for CO, CO2, CH4, and other noncondensable gases. A Varian CP 3800 with a Petrocol DH100 fused silica capillary column and a flame ionization detector (FID) were used for organic liquid products so that a complete product distribution could be provided.


## 2.1. Catalyst Preparation

Fe-Cu nanoparticles were prepared by coprecipitation in a water-in-oil microemulsion [11–15]. The precipitation was performed in the single-phase microemulsion operating region. For this purpose, a water solution of metal precursor, Fe(NO3)3-9H2O (Fluka puriss, p.a. ACS: 98–100%), and Cu(NO3)2-4H2O (Fluka, purum, p.a. > 97%) were added to a mixture of an oil phase (Chloroform, Aldrich, >99%) and mixed surfactants contain Triton X-100 and SDS. The HLB values of Triton X-100 and SDS are 13.4 and 40, respectively. Besides, 1-butanol as a cosurfactant was added to system in order to obtain a proper microemulsion.For preparation of various sizes of hematite nanoparticles, reverse microemulsions were prepared with different HLB values through varying the weight ratio of Triton X-100 and SDS. For a quaternary system of surfactant (S, g), oil (O, g), alcohol (A, g), and water (W, g), the following symbols were defined; α represents the mass fraction of oil in water plus oil, α=O/(W+O), β the mass ratio of surfactant in the whole system, β=S/(W+O+S+A), and ε the mass fraction of alcohol in the whole system, ε=A/(W+O+S+A) [4–7]. In the prepared microemulsion system, the parameters are, α=0.62, β=0.03, and ε=0.28. After stirring well and stabilizing for 24 h, a transparent mixture was obtained. Then, hydrazine was added to reduce metal precursor. The resulting mixture was decanted overnight. The solid was recovered by centrifuging and then washing thoroughly with distilled water and ethanol for several times. Lanthanum promoter was added by wet impregnation method with La(NO3)3 precursor on its optimal value after treatment in air as described previously [10–12, 17]. The promoted catalysts were dried at 383 K for 16 h and calcined at 723 K for 3 h in air. The catalyst compositions were designated in terms of the atomic ratios as 100Fe/5.64Cu/2La.


## 2.2. Catalyst Characterization

Elemental analysis was performed to determine the composition of the elements in the bulk of catalysts. The surface area was calculated from the Brunauer-Emmett-Teller (BET) equation and pore volume, average pore diameter, and pore size distribution of the catalysts were determined by N2 physisorption using a micromeritics ASAP 2010 automated system. A 0.5 g catalyst sample was degassed in the micromeritics ASAP 2010 at 100°C for 1 h and then at 573 K for 2 h prior to analysis. The analysis was done using N2 adsorption at 77 K. Both the pore volume and the average pore diameter were calculated by Barrett-Joyner-Hallender (BJH) method from the adsorption isotherm. Assuming that the Fe2O3 particles are spherical, the corresponding particle size (dBET) can be estimated as [18]
(1)dBET=6ρA,
where ρ is the true density of Fe2O3, that is, 5.24 g/cm3, and A is the specific surface area of samples.The XRD spectrum of the catalysts was collected by an X-ray diffractometer, Philips PW1840 X-ray diffractometer, using monochromatizedCu/Kα radiation (40 kV, 40 mA), and a step scan mode at a scan rate of 0.02° (2θ) per second from 10–80°. XRD peak identification was recognized by comparison to the JCPDS database software. The average crystallite size of samples, dXRD, can be estimated from XRD patterns by applying full-width half-maximum (FWHM) of characteristic peak (104) Fe2O3 located at 2θ=33.3° peak to Scherrer equation:
(2)dXRD=0.9λFWHMcosθ,
where λ is the X-ray wavelength (1.5406 Å in this study) and θ is the diffraction angle for the (104) plane.Temperature programmed reduction (TPR) measurements of the calcined catalysts were recorded by using a Micromeritics TPD-TPR 2900 system. The catalyst samples (50 mg) were purged with argon at 473 for 30 min and cooled to 323 K. The samples were heated from 350 to 1100 K at a rate of 10 K/min under flow of 5.1% hydrogen in argon gas mixture. The consumption of hydrogen was monitored by a thermal conductivity detector (TCD).The morphology of prepared catalysts was observed with a transmission electron microscope (TEM, LEO 912 AB, Germany). An appropriate amount of Fe2O3 suspension directly taken from the reaction solution was dropped onto the carbon-coated copper grids for TEM observation. The average particle size (dTEM) and particle size distribution were determined by TEM images considering more than 100 particles.


## 2.3. Catalytic Performance

The catalysts were tested in a fixed-bed microreactor. A detailed description of the experimental setup and procedures has been provided elsewhere [15, 16]. The catalyst samples (3.0 g catalyst diluted with 12 g quartz, 100–180 μm) were activated by a 5% (v/v) H2/N2 gas mixture with space velocity of 15.1 nl·h-1·gFe-1 at 0.1 MPa by increasing temperature from ambient to 673 K at 5 K/min, then maintained for one hour, and subsequently reduced to 543 K. The pretreatment was followed by the synthesis gas stream with H2/CO = 1 and space velocity of 3.07 nl·h-1·gFe-1 for 24 h in 0.1 Mpa and 543 K. After catalyst pretreatment, synthesis gas was feed to the reactor at 563 K, 17 bar, (H2/CO)feed=1 and a space velocity of 4.9 nl·h-1·gFe-1.The products were analyzed by means of three gas chromatographs, a Shimadzu 4C gas chromatograph equipped with two subsequent connected packed columns: Porapak Q and Molecular Sieve 5A, and a thermal conductivity detector (TCD) with Ar as carrier gas for hydrogen analyzing. A Varian CP 3800 with a chromosorb column and a thermal conductivity detector (TCD) were used for CO, CO2, CH4, and other noncondensable gases. A Varian CP 3800 with a Petrocol DH100 fused silica capillary column and a flame ionization detector (FID) were used for organic liquid products so that a complete product distribution could be provided.


