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1. Introduction

Water pollution is one of the major environmental issues that arises from the discharge of organic dyes in wastewater, which is a threat to both aquatic and human life [1]. Various methods used for the removal of these organic dyes from wastewater are reported in the literature [2], such as advanced oxidation, biological methods, and adsorption processes. [3] Among these methods, heterogeneous photocatalysis under UV light or artificial light is a popular choice [4]. In this regard, different types of metal and metal oxide nanoparticles (NPs) have gained significant attention as efficient photocatalysts. Compared to physical, chemical, and biological methods, dye degradation using NPs as photocatalysts offers various benefits, as NPs are effective, stable, inexpensive, easily prepared, and also possess efficient optical and electrical properties [5]. Among the various metal oxides, CrO2 has attracted great scientific interest in the fields of materials science and physical chemistry, since it is the only half-metallic (HM) ferromagnetic (FM) material in 3d transition metal dioxide form [6]. It offers various advantages, such as low cost [7], high thermal stability [8], and low toxicity [9]; thus, it can potentially be applied for the degradation of methylene blue [10] and methyl orange dyes [11]. However, the degradation ability of CrO2 is severely affected by its inability to fully absorb photons in the UV region; this is because of its large band gap (3.7 eV) [12]. In order to enhance the photo catalytic activity of CrO2 and reduce its band gap [6], it is typically doped with different types of noble metals, which creates defects and additional energy levels in its microstructure [13,14]. Thus far, various types of metals and their oxides have been used as dopants, including Ru, Ti, and Sn [12,15].

Among the different elements, zirconium has been considered as an important material because of its various unique properties, which can be used for a number of applications. Zr doping in metal oxide (such as CrO2) nanoparticles produces many structural defects, e.g., interstitial defects and oxygen vacancies. The discussion of doping in this paper focuses on a solid solution obtained by combining a dopant (Zr) and a host metal oxide (CrO2), with the addition of oxygen. The charge of the Zr is then compensated for by an ionic defect that is gradually replaced by holes. When the equilibrium is disturbed as a result of the oxygen, the lattice defect is gradually replaced by electrons. The stoichiometric region of CrO2 is replaced by two regions: the byproduct of reduction, e.g., oxygen vacancies (electrons), and the byproduct of oxidation, e.g., cation vacancies (holes) in the region of higher oxygen vacancies [16]. Various authors have previously studied Zr-doped metal oxides for the degradation of different dyes. Desta et al. studied Zr4+ doped TiO2 for the degradation of MB dye [17]. Khan et al. studied the effect of Zr doping in CeO2 for the degradation of MB dye [16]. Subash et al. investigated the effect of Zr-loading on a Ag-ZnO composite for the degradation of red 120 dye [18]. Sulaiman et al. used m-ZrO2, c-ZrO2, and t-ZrO2 for the degradation of MO dye [19]. Kumar et al. used ferromagnetic ZrO2 nanoparticles for the degradation of MB dye [20].

Chromium IV oxide can be used as a heterogeneous catalyst [9], and the dopant Zr can be used as a catalyst support [10,11], dielectric material [6], high-performance ceramic material [13] and in chemical sensors [15], solid oxide fuel cells [21,22], and as a photocatalyst [23]. It is a semiconductor metal oxide which is considered to be a suitable material because of its chemical and photochemical stability in aqueous medium. Zr doping of CrO2 not only enhances photocatalytic activity by increasing the surface area, but also stabilizes the structure at high temperature [21]; thus, the selective trapping of electrons occurs on Zr4+ in contrast to Cr4+ [22]. Therefore, the addition of a second element such as Zr enhances the thermal stability, increases the surface area of the host, and also helps to improve the separation rate of photo-induced electrons and holes. However, to the best of our knowledge, Zr-doped CrO2 has been rarely reported as a photocatalyst for the degradation of dyes.

