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Kinetics of Iron Removal From Ti-Extraction Blast Furnace Slag by Chlorination Calcination

  • Siqi He , Tongjiang Peng EMAIL logo , Hongjuan Sun , Dongshan Luo , Qing Xiao and Qian Geng
Published/Copyright: December 18, 2019
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Open Chemistry
From the journal Open Chemistry Volume 17 Issue 1

Abstract

In this research, ammonium chloride was used to calcine Ti-extraction blast furnace slag (EBFS) with the aim of removing iron from it. The influences of calcination temperature, ammonium chloride to EBFS mass ratio and particle size on the rates of iron removal were investigated. The results show that the rate of iron removal increased to almost 100% with increases in calcination temperature and the NH4Cl to EBFS mass ratio, but decreased with increases in particle size. Iron is removed in the form of ferric chloride gas, and ammonium chloride can be recycled by recrystallization after decomposition. The bagdasarrym model was used to describe the calcination process at temperatures below 261°C, which was controlled by nonisothermal crystallization. The reaction kinetic equation was obtained and the apparent activation energy of 67.21 kJ/mol. Ferric chloride reaction product existed in the calcined slag in an amorphous solid state. The shrinking core model was used to describe the calcination process at temperatures above 261°C, which was controlled by surface chemical reactions. The reaction kinetic equation was obtained and the apparent activation energy was found to be 42.05 kJ/mol.

Keywords: Ti-extraction blast furnace slag; iron removal; chlorination calcination; kinetics

1 Introduction

In Panzhihua, China, over 60 million tons of Ti-bearing blast furnace slag (TBFS) is produced. It causes severe environmental problems such as groundwater contamination via the leaching of hazardous heavy metals, while particulates are emitted into the surrounding air [1]. At present, high-temperature carbonization-low-temperature chlorination is the main process used to utilise TBFS [2]. This process has a high titanium extraction rate; however, it produces a chlorine-containing waste residue called Ti-extraction blast furnace slag (EBFS), which is difficult to treat and can cause serious environmental pollution.

After chlorine removal, EBFS is mainly used to produce low-value-added products such as cement mortar admixtures [3] and bricks [4, 5]. Based on its complex composition and amorphous phase structure, our research group used EBFS to produce glass-ceramics with good properties [6, 7]. The chloride component escapes from EBFS during a calcination process; however, deleterious impurities can remain, usually in the form of iron compounds, which can discolour glass-ceramic products. This limits the commercial applications of glass-ceramics. Therefore, it is necessary to remove iron from EBFS before using it in glass-ceramics. Iron can be removed by two methods including: 1) a physical separation process that aims to remove iron-containing minerals, and 2) chemical treatment that dissolves iron compounds bonded at the surface or existing as mineral grains [8]. The appropriate method for the removal of iron from an industrial solid waste depends on its mineralogical form and iron distribution.

Based on a mineralogical study of EBFS, this work aims to investigate the iron removal from EBFS by ammonium chloride calcination. The iron component in EBFS reacts with ammonium chloride to form ferric chloride, which escapes from the slag in a gaseous state at a certain temperature. The process conditions, such as calcination temperature, mass ratio of NH4Cl to EBFS and particle size, were assessed. Furthermore, the

chlorination calcination kinetics of iron was studied, which can provide a theoretical guide for future process optimization and industrial applications.

2 Materials And Methods

2.1 Mineralogical analysis of EBFS

Samples of EBFS were collected from Panzhihua Iron and Steel Co. Ltd., Sichuan, China. X-ray Fluorescence (XRF) was used to analyse the chemical components of EBFS, X-ray Diffraction (XRD) was used for mineral phase analysis, X-ray Photoelectron Spectroscopy (XPS) was used for valence analysis of the iron in EBFS, Scanning Electron Microscope-Energy Dispersive Spectroscopy (SEM-EDS) was used to analyse the morphology and iron distribution of EBFS, and Thermogravimetric Analysis-Differential Scanning Calorimetry (TG-DSC) was used for thermal stability analysis.

2.2 Process of calcination with ammonium chloride

Calcination was carried out in a furnace with programmed temperature control. Firstly, a certain amount of ammonium chloride was put into a 10 g EBFS sample and stirred in a 100 mL ceramic crucible, which was then placed in the furnace. The experiments were repeated under various experimental conditions. The process design is represented in Table 1. After being calcined, The calcined product obtained below 260°C was leached in water to obtain the leached product. The leached product and the calcined product obtained above 261°C was characterized by XRF. The % iron removal (R) was calculated according to Equation (1):

Table 1

Design of the experiment.

