Photocatalytic intrinsic reaction kinetics. II: Effects of oxygen concentration on the kinetics of the photocatalytic degradation of dichloroacetic acid

2005 ◽  
Vol 60 (15) ◽  
pp. 4311-4322 ◽  
Author(s):  
Cristina Susana Zalazar ◽  
Carlos Alberto Martin ◽  
Alberto Enrique Cassano
Keyword(s):  
Photocatalytic Degradation ◽  
Reaction Kinetics ◽  
Oxygen Concentration ◽  
Dichloroacetic Acid ◽  
Kinetics Of

Reaction kinetics of photocatalytic degradation of sulfosalicylic acid using TiO2 microspheres

2009 ◽  
Vol 163 (2-3) ◽  
pp. 1101-1106 ◽  
Author(s):  
Chuan Wang ◽  
Xianghua Zhang ◽  
Hong Liu ◽  
Xiangzhong Li ◽  
Wenzhao Li ◽  
...  
Keyword(s):  
Photocatalytic Degradation ◽  
Reaction Kinetics ◽  
Sulfosalicylic Acid ◽  
Tio2 Microspheres ◽  
Kinetics Of

Kinetics of TiO2/Polyurethane Films for Degradation of Organic Pollutants in Water

2012 ◽  
Vol 610-613 ◽  
pp. 1560-1564
Author(s):  
Ruo Kun Jia ◽  
Yang Yu ◽  
Song Zhu Lin ◽  
Na Bai
Keyword(s):  
Photocatalytic Degradation ◽  
Reaction Kinetics ◽  
Sol Gel ◽  
Initial Concentration ◽  
First Order ◽  
Film Forming ◽  
Polyurethane Film ◽  
Degradation Reaction ◽  
Phenolic Wastewater ◽  
Kinetics Of

In this paper,TiO2was prepared by the sol-gel Method,which has high activity and oxidation abilities .The polyurethane is famous for its transmittance and film forming properties,we use polyurethane and titanium dioxide to produce TiO2/polyurethane films. In this paper, phenolic wastewater was considered as the research object,Discussed photocatalytic properties and photocatalytic reaction kinetics model of TiO2/polyurethane film at 253.7nm UV irradiation.The results show that degradation rate of phenolic wastewater approached to 14.6mg.L-1.h-1.m2-1 when Ti02dosage of 60 mg/L,reaction time of 240 min,Phenolic wastewater initial concentration of 10mg/L and pH5.0.The dosage of TiO2,wastewater initial concentration and pH have significant influence on apparent first-order rate constants of photocatalytic degradation,Reaction kinetics of photocatalytic degradation to phenolic wastewater accordances with the quasi-one grade equation of Langmuir-Hinshelwood.

Impact Of Synthesis Route on the Water Oxidation Kinetics of Hematite Photoanodes

2020 ◽  
Author(s):  
Camilo A. Mesa ◽  
Ludmilla Steier ◽  
Benjamin Moss ◽  
Laia Francàs ◽  
James E. Thorne ◽  
...  
Keyword(s):  
Oxygen Vacancy ◽  
Reaction Kinetics ◽  
Water Oxidation ◽  
Oxidation Kinetics ◽  
Oxidation Reaction ◽  
Charge Accumulation ◽  
Optical Signals ◽  
Current Voltage ◽  
Voltage Performance ◽  
Kinetics Of

<p><i>Operando</i> spectroelectrochemical analysis is used to determine the water oxidation reaction kinetics for hematite photoanodes prepared using four different synthetic procedures. Whilst these photoanodes exhibit very different current / voltage performance, their underlying water oxidation kinetics are found to be almost invariant. Lower photoanode performance was found to correlate with the observation of optical signals indicative of charge accumulation in mid-gap oxygen vacancy states, indicating these states do not contribute directly to water oxidation.</p>

Chemical Analysis and Reaction Kinetics of EA-2192 in Decontamination Solution for the MMD-1 Project

2003 ◽  
Author(s):  
David J. McGarvey ◽  
H. D. Durst ◽  
William R. Creasy ◽  
Jill L. Ruth ◽  
Kevin M. Morrissey
Keyword(s):  
Chemical Analysis ◽  
Reaction Kinetics ◽  
Kinetics Of ◽  
Decontamination Solution

Kinetics of catalytic conversion of methanol at higher pressures

1980 ◽  
Vol 45 (12) ◽  
pp. 3402-3407 ◽  
Author(s):  
Jaroslav Bartoň ◽  
Vladimír Pour
Keyword(s):  
Low Temperature ◽  
Reaction Kinetics ◽  
Water Vapour ◽  
Kinetic Data ◽  
Catalytic Conversion ◽  
The Given ◽  
Kinetics Of

The course of the conversion of methanol with water vapour was followed on a low-temperature Cu-Zn-Cr-Al catalyst at pressures of 0.2 and 0.6 MPa. The kinetic data were evaluated together with those obtained at 0.1 MPa and the following equation for the reaction kinetics at the given conditions was derived: r = [p(CH3OH)p(H2O)]0.5[p(H2)]-1.3.

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