Kinetics and mechanism of color removal of methylene blue with hydrogen peroxide catalyzed by some supported alumina surfaces

Salem, Ibrahim A.; El-Maazawi, M.

doi:10.1016/s0045-6535(00)00009-6

Cited by 208 publications

(101 citation statements)

References 18 publications

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“…Various techniques like precipitation, ion exchange, chemical oxidation and adsorption have been used for the removal of toxic pollutant from, wastewater [3][4][5] . Over the years, a number of workers have used different waste materials.…”

Section: Introductionmentioning

confidence: 99%

Antimicrobial Activity of Some Medicinal Plants from Malaysia

Philip¹,

Malek²,

Sani³

et al. 2009

American J. of Applied Sciences

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Problem statement: It is well documented that lead is one of contaminants of industrial wastewaters and its pollution exists in the wastewater of many industries. As a result, recent research has focused on the development of cost effective alternatives using various natural sources and industrial wastes. In this setting, the use of low-cost agricultural materials, waste and residues for recovering heavy metals from contaminated industrial effluent has emerged as a potential alternative method to high cost adsorbents. In the present study, adsorption of lead(II) ions onto Orange Peel (OP), a typical agricultural byproduct, was investigated systematically with the variation in the parameters of pH, sorbent dosage, contact time and the initial concentration of adsorbate. Langmuir and Freundlich isotherms were used to analyze the equilibrium data. Kinetic and thermodynamic parameters were also calculated to describe the adsorption mechanism. Approach: The Orange Peel (OP) was obtained from a local market in the south of Jordan. The orange peel was cut into small pieces using scissors. Then OP was dried at 100°C for 24 h using hot air oven. Qualitative analyses of the main functional groups involved in metal adsorption were performed using a Fourier transformed infrared spectrometer (Perkin-Elmer FTIR 1605, ¨Uberlingen, Germany). Biosorption experiments were carried out in a thermostatic shaker at 180 rpm and at an ambient temperature (20±2°C) using 250 mL shaking flasks containing 100 mL of different concentrations and initial pH values of Pb(II) solutions, prepared from reagent grade salt Pb(NO 3 ) 2 (Merck). The initial pH values of the solutions were previously adjusted with 0.1 M HNO 3 or NaOH and measured using a hand held pH meters (315i/SET). The sorbent (0.2-1.0 g) was added to each flask and then the flasks were sealed up to prevent change of volume of the solution during the experiments. After shaking the flasks for predetermined time intervals, the samples were withdrawn from the flasks and filtered through a Whatman filter paper. The filtrate was analyzed by AAS (Perkin Elmer Analyst 300). Results: Four kinetic models are the pseudo-first-order, pseudo-second-order, Elovich and intraparticle diffusion equations, were selected to interpret the adsorption data. Kinetic parameters such as the rate constants, equilibrium adsorption capacities and related correlation coefficients, for each kinetic model were calculated and discussed. The linear Langmuir and Freundlich models were applied to describe equilibrium isotherms and both models fitted well. The monolayer adsorption capacity was found as 21.1 mg g −1 at pH 6 and 20°C.The dimensionless separation factor (R L ) has shown that orange peel can be used for removal of Pb(II) from aqueous solutions. The nagative free energy of adsorption indicated that the adsorption of lead (II) ions onto orange peel was feasible and spontaneous. Conclusion: The sorption capacity of the orange peel is comparable to the other available adsorbents and it is quite c...