## 3. Results and Discussion

### 3.1. Catalyst Characterization

Nanostructure iron catalysts were characterized by X-ray diffraction (XRD) measurement after calcinations (Figure1). As shown in Figure 1, XRD patterns of samples very close to the ones with cubic hematite structured Fe2O3 crystal in JCPDS database. The characteristic peaks corresponding to (012), (104), (110), (113), (024), (116), (018), (214), and (300) planes are located at 2θ=24.3, 33.3, 35.8, 40.8, 49.6, 54.1, 57.6, 64.1, and 65.6°, respectively. Diffraction data indicates that the presence of lanthanum and copper and also subsequent treatment by dried air do not affect the hematite crystalline phases in different catalyst preparation methods. This shows that the formed hematite structure remains stable during subsequent aqueous impregnation and thermal treatment. It was also shown in Figure 1 that the microemulsion system only modules the physical properties of reaction medium without changing the reaction paths and arrangements of crystal structure. The characteristic peak at 2θ=33.3° which corresponds to the hematite 104 plane was used to calculate the average metal particle size by the Scherrer equation. The calculated values of dXRD of the samples are listed in Table 1.Table 1
Average particle size determined by TEM, BET, and XRD techniques.
HLB
d
BET (nm)
d
XRD (nm)
d
TEM(nm)
13.9
16.8
15.4
14
23.7
20.3
18.8
17
31.2
22.1
20.6
21
40
26.3
24.8
24Figure 1
X-ray diffraction patterns of the prepared catalysts after calcinations ((a) HLB = 13.9, (b) HLB = 23.7, (c) HLB = 31.2, and (d) HLB = 40).Textural properties and pore size distributions of the fresh iron-based catalysts are shown in Table2 and Figures 2 and 3, respectively. N2 adsorption-desorption isotherms of catalysts are presented in Figure 3. As shown in this Figure, the prepared catalysts show type IV of Brunauer’s classification isotherms with H1-type hysteresis loop at the relative pressure of P/P0=0.8–0.95. This hysteresis loop is characterized as hexagonal mesoporous materials with cylindrical channels [19].Table 2
Textural properties of prepared catalysts.
HLB
BET surface area (m2/g)
Average pore size (nm)a
Pore volume  (cm3/g)a
13.9
68.2
16.2
0.14
23.7
56.4
19.6
0.16
31.2
51.8
22.3
0.19
40
43.5
25.9
0.21
aThese values were calculated by BJH method from desorption isotherm.N2 adsorption-desorption hysteresis at 77 K of prepared catalysts after calcinations ((a) HLB = 13.9, (b) HLB = 23.7, (c) HLB = 31.2, and (d) HLB = 40).
(a)
(b)
(c)
(d)Adsorption BJH pore size distribution of prepared catalysts after calcinations ((a) HLB = 13.9, (b) HLB = 23.7, (c) HLB = 31.2, and (d) HLB = 40).
(a)
(b)
(c)
(d)The pore size distributions of the catalysts which were calculated by Barrett-Joyner-Halenda (BJH) method for adsorption step are presented in Figure3 and Table 2. Since all pore size values are fairly close to the dimension of particles, it deduces that the measured pore size is mainly caused by the inter particle voids.The TEM photographs for the prepared samples are demonstrated in Figure4 and Table 1 and also the particle size distribution determined by TEM images are shown in Figure 5. The average particle size (dTEM) and particle size distribution were obtained from TEM images by considering more than 100 particles. As shown in Figures 4 and 5, the average range of particle size and particle size distribution increases as HLB value increases.TEM image of prepared catalysts after calcinations ((a) HLB = 13.9, (b) HLB = 23.7, (c) HLB = 31.2, and (d) HLB = 40).
(a)
(b)
(c)
(d)Relative particle size distribution of prepared catalysts after calcinations ((a) HLB = 13.9, (b) HLB = 23.7, (c) HLB = 31.2, (d) HLB = 40).
(a)
(b)
(c)
