Structural features of La0.55Ca0.45A0.50Co0.50O3 (A = Mg, Mn) nanoparticles over photo-degradation of methyl blue
Hamid Yousefi
1
(School of Physics, Damghan University (DU), Damghan, Islamic Republic of Iran)
Ahmad Gholizadeh
2
(School of Physics, Damghan University (DU), Damghan, Islamic Republic of Iran)
Zahra MirbeigSabzevari
3
(School of Chemistry, Damghan University (DU), Damghan, Islamic Republic of Iran)
Azim Malekzadeh
4
(School of Chemistry, Damghan University (DU), Damghan, , Islamic Republic of Iran)
Keywords:
Abstract :
Structural features of La0.55Ca0.45A0.50Co0.50O3 (A = Mg, Mn) nanoparticles over photo-degradation of methyl blue
Abstract:
La0.55Ca0.45A0.5Co0.5O3(A = Mg, Mn) nanoparticles prepared by citrate method were characterized using X-ray diffraction measurement, transmission electron microscopy, Fourier transform infrared and UV-Vis spectroscopy. The structural analysis using X’Pert package and Fullprof program is an evidence for the presence of the perovskite structure. The calculated value of crystallite size, particle size and band gap energy of La0.55Ca0.45Mg0.5Co0.5O3 is much less than La0.55Ca0.45Mg0.5Co0.5O3. The photocatalytic activity of the product was studied for degradation of an aqueous solution of methyl blue under solar condition. The effects of three operational parameters including irradiation time, pH, and the catalyst amount on the dye degradation were analyzed using optical absorption spectra. The degradation efficiency of MB solutions in the presence of 10 mg La0.55Ca0.45Mn0.5Co0.5O3 nanoparticles under visible light indicate to be higher than La0.55Ca0.45Mg0.5Co0.5O3 nanoparticles. 96 % degradation is obtained in an aqueous solution at pH = 2.33 and containing 30 mg La0.55Ca0.45Mg0.5Co0.5O3 catalyst after 30 minutes.
Keywords: Nanoparticles; Cobaltite Perovskite; Structural Properties; UV-Visible; Photo-Degradation.
1. Introduction
Different types of dyes are used in many industries such as textile, leather, paper and plastics in order to colorize their products and also consuming substantial volumes of water. A certain amount of them are lost in the process of their manufacturing and utilization and often cause environmental problems. Nowadays, regulation on the discharge of dye-polluted colored wastewater has been getting stringent in many countries [1-4]. The presence of even very small amounts of dyes in water, less than 1 ppm for some dyes, is highly visible and undesirable. It is estimated that more than 100,000 commercially available dyes with over 7×105 tons of dyestuff are produced annually [5-8].
The removal of color from textile dye baths is one of the most challenging problems in the field of environmental chemistry. Different techniques were applied such as adsorption, oxidation, reduction, electrochemical, and membrane filtration [9]. Several methods like physical, chemical and biological methods have been investigated for the removal of dye materials from contaminated water. Among the proposed methods, removal of dyes by adsorption technologies is regarded as one of the most competitive methods because of its high efficiency, economic feasibility and simplicity of design/operation. Moreover, adsorption of dyes on inorganic supports like silica is important in order to produce pigments [10-12].
The photocatalytic process gives degraded products which are in desorption from the interface region makes the water less toxic [13]. The higher the mobility of the photo-generated carriers (including holes and electrons), the better the performance of the photo-catalyst is. Additionally, the valence band position of a semiconductor and the incident photon energy also play an important roles in deciding the photocatalytic activity of the semiconductor. Oxidative activity and the photocatalytic property of the material are higher when the valence band of a semiconductor is deeper [14]. These materials, for their activation demand higher photon energy, which could be near-UV or in UV range [15-18]. However, since UV occupies just 4% of whole solar energy, the technology becomes difficult to widen the application. Therefore, it is indispensable and urgent to develop a sunlight sensitive photocatalyst for wastewater treatment. Develop a sunlight sensitive photocatalyst either need an appropriately band-gap engineered material or the material to possess satisfactory characteristics which are brought out by its defect nature [14].
