Heterogeneous photocatalytic degradation of methylene blue aqueous solution under the coexistence of metalloporphyrin polymer and air An Taicheng, Gao Jinzhang#, Chen Hui#, Zhu Xihai( #Department of Chemistry, Northwest Normal University, Lanzhou, 730070; School of Chemistry and Chemical Engineering, Zhongshan University, Guangzhou, 510275, China.) Received Sep. 21, 2000; Supported by the National Natural Science Foundation of China (No.29977030) and Natural Science Foundation of Gansu (No. zs-981-A24-058-Y) Abstract High pressure mercury lamp (HPML) was used for irradiation, the kinetics of photocatalytic degradation of methylene blue (MB) in water with air sparging has been investigated in the presence of Polymeric[Co(II)meso-Tetra(4,4'-Biphenylbisulfony)-phenyl porphyrin]. Chemical Oxygen Demand (COD) proximately dropped by half, with the decolourizing efficiency being about 50-60% after 8 hours. The changes of the visible spectra and the kinetics curve of reaction were measured. It was observed that photocatalytic degradation of MB obey pseudo first-order reaction with the apparent first-order decay constant k= 0.3544 h-1, half life 1.96 h. Compared with HPML, natural sunlight (NSL) had similar effect on the photocatalytic degradation of MB. The effects of a variety of factors such as pH, irradiation sources and initial concentration of MB were discussed. MB in water could degrad within 3 h in the presence of metalloporphyrin polymer and diluted solution of hydrogen peroxide.Keywords Photocatalytic degradation, Methylene blue, Metalloporphyrin, Kinetics The issue of treatment of organic pollutants
in water is an ever increasingly global problem because many organic contaminants are
inevitable byproducts of industry and agriculture. In 1980s, the total production of
synthesized dyes alone was more than 800 thousand tons per year. In the course of
production and utilization, a significant amount of dye-containing wastewater was
discharged into receiving water. 1.1 Materials Polymeric Co[meso-Tetra (4,4'-Biphenylbisulfony)phenyl-porphyrin] (Co[P(TBPSOPP)]) was prepared, purified and characterized as previously reported [10], and visible spectra of polymeric ligand exhibits a soret band at 422.1 nm, with the Q bands at 524.2, 558.7, 599.0, and 658.2 nm. The soret band varied little and the Q bands decreased from 5 to 2 with the ligand coordinating with metals. MB was obtained from Chmond Rd. (London) and used without further purification. The tanked oxygen was used and air was sparged with an air pump. The other reagents were analytical grade and all the solutions were prepared with double-distilled water. 1.2 Recommended procedure 5 mg of Co[P(TBPSOPP)] was added into a quartz double-layered reactor (self-designed) containing 35 ml of 3.74 mg/L MB solution, then stirred with 78HW-1 magnetic stirrer prior to irradiation with 450 W HPML. With air sparging, photocatalytic degradation took place in the reactor. Water was recycled in a 501 model thermostatic bath and the temperature of the reactor kept at 20°C except for the temperature experiments. The absorbance of the sample solution were determined on model UV-754 spectrophotometer at 664 nm with glass cells (10 mm optical path length) every hour after standing for 5 minutes. Experiments performed under NSL were carried out in August and September in Lanzhou, Gansu, China (East longitude 103°53' and North latitude 36°03'). 1.3 Calibration curve A calibration curve was obtained for MB and found to be linear in the range of 0.75-7.5 mg/L. The MB concentrations and absorbances were well correlated with the regression equation as follows: A=0.0139 +0.1439×C (R = 0.9979) where A is the absorbance of the MB; C is the concentration of MB (mg/L) and R is the regression coefficient for the straight line. 2. RESULTS 2.1 The kinetics of photocatalytic degradation of MB solution In the presence of Co[P(TBPSOPP)], the change of the visible spectra and the kinetics of photocatalysis of MB were investigated at pH 6.6. The contrast degradation curve of MB is shown in Fig. 1. From the relevant data, it can be seen that MB dramatically decrease with the increase of irradiation time . It was found that the logarithmic values of the concentrations of MB solution was presented in Fig.2 as a straight line with the increase of irradiation time. This indicates that the photocatalytic degradation of MB obeyed pseudo first-order kinetics. The rate equation can be represented as follows: lnCt = lnC0 -kt
a: No catalyst and in the dark; b: Absorption under 5mg catalyst and no illumination. c: No catalyst plus HPML; d: Absorption under 5 mg catalyst , HPML plus air pumping; e: Absorption under 5 mg catalyst, HPML, air pumping plus H2O2. Compared with HPML, NSL
had similar effect on the photocatalytic degradation of MB. The process also conformed the
pseudo first-order kinetics.( Fig.2 ) The kinetics regression equations were shown below
respectively:
a: NSL; b: 450 W HPML. 2.2 Determination of COD
2.3 Determination of decolourization
rate
*The absorbance of Pt-Co standard chromaticity was determined with a model 721 spectrophotometer [12] .2.4 Recovery of photocatalyst 3.1 The contrast disappearance of MB Results of the photo-decomposition of MB in various conditions are presented in Fig. 1. It was shown that the concentrations of MB decreased with the increase of irradiation time. From curve (a) of Fig. 1 the absorbance did not vary at all and the slope is plat. It is well known that MB can be absorbed onto solid easily, but from curve (b), only a small amount of MB could be absorbed onto photocatalyst without irradiation. Only 10 per cent of MB could be photodegraded when illuminated with HPML in the absence of metalloporphyrin in curve (c), although MB have been used as a sensitizer in previous reports [13,14] for the photocatalytic degradation of organic contaminants in water. In curve (d), with added photocatalyst and illuminated with HPML, MB decreased rapidly and photocatalytically degraded completely within 8 hours with air sparging. The significantly greater slope was obtained for curve (e). The degradation rate greatly speeded up, and the decomposition of MB completely finished within 3 hours in the presence of 2.5×10-2 mol/L hydrogen peroxide. 3.2 Effect of pH The effect of pH was studied in the pH range of 2.90-12.00 by adjusting pH with diluted sodium hydroxide or hydrochloride acid solution. The results shown in Fig. 3 indicate that the effect of pH on photocatalytic degradation rate was noticeable. The degradation rates of MB increase distinctly with the increase of the pH value. Fig.3 The pH effect on the degradation a: pH 2.9; b: pH 4.2; c: pH 6.6; d: pH 9.3; e: pH 12.0. 3.3 Effect of working temperature Table 3. The kinetic parameters of temperature effect
3.4 Effect of oxidants a: Air-Sparge; b: Oxygen-sparge; c: H2O2 plus air-sparge. 3.5 Effect of initial concentration
of MB Table 4 the kinetic parameters in various initial concentration of MB
3.6 Effect of amount of photocatalyst MB aqueous solution can be degraded with irradiation with both HPML and NSL in the presence of Co[P(TBPSOPP)]. The degradation of MB in water obeys pseudo first-order reaction. Photocatalyst can be deposited and recycled without second pollution. After 8 hrs photocatalytic degradation, the dyestuff (MB) can be completely decolourized with the solution becoming colorless; the COD concentrations of dyestuff also dropped apparently. The photocatalytic degradation of MB in water could be greatly accelerated in the presence of hydrogen peroxide. REFERENCES [1] Matihews P W. Wat. Res., 1991, 25 (10): 1169. [2] Wang Q Q, Jiang W C, Bao Y Y et al. Environment pollution & control, 1992, 14 (1): 2. [3] Ollis D F, Pelizzetti E, Serpone N. Environ. Sci. & Technol., 1991, 25 (9): 1523. [4] Wang Q Q, Jiang W C. (Huanjing Kexue yu Jishu), 1994, 66 (3): 1. [5] Matthews R W. Pure & Appl, 1992, 64 (9): 1285. [6] Polo E, Amadelli R, Carassiti V et al. Inorg. Chim. Acta, 1992, 192: 1. [7] Chen H, An T C, Fang Y J et al. J. Mol. Catal. A: Chem., 1999, 147 (1-2): 165. [8] Chen H, An T C, Fang Y J et al. Indian J. Chem., B: 1999, 38 (7): 185. [9] Maldotti A, Bartocci C et al. Inorg.Chem., 1996, 35: 1126-1131. [10] Wan R M, Li S B, Wang Y P et al. J.Appl.Polym.Sci., 1998, 67: 2027. [11] EPA of China. The Methods for Water and Wastewater monitoring & Analysis (3rd edition), Beijing: China Environmental Technolge & Science Press, 1989, 354. [12] Zhou J J. Electroplating and Environmental Protection, 1988, 8 (2): 35. [13] Acher A, Fischer E, Zellingher R et al. Wat. Res. 1990, 24 (7): 837. [14] Li X Z. Technology of water treatment, 1984, 10 (1): 7. [15] Fujihira M et al. Bull. Chem. Soc. Jpn., 1982, 55: 666. [16] Wei H B, T Li, Yan X S. Advance Environ. Sci., 1994 , 2: 50. |
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