(d)The particle size of samples which were determined by XRD, BET, and TEM techniques are summarized in Table1. Particle sizes which were estimated by different techniques provide different physical explanation. The particle size obtained from XRD pattern (dXRD) indicates the average crystallite size of particles. The dBET value is calculated from surface area which is measured by nitrogen adsorption-desorption assuming that the particles are spherical and nonporous. The dXRD and dBET possess the cumulative and comprehensive information on particle size, although they are derived indirectly. However, the dTEM value is a direct evidence of average particle size of Fe2O3 suspension and thus in this work, it has been used for further calculations.As shown in Table1, the particle size is increased and the particle size distribution becomes wider with the increase of HLB value. In fact, nanoparticles are formed in the internal structure of the microemulsion, which is determined by the HLB value of surfactant. The results show that the size of different droplets determines the hematite particle size, depending on the HLB value of surfactant.The effects of the iron particle size on the reduction behavior of the catalysts were measured by H2-TPR. The profiles of H2-TPR are presented in Figure 6. As shown in Figure 6, all catalysts present two main reduction peaks at about 700 and 900 K in the H2-TPR profiles. It has been postulated that the first stage corresponds to the reductions of α-Fe2O3 to magnetite (Fe3O4) and CuO to Cu, whereas the second stage corresponds to the subsequent reduction of Fe3O4 to metallic iron (α-Fe) [15, 16]. It is also found that the first stage can be further separated into two peaks, the first peak corresponds to the reduction of the solid solution of CuO and part of α-Fe2O3 to Cu and Fe3O4, and the second small peak is ascribed to the reduction of the residual α-Fe2O3 to Fe3O4. The presence of Cu in iron catalyst reduces α-Fe2O3 to Fe3O4 at lower temperature rather than Cu-free samples. As CuO reduces, Cu crystallites nucleate and provide H2 dissociation sites, which in turn lead to reactive hydrogen species capable of reducing iron oxides at relatively low temperatures [8, 9].Figure 6
TPR profiles of prepared catalysts after calcinations ((a) HLB = 13.9, (b) HLB = 23.7, (c) HLB = 31.2, and (d) HLB = 40).The TPR profiles in Figure6 clearly show that the first reduction peaks of the catalysts shift to the lower temperature with the decrease of the iron particle size. The probable reason is higher interaction between iron and copper oxides in homogeneous phase of the catalyst prepared via microemulsion system. This suggests that the microemulsion technique promotes the dispersion of Cu promoter, which subsequently enhances the effect of Cu promoter, improves the reduction of the α-Fe2O3, and decreases the reduction temperature for first peak in H2-TPR profile.The amount of the consumed H2 during different reduction stages which is obtained from integrating the area of the corresponding reduction peak is summarized in Table 3. The overall H2 consumption [mol H2/mol M(Fe + Cu)] of the first reduction peaks can be assigned to the reduction of CuO and also the reduction of α-Fe2O3 to Cu and Fe3O4, respectively. In the first stage of reduction, CuO and Fe2O3 reacted with hydrogen based on the following reactions:
(3)3Fe2O3+H2⟶2Fe3O4+H2O(molH2molFe=0.166forcompletereduction),(4)CuO+H2⟶Cu+H2O(molH2molCu=1forcompletereduction).
The peaks at 851 K (mol H2/mol Fe) correspond to the reduction of Fe3O4 to Fe as below:
(5)Fe3O4+4H2⟶3Fe+4H2O(molH2molFe=1.33forcompletereduction).Table 3
Quantitative results of H2 consumption for catalysts in H2-TPRa.
HLB
Peak (K)
H2 consumption
% Reduction
mol H2/mol Mb
mol H2/mol Fe
13.9
533
0.171
93
850
1.24
23.7
558
0.163
87
851
1.16
31.2
608
0.154
84
842
1.12
40
640
0.142
79
852
1.06
aThe H2 consumption was measured from the area under the corresponding peak.
bM = Fe + Cu.The peaks at higher temperature (above 900 K) may be due to the reduction of FeO to Fe and the H2 consumptions which are consistent with theoretical values.As shown in Figure6 and Table 3, smaller crystal size of the catalyst has also influence on the reduction of Fe3O4 to α-Fe as well as first reduction step. The results show that the amount of the catalyst reduction increased with decreasing the catalyst crystal size.


### 3.2. Catalytic Activity

The effect of the catalyst particle size on catalyst activity, product selectivity, and hydrocarbon distribution at the same time-on stream is listed in Table4. It was found that the CO and H2 conversion was increased while the HLB value of surfactant decreased. It is also shown in this table that the methane and CO2 selectivity increased while the catalyst particle size decreased. Moreover, higher hydrocarbon selectivity and chain growth probability (α) decreased when the crystal size decreased.Table 4
Catalysts activity and products selectivity after 35 h time-on-stream.
HLB
X
CO
a
HCb
O/Pc
α
d
CO2 (%)e
Products  selectivity
CH4
C2–C4
C5–C12
C12+
40
67.2
21.3
1.1
0.83
31.3
13.7
41.7
35.0
9.6
31.2
71.5
22.2
1.0
0.8
32.2
14.6
47.6
31.5
6.3
23.7
75.2
22.8
1.0
0.78
33.1
15.6
53.2
27.4
3.8
13.9
77.5
23.5
0.9
0.75
34.5
17.6
57.5
22.8
2.1
Reaction conditions: 563 K, 1.7 Mpa, and H2/CO = 1 and space velocity = 4.9 nl · h−1 · gFe-1.
aCarbon monoxide conversion (mol%).
bHydrocarbon production, gCH2/gFe/s (×105), and CH4 free.
cOlefin to paraffin ratio.
dChain growth probability.
eCO2  selectivity: selectivity to oxygenates was negligible (<2.0%) in all cases.Olefin-to-paraffin ratio in products and olefin and paraffin production rates after 35 h time-on-stream are shown in Figures7 and 8. As listed in Table 4 and shown in Figures 7 and 8, olefin selectivity is decreased by reduction of the HLB value of the surfactant (catalyst particle size decreased). Also as shown in Figures 7 and 8, olefin selectivity decreases with increasing the olefins carbon number.Figure 7
Olefin-to-paraffin ratio in products after 35 h time-on-stream, reaction conditions: 583 K, 17 bar,(H2/CO)feed=1, and space velocity of 4.9 nl·h-1·gFe-1 ((a) HLB = 13.9, (b) HLB = 23.7, (c) HLB = 31.2, and (d) HLB = 40).Olefin and paraffin production rates after 35 h time-on-stream, and reaction conditions: 583 K, 17 bar,(H2/CO)feed=1, space velocity of 4.9 nl·h-1·gFe-1 ((a) HLB = 13.9, (b) HLB = 23.7, (c) HLB = 31.2, and (d) HLB = 40).
(a)
(b)
(c)
(d)The catalytic properties of nanoparticles depend on the size of catalysts active site. Thus, different sizes of nanoparticles have different catalytic activity and selectivity. The dynamic surface restructuring of nanoparticles should also depend on their size; that is, smaller nanoparticles have higher surface energies. For the heterogeneous catalytic reactions, adsorption equilibrium constant of feed increased with decreasing the particle size [13, 14]. By increasing the adsorption equilibrium constant of hydrogen and carbon monoxide on surface of iron catalysts in small particles, the catalyst reduction and FTS reaction increased. Also, higher activity of the iron catalyst with lower particle size (Table 4) may be related to the reduction ability of the catalysts that increased with the particle size (Figure 6 and Table 3).It is postulated that 1-alkenes are primary products of the FTS reaction over iron-based catalyst and may be transformed to paraffin by hydrogenation as a secondary reaction [20, 21]. Secondary reactions occur when primary products desorbed from a site and then interact with another catalytic site before leaving the catalyst particles. Secondary reactions can influence the type and molecular weight of the hydrocarbon products. Hydrogenation of 1-alkenes to paraffin is the most famous secondary reaction in FT synthesis. Thus, the extent of secondary reactions can also be observed from the dependency of the On/Pn ratio or olefin content on chain length. The ratio of olefins to paraffins depends on catalyst type, structure, and the reaction conditions. Slow removal of reactive products (e.g., α-olefins) due to the reduction of diffusion coefficients with increasing chain length can influence the FTS reaction rate and selectivity. The results presented in Table 4 show that the olefin/paraffin ratios are decreased with increasing catalyst particle size.Van der Laan and Beenackers emphasized the solubility impact (vapor-liquid equilibrium) over diffusion as the main contributor on secondary reactions [21]. As shown in Table 4, the secondary reactions are increased (O/P decreased) in the lower iron particle size because of some difficulties of olefin diffusion in nanoparticles with narrow pores. On the other hand, the steric hindrance can limit the competitive adsorption of bigger molecules on smaller crystal sizes. Thus, increasing the adsorption equilibrium constant by decreasing iron particle size is more for hydrogen than that of carbon monoxide [8–12]. Higher hydrogen concentrations on smaller particles enhance the hydrogenation of olefin. The results presented in Figures 7 and 8 and Table 4 show that the olefin/paraffin ratios are decreased with increasing the catalyst particle size of the samples.Anderson-Schultz-Floury (ASF) distribution of FTS products on catalysts is presented in Figure9. Product distribution shows a slight shift to the lower molecular weight hydrocarbons by decreasing the HLB value of the surfactant. The trend lines are plotted to determine the chain growth probability, α. As listed in Table 4, the chain growth probabilities were 0.83, 0.8, 0.78, and 0.75 for 40, 31.2, 23.7, and 13.9 HLB value of surfactant, respectively. This confirms the higher molecular weight hydrocarbons production using higher HLB value of surfactant in preparation of catalyst. As mentioned in the previous section, higher HLB value of surfactant produced higher particle size of catalysts.Figure 9
Overall products distributions on catalysts after 35 h time-on-stream, reaction conditions: 583 K, 17 bar,(H2/CO)feed=1, space velocity of 4.9 nl·h-1·gFe-1 ((a) HLB = 13.9, (b) HLB = 23.7, (c) HLB = 31.2, and (d) HLB = 40).Figure9 and Table 4 also show the effects of the catalyst particle size on the selectivity of Fischer-Tropsch synthesis products. Comparison of the product distributions of the catalysts clearly shows that the product distribution shift to the lower molecular weight hydrocarbons by decreasing the HLB value of the surfactant (or decreasing the catalyst particle size).The most accepted mechanism for FTS reaction is C1 insertion which leads to the carbide theory [21]. These C1 species have various hydrogenation degrees as follows: CO, HCO, HCOH, CH, and CH2. Literature results [19, 20] have discussed that light hydrocarbons are built up by monomers that exhibited higher degree of hydrogenation, that is, CH2. Obviously, heavy hydrocarbons are built up due to monomers except CH2 species with lower degree of hydrogenation. With increasing the hydrogen concentration on the surface of the catalyst, the concentration of C1 monomers with higher degree of hydrogenation are increased. Increasing the concentration of hydrogen on the surface of the catalysts as a result of reduction of the catalyst particle size increases the concentration of C1 monomers and ultimately leads to the higher selectivity to the lower hydrocarbons being enhanced.