In this work, we prepared La0.55Ca0.45(Mg or Mn)0.5Co0.5O3 by citrate precursor method. First, geometric parameters of the samples including crystallite size and particle size are studied using X-ray diffraction (XRD) measurement and transmission electron microscopy (TEM). Then, attempt was made to explain their structural properties and the influence of substituting Mg and Mn on the photocatalytic activity of La0.55Ca0.45(Mg or Mn)0.5Co0.5O3 in removal of dyes by chemical oxidation method. The chemical structure of Methyl Blue (MB, C37H27N3Na2S3O9, triphenyl methane) as a kind of dye that has been used widely is shown in Fig. 1 [19]. The samples have been used as photocatalyst under ambient sunlight for decolorisation of Methyl blue.
2. Experimental Section
The samples of La0.55Ca0.45A0.5Co0.5O3 (A = Mg, Mn) were prepared according to the literature by the citrate method using metal nitrate precursor in the presence of citric acid [20-21]. Solutions of appropriate mole numbers of metal nitrates and citric acid (equal to the total number of nitrate ions moles) in 15 mL distilled water were evaporated at 80°C and 150°C overnight. The samples were completely powdered after each drying. Resulting materials were powdered and calcined at 900°C for 5 h.
The XRD pattern has been recorded using a Bruker AXS diffractometer D8 ADVANCE (Bruker-AXS, Karlsruhe, Germany) with CuKα radiation in the range of 2θ=10-80° at room temperature (RT). The crystallite size of the samples is calculated by using Scherrer’s equation as follows [22]:
(1)
Here, βhkl is the full-width at half-maximum of the diffraction peak at around 47o. In this method, increase of peak broadening is due to decrease of crystallite size. The particle size of C60M50 sample was investigated by the TEM (LEO Model 912AB, GmbH, Oberkochen, Germany) analysis. Size distribution histogram is fitted by using a log-normal function as follow [23]:
(2)
Where σd is the standard deviation of the diameter and DTEM is the mean diameter obtained from the TEM results.
The FT-IR spectra of samples were recorded with a PERKIN-ELMER FT-IR spectrometer (Perkin-Elmer Spectrum RXI FT-IR System) in the wave number range of 300-4000 cm-1. Optical absorption spectra of the samples have been recorded between 200 and 1000 nm wavelengths with a HP-UV-Vis system (Analytic Jena AG, Jena, Germany) to study optical and photocatalytic characteristics of the samples. Band gap energies of the samples have been calculated using optical absorption spectra recorded between 200 and 1100 nm wavelengths same as the literature [24]. The following relation holds between the optical absorption coefficient, α (λ), and the optical band gap energy of a direct band transition, 
. Here, B is an energy-independent constant and 
is optical absorption coefficient calculated from the absorption spectra (A(λ)) and also the mean particle size of the sample (t). Band gap energy of the samples is estimated by extrapolating the linear part of 
vs. 
plot. Then, the photocatalytic activity of nanoparticles for degradation of methyl blue aqueous solution are investigated using absorption spectra at wavelengths range of 300-700 nm. Before lighting, the suspension is sufficiently stirred for 30 min to reach adsorption-desorption equilibrium between the catalysts and methyl blue so that the adsorption in the dark can be discounted. The effect of value of the absorbant, contact time, and pH are studied to obtain optimal conditions.
3. Results and Discussions
3.1. Structural Characterization
X-ray diffraction patterns of La0.55Ca0.45A0.5Co0.5O3 (A = Mg, Mn) are shown in Fig. 2. XRD data were analyzed using both the commercial X’Pert High Score package and Fullprof program. Identification of structure type using X’pert package confirms the existence of the main phase with perovskite structure without presence of impurity phases in the samples. Rietveld analysis of the samples by using Fullprof program indicates all the diffraction peaks of La0.55Ca0.45Mn0.5Co0.5O3 be quite well indexed in rhombohedra structure with the space group R-3c. However, it shows presence of two-phase orthorhombic system including Pnma II and final Pnma I phases for La0.55Ca0.45Mg0.5Co0.5O3. The best fit with the least difference is carried out as shown in Fig. 2. The crystallite size and the lattice parameters of the samples are given in Table 1. The crystallite size of La0.55Ca0.45Mn0.5Co0.5O3 is much less than La0.55Ca0.45Mg0.5Co0.5O3.
TEM micrograph and particle size distribution of La0.55Ca0.45A0.5Co0.5O3 (A = Mg, Mn) are shown in Fig 3. Fitting of the size distribution histogram by using a log-normal function indicate that the mean diameter calculated for La0.55Ca0.45Mn0.5Co0.5O3 and La0.55Ca0.45Mg0.5Co0.5O3 nanoparticles are 46 nm and 84 nm, respectively. The result is different from the crystallite size calculated by XRD measurement. The difference is related to the irregular shape of nanoparticles with spherical, spheroidal and polygon morphologies which are observed in the TEM micrographs.
2.2. Optical Characterization
Variation of (αhυ)2 with photon energy hυ for the nanoparticles is shown in Fig. 4. One can observe that the plots are linear over a wide range of photon energy suggesting direct transitions. The direct band gap energies of the nanoparticles 1.91 eV and 2.85 eV were calculated using Tauc equation, from the intersections of the straight line with the energy axis [24]. The values of the band gap energy show metallic behaviour for La0.55Ca0.45Mn0.5Co0.5O3, but, semiconductor for La0.55Ca0.45Mg0.5Co0.5O3.
2. 3. Photocata1tic degradation of MB
For all the experiments mentioned here, the MB dye concentration was kept constant to 25mg per 1 liter of water. This was used as stalk solution, out of which 20 ml solution was used for all individual experiments. In this aliquot, 10 mg (500 mg/l) of catalyst was added and the solution was subjected to ambient sunlight.
The absorption spectra of the samples were recorded by measuring the absorbance at 607 nm corresponding to the maximum absorption wavelength of MB with UV–visible absorption spectroscopy. The photocatalytic degradation rate (DC) was calculated by the following formula [25-26]:
(3)
Where Ao is the initial absorbance of MB solution without any exposure, At is the absorbance of MB after photo irradiation for time (t).
The photocatalytic reaction rate depends on the concentration of the organic pollutants and can be described by the following kinetic model [27]:
(4)
Where C is the concentration of MB (mg/L) at any time, t is the irradiation time, k is the first-order rate constant of the reaction and K is the adsorption constant of the pollutant on the photocatalyst. This equation can be simplified to a pseudo-first-order equation [28]:
(5)
In which kobs is the observed first-order rate constant of the photodegradation reaction.
The observed first-order rate constant for the photocatalytic degradation of MB on the nanocrystallines was calculated using plots of Ln C/C0 versus irradiation time.
Fig.5 shows the degradation efficiency of MB solutions in the presence 10 mg of La0.55Ca0.45A0.5Co0.5O3 (A = Mn, Mg ) nanoparticles under visible light. From this figure, it could be seen that the degradation efficiency of MB with the photo-catalysts in acidic solution is more efficient than natural than basic solution. Also, the degradation efficiency of MB solutions in the presence of La0.55Ca0.45Mn0.5Co0.5O3 nanoparticles is higher than La0.55Ca0.45Mg0.5Co0.5O3 nanoparticles.
The reactivity of nanosized materials is often altered or enhanced with respect to their bulk counterparts due to size-dependent changes in their redox potentials and high density of the active surface states associated with large surface-to-volume ratio. Moreover, recombination of electron-hole pairs within the semiconductor particle is drastically reduced as particle size decreases [29]. So, better photocatalytic activity of La0.55Ca0.45Mn0.5Co0.5O3 than La0.55Ca0.45Mg0.5Co0.5O3 can be related to smaller particle size calculated by using XRD measurement and TEM and also observed metallic behaviour in this sample with respect to other. So we use La0.55Ca0.45Mn0.5Co0.5O3 nanopatricles and study to detect optimum term for this aqueous. In below, photocatalytic activity of this sample is subjected further.
We use different values of HCl (0.1N) (Fig. 6) in the solution to discover that in which pH of the aqueous with La0.55Ca0.45Mn0.5Co0.5O3 catalyst has maximum degradation efficiency. After examine the 0.01, 0.05, 0.1 cc of the acid, we found that the solution with 0.1 cc HCl (pH = 2.33) and La0.55Ca0.45Mn0.5Co0.5O3 nanocatalyst has maximum degradation efficiency between acidic solutions. Fig. 7 shows that the adsorption capacity decreases below pH = 3. These variations in adsorption capacities of different catalysts highly dependent on the zero point charges. Because of the amphoteric behaviour of most of the semiconductor oxides, an important parameter in the reaction on the semiconductor particle surface is the pH of dispersions, since it influences the surface charge properties of photo-catalyst, the anionic dye molecule is negatively charged, and so low pH favors adsorption on the catalyst surface [30].
Fourier transform infrared (FT-IR) spectroscopy results of fresh La0.55Ca0.45A0.50Co0.50O3 (A = Mn, Mg) and used one after photocatalytic tests at pH = 2.33 are shown in Fig. 8. Similar FT-IR spectrum is observed for fresh and spent samples. The broad absorption band at 615 cm-1 is related to the asymmetrical lengthening of the Mn-O vibrations of MnO6 octahedral in perovskite structure [31]. A sharper band was related to a more symmetrical structure. The widening of this band and/or the appearance of a shoulder was reported to be an indication of a structure with lower symmetry. A shoulder in the perovskites at 540 cm-1 is cited to be a characteristic of a rhombohedral structure [32]. Results of Fig. 8 can be accounted for a more symmetric rhombohedra perovskite structure after degradation. No MB residual, however, is observed after photocatalytic degradation over La0.55Ca0.45A0.50Co0.50O3 nanoparticles. It can be concluded that adsorption of MB over the surface of the catalysts is followed by degradation. The peaks at 1636 and 3422 cm-1 in fresh sample are assigned to the O-H vibrations of trace of water on the sample. The La0.55Ca0.45A0.50Co0.50O3 is found to be an efficient photocatalyst under solar irradiation.
The degradation of MB on La0.55Ca0.45Mn0.5Co0.5O3 were done by varying catalyst amounts from 5 to 50 mg for the dye solution at maximized pH of 2.33 (Fig. 9). Maximum degradation is observed with 30 mg of the catalyst. This could be due to the fact that by increasing the mass of catalyst, higher surface area and active sites of the catalyst is available. In addition, of excess amount of La0.55Ca0.45Mn0.5Co0.5O3 above this dosage did not significantly enhance the degradation as shown in Fig.9. This is due to aggregation of catalyst particles, which reduced the surface area between the reaction solution and the photocatalyst. The increase in opacity and light scattering by the particles may be other reasons for the degradation rate [33-34]. This phenomenon can be ascribed to the reason that the number of the reactive sites can be increased when the amount of the catalysts was increasing. However, these nanoparticles may have a tendency to aggregate when their quantity is in excess, thus contributing to the decrease of the reactive sites. Besides, excess amount of the catalyst may exist as the scavenger of hydroxyl radicals [35-37]. Therefore, we choose 30 mg catalyst as the optimum amount of La0.55Ca0.45Mn0.5Co0.5O3 in aqueous solution and investigate the degradation of MB in this solution (Fig. 9).
Photo-Fenton degradation of MB in aqueous solution in the presence of La0.55Ca0.45Mn0.5Co0.5O3 photocatalysts at room temperature under pH = 2.33 are shown in Fig. 10. In general, the kinetics of photocatalytic degradation of organic pollutants on the semiconducting oxide has been established and can be described well by the apparent first-order reaction in 
, where kapp is the apparent rate constant, c0 is the concentration of MB after darkness adsorption for 30 min and ct is the concentration of MB at time t. The inset of Fig. 11 shows the linear relation of 
versus irradiation time for degradation of MB [38]. Also, the photocatalytic degradation of MB over La0.55Ca0.45Mn0.5Co0.5O3 catalyst, obeys the pseudo-zero-order kinetics in terms of modified Langmuir-Hinshelwood (LW-H) model [39].
5. Conclusions
La0.55Ca0.45A0.5Co0.5O3(A = Mg, Mn) nanoparticles prepared by citrate method were characterized using X-ray diffraction measurement, transmission electron microscopy, Fourier transform infrared and UV-Vis spectroscopy. The structural characterization of the samples using X’Pert package and Fullprof program is evidence for the presence of the rhombohedral structure (space group R-3c) in La0.55Ca0.45Mn0.5Co0.5O3 and orthorhombic structure (two phase system Pnma I and Pnma II) in La0.55Ca0.45Mg0.5Co0.5O3. The calculated value of crystallite size and particle size of La0.55Ca0.45Mn0.5Co0.5O3 is much less than La0.55Ca0.45Mg0.5Co0.5O3. La0.55Ca0.45A0.5Co0.5O3 (A = Mg, Mn). Nanoparticles prepared by the citrate-nitrate method were characterized by FT-IR and UV-Vis spectroscopy. The values of the band gap energy calculated using Tauc equation are 1.31 eV and 3.58 eV that show metallic behaviour for La0.55Ca0.45Mn0.5Co0.5O3, but semiconductor behaviour for La0.55Ca0.45Mg0.5Co0.5O3. There is no difference between the FT-IR of the fresh and used samples with the same concentration. No MB residual is observed after photocatalytic degradation for all solutions that we examined in this work over La0.55Ca0.45A0.5Co0.5O3 (A = Mn, Mg) nanoparticles. Also adsorption of MB over the surface of La0.55Ca0.45A0.5Co0.5O3 (A = Mn, Mg) nanoparticles is followed by the degradation. The photocatalytic activity of the product was studied for degradation of an aqueous solution of methyl blue under solar condition. The result show that three operational parameters including irradiation time, pH, and the catalyst amount strongly affect the dye degradation. The degradation efficiency of MB solutions in the presence of 10 mg La0.55Ca0.45Mn0.5Co0.5O3 nanoparticles under visible light indicate to be higher than La0.55Ca0.45Mg0.5Co0.5O3 nanoparticles. Also, the solution with 0.1 cc HCl (pH = 2.33) and 30 mg of La0.55Ca0.45Mn0.5Co0.5O3 nanocatalyst has 96 % degradation efficiency after 30 minutes between asidic solutions.
References
[1] Tanaka, K., Kanjana, P., and Teruaki, H.. (2000). Photocatalytic degradation of commercial azo dyes. Water research 34, 327-333.
[2] Lachheb, H., et al. (2002). Photocatalytic degradation of various types of dyes (Alizarin S, Crocein Orange G, Methyl Red, Congo Red, Methylene Blue) in water by UV-irradiated titania. Applied Catalysis B: Environmental 39, 75-90.
[3] Crini, G. (2006). Non-conventional low-cost adsorbents for dye removal: a review. Bioresource technology 97, 1061-1085.
[4] Ravikumar, K., B. Deebika, and Balu. K. (2005). Decolourization of aqueous dye solutions by a novel adsorbent: application of statistical designs and surface plots for the optimization and regression analysis. Journal of hazardous materials 122, 75-83.
[5] McMullan, Geoffrey, et al. (2001). Microbial decolourisation and degradation of textile dyes. Applied Microbiology and Biotechnology 56, 81-87.
[6] Soltani, N., et al. (2012). Visible light-induced degradation of methylene blue in the presence of photocatalytic ZnS and CdS nanoparticles. International journal of molecular sciences 13, 12242-12258.
[7] Pearce, C. I., Lloyd J. R., and Guthrie J. T. (2003). The removal of colour from textile wastewater using whole bacterial cells: a review. Dyes and pigments 58, 179-196.
[8] Lee, Jae-Wook, et al. (2006). Evaluation of the performance of adsorption and coagulation processes for the maximum removal of reactive dyes. Dyes and pigments 69, 196-203.
[9] Salem, I.A., and Mohamed S. El-M. (2000). Kinetics and mechanism of color removal of methylene blue with hydrogen peroxide catalyzed by some supported alumina surfaces. Chemosphere 41, 1173-1180.
[10] Haque, E., Jong, W.J., and Sung H. J. (2011). Adsorptive removal of methyl orange and methylene blue from aqueous solution with a metal-organic framework material, iron terephthalate (MOF-235). Journal of Hazardous materials 185, 507-511.
[11] Jesionowski, T. (2005). Characterization of pigments obtained by adsorption of CI Basic Blue 9 and CI Acid Orange 52 dyes onto silica particles precipitated via the emulsion route. Dyes and pigments 67, 81-92.
[12] Jesionowski, T., Agnieszka, A., and Andrzej, K. (2008). Adsorption of basic dyes from model aqueous solutions onto novel spherical silica support. Coloration Technology 124, 165-172.
[13] Herrmann, J.-M. (1999). Heterogeneous photocatalysis: fundamentals and applications to the removal of various types of aqueous pollutants. Catalysis today 53, 115-129.
[14] Kitture, R., et al. (2011). Catalyst efficiency, photostability and reusability study of ZnO nanoparticles in visible light for dye degradation. Journal of Physics and Chemistry of Solids 72, 60-66.
[15] Keshmiri, M., Madjid M., and Tom T. (2004). Development of novel TiO2 sol–gel-derived composite and its photocatalytic activities for trichloroethylene oxidation. Applied Catalysis B: Environmental 53, 209-219.
[16] Su, C., Hong, B-Y., and Tseng. C.-M., (2004). Sol–gel preparation and photocatalysis of titanium dioxide. Catalysis Today 96, 119-126.
[17] Sivalingam, G., et al., (2003). Photocatalytic degradation of various dyes by combustion synthesized nano anatase TiO2. Applied Catalysis B: Environmental 45, 23-38.
[18] Nagaveni, K., et al. (2004). Solar photocatalytic degradation of dyes: high activity of combustion synthesized nano TiO2. Applied Catalysis B: Environmental 48, 83-93.
[19] www.sigmaaldrich.com.
[20] Gholizadeh, A., Malekzadeh, A., Ghiasi, M., (2016). Structural and magnetic features of La0.7Sr0.3Mn1-xCoxO3 nano-catalysts for ethane combustion and CO oxidation. Ceramics International 42, 5707–5717.
[21] Gholizadeh A, Malekzadeh A., (2017). Structural and redox features of La0.7Bi0.3Mn1-xCoxO3 nanoperovskites for ethane combustion and CO oxidation. International Journal of Applied Ceramic Technology 14, 404–412.
[22] Gholizadeh, A., (2017). La1-xCaxCo1-yMgyO3 nano-perovskites as CO oxidation catalysts: structural and catalytic properties. Journal of the American Ceramic Society 100, 813–1249.
[23] Gholizadeh, A., Yousefi, H., Malekzadeh, A., Pourarian, F., (2016). Calcium and strontium substituted lanthanum manganite–cobaltite (La1-x(Ca,Sr)xMn0.5Co0.5O3] nano-catalysts for low temperature CO oxidation. Ceramics International 42, 12055–12063.
[24] Gholizadeh, A., Tajabor, N., (2010). Influence of N2- and Ar-ambient annealing on the physical properties of SnO2:Co transparent conducting films. Materials Science in Semiconductor Processing, 13, 162–166.
[25] Wang, K., et al., (2009). Photocatalytic degradation of methylene blue on magnetically separable FePc/Fe3O4 nanocomposite under visible irradiation. Pure and Applied Chemistry 81, 2327-2335.
[26] Abdollahi, Y., et al., (2011). Photocatalytic degradation of p-Cresol by zinc oxide under UV irradiation. International journal of molecular sciences 13, 302-315.
[27] Taghvaei, V., Aziz, H.-Y., and Mahdi, B. (2010). Hydrothermal and template-free preparation and characterization of nanocrystalline ZnS in presence of a low-cost ionic liquid and photocatalytic activity. Physica E: Low-dimensional Systems and Nanostructures 42, 1973-1978.
[28] Xu, Xin, et al., (2011). Fabrication and photocatalytic performance of a ZnxCd1-xS solid solution prepared by sulfuration of a single layered double hydroxide precursor. Applied Catalysis B: Environmental 102, 147-156.
[29] Zhang, F., Weijie, S., and Jing, L., (2015). Effective removal of methyl blue by fine-structured strontium and barium phosphate nanorods. Applied Surface Science 326, 195-203.
[30] Alkaim, A. F., et al., (2014). Effect of pH on adsorption and photocatalytic degradation efficiency of different catalysts on removal of methylene blue. Asian Journal of Chemistry 26, 8445-8448.
[31] Pecchi, G., Claudia, C., and Octavio, P., (2009). Thermal stability against reduction of LaMn1-yCoyO3 perovskites. Materials Research Bulletin 44, 846-853.
[32] M. Khazaei, A. Malekzadeh, F. Amini, Y. Mortazavi, A. Khodadadi, Effect of citric acid concentration as emulsifier on perovskite phase formation of nano-sized SrMnO3 and SrCoO3 samples. Crystal Research and Technology 45 (2010) 1064.
