Effects of salts on the kinetics of oxidation of alkenes by thallic salts in aqueous solutions

1981 ◽  
Vol 46 (3) ◽  
pp. 693-700 ◽  
Author(s):  
Milan Strašák ◽  
Jaