Photocatalytic Activity Investigation

Photocatalytic Activity InvestigationThe photocatalytic activity of the modified samples was investigated by the determination of the remaining concent ration of the nominated pollutant, acetaldehyde, over various time intervals. Figures. 5 and 6 show the photodecomposition activity of different modified TiO nanoparticles chthonic 8w visible fall down irradiation in the continuous turn tail reactor with a flow rate of 95 ml/min.According to Figures. 5 and 6, all the modified samples show much higher photocatalytic activity than the small TiO, confirming that N and Co doping is an effective way of improving the photocatalytic activity. The highest activity was observed for 1%Co-N-TiO sample, and the 50 min irradiation by visible light resulted in 44.2% of acetaldehyde degradation for this sample.The increased visible light absorption and specific surface atomic number 18a are key factors that influenced the photoactivity of the different modified samples under visible light irra diation compared to pure TiO2.The decrease in the particle size and increase in the BET surface area (Table 1) contribute to the improvement of the acetaldehyde degradation. Table 1 shows that the crystallite size of samples decreases from 21.9 to 14.7 nm this decrease may be beneficial for the photocatalytic activity. Compared with the N-TiO2 sample, Co-N/TiO2 photocatalysts have a with child(p)r surface area, which increases the photoactivity rate because of the large amounts of acetaldehyde molecules being adsorbed on the photocatalytic surface and easily reacted by photogenerated oxidizing species.The light absorption characteristics of the modified samples are extended towards the visible light region subsequently N and Co doping, which implies that the formation of photogenerated charge carriers will be increased under visible light irradiation. Also, cobalt doping with a low cobalt satisfy can act as a charge trap to prevent electron-hole recombination and improve the in terfacial charge channelise to degrade acetaldehyde. After the optimal doping ratio of cobalt was exceeded (1wt % Co-N-TiO2), reduced photocatalytic activity was observed. This result can be due to the coverage of the surface of photocatalyst with increased cobalt ions (Co2+) which inhibited interfacial charge transfer due to inadequate amount of light energy available for activation of all the photocatalyst particles. Also due to excessive concentration, Co particles acting as recombination centers for photogenerated electrons and holes .establish on the acetaldehyde degradation results in this study, it is therefore evident that photocatalytic activity is strongly dependent on the doping ratio rather than the band gap of the samples and activities of the Co-N-TiO2 co-doped samples are higher than those of N-TiO2 or pure TiO2.** Fig. 5 **** Fig. 6 **Kinetic studyThe Langmuir-Hinshelwood kinetic model has been extensively used to describe heterogeneous photocatalysis on si dioxid e . This model successfully describes the kinetic of Eq. (3), which is the reaction between hydroxyl radical and adsorbed acetaldehyde. When the photocatalytic reaction obeys a Langmuir-Hinshelwood model, the relationship between the rate of reaction r (mol g-1 min-1) and the acetaldehyde concentration Cact. (mol l-1) can be described as follows in Eq. (4)Where k is the rate constant (mol g-1 min-1) and Ka is the adsorption constant (l mol-1). many as resumeptions were used in Eq. (4). Only acetaldehyde is adsorbed on the catalyst surface and all intermediates and products desorbed immediately after chemical reaction therefore, they have not been discover in Eq. (4).The mathematical modelling for the plug photoreactor at unsteady condition with the assumption of isothermal condition, ignored diffusion resistance and constant flow rate, the stool balance equation inside the continuous photoreactor would become as follows in Eq. (5)Where Q is the intensivenesstric flow rate (l min- 1), W is the weight of catalyst (g), V is the volume of the reactor (l), and t is the time of experiment (min).Kinetic parameters (k, K) were calculated using the Nelder-Mead method, which was used through computer programming in MATLAB by minimization of sum of squared of relative error, the difference between the calculated and experimental outlet concentration results, as the following objective functionBy minimization of Eq. (6), kinetic parameters (k, Ka) are predicted and shown in Table 3. A good agreement among the predicted and experimental data were found that are shown in Fig. 7.