ParametersLevels
Time (min)0, 5, 10, 15, 20, 25, 30, 35, 40, 50, 60
Temperature (°C)180, 220, 260, 290, 310, 335, 350
Mass ratio of NH4Cl to EBFS1.0, 1.5, 2.0, 2.5
Average particle size (μm)300, 200, 100, 74
(1)R=m2m1×100%

where m1 and m2 are the masses of Fe2O3 in the EBFS and calcined product or leached product, respectively.

Ethical approval: The conducted research is not related to either human or animal use.

3 Results And Discussion

3.1 Characterization of EBFS samples

The loss on ignition (LOI) of EBFS was 12.92%. On the basis of the XRF results, it contained 4.39% Fe2O3 (Table 2). XRD of the EBFS (Figure 1) shows that the main diffraction peaks are d111=2.49 Å, d200=2.16 Å, d220=1.52 Å and d311=1.30 Å, which are characteristic peaks of its titanium carbide (TiC) (reference code: 00-032-1383) [9]. Besides, there are some amorphous substances in EBFS, the chemical bond in amorphous compounds is easier to break and synthesize than that in the crystal of the same substance. So the EBFS sample had high reactivity [10]. XPS was used to characterize the Fe oxidation state (Figure 2). The supported Fe2O3 was characterized by a spin-coupled doublet for curve fitting of Fe2p3/2 and Fe2p1/2 at 712.2 eV and 725.6 eV, respectively [11, 12]. The supported FeO was characterized by a spin-coupled doublet for curve fitting of Fe2p3/2 and Fe2p1/2 at 711 eV and 723.7 eV, respectively, which indicates that both Fe2+ and Fe3+ species were present in the EBFS [13]. Figure 3 shows the SEM-EDS determined distribution of iron in the EBFS samples. The EBFS particles had no specific morphology and could be divided into two types: those with smooth and dense surfaces, and those with rough and loose surfaces. Surface scanning analysis indicates that the distribution of iron was very dispersed. Hence, it would be difficult to remove iron by beneficiation and a chemical method would be better.

Figure 1 XRD pattern of EBFS samples. 1=titanium carbide.
Figure 1

XRD pattern of EBFS samples. 1=titanium carbide.

Figure 2 XPS spectra in the Fe2p region of EBFS.
Figure 2

XPS spectra in the Fe2p region of EBFS.

Figure 3 SEM-EDS images of EBFS.
Figure 3

SEM-EDS images of EBFS.

Table 2

Chemical composition of EBFS samples (%).

CaOSiO2Al2O3TiO2MgOFe2O3ClSO3
32.4527.7213.378.687.62 4.392.960.84
MnOK2ONa2OBaOSrO P2O5ZrO2Y2O3
0.810.670.260.10.06 0.040.030.01

3.2 Effect of experimental conditions on iron removal

3.2.1 Effect of calcination temperature

The mixture of NH4Cl and EBFS was calcined at 180, 220, 260, 290, 310, 335 and 350°C for 1 h, with the mass ratio of NH4Cl to EBFS and the particle size of EBFS held at 1.8:1 and 250 μm, respectively. The results shown in Figure 4 revealed that temperature had a strong influence on the iron removal rate, which was > 60% at temperatures > 335°C. Figure 5 shows the TG-DSC diagram for the mixture of NH4Cl and EBFS, which has four endothermic peaks and two mass-loss regions from 170–350°C. The DSC curve of the mixture shows two small endothermic peaks at 172.1°C and 210.9°C due to the reaction of solid ammonium chloride with iron components in the EBFS. The DSC curve also shows a sharp endothermic peak at 261.1°C due to ammonium chloride being decomposed into ammonia and hydrogen chloride, resulting in a mass loss of 17.2% [14]. The DSC curve shows a small endothermic peak at 310.2°C due to the reaction of gaseous hydrogen chloride with iron components in the EBFS that formed ferric chloride gas, resulting in a mass loss of 5.2%. The reaction temperature is slightly lower than the thermodynamic calculation temperature of the reaction between Fe2O3 and HCl. It may be that other components in EBFS play a catalytic role in the reaction [15]. Therefore, an increase in the removal rate with increases in temperature could be attributed to a change of the state of the calcination additives leading to an increase in the reaction area between EBFS and the calcination additives.

Figure 4 Effect of temperature on iron removal rates with time.
Figure 4

Effect of temperature on iron removal rates with time.

3.2.2 Effect of the NH4Cl to EBFS ratio

The effect of increasing the mass ratio of NH4Cl to EBFS on iron removal is shown in Figure 6, with the calcination temperature and average particle size held at 335°C and 250 μm, respectively. An increase in the NH4Cl to EBFS mass ratio was observed to have some influence on the iron removal rate. At low ratios, the NH4Cl decomposed less hydrogen chloride gas, resulting in a low overall concentration of hydrogen chloride in the reaction system. Meanwhile, an increase in the ratio contributed to an increased concentration of hydrogen chloride gas in the reaction system, thus increasing the reaction rate of calcination additives and iron-containing particles in the EBFS.

Figure 5 TG-DSC analysis of the NH4Cl and EBFS mixture.
Figure 5

TG-DSC analysis of the NH4Cl and EBFS mixture.

Figure 6 Effect of various NH4Cl to EBFS mass ratios on iron removal rate over time.
Figure 6

Effect of various NH4Cl to EBFS mass ratios on iron removal rate over time.

3.2.3 Effect of particle size

The influence of average particle size fractions on the removal rate of iron is shown in Figure 7, with the reaction temperature and mass ratio of NH4Cl to EBFS held at 335°C and 2.0:1. The results indicate that iron removal rates increased with decreases in the EBFS particle size. A decrease in particle size would contribute to an increase in the specific surface area, leading to much-improved heat and mass transfer rates and facilitating faster liberation of the iron component [16].

Figure 7 Effect of various particle sizes on iron removal rate over time.
Figure 7

Effect of various particle sizes on iron removal rate over time.

3.3 Phase analysis of calcined products and condensated products

As seen in the XRD patterns of the calcined product at 220, 260, 335 and 350°C with the mass ratio of NH4Cl to EBFS and the particle size held at 1.8:1 and 250 μm in Figure 8, comparing with XRD of EBFS (Figure 1), the number and the intensity of the diffraction peaks of titanium carbide (TiC) decreased until they disappeared after calcination. The diffraction peaks of ammonium chloride appeared in the calcined products at 220 and 260°C. However, there is no diffraction peaks of ammonium chloride in the calcined products at 335 and 350°C. This is consistent with the

Figure 8 XRD patterns of the calcined product obtained at different temperatures: 1-Ammonium Chloride, 2- Titanium Carbide.
Figure 8

XRD patterns of the calcined product obtained at different temperatures: 1-Ammonium Chloride, 2- Titanium Carbide.

TG-DSC result (Figure 5) that ammonium chloride being decomposed into ammonia and hydrogen chloride when the temperature is higher than 261°C. This phenomenon shows that ammonium chloride will not remain in the calcined product when the calcination temperature is higher than 261°C, which is beneficial to the application of EBFS after iron removal. There are no diffraction peaks of ferric chloride in calcined product. The reason is that ferric chloride is gaseous when the calcination temperature is higher than 310.2°C, and ferric chloride may exist in amorphous state when the temperature is less than 310.2°C.

Gas produced by calcination of EBFS at 335°C, and the products of gas condensation show three distinct color ranges on the wall of quartz tube (Figure 9). The XRD pattern of the condensated products in three color ranges shown in Figure 9A, B, C revealed that white condensated product was calcination additive ammonium

Figure 9 XRD patterns of condensation products of volatile gases calcined at 335 C: 1- Ammonium Chloride (NH4Cl), 2- Ammonium Aqua Iron Chloride((NH4)2FeCl5H2O), 3- Iron Chloride Hydrate (FeCl3·6H2O).
Figure 9

XRD patterns of condensation products of volatile gases calcined at 335 C: 1- Ammonium Chloride (NH4Cl), 2- Ammonium Aqua Iron Chloride((NH4)2FeCl5H2O), 3- Iron Chloride Hydrate (FeCl3·6H2O).

chloride which is formed by hydrogen chloride gas and ammonia gas decomposed from ammonium chloride, yellow condensated product was the mixture of ammonium chloride and ammonium aqua iron chloride, brown condensated product was iron chloride hydrate. This phenomenon shows that iron can be successfully removed by calcination with ammonium chloride. Iron exists in the form of ferric chloride and can be recovered by condensation, the calcination additives ammonium chloride can also be recycled by recrystallization after decomposition.