[33] Vinu, R., and Giridhar, M., (2008). Kinetics of sonophotocatalytic degradation of anionic dyes with nano-TiO2. Environmental science & technology 43, 473-479.
[34] Schrank, S.G., et al., (2005). Applicability of Fenton and H2O2/UV reactions in the treatment of tannery wastewaters. Chemosphere 60, 644-655.
[35] Yang, X., et al., (2015). Rapid degradation of methylene blue in a novel heterogeneous Fe3O4@ rGO@ TiO2-catalyzed photo-fenton system. Scientific reports 22, 10632-10639.
[36] Kuang, Ye, et al., (2013). Heterogeneous Fenton-like oxidation of monochlorobenzene using green synthesis of iron nanoparticles. Journal of colloid and interface science 410, 67-73.
[37] Bel Hadjltaief, H., et al., (2013), Influence of operational parameters in the heterogeneous photo-Fenton discoloration of wastewaters in the presence of an iron-pillared clay. Industrial & Engineering Chemistry Research 52, 16656-16665.
[38] Wang, F., et al., (2010). Visible-light-induced photocatalytic degradation of methylene blue with polyaniline-sensitized composite photocatalysts. Superlattices and Microstructures 48,170-180.
[39] Zhou, M., Jiaguo, Y., and Huogen, Y., (2009). Effects of urea on the microstructure and photocatalytic activity of bimodal mesoporous titania microspheres. Journal of Molecular Catalysis A: Chemical 313, 107-113.
D (nm) | lattice Parameters | A (%) | Space group | Structure | Abbreviation sample # | Sample |
24 | a = b =c = 5.388 (Å), α = β = γ = 60.371 (°) | ----- | R-3c | Rhombohedral | Mn | La0.55Ca0.45Mn0.5Co0.5O3 |
32 | a = 5.3004(Å) , b = 7.7650 (Å) , c = 5.5582(Å) | 90 | Pnma I | Orthorhombic | Mg | La0.55Ca0.45Mg0.5Co0.5O3 |
| a = 5.4081(Å) , b = 7.6219(Å) , c = 5.2994(Å) | 10 | Pnma II |
|
Table 1: Crystallite size, structure type and unit cell parameters of the samples. A is the Pnma I or Pnma II Share (%)
Figures captions
Fig. 1: Chemical structure of methyl blue dye.
Fig. 2: Rietveld analysis of La0.55Ca0.45A0.5Co0.5O3 using Fullprof program. The circle sings represent the raw data. The solid line represents the calculated profile. Vertical bars in (Mn) indicate the position of Bragg peaks for rhombohedral with space group R-3c and in (Mg) the position of Bragg peaks for orthorhombic structure with space groups Pnma II and Pnma I, respectively. The lowest curve is the difference between the observed and the calculated patterns.
Fig. 3: TEM micrographs and size distribution histograms of La0.55Ca0.45A0.5Co0.5O3.
Fig. 4: The plot of the Tauc’s equation to obtain band gap of La0.55Ca0.45A0.5Co0.5O3 nanoparticles.
Fig. 5: Degradation efficiency of MB with the photocatalyst in natural, basic (in 360 min) and asidic solutions (in 300 min).
Fig. 6: Degradation efficiency of MB with the photocatalysts in asidic solutions.
Fig. 7: Effect of pH on adsorption capacity of methyl blue on La0.55Ca0.45Mn0.5Co0.5O3 catalyst (b) Absorption spectrum of a 25 ppm MB solution in different pH.
Fig. 8: FT-IR spectrum of fresh and used La0.55Ca0.45Mn0.5Co0.5O3 photocatalyst.
Fig. 9: Effect of the amount of catalyst on the degradation of MB (C0 = 25 ppm, pH = 2.33, time of irradiation = 30 min, temperature = 28–32 ºC).
Fig. 10: Photo-Fenton degradation of MB in the presence of catalyst at room temperature under pH = 2.33.
Fig. 11: Photodegradation of methyl blue (MB) under solar irradiation in the presence of La0.55Ca0.45Mn0.5Co0.5O3 sample (inset shows its 
vs. time graph).
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