To date, various methods such as sol gel [23], coprecipitation [24], hydrothermal [25], sonication [26], ball mill [27], and flame pyrolysis [28] have been reported in the literature for the preparation of nanoparticle-based photocatalysts and their composites. However, such methods are often expensive, hazardous, and counterproductive to the fabrication of scalable and environmentally friendly composite materials. Therefore, in the current research, an eco-friendly, solid-state reaction [29] has been reported for the first time to prepare a Zr-doped, chromium IV oxide photocatalyst. In order to obtain an optimized dopant percentage, different samples were prepared by varying the amount of zirconium. The structure, morphology, and specific surface area of the as-prepared composites were investigated through X-ray diffraction, scanning electron microscopy, Brunauer–Emmett–Teller (BET), and UV–visible absorption. Additionally, the band gaps of the synthesized Zr/CrO2 materials were determined through diffused reflectance spectroscopy (DRS). Finally, photocatalytic experiments were carried out using the different samples under visible light.

2. Results and Discussion 2.1. Structural and Morphological Characterization

The prepared Zr/CrO2 photocatalysts were characterized by their crystal structure, crystallite size, and phase composition by X-Ray diffraction technique. Figure 1a shows the XRD patterns of the synthesized Zr1CrO2, Zr3CrO2, Zr5CrO2, Zr7CrO2, and Zr9CrO2 materials, which were tetragonal in structure and single phase due to the presence of (110), (101), (200), and (111) diffraction planes. The lattice parameters of CrO2(a=b=4.421 Å, c=2.916 Å)were almost similar to those of TiO2 (a=b=4.593 Å, c=2.959 Å), which is considered an efficient photocatalyst [30]. When doping a metal, the size of the dopant is an important parameter. First, the dopant size should approximately match that of the host metal (Cr or O). Second, if it is necessary to occupy the distance between the host atoms, an appropriately sized dopant is required; in the case of Cr-O, Zr, has an atomic radius of 0.160 nm. The (4+) ionic radius is 0.080 nm smaller than the distance between the Cr-O, which is 0.18 nm to 0.21 nm. It is clear from the XRD pattern in Figure 1b that the two most intensive peaks at (110) and (101) were slightly shifted towards the high angle (2θ) with low d-spacing after the incorporation of Zr in CrO2. This indicated that the Cr atoms had been replaced by Zr in the tetragonal structure of CrO2 due to substitution, which distorted the crystal structure of the host material on the basis of differences in the ionic radii of chromium and zirconium atoms [31,32]. The XRD pattern of Zr/CrO2 showed few peaks of Cr2O3, which is considered to be one of the most stable oxides of chromium [33]; at high temperatures, CrO2 is converted to Cr2O3. The crystallite size obtained using the Scherrer equation [34] revealed an average size of the NPs of between 33.9 nm and 45 nm. Notably, with varying zirconium doping from 1 to 9 wt.%, the peak intensities also increased, along with the zirconium concentration.

SEM was used for crystal morphology and shape observations of all the synthesized samples. The SEM images are shown in Figure 2. These images indicate that the shape and morphology of Zr/CrO2 photocatalysts change with increasing Zr concentration. The particles seemed to agglomerate with an increase of Zr content and exhibit a flake shaped morphology, with average crystalline sizes of 33.9 nm to 45.3 nm. The particles were dispersed properly in all samples, which is evident in Figure 2. To determine the elemental composition of all the samples, EDX was used, as shown in Figure 3. The EDX analysis showed that the material was in pure form with no elemental impurities present in the samples, while the concentration of Zr increased gradually.

In order to further confirm the synthesis of all as-prepared Zr/CrO2-based photo catalysts, FTIR spectra were measured, as shown in Figure 4 and Table 1. After calcinations, the synthesized photocatalysts were free from impurities and moisture. The IR spectra exhibited peaks at 3100, 3010, and 1986 cm−1 belonging to C-H, C-C, and C=O functional groups. The peaks at 3400 and 1239 cm−1 represented O-H and C-O functional groups [35]. Different modes of vibration of CrO2 and Zr-O were also visible in the IR spectra. For instance, the presence of Zr-O was represented by the vibrational mode at 815 cm−1, while the peaks at 503 and 428 cm−1 corresponded to the vibration of Cr18O18O and Cr16O2, the peaks at 1110 and 653 cm−1 possibly pointed to the vibrational mode of Cr-O and O-O in CrOO, and the vibrational mode of O-Cr-O appeared at 1789 cm−1 [36]. The stretching vibrational peak at 815 cm−1 indicated the presence of Zr-O [37].

The as-prepared Zr/CrO2 photocatalysts (Zr1CrO2, Zr3CrO2, Zr5CrO2, Zr7CrO2, and Zr9CrO2) were also investigated for absorption in the 200–800 nm wavelength region, as shown in Figure 5a. Pure CrO2 absorbance peaks appeared at 257 nm and 346 nm [33]; however, after doping, the absorbance peaks shifted to a higher wavelength [38]. For band gap studies, the Diffuse Reflectance Spectroscopy (DRS) technique was used. From the DRS spectra, the band gap of the as-prepared photocatalysts was calculated using the Tauc, Davis and Mott relation, given by (αhν)1/2 = A(hν–Eg), where α, ν, A, and Eg are the absorption coefficient, light frequency, proportionality constant, and band gap, respectively [39,40,41]. From the plot for (αhν)1/2 vs. energy (hν) shown in Figure 5b, the band gap could be evaluated by extrapolating the straight line to the axis intercept. By using the DRS technique, followed by the numerical relation given above, the band gaps of all the samples were calculated. The DRS studies of the prepared material showed band gaps of 4.3, 3.2, 2.9, 2.87, 2.7, and 2.4 eV for pristine CrO2, Zr1CrO2, Zr3CrO2, Zr5CrO2, Zr7CrO2, and Zr9CrO2, respectively, as shown in Table 2. The DRS study revealed that after doping, the band gap decreased from 4.3 eV to 2.4 eV, which made the samples capable of absorbing light in the UV region, ultimately enhancing their photocatalytic degradation capabilities.

BET was employed to determine the surface area and pore size of the prepared material. The results, shown in Table 3, indicated that by increasing the doping concentration of zirconium in chromium IV oxide, the surface area of the host metal oxide (CrO2) also increased, which indicated that the maximum loading of the dopant and the degradation capacity of the material had been enhanced due to the large surface area, as shown [42].

2.2. Studies of Zr/CrO2 Photo-Catalysts for the Degradation of Dyes

2.2.1. The Degradation Study of MB and MO Dyes

Both MB and MO are heterocyclic aromatic compounds, which are also known as azo dyes bearing the functional group(R−N=N−Ŕ). Both R and Ŕ are aryl groups that can be degraded using OH radicals produced by metal-doped metal oxide nanoparticles that are activated by UV light in the presence of aqueous media, producing carbon dioxide, water, and minerals as byproducts. These dyes are known to alter the physicochemical properties of soil and poison water bodies, and can cause serious damage to the flora and fauna in the environment. The UV-visible spectroscopic technique was used to study the effect of dopant concentration and time during the degradation of methylene blue (MB) and methyl orange (MO) in aqueous media in the presence of catalysts. During the experiments, the concentrations both of dyes (MB and MO) and photocatalysts were kept constant. The mixtures were prepared by dissolving 0.2 g of photocatalysts in 50 mL aqueous solution of each dye; before placing them under UV-light irradiation, these mixtures were kept in a dark place for 20 min to achieve complete adsorption and desorption equilibrium. The zero-time readings were taken, and the mixtures were studied under UV-light from 0–140 min.

The photocatalytic experiments showed that as the dopant concentration increased, the efficiency of the photocatalyst also increased. However, this trend was followed only up to 5 wt.%. After further increasing the amount of dopant, the efficiency of the samples dropped; this was due to the recombination of photoexcited electrons and holes and the energy absorbed by electrons during excitation that were released in the form of radiation [43]. The photocatalysts showed maximum efficiency from 1 wt.% to 5 wt.%, beyond which the efficiency decreased for the Zr7CrO2 and Zr9CrO2 samples. This fact can be clearly seen from the UV/Visible degradation study of MB and MO dyes. Initially, the degradation rates of MB and MO dyes were fast due to high concentration of dye molecules; however, the rate decreased gradually due to the deficiency of dye molecules [44,45]. The effect of contact time and dopant concentration on catalysts with MB and MO dyes are shown in Figure 6 and Figure 7, respectively, which indicate that by increasing the time, the catalytic efficiency also increases up to 140 min.

2.2.2. The MB and MO Kinetic Study

The reaction (degradation) kinetics of both MB and MO were studied by placing the prepared mixtures under UV-light for different intervals of time, i.e., 0–140 min. The initial rate (r0) of degradation of methylene blue and methyl orange increased for Zr1CrO2, Zr3CrO2, and Zr5CrO2 as the concentration of zirconium increased, while the initial rate(r0) decreased in the case of Zr7CrO2 and Zr9CrO2 due to the recombination of photoexcited electrons and holes. The Langmuir-Hinshelwood model can be used to understand the kinetics of photocatalytic degradation of MB and MO dyes as [46,47]:

r0=−dcdt=kKc1+KC

wherer0denotes the initial reaction rate(mg L−1 min−1),Crepresents the dye concentration(mg L−1),andtrepresents the reaction time(min). In addition,kandKcrepresent the Langmuire-Hinshelwood reaction rate constant(mg L−1 min−1)and langmuire adsorption equilibrium constant(L mg−1). For small amounts of pollutants(KC <<1), pseudo-first-order kinetics can be applied, as given by the following equations:

r0=−dcdt=−kKC

lnC0C=kKt= kappt

where apparent constant(kapp)is the kinetics parameter, andC0andCare initial and residual concentrations of MB and MO dyes in the aqueous phase before and after light irradiation, respectively. The(kapp)can be found from (lnC0C)vs. irradiation time. For all photocatalysts, the initial degradation rates (r0= kapp × C0) of10 mg L−1 MB and MO were calculated, and the results are shown in Figure 8a,b, respectively.

To find the rate of degradation of MB and MO dyes, the pseudo first order kinetics can be applied, as given by the following equation as [48]:

lnC0Ct= Kt

whereC0represents the initial concentration before irradiation,Ctrepresents the concentration after irradiation,t represents the time of irradiation, and K is a constant which can be found as a slope after plotting, as shown in Figure 9a,b.

The photocatalytic efficiency of the prepared catalysts is dependent on the concentration of dopant (Zr4+) in (CrO2) nanoparticles. As the concentration of the dopant increases, the photocatalytic efficiency also increases up to 5 wt.%, whereas for 7 wt.% and 9 wt.%, the catalytic efficiency decreases due the recombination of holes and photoexcited electrons. The dopant enhanced the photocatalytic efficiency of the host materials due to the presence of(Zr4+)ions, which gain electrons during photo-excitation by converting to(Zr3+), which is transferred to O2 generating superoxide radical O2•−, preventing photo-corrosion.

2.2.3. MB and MO Percent Photo Catalytic Degradation Curve of Zr-doped CrO2 as Function of time

To study the effects of contact time and dopant concentration on the percent degradation of MB and MO,10 ppm (10mgL)dye solutions were prepared in deionized water. The amount of prepared catalysts and dyes (MB and MO) were kept constant. The efficiencies of the prepared photocatalysts varied for different dopant concentrations. The MB dye was degraded up to 50.5%, 57.4%, and 64.4% byZr1CrO2, Zr3CrO2, and Zr5CrO2photocatalysts after 140 min, respectively, whereas 41.8% and 37.6% of MB dye was degraded byZr7CrO2and Zr9CrO2 , respectively (see Figure 10a,b). In the case of MO degradation, photocatalysts followed the same pattern as above. The MO dye was degraded up to 48.4%, 52.2%, and 55.4% byZr1CrO2, Zr3CrO2, and Zr5CrO2photocatalysts, respectively, after 140 min, whereas 38.3% and 26.5% of MO dye degraded byZr7CrO2andZr9CrO2 respectively (see Figure 11a,b). On the basis of percentage of degradation of MB and MO dyes, it is clear that after 5 wt.% doping, the photocatalytic efficiency did not increase, because the doping crossed the optimum level; as a result, the electrons and holes were recombined, also known as photo-corrosion [49].

