Rate constant of the hydroxy radical + hydrogen peroxide .fwdarw. hydroperoxo radical + water reaction

1983 ◽  
Vol 87 (22) ◽  
pp. 4467-4470 ◽  
Author(s):  
John J. Lamb ◽  
Luisa T. Molina ◽  
Craig A. Smith ◽  
Mario J. Molina
Keyword(s):  
Hydrogen Peroxide ◽  
Rate Constant ◽  
Hydroxy Radical

scholarly journals Photochemical Degradation of Sulfadiazine

2013 ◽  
Vol 39 (3) ◽  
pp. 79-91 ◽  
Author(s):  
Natalia Lemańska-Malinowska ◽  
Ewa Felis ◽  
Joanna Surmacz-Górska
Keyword(s):  
Hydrogen Peroxide ◽  
Uv Radiation ◽  
Hydroxyl Radicals ◽  
Rate Constant ◽  
Photochemical Degradation ◽  
Photochemical Processes

Abstract The photochemical degradation of the sulfadiazine (SDZ) was studied. The photochemical processes used in degradation of SDZ were UV and UV/H2O2. In the experiments hydrogen peroxide was applied at different concentrations: 10 mg/dm3 (2.94*10-4 M), 100 mg/dm3 (2.94*10-3 M), 1 g/dm3 (2.94*10-2 M) and 10 g/dm3 (2.94*10-1 M). The concentrations of SDZ during the experiment were controlled by means of HPLC. The best results of sulfadiazine degradation, the 100% removal of the compound, were achieved by photolysis using UV radiation in the presence of 100 mg H2O2/dm3 (2.94*10-3 M). The determined rate constant of sulfadiazine reaction with hydroxyl radicals kOH was equal 1.98*109 M-1s-1.

scholarly journals THE RATE CONSTANT OF THE REACTION BETWEEN FERROUS IONS AND HYDROGEN PEROXIDE IN ACID SOLUTION

1957 ◽  
Vol 35 (5) ◽  
pp. 428-436 ◽  
Author(s):  
T. J. Hardwick
Keyword(s):  
Hydrogen Peroxide ◽  
Acid Solution ◽  
Sulphuric Acid ◽  
Acid Concentration ◽  
Rate Constant ◽  
Perchloric Acid ◽  
Ferrous Ion ◽  
Ferrous Ions ◽  
Bimolecular Rate Constant

Identical values of the bimolecular rate constant of the ferrous ion – hydrogen peroxide reaction were obtained from intercomparisons of the methods previously used in following this reaction. In perchloric acid the bimolecular rate constant is unaffected by acid concentration; in sulphuric acid it increases slightly in acid concentrations above 10−2N. The results agree with and explain the differences between those obtained by Baxendale and by Dainton, but are only in marginal agreement with those recently reported by Weiss.

The Rate Constant of the Reaction between Hydrogen Peroxide and Ferrous Ions

1953 ◽  
Vol 21 (8) ◽  
pp. 1419-1420 ◽  
Author(s):  
William Taylor ◽  
Joseph Weiss
Keyword(s):  
Hydrogen Peroxide ◽  
Rate Constant ◽  
Ferrous Ions

Kinetics of the oxidation of diphenyl sulfide with hydrogen peroxide catalyzed by sodium metavanadate

1982 ◽  
Vol 60 (7) ◽  
pp. 848-852 ◽  
Author(s):  
Yoshiro Ogata ◽  
Kazushige Tanaka
Keyword(s):  
Hydrogen Peroxide ◽  
Rate Constant ◽  
Reaction Rate ◽  
Catalytic Amount ◽  
Probable Mechanism ◽  
Initial Concentration ◽  
Sodium Metavanadate ◽  
Low Concentration ◽  
Diphenyl Sulfide ◽  
Kinetics Of

The oxidation of diphenyl sulfide (Ph2S) by hydrogen peroxide in the presence of a catalytic amount of sodium metavanadate (NaVO3) has been studied kinetically by means of iodometry of hydrogen peroxide. The reaction rate is expressed as: v = k[NaVO3]st[Ph2S]2, when the concentration of catalyst is very low and [Ph2S]0/[H2O2]0 > 2, where []st and []0 mean stoichiometric and initial concentration, respectively. The effective oxidant may consist of polymeric as well as monomeric peroxyvanadate in view of the effect of concentration of catalyst on the rate. The main oxidizing species at low concentration of catalyst seems to be diperoxyvanadate VO5−. The rate constant k2 in v = k2[Ph2S]2 tends to decrease with initial concentration of H2O2, which is present in excess of the catalyst. A probable mechanism for the oxidation is discussed.

Influence of Natural Organic Matter on Oxidation of Volatile Organic Compounds by the H2O2/VisUV Process

1997 ◽  
Vol 2 (3) ◽  
Author(s):  
James M. Symons ◽  
Charlene M. Baker ◽  
H. William Prengle
Keyword(s):  
Hydrogen Peroxide ◽  
Rate Constant ◽  
Reaction Rate ◽  
Tap Water ◽  
Reaction Rate Constant ◽  
Photon Flux ◽  
Excess Hydrogen ◽  
Volatile Organic ◽  
Natural Organic Material ◽  
Experimental Runs

AbstractThis paper presents experimental research to determine the affect of background natural organic material (NOM) on the conversion of five (5) VOC's: 1,1,1-trichloroethane (TCA), benzene (BNZ), trichloroethylene (TCE), 1,4-dichlorobenzene (DCB), and tetrachloroethylene (PCE). Experiments were conducted using DI water and Houston tap water ([TOC] = 3.6 mg/L) as solvents. In addition, the affects of buffer form and excess hydrogen peroxide were determined. Experimental runs were conducted in a photochemical-flow-stirred-tank reactor (pcfSTR), using a 450 W visible/ultraviolet radiation source. The data were analyzed using the Prengle- Shimoda reaction rate model, yielding the reaction rate constant ka (μmols A conv/min, Lr, photon flux) for comparison purposes. Analysis of the experimental data indicated the following conclusions: 1) At the concentrations used for bicarbonate or phosphate buffer, little or no affect was observed; 2) The presence of NOM surpressed the reaction rate for three of the compounds, TCA, BNZ, and PCE at the 95 % confidence level; and 3) Excess hydrogen peroxide, beyond the stoichiometric value, increased the reaction rate constant for all five compounds. The greatest increase was seen for DCB.

Theory of Copper-Electrolyte Slimes Decoppering in the Presence of Hydrogen Peroxide

2019 ◽  
Vol 946 ◽  
pp. 585-590
Author(s):  
V.G. Lobanov ◽  
K.D. Naumov ◽  
A.A. Korolev
Keyword(s):  
Hydrogen Peroxide ◽  
Dissolution Rate ◽  
Rate Constant ◽  
Chemical Transformations ◽  
Composition Effect ◽  
Rotating Disc ◽  
Copper Dissolution ◽  
Copper Leaching ◽  
Copper Electrolyte ◽  
Dissolution Rate Constant

The problem of copper leaching from copper-electrolyte slimes is discussed. To intensify the long and costly process, it is proposed to use a leaching system containing sulfuric acid and hydrogen peroxide as an oxidizing agent. The chemical transformations possible variants at the treatment of slime under the specified conditions and the thermodynamic parameters of the predicted reactions are considered. Solution composition effect on the copper dissolution rate at room temperature was studied in the presence of hydrogen peroxide using the rotating disc technique. It is found that dissolution rate constant at using hydrogen peroxide slightly inferior to dissolution rate constant under autoclaved conditions in an oxygen atmosphere.

Sign in / Sign up

Export Citation Format

Share Document