## 3.1. Catalyst Characterization

Nanostructure iron catalysts were characterized by X-ray diffraction (XRD) measurement after calcinations (Figure1). As shown in Figure 1, XRD patterns of samples very close to the ones with cubic hematite structured Fe2O3 crystal in JCPDS database. The characteristic peaks corresponding to (012), (104), (110), (113), (024), (116), (018), (214), and (300) planes are located at 2θ=24.3, 33.3, 35.8, 40.8, 49.6, 54.1, 57.6, 64.1, and 65.6°, respectively. Diffraction data indicates that the presence of lanthanum and copper and also subsequent treatment by dried air do not affect the hematite crystalline phases in different catalyst preparation methods. This shows that the formed hematite structure remains stable during subsequent aqueous impregnation and thermal treatment. It was also shown in Figure 1 that the microemulsion system only modules the physical properties of reaction medium without changing the reaction paths and arrangements of crystal structure. The characteristic peak at 2θ=33.3° which corresponds to the hematite 104 plane was used to calculate the average metal particle size by the Scherrer equation. The calculated values of dXRD of the samples are listed in Table 1.Table 1
Average particle size determined by TEM, BET, and XRD techniques.
HLB
d
BET (nm)
d
XRD (nm)
d
TEM(nm)
13.9
16.8
15.4
14
23.7
20.3
18.8
17
31.2
22.1
20.6
21
40
26.3
24.8
24Figure 1
X-ray diffraction patterns of the prepared catalysts after calcinations ((a) HLB = 13.9, (b) HLB = 23.7, (c) HLB = 31.2, and (d) HLB = 40).Textural properties and pore size distributions of the fresh iron-based catalysts are shown in Table2 and Figures 2 and 3, respectively. N2 adsorption-desorption isotherms of catalysts are presented in Figure 3. As shown in this Figure, the prepared catalysts show type IV of Brunauer’s classification isotherms with H1-type hysteresis loop at the relative pressure of P/P0=0.8–0.95. This hysteresis loop is characterized as hexagonal mesoporous materials with cylindrical channels [19].Table 2
Textural properties of prepared catalysts.
HLB
BET surface area (m2/g)
Average pore size (nm)a
Pore volume  (cm3/g)a
13.9
68.2
16.2
0.14
23.7
56.4
19.6
0.16
31.2
51.8
22.3
0.19
40
43.5
25.9
0.21
aThese values were calculated by BJH method from desorption isotherm.N2 adsorption-desorption hysteresis at 77 K of prepared catalysts after calcinations ((a) HLB = 13.9, (b) HLB = 23.7, (c) HLB = 31.2, and (d) HLB = 40).
(a)
(b)
(c)
(d)Adsorption BJH pore size distribution of prepared catalysts after calcinations ((a) HLB = 13.9, (b) HLB = 23.7, (c) HLB = 31.2, and (d) HLB = 40).
(a)
(b)
(c)
(d)The pore size distributions of the catalysts which were calculated by Barrett-Joyner-Halenda (BJH) method for adsorption step are presented in Figure3 and Table 2. Since all pore size values are fairly close to the dimension of particles, it deduces that the measured pore size is mainly caused by the inter particle voids.The TEM photographs for the prepared samples are demonstrated in Figure4 and Table 1 and also the particle size distribution determined by TEM images are shown in Figure 5. The average particle size (dTEM) and particle size distribution were obtained from TEM images by considering more than 100 particles. As shown in Figures 4 and 5, the average range of particle size and particle size distribution increases as HLB value increases.TEM image of prepared catalysts after calcinations ((a) HLB = 13.9, (b) HLB = 23.7, (c) HLB = 31.2, and (d) HLB = 40).
(a)
(b)
(c)
(d)Relative particle size distribution of prepared catalysts after calcinations ((a) HLB = 13.9, (b) HLB = 23.7, (c) HLB = 31.2, (d) HLB = 40).
(a)
(b)
(c)