3. Tentative Mechanism The proposed mechanisms of Zr-doped CrO2 nanoparticles for the degradation of MB and MO dyes are as follows:

  • After illumination with UV light, the electrons move from the conduction band to the valence band, leaving a positive hole in the valence band.

    CrO2 + hv → CrO2 (h+ vb) + CrO2 (e− cb)

  • The electrons in the conduction band of Zr-doped CrO2 can be trapped by dopant Zr4+, thereby holding up the recombination process of electrons.

    CrO2 (e−) + Zr4+ → CrO2 + Zr3+ (unstable)

  • The trapped electrons (Zr4+→Zr3+) were scavenged by molecular oxygen, which is adsorbed on the surface of CrO2 to generate superoxide radicals, in turn producing hydrogen peroxide (H2O2), hydroperoxyl (HO2•), and hydroxyl (•OH) radicals.

    CrO2 (e−) + O2 → CrO2 + O2• −

    CrO2 (e−) + O2• − + H2O → CrO2 + HO2• + HO−

    CrO2 (e−) + HO• + H+ → CrO2 + H2O2

    CrO2 (e−) + H2O2 → CrO2 + HO2• + HO−

  • Finally, the holes act as oxidizing agents and electrons act as reducing agents for the degradation of MB and MO dyes in aqueous solution.

    •OH (hv) + Pollutant → Degradation product

4. Materials and Methods 4.1. Materials The chemicals used for the preparation of zirconium-doped, chromium IV oxide photocatalysts were of analytical grade, and used as such without further purification. Zirconium metal powder, CrO2 powder, DI water, methylene blue, and methyl orange were purchased from Merck Ltd. (Darmstadt, Germany‎). Ethanol was purchased from Sigma-Aldrich (St. Louis, MO, USA). 4.2. Synthesis of Zr/CrO2 Photocatalyst by Solid-State Reaction Method Zirconium-doped, chromium IV oxide photocatalysts (Zr/CrO2) were prepared by a solid-state, environmentally friendly reaction at room temperature. Zirconium metal powder and chromium IV oxide powder were mixed in definite molar ratios (1:1, 3:1, 5:1, 7:1, and 9:1) using a mortar and pestle with a small amount of ethanol, and ground for several minutes until the powder was sufficiently mixed. After mixing, the prepared photocatalysts were calcined at 450 °C in a muffle furnace for 1 h to remove any impurities. The prepared photocatalysts were then characterized by various techniques, i.e., XRD, SEM, EDX, FT-IR, UV-Vis, and BET, and were used for the degradation of methylene blue and methyl orange as such. Degradation studies were carried out by UV/Visible spectrophotometer (Perkin Elmer lambda 35, Waltham, MA, USA). 4.3. Photocatalytic Experiments The photocatalytic activity was examined by dissolving 0.2 g of each catalyst (solid), i.e., Zr1CrO2, Zr3CrO2, Zr5CrO2, Zr7CrO2, and Zr9CrO2, in 50 mL aqueous solution of MB and MO dyes (10 ppm). The reaction vessel was placed in the dark for complete desorption and adsorption equilibrium for 20 min with continuous stirring. Zero-time readings were taken before the samples were placed under UV light (10 watt) at 15 cm distance for maximum utilization of the light at different intervals of time (10–140 min) for their complete mineralization. Afterwards, all samples were filtered through a 0.45 μm (PVDF) filter and then analyzed using a UV/Visible spectrophotometer (Carry 50) to determine the degradation, reaction kinetics, and concentration. 5. Conclusions Zr-doped CrO2 nanoparticles were prepared on the basis of different concentrations of dopant (Zr) through a one-step, solid-state reaction method. XRD analysis confirmed the doping of Zr in CrO2 by replacing the Cr with Zr. This optical study verifies that as the dopant concentration increases, the absorbance peaks shifts to higher wavelengths and lower energy as a result of the decreasing band gap of the host material. Moreover, other techniques such as FT-IR and EDX confirmed the Zr doping in CrO2, which shows that the photocatalysts are suitable for UV light absorption due to the reduction in the band gap. It was also observed that as the concentration of dopant increases, the photocatalytic efficiency of the catalysts also increases up to 5 wt.%. Therefore, Zr-doped CrO2 photocatalysts could potentially be used for wastewater treatment.