3.4 Calcination kinetics analysis

3.4.1 Temperatures less than 261°C

Ammonium chloride is solid at calcination temperatures lower than 261°C, so the chlorination reaction is a solid-solid reaction that forms a solid phase. The typical rate-controlling step of solid-solid reaction are the interfacial chemical reaction, diffusion control and nonisothermal crystallization process. The step with the highest kinetic resistance is the rate controlling step [17, 18]. Table 3 shows the integrated rate equations. Experimental data obtained at 180, 220 and 260°C were compared with the three models, with the results shown in Figure 10 [19, 20, 21]. It can be seen that the plots of ln[-ln(1-rFe)] had a very good linear relationship with lnt, with a fitting degree higher than 0.9. This indicates that the calcination rate was controlled by regional nucleation reactions, the most appropriate reaction model is the bagdasarrym model [19]. The reaction rate constant lnk and its model equation at different temperatures are presented in Table 4. According to the kinetic equation, we can know that when n ≈ 1, the number of growth directions of the product nucleus is α = 0. So, it can be judged that the chlorination calcination reaction is completed in one step and the chlorination product is amorphous at temperatures < 261°C [22]. This is consistent with the conclusions of the experiment—that ferric chloride in the calcined product obtained at < 261°C is in an amorphous phase. The relationship between reaction rate and temperature is well established and can be modelled with the Arrhenius equation, as expressed below.

Figure 10 Comparison between plots of (a) (1 − rFe)-2/3 − 1 and (b) 1 − 2rFe/3 − (1 −rFe)2/3 vs time, (c) ln[−ln(1 − rFe)] vs lnt .
Figure 10

Comparison between plots of (a) (1 − rFe)-2/3 − 1 and (b) 1 − 2rFe/3 − (1 −rFe)2/3 vs time, (c) ln[−ln(1 − rFe)] vs lnt .

Table 3

Integrated rate equations for the solid-solid reaction.

Rate-controlling stepRate equation
Interfacial chemical reaction(1-rFe)-2/3-1=kr1t
Diffusion control1-2rFe/3-(1-rFe)2/3=kr2t
Nonisothermal crystallizationln[-ln(1-rFe)]=lnkr3+nlnt
rFe- iron removal degree; t- time (min); kr- apparent rate constant (min-1); n- n=δ+α, δ is the number of steps in series reaction and α is the number of growth directions of product nuclei.
Table 4

Parameters of ln[-ln(1-rFe)] vs lnt obtained at temperatures of 160°C, 200°C and 230°C.

Temperature (°C)Apparent rate constant lnkFitting equation
180-8.40582ln[-ln(1-rFe)]= -8.40582+1.31927lnt
220-7.02595ln[-ln(1-rFe)]= -7.02595+1.37603lnt
260-5.72542ln[-ln(1-rFe)]= -5.72542+1.27014lnt
(2)kr=Ae−Ea/RT
(3)lnkr=−EaRT+lnA

where kr is the rate constant, A is the frequency factor, Ea is the apparent activation energy (J/mol), R is the mole gas constant (R = 8.314 J/mol) and T is the thermodynamic temperature.

The corresponding relationship between lnkr and 1/T is shown in Figure 11. The apparent activation energy of iron removal is estimated to be 67.21 kJ/mol according to the slopes of the straight lines in Figure 11, with A estimated as is 12.23 × 103 according to the intercept. Therefore, the semi-empirical kinetic equation is

Figure 11 Arrhenius plot between lnkr and 1/T for the calculation of activation energy. The values of Kr were calculated by using the bagdasarrym model.
Figure 11

Arrhenius plot between lnkr and 1/T for the calculation of activation energy. The values of Kr were calculated by using the bagdasarrym model.

ln[−ln(1−rFe)]=ln12.23×103e−67210RT+lnt

where rFe is the fraction of Fe removed, R is the molar gas constant (R = 8.314 J/mol), T is the calcination temperature (K), t is the reaction time (min).

Because the ferric chloride calcined product is in an amorphous solid state at calcination temperatures below 261°C, solid ferric chloride cannot escape from the reaction system to achieve the purpose of iron removal. Hence, the dynamics of different NH4Cl:EBFS mass ratios and EBFS particle sizes at calcination temperatures below 261°C are not discussed.

3.4.2 Temperatures above 261°C

Ammonium chloride decomposes into ammonia gas and hydrogen chloride gas at calcination temperatures higher than 261°C. The reaction product, ferric chloride, is a gas at this temperature, so the reaction between hydrogen chloride and the iron component of EBFS is a solid-gas reaction. Because EBFS particles have dense surfaces, which can be considered as non-porous particles, and the iron-containing particles gradually shrink during calcination, so the most appropriate reaction model is the shrinking core model [23, 24, 25]. In the chlorination calcination system, the ferric chloride gas is formed by chlorination of iron-containing minerals. Because the iron-containing minerals are widely distributed and the total iron content in EBFS is relatively low, the release of ferric chloride gas does not have a significant impact on the morphology of the EBFS particles. This results in the calcination process being controlled by diffusion through the EBFS particle layer or chemical reactions at the surfaces of the EBFS particles [17]. Integrated rate equations for the shrinking core model are shown in Table 5 [20].

Table 5

Integrated rate equations for the shrinking core model.

Rate-controlling stepRate equation
Diffusion control through the particle layer1 + 2(1 - rFe) - 3(1 - rFe)2/3 = kr1t
Surface chemical reaction1 - (1 - rFe )1/3 = kr2t
rFe- iron removal degree; t- time (min); kr- apparent rate constant (min-1).

The linear regression analysis of experimental data obtained at temperatures of 290, 310, 335 and 350°C using the equations in Table 5. Figure 12 compares the plots of 1 − 2(1 − rFe)− 3(1 − rFe)2/3 and 1 − (1 − rFe)1/3 versus time at calcination temperatures of 290, 310, 335 and 350°C with a NH4Cl to EBFS mass ratio of 1.8:1 and average particle size of 250 μm. The results show that there are very good linear relationships in the plots of 1 − (1 − rFe)1/3 vs time.

Figure 12 Comparison of plots of (a) 1 + 2(1 − rFe)− 3(1 − rFe)2/3 and (b) 1 − (1 −rFe)1/3 vs time.
Figure 12

Comparison of plots of (a) 1 + 2(1 − rFe)− 3(1 − rFe)2/3 and (b) 1 − (1 −rFe)1/3 vs time.

This indicates that the calcination rate was controlled by chemical reaction. Fitting the experimental data presented in Figures. 6–7 with chemically-controlled model. The fitting results of the model to the experimental data is shown in Figure 13. The reaction rate constant kr and its fitting equation are presented in Table 6.

Figure 13 Plots of 1 − (1 − rFe)1/3 vs time for different parameters: (a) ratio of NH4Cl to EBFS mass and (b) particle size.
Figure 13

Plots of 1 − (1 − rFe)1/3 vs time for different parameters: (a) ratio of NH4Cl to EBFS mass and (b) particle size.

Table 6

Parameters of 1 − (1 − rFe)1/3 vs time for all experimental data.

Apparent rate constant kFitting equation
Temperature (°C.)
2900.007381 - (1 - rFe)1/3 = 0.00738 t
3100.008361 - (1 - rFe)1/3 = 0.00836 t
3350.015511 - (1 - rFe)1/3 = 0.01551 t
3500.015731 - (1 - rFe)1/3 = 0.01573 t
Ratio of NH4Cl to EBFS mass (g/g)
1.00.004451 - (1 - rFe)1/3 = 0.00445 t
1.50.006791 - (1 - rFe)1/3 = 0.00679 t
2.00.008691 - (1 - rFe)1/3 = 0.00869 t
2.50.009711 - (1 - rFe)1/3 = 0.00971 t
Particle size (μm)
3000.008531 - (1 - rFe)1/3 = 0.00853 t
2000.009411 - (1 - rFe)1/3 = 0.00941 t
1000.009661 - (1 - rFe)1/3 = 0.00966 t
740.012331 - (1 - rFe)1/3 = 0.01233 t

The apparent rate constant kr is affected by the calcination temperature, concentration of calcination additives and EBFS particle radius. The empirical formulas can be established as per Eq. (4) [26]. Therefore, the apparent rate constant can be calculated by the relationships between kr and each factor.

(4)kr=kCoMρr0

Where kr is the apparent rate constant, k is the reaction rate constant, C0 is the concentration of hydrogen chloride gas, M is the molecular weight of solid reactant, r0 is the initial radius of solid reactant, and ρ is the density of solid reactant (ρ = 1.8944 g/cm3).

The relationship between kr and calcination temperature obeys the Arrhenius equation as expressed in Reactions (2) and (3), with the results shown in Figure 14a. The apparent activation energy of iron removal is calculated to be 42.05 kJ/mol, the relationship between kr

Figure 14 Relationships between lnkr and 1/T, ln(C0), and lnr0: (a) Arrhenius plot of the calcination process at 290, 310, 335 and 350 °C; (b) relationship between lnk and ln(C0); and (c) relationship between lnk and lnr0.
Figure 14

Relationships between lnkr and 1/T, ln(C0), and lnr0: (a) Arrhenius plot of the calcination process at 290, 310, 335 and 350 °C; (b) relationship between lnk and ln(C0); and (c) relationship between lnk and lnr0.

and T can be expressed as per Equation (5). It is generally believed that high values of activation energy (>40 kJ/ mol) indicate chemical control, whereas values <20 kJ/ mol imply diffusion-controlled processes [18, 19, 20, 21, 22, 23, 24, 25, 26, 27, 28], so the calcination rate was controlled by chemical reaction.

(5)kr=55.65e−42051/RT

Equation (4) shows that the apparent rate constant kr is positively proportional to the concentration of calcination additives. The concentration of hydrogen chloride gas can be calculated by the mass ratio of NH4Cl to EBFS. When κMρr0is regarded as a constant, A1, Equation. (4) can be transformed into:

(6)lnkr=lnC0+lnA1

The plot of lnkr versus lnC0 is shown in Figure 14b. The slope of the fitting line is 0.86725, so the relationship between kr and C0 is:

(7)kr=A1C00.86725

The radius of EBFS can be calculated by its particle size. When κC0Mρis regarded as the constant A2, Eq. (4) can be transformed into:

(8)lnkr=lnA2−lnr0

The plots of lnkr versus lnr0 are presented in Figure 14c. The slope of the fitting line is 0.61079, so the relationship between kr and r0 can be written as:

(9)kr=A2r00.61079

The relationships between the three factors and kr are established in Eqs. (5), (7) and (9). The semi-empirical kinetic equation can be obtained by synthesizing the three relationships.

kr=kC0Mρr0=kC00.86725Mρr00.61079=C00.86725Mρr00.61079A3e−EaRT      =C00.86725Mρr00.61079A3e−42051RT=A′C00.86725Mr00.61079e−42051RT

Where A3 is a frequency factor, and A′=MA3ρ.

The Arrhenius equation obtained from Figure 14a is kr = 55.65e-42051/RT, then A′c00.86725r00.61079= 55.65.

Substituting C0 = 4.68 mol/L and r0 = 100 × 10-6 m gives A’ = 5.26 × 10-2. Therefore, the semi-empirical kinetic equation is

1−(1−rFe)13=5.26×10−2×C00.86725r00.61079×e−42051RT×t

where rFe is the fraction of Fe removed, C0 is the concentration of hydrogen chloride gas, r0 is the initial radius of solid reactant, R is the molar gas constant (R = 8.314 J/mol), T is the calcination temperature (K), t is the reaction time (min).

4 Conclusions

The main minerals of EBFS are titanium carbide (TiC) and some amorphous substances. EBFS contains about 4.39% Fe2O3 and the distribution of the iron component is very dispersed. Besides, both Fe2+ and Fe3+ species were present in the EBFS. Removal of the iron component from EBFS uses ammonium chloride calcination. It was found that the increase of calcination temperature, mass ratio of NH4Cl to EBFS and the decrease of slag particle size are beneficial to iron removal from EBFS. Iron is removed in the form of ferric chloride gas, the separation and recovery of ferric chloride and ammonium chloride which decomposition from reaction system can be carried out by recrystallization. The bagdasarrym model was used to describe the calcination process at temperatures below 261°C. The calculated apparent activation energy was 67.21 kJ/mol and the reaction product was ferric chloride in an amorphous solid state. The kinetic equation is ln[−ln(1−rFe)]=ln12.23×103e−67210RT+lnt. The experimental results at calcination temperature above 261 °C are matched the shrinking core model with surface chemical control, and the apparent activation energy of iron removal in the calcination reaction was estimated to be 42.05 kJ/mol. The relationships between the rate constants and the process parameters were established. The kinetic equation is 1−(1−rFe)13=5.26×10−2×C00.86725r00.61079×e−42051RT×t.

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Received: 2019-06-01
Accepted: 2019-08-29
Published Online: 2019-12-18

© 2019 Siqi He et al., published by De Gruyter

This work is licensed under the Creative Commons Attribution 4.0 Public License.

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https://doi.org/10.1515/chem-2019-0124
Keywords for this article
Ti-extraction blast furnace slag; iron removal; chlorination calcination; kinetics
Creative Commons
BY 4.0

Articles in the same Issue

  1. Regular Articles
  2. Research on correlation of compositions with oestrogenic activity of Cistanche based on LC/Q-TOF-MS/MS technology
  3. Efficacy of Pyrus elaeagnifolia subsp. elaeagnifolia in acetic acid–induced colitis model
  4. Anti-inflammatory and antinociceptive features of Bryonia alba L.: As a possible alternative in treating rheumatism
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  7. Phytic Acid Extracted from Rice Bran as a Growth Promoter for Euglena gracilis
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  9. Topological Indices of Hyaluronic Acid-Paclitaxel Conjugates’ Molecular Structure in Cancer Treatment
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  13. Specific, highly sensitive and simple spectrofluorimetric method for quantification of daclatasvir in HCV human plasma patients and in tablets dosage form
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  27. Phytochemical screening and estrogenic activity of total glycosides of Cistanche deserticola
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  95. Computing Topological Indices for Para-Line Graphs of Anthracene
  96. Zagreb Polynomials and redefined Zagreb indices of Dendrimers and Polyomino Chains
  97. Topological Descriptor of 2-Dimensional Silicon Carbons and Their Applications
  98. Topological invariants for the line graphs of some classes of graphs
  99. Words for maximal Subgroups of Fi24‘
  100. Generators of Maximal Subgroups of Harada-Norton and some Linear Groups
  101. Special Issue on POKOCHA 2018
  102. Influence of Production Parameters on the Content of Polyphenolic Compounds in Extruded Porridge Enriched with Chokeberry Fruit (Aronia melanocarpa (Michx.) Elliott)
  103. Effects of Supercritical Carbon Dioxide Extraction (SC-CO2) on the content of tiliroside in the extracts from Tilia L. flowers
  104. Impact of xanthan gum addition on phenolic acids composition and selected properties of new gluten-free maize-field bean pasta
  105. Impact of storage temperature and time on Moldavian dragonhead oil – spectroscopic and chemometric analysis
  106. The effect of selected substances on the stability of standard solutions in voltammetric analysis of ascorbic acid in fruit juices
  107. Determination of the content of Pb, Cd, Cu, Zn in dairy products from various regions of Poland
  108. Special Issue on IC3PE 2018 Conference
  109. The Photocatalytic Activity of Zns-TiO2 on a Carbon Fiber Prepared by Chemical Bath Deposition
  110. N-octyl chitosan derivatives as amphiphilic carrier agents for herbicide formulations
  111. Kinetics and Mechanistic Study of Hydrolysis of Adenosine Monophosphate Disodium Salt (AMPNa2) in Acidic and Alkaline Media
  112. Antimalarial Activity of Andrographis Paniculata Ness‘s N-hexane Extract and Its Major Compounds
  113. Special Issue on ABB2018 Conference
  114. Special Issue on ICCESEN 2017
  115. Theoretical Diagnostics of Second and Third-order Hyperpolarizabilities of Several Acid Derivatives
  116. Determination of Gamma Rays Efficiency Against Rhizoctonia solani in Potatoes
  117. Studies On Compatibilization Of Recycled Polyethylene/Thermoplastic Starch Blends By Using Different Compatibilizer
  118. Liquid−Liquid Extraction of Linalool from Methyl Eugenol with 1-Ethyl-3-methylimidazolium Hydrogen Sulfate [EMIM][HSO4] Ionic Liquid
  119. Synthesis of Graphene Oxide Through Ultrasonic Assisted Electrochemical Exfoliation
  120. Special Issue on ISCMP 2018
  121. Synthesis and antiproliferative evaluation of some 1,4-naphthoquinone derivatives against human cervical cancer cells
  122. The influence of the grafted aryl groups on the solvation properties of the graphyne and graphdiyne - a MD study
  123. Electrochemical modification of platinum and glassy carbon surfaces with pyridine layers and their use as complexing agents for copper (II) ions
  124. Effect of Electrospinning Process on Total Antioxidant Activity of Electrospun Nanofibers Containing Grape Seed Extract
  125. Effect Of Thermal Treatment Of Trepel At Temperature Range 800-1200˚C
  126. Topical Issue on Agriculture
  127. The effect of Cladophora glomerata exudates on the amino acid composition of Cladophora fracta and Rhizoclonium sp.
  128. Influence of the Static Magnetic Field and Algal Extract on the Germination of Soybean Seeds
  129. The use of UV-induced fluorescence for the assessment of homogeneity of granular mixtures
  130. The use of microorganisms as bio-fertilizers in the cultivation of white lupine