(d)The particle size of samples which were determined by XRD, BET, and TEM techniques are summarized in Table1. Particle sizes which were estimated by different techniques provide different physical explanation. The particle size obtained from XRD pattern (dXRD) indicates the average crystallite size of particles. The dBET value is calculated from surface area which is measured by nitrogen adsorption-desorption assuming that the particles are spherical and nonporous. The dXRD and dBET possess the cumulative and comprehensive information on particle size, although they are derived indirectly. However, the dTEM value is a direct evidence of average particle size of Fe2O3 suspension and thus in this work, it has been used for further calculations.As shown in Table1, the particle size is increased and the particle size distribution becomes wider with the increase of HLB value. In fact, nanoparticles are formed in the internal structure of the microemulsion, which is determined by the HLB value of surfactant. The results show that the size of different droplets determines the hematite particle size, depending on the HLB value of surfactant.The effects of the iron particle size on the reduction behavior of the catalysts were measured by H2-TPR. The profiles of H2-TPR are presented in Figure 6. As shown in Figure 6, all catalysts present two main reduction peaks at about 700 and 900 K in the H2-TPR profiles. It has been postulated that the first stage corresponds to the reductions of α-Fe2O3 to magnetite (Fe3O4) and CuO to Cu, whereas the second stage corresponds to the subsequent reduction of Fe3O4 to metallic iron (α-Fe) [15, 16]. It is also found that the first stage can be further separated into two peaks, the first peak corresponds to the reduction of the solid solution of CuO and part of α-Fe2O3 to Cu and Fe3O4, and the second small peak is ascribed to the reduction of the residual α-Fe2O3 to Fe3O4. The presence of Cu in iron catalyst reduces α-Fe2O3 to Fe3O4 at lower temperature rather than Cu-free samples. As CuO reduces, Cu crystallites nucleate and provide H2 dissociation sites, which in turn lead to reactive hydrogen species capable of reducing iron oxides at relatively low temperatures [8, 9].Figure 6
TPR profiles of prepared catalysts after calcinations ((a) HLB = 13.9, (b) HLB = 23.7, (c) HLB = 31.2, and (d) HLB = 40).The TPR profiles in Figure6 clearly show that the first reduction peaks of the catalysts shift to the lower temperature with the decrease of the iron particle size. The probable reason is higher interaction between iron and copper oxides in homogeneous phase of the catalyst prepared via microemulsion system. This suggests that the microemulsion technique promotes the dispersion of Cu promoter, which subsequently enhances the effect of Cu promoter, improves the reduction of the α-Fe2O3, and decreases the reduction temperature for first peak in H2-TPR profile.The amount of the consumed H2 during different reduction stages which is obtained from integrating the area of the corresponding reduction peak is summarized in Table 3. The overall H2 consumption [mol H2/mol M(Fe + Cu)] of the first reduction peaks can be assigned to the reduction of CuO and also the reduction of α-Fe2O3 to Cu and Fe3O4, respectively. In the first stage of reduction, CuO and Fe2O3 reacted with hydrogen based on the following reactions:
(3)3Fe2O3+H2⟶2Fe3O4+H2O(molH2molFe=0.166forcompletereduction),(4)CuO+H2⟶Cu+H2O(molH2molCu=1forcompletereduction).
The peaks at 851 K (mol H2/mol Fe) correspond to the reduction of Fe3O4 to Fe as below:
(5)Fe3O4+4H2⟶3Fe+4H2O(molH2molFe=1.33forcompletereduction).Table 3
Quantitative results of H2 consumption for catalysts in H2-TPRa.
HLB
Peak (K)
H2 consumption
% Reduction
mol H2/mol Mb
mol H2/mol Fe
13.9
533
0.171
93
850
1.24
23.7
558
0.163
87
851
1.16
31.2
608
0.154
84
842
1.12
40
640
0.142
79
852
1.06
aThe H2 consumption was measured from the area under the corresponding peak.
bM = Fe + Cu.The peaks at higher temperature (above 900 K) may be due to the reduction of FeO to Fe and the H2 consumptions which are consistent with theoretical values.As shown in Figure6 and Table 3, smaller crystal size of the catalyst has also influence on the reduction of Fe3O4 to α-Fe as well as first reduction step. The results show that the amount of the catalyst reduction increased with decreasing the catalyst crystal size.


## 3.2. Catalytic Activity

The effect of the catalyst particle size on catalyst activity, product selectivity, and hydrocarbon distribution at the same time-on stream is listed in Table4. It was found that the CO and H2 conversion was increased while the HLB value of surfactant decreased. It is also shown in this table that the methane and CO2 selectivity increased while the catalyst particle size decreased. Moreover, higher hydrocarbon selectivity and chain growth probability (α) decreased when the crystal size decreased.Table 4
Catalysts activity and products selectivity after 35 h time-on-stream.
HLB
X
CO
a
HCb
O/Pc
α
d
CO2 (%)e
Products  selectivity
CH4
C2–C4
C5–C12
C12+
40
67.2
21.3
1.1
0.83
31.3
13.7
41.7
35.0
9.6
31.2
71.5
22.2
1.0
0.8
32.2
14.6
47.6
31.5
6.3
23.7
75.2
22.8
1.0
0.78
33.1
15.6
53.2
27.4
3.8
13.9
77.5
23.5
0.9
0.75
34.5
17.6
57.5
22.8
2.1
Reaction conditions: 563 K, 1.7 Mpa, and H2/CO = 1 and space velocity = 4.9 nl · h−1 · gFe-1.
aCarbon monoxide conversion (mol%).
bHydrocarbon production, gCH2/gFe/s (×105), and CH4 free.
cOlefin to paraffin ratio.
dChain growth probability.
eCO2  selectivity: selectivity to oxygenates was negligible (<2.0%) in all cases.Olefin-to-paraffin ratio in products and olefin and paraffin production rates after 35 h time-on-stream are shown in Figures7 and 8. As listed in Table 4 and shown in Figures 7 and 8, olefin selectivity is decreased by reduction of the HLB value of the surfactant (catalyst particle size decreased). Also as shown in Figures 7 and 8, olefin selectivity decreases with increasing the olefins carbon number.Figure 7
Olefin-to-paraffin ratio in products after 35 h time-on-stream, reaction conditions: 583 K, 17 bar,(H2/CO)feed=1, and space velocity of 4.9 nl·h-1·gFe-1 ((a) HLB = 13.9, (b) HLB = 23.7, (c) HLB = 31.2, and (d) HLB = 40).Olefin and paraffin production rates after 35 h time-on-stream, and reaction conditions: 583 K, 17 bar,(H2/CO)feed=1, space velocity of 4.9 nl·h-1·gFe-1 ((a) HLB = 13.9, (b) HLB = 23.7, (c) HLB = 31.2, and (d) HLB = 40).
(a)
(b)
(c)
(d)The catalytic properties of nanoparticles depend on the size of catalysts active site. Thus, different sizes of nanoparticles have different catalytic activity and selectivity. The dynamic surface restructuring of nanoparticles should also depend on their size; that is, smaller nanoparticles have higher surface energies. For the heterogeneous catalytic reactions, adsorption equilibrium constant of feed increased with decreasing the particle size [13, 14]. By increasing the adsorption equilibrium constant of hydrogen and carbon monoxide on surface of iron catalysts in small particles, the catalyst reduction and FTS reaction increased. Also, higher activity of the iron catalyst with lower particle size (Table 4) may be related to the reduction ability of the catalysts that increased with the particle size (Figure 6 and Table 3).It is postulated that 1-alkenes are primary products of the FTS reaction over iron-based catalyst and may be transformed to paraffin by hydrogenation as a secondary reaction [20, 21]. Secondary reactions occur when primary products desorbed from a site and then interact with another catalytic site before leaving the catalyst particles. Secondary reactions can influence the type and molecular weight of the hydrocarbon products. Hydrogenation of 1-alkenes to paraffin is the most famous secondary reaction in FT synthesis. Thus, the extent of secondary reactions can also be observed from the dependency of the On/Pn ratio or olefin content on chain length. The ratio of olefins to paraffins depends on catalyst type, structure, and the reaction conditions. Slow removal of reactive products (e.g., α-olefins) due to the reduction of diffusion coefficients with increasing chain length can influence the FTS reaction rate and selectivity. The results presented in Table 4 show that the olefin/paraffin ratios are decreased with increasing catalyst particle size.Van der Laan and Beenackers emphasized the solubility impact (vapor-liquid equilibrium) over diffusion as the main contributor on secondary reactions [21]. As shown in Table 4, the secondary reactions are increased (O/P decreased) in the lower iron particle size because of some difficulties of olefin diffusion in nanoparticles with narrow pores. On the other hand, the steric hindrance can limit the competitive adsorption of bigger molecules on smaller crystal sizes. Thus, increasing the adsorption equilibrium constant by decreasing iron particle size is more for hydrogen than that of carbon monoxide [8–12]. Higher hydrogen concentrations on smaller particles enhance the hydrogenation of olefin. The results presented in Figures 7 and 8 and Table 4 show that the olefin/paraffin ratios are decreased with increasing the catalyst particle size of the samples.Anderson-Schultz-Floury (ASF) distribution of FTS products on catalysts is presented in Figure9. Product distribution shows a slight shift to the lower molecular weight hydrocarbons by decreasing the HLB value of the surfactant. The trend lines are plotted to determine the chain growth probability, α. As listed in Table 4, the chain growth probabilities were 0.83, 0.8, 0.78, and 0.75 for 40, 31.2, 23.7, and 13.9 HLB value of surfactant, respectively. This confirms the higher molecular weight hydrocarbons production using higher HLB value of surfactant in preparation of catalyst. As mentioned in the previous section, higher HLB value of surfactant produced higher particle size of catalysts.Figure 9
Overall products distributions on catalysts after 35 h time-on-stream, reaction conditions: 583 K, 17 bar,(H2/CO)feed=1, space velocity of 4.9 nl·h-1·gFe-1 ((a) HLB = 13.9, (b) HLB = 23.7, (c) HLB = 31.2, and (d) HLB = 40).Figure9 and Table 4 also show the effects of the catalyst particle size on the selectivity of Fischer-Tropsch synthesis products. Comparison of the product distributions of the catalysts clearly shows that the product distribution shift to the lower molecular weight hydrocarbons by decreasing the HLB value of the surfactant (or decreasing the catalyst particle size).The most accepted mechanism for FTS reaction is C1 insertion which leads to the carbide theory [21]. These C1 species have various hydrogenation degrees as follows: CO, HCO, HCOH, CH, and CH2. Literature results [19, 20] have discussed that light hydrocarbons are built up by monomers that exhibited higher degree of hydrogenation, that is, CH2. Obviously, heavy hydrocarbons are built up due to monomers except CH2 species with lower degree of hydrogenation. With increasing the hydrogen concentration on the surface of the catalyst, the concentration of C1 monomers with higher degree of hydrogenation are increased. Increasing the concentration of hydrogen on the surface of the catalysts as a result of reduction of the catalyst particle size increases the concentration of C1 monomers and ultimately leads to the higher selectivity to the lower hydrocarbons being enhanced.


## 4. Conclusion

Nanosized iron oxide particles have been successfully synthesized by reverse microemulsion with different HLB values. The iron oxide particle size and particle size distribution are increased by decreasing of HLB values. It was found that the CO and H2 conversion is increased as the HLB value of the surfactant is reduced. Also the methane and CO2 selectivity is increased at the same time as the catalyst particle size is decreased. In addition, higher hydrocarbon selectivity and chain growth probability (α) show a descending trend in carbon number when the crystal size decreases.



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*Source: 781595-2013-10-31.xml*