Figure 1.(a) Comparison of XRD spectra of Zr1CrO2, Zr3CrO2, Zr5CrO2, Zr7CrO2, and Zr9CrO2; (b) XRD spectra demonstrating peak shifts of (110) and (101) diffraction planes.

Figure 2. SEM images of (a) Zr1CrO2, (b) Zr3CrO2, (c) Zr5CrO2, (d) Zr7CrO2, and (e) Zr9CrO2 photocatalysts.

Figure 3. EDX spectra of (a) Zr1CrO2, (b) Zr3CrO2, (c) Zr5CrO2, (d) Zr7CrO2, and (e) Zr9CrO2 photocatalysts.

Figure 4. The FT-IR spectra of Zr-doped CrO2 photocatalysts.

Figure 5.(a) UV-Vis spectra; (b) Band gaps of Zr-doped CrO2 photocatalysts.

Figure 6.(a) Zr1CrO2, (b) Zr3CrO2, (c) Zr5CrO2, (d) Zr7CrO2, and (e) Zr9CrO2 degradation of MB dye vs. contact time.

Figure 7.(a) Zr1CrO2, (b) Zr3CrO2, (c) Zr5CrO2, (d) Zr7CrO2, and (e) Zr9CrO2 degradation of MO dye vs. contact time.

Figure 8.(a) Methylene blue and (b) Methyl orange initial rate (r0).

Figure 9. Photocatalytic degradation curve of (a) Methylene blue (b) Methyl orange.

Figure 10.(a) Methylene blue (b) Methyl orange percent photocatalytic degradation.

Figure 11.(a) Methylene blue (b) Methyl orange percent degradation at 140 min.

Peak Number Functional Group Peak Position cm−1 Mode
1Cr16O2428Stretching
2Cr18O18O503Stretching
3CrOO (O-O)653Stretching
4Zr-O815Bending
5Cr-O1110Stretching
6C-O-C1239Stretching
7O52CrO1789Bending
8CO21986Bending
9C-C3010Bending
10C-H3100Vibration
11OH3400Stretching

Samples CrO2 Zr1CrO2 Zr3CrO2 Zr5CrO2 Zr7CrO2 Zr9CrO2
Band gap (E) eV4.33.22.92.872.72.4

Samples Pore Size (cm3/g) BET S.A. (m2/g)
Zr1CrO24.83.5
Zr3CrO2128.7
Zr5CrO213.49.9
Zr7CrO211.18.1
Zr9CrO211.28.2

Author Contributions

Conceptualization, Z.M. and M.B.; data curation, F.A., M.S. and N.A.; formal analysis, M.R.S., S.F.A., M.A.F.S. and E.M.A.; funding acquisition, M.R.S.; investigation, Z.M., F.A., M.S., N.A. and M.B.; methodology, A Z.M. and M.B.; visualization, M.R.S.; writing-original draft, Z.M., F.A., M.S., N.A. and M.B.; writing-review and editing, Z.M., F.A., M.S., N.A., M.B., M.R.S., S.F.A. and M.K.; All authors have read and agreed to the published version of the manuscript.

Funding

The authors extend their appreciation to the Deanship of Scientific Research at King Saud University for funding this work through Research Group no. RG-1441-453.

Institutional Review Board Statement

Not applicable.

Informed Consent Statement

Not applicable.

Data Availability Statement

Data is contained within the article.

Acknowledgments

The authors extend their appreciation to the Deanship of Scientific Research at King Saud University for funding this work through Research Group no. RG-1441-453. The authors also thankful to department of Physics, Kohat University of Science and Technology, Pakistan for its co-operation by providing synthesis and characterization facility at the nanotech lab for the synthesized material.

Conflicts of Interest

The authors declare that they have no conflicts of interest.

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Zahir Muhammad

1,

Farman Ali

1,

Muhammad Sajjad

2,

Nisar Ali

3,

Muhammad Bilal

4,*,

Mohammed Rafi Shaik

5,*,

Syed Farooq Adil

5,

Mohammed A.F. Sharaf

6,

Emad Mahrous Awwad

7 and

Mujeeb Khan

5,*

1Department of Chemistry, Hazara University Mansehra, Dhodial 21300, Pakistan

2Department of Physics, Kohat University of Science and Technology, Kohat 26000, Pakistan

3Key Laboratory for Palygorskite Science and Applied Technology of Jiangsu Province, National & Local Joint Engineering Research Center for Deep Utilization Technology of Rock-salt Resource, Faculty of Chemical Engineering, Huaiyin Institute of Technology, Huaian 223003, China

4School of Life Science and Food Engineering, Huaiyin Institute of Technology, Huaian 223003, China

5Department of Chemistry, College of Science, King Saud University, P.O. Box 2455, Riyadh 11451, Saudi Arabia

6Department of Industrial Engineering, College of Engineering, King Saud University, P.O. Box 800, Riyadh 11421, Saudi Arabia

7Department of Electrical Engineering, College of Engineering, King Saud University, P.O. Box 800, Riyadh 11421, Saudi Arabia

*Authors to whom correspondence should be addressed.

Word count: 5271

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© 2021. This work is licensed under http://creativecommons.org/licenses/by/3.0/ (the “License”). Notwithstanding the ProQuest Terms and Conditions, you may use this content in accordance with the terms of the License.

Abstract

Degradation of organic dyes and their byproducts by heterogeneous photocatalysts is an essential process, as these dyes can be potentially discharged in wastewater and threaten aquatic and xerophyte life. Therefore, their complete mineralization into nontoxic components (water and salt) is necessary through the process of heterogeneous photocatalysis. In this study, Zr/CrO2 (Zirconium-doped chromium IV oxide) nanocomposite-based photocatalysts with different compositions (1, 3, 5, 7 & 9 wt.%) were prepared by an environmentally friendly, solid-state reaction at room temperature. The as-prepared samples were calcined under air at 450 °C in a furnace for a specific period of time. The synthesis of Zr/CrO2 photocatalysts was confirmed by various techniques, including XRD, SEM, EDX, FT-IR, UV-Vis, and BET. The photocatalytic properties of all samples were tested towards the degradation of methylene blue and methyl orange organic dyes under UV light. The results revealed a concentration-dependent photocatalytic activity of photocatalysts, which increased the amount of dopant (up to 5 wt.%). However, the degradation efficiency of the catalysts decreased upon further increasing the amount of dopant due to the recombination of holes and photoexcited electrons.

Details

Title
Zirconium-Doped Chromium IV Oxide Nanocomposites: Synthesis, Characterization, and Photocatalysis towards the Degradation of Organic Dyes
First page
117
Publication year
2021
Publication date
2021
Publisher
MDPI AG
e-ISSN
20734344
Source type
Scholarly Journal
Language of publication
English
DOI
https://doi.org/10.3390/catal11010117
ProQuest document ID
2478827114
Copyright
© 2021. This work is licensed under http://creativecommons.org/licenses/by/3.0/ (the “License”). Notwithstanding the ProQuest Terms and Conditions, you may use this content in accordance with the terms of the License.