  131. Lyophilized apples on flax oil and ethyl esters of flax oil - stability and antioxidant evaluation
  132. Production of phosphorus biofertilizer based on the renewable materials in large laboratory scale
  133. Human health risk assessment of potential toxic elements in paddy soil and rice (Oryza sativa) from Ugbawka fields, Enugu, Nigeria
  134. Recovery of phosphates(V) from wastewaters of different chemical composition
  135. Special Issue on the 4th Green Chemistry 2018
  136. Dead zone for hydrogenation of propylene reaction carried out on commercial catalyst pellets
  137. Improved thermally stable oligoetherols from 6-aminouracil, ethylene carbonate and boric acid
  138. The role of a chemical loop in removal of hazardous contaminants from coke oven wastewater during its treatment
  139. Combating paraben pollution in surface waters with a variety of photocatalyzed systems: Looking for the most efficient technology
  140. Special Issue on Chemistry Today for Tomorrow 2019
  141. Applying Discriminant and Cluster Analyses to Separate Allergenic from Non-allergenic Proteins
  142. Chemometric Expertise Of Clinical Monitoring Data Of Prolactinoma Patients
  143. Chemomertic Risk Assessment of Soil Pollution
  144. New composite sorbent for speciation analysis of soluble chromium in textiles
  145. Photocatalytic activity of NiFe2O4 and Zn0.5Ni0.5Fe2O4 modified by Eu(III) and Tb(III) for decomposition of Malachite Green
  146. Photophysical and antibacterial activity of light-activated quaternary eosin Y
  147. Spectral properties and biological activity of La(III) and Nd(III) Monensinates
  148. Special Issue on Monitoring, Risk Assessment and Sustainable Management for the Exposure to Environmental Toxins
  149. Soil organic carbon mineralization in relation to microbial dynamics in subtropical red soils dominated by differently sized aggregates
  150. A potential reusable fluorescent aptasensor based on magnetic nanoparticles for ochratoxin A analysis
  151. Special Issue on 13th JCC 2018
  152. Fluorescence study of 5-nitroisatin Schiff base immobilized on SBA-15 for sensing Fe3+
  153. Thermal and Morphology Properties of Cellulose Nanofiber from TEMPO-oxidized Lower part of Empty Fruit Bunches (LEFB)
  154. Encapsulation of Vitamin C in Sesame Liposomes: Computational and Experimental Studies
  155. A comparative study of the utilization of synthetic foaming agent and aluminum powder as pore-forming agents in lightweight geopolymer synthesis
  156. Synthesis of high surface area mesoporous silica SBA-15 by adjusting hydrothermal treatment time and the amount of polyvinyl alcohol
  157. Review of large-pore mesostructured cellular foam (MCF) silica and its applications
  158. Ion Exchange of Benzoate in Ni-Al-Benzoate Layered Double Hydroxide by Amoxicillin
  159. Synthesis And Characterization Of CoMo/Mordenite Catalyst For Hydrotreatment Of Lignin Compound Models
  160. Production of Biodiesel from Nyamplung (Calophyllum inophyllum L.) using Microwave with CaO Catalyst from Eggshell Waste: Optimization of Transesterification Process Parameters
  161. The Study of the Optical Properties of C60 Fullerene in Different Organic Solvents
  162. Composite Material Consisting of HKUST-1 and Indonesian Activated Natural Zeolite and its Application in CO2 Capture
  163. Topical Issue on Environmental Chemistry
  164. Ionic liquids modified cobalt/ZSM-5 as a highly efficient catalyst for enhancing the selectivity towards KA oil in the aerobic oxidation of cyclohexane
  165. Application of Thermal Resistant Gemini Surfactants in Highly Thixotropic Water-in-oil Drilling Fluid System
  166. Screening Study on Rheological Behavior and Phase Transition Point of Polymer-containing Fluids produced under the Oil Freezing Point Temperature
  167. The Chemical Softening Effect and Mechanism of Low Rank Coal Soaked in Alkaline Solution
  168. The Influence Of NO/O2 On The NOx Storage Properties Over A Pt-Ba-Ce/γ-Al2O3 Catalyst
  169. Special Issue on the International conference CosCI 2018
  170. Design of SiO2/TiO2 that Synergistically Increases The Hydrophobicity of Methyltrimethoxysilane Coated Glass
  171. Antidiabetes and Antioxidant agents from Clausena excavata root as medicinal plant of Myanmar
  172. Development of a Gold Immunochromatographic Assay Method Using Candida Biofilm Antigen as a Bioreceptor for Candidiasis in Rats
  173. Special Issue on Applied Biochemistry and Biotechnology 2019
  174. Adsorption of copper ions on Magnolia officinalis residues after solid-phase fermentation with Phanerochaete chrysosporium
  175. Erratum
  176. Erratum to: Sand Dune Characterization For Preparing Metallurgical Grade Silicon
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