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Section: Introductionmentioning

confidence: 99%

Antimicrobial Activity of Some Medicinal Plants from Malaysia

Philip¹,

Malek²,

Sani³

et al. 2009

American J. of Applied Sciences

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“…The formation of surface precursor complex is one of the kinetic rate-limiting steps in heterogeneous oxidative degradation of organic pollutants, closely related to the nature of surface charge. [37] It has been reported that the catalytic removal of MB in the presence of H 2 O 2 and MnO x follows a radical oxidation pathway. [38] This pathway may be taken due to H 2 O 2 as a source of OH radicals when decomposed homolytically.…”

Section: Catalytic Effectsmentioning

confidence: 99%

Efficient and green oxidative degradation of methylene blue using Mn-doped ZnO nanoparticles (Zn₁₋_xMn_xO)

Khaksar

Amini

Boghaei

2015

Journal of Experimental Nanoscience

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Mn-doped ZnO nanoparticles, Zn 1¡x Mn x O, were synthesised by a polyethylene glycol (PEG) solÀgel method and the physicochemical properties of compounds were characterised by atomic absorption spectroscopy (AAS), energy-dispersive X-ray analysis, X-ray diffraction, scanning electron microscopy and transmission electron microscopy. The catalytic degradation of an organic dye, methylene blue (MB), in the presence of Zn 1¡x Mn x O as the catalyst and hydrogen peroxide (H 2 O 2 ) as the oxidant at room temperature in water has been studied. Effects of oxidant, catalyst amount, catalyst composition, pH value of the solution and an OH-radical scavenging agent on the degree of the decomposition of MB dye were also studied.

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“…Excess use of various dyes in the textile industry has led to the severe surface water and groundwater contamination due to release of toxic and colored effluents (Salem and El-Maazawi, 2000). It is important for the sake of increasing amount, its selection and resistance to biological destruction (Fung et al, 1999;Sohrabi and Ghavamia 2008).…”

Section: Introductionmentioning

confidence: 99%

Synthesis of α-Bi4V2O11 and its Sonocatalytic Activity for the Degradation of Rhodamine B

Kumar¹,

Sahare²

2014

JLA

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A simple method for preparing highly sonoactive nano-sized bismuth vanadate (α-Bi4V2O11) was prepared by combustion technique. The prepared α-Bi4V2O11 powders were characterized by X-ray diffraction (XRD) and transmission electron microscope (TEM). High-resolution TEM images displayed well defined Braggs planes having interplaner distances (dhkl) 3.04Å and 3.12Å, which were in good agreement with the (025) at 2θ = 30.56 o and (133) at 2θ = 28.04 o planes observed in the XRD pattern of monoclinic α-phase of bismuth vanadate respectively. The ultrasonic degradation of Rhodamine B (Rh B) was studied in the absence of catalyst and in the presence of catalyst. The rate of degradation of catalyzed reaction was higher than that obtained with in the absence of the catalysts. The observed pseudo-first-order rate constant increased from 0.010 min -1 to 0.017 min -1 as the concentration of catalyst Rh B increased from 0.03 mg/ml to 0.33 mg/ml. The possible reaction mechanism of sonocatalytic degradation of Rh B over α-Bi4V2O11 has also been discussed. Thus, in this paper we have concluded that bismuth vanadate is a stable and efficient catalyst for the industrial waste-water treatment.

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Kinetics and mechanism of color removal of methylene blue with hydrogen peroxide catalyzed by some supported alumina surfaces

Cited by 208 publications

References 18 publications

Antimicrobial Activity of Some Medicinal Plants from Malaysia

Antimicrobial Activity of Some Medicinal Plants from Malaysia

Efficient and green oxidative degradation of methylene blue using Mn-doped ZnO nanoparticles (Zn₁₋_xMn_xO)

Synthesis of α-Bi4V2O11 and its Sonocatalytic Activity for the Degradation of Rhodamine B

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Kinetics and mechanism of color removal of methylene blue with hydrogen peroxide catalyzed by some supported alumina surfaces

Cited by 208 publications

References 18 publications

Antimicrobial Activity of Some Medicinal Plants from Malaysia

Antimicrobial Activity of Some Medicinal Plants from Malaysia

Efficient and green oxidative degradation of methylene blue using Mn-doped ZnO nanoparticles (Zn1−xMnxO)

Synthesis of α-Bi4V2O11 and its Sonocatalytic Activity for the Degradation of Rhodamine B

Contact Info

Product

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Efficient and green oxidative degradation of methylene blue using Mn-doped ZnO nanoparticles (Zn₁₋_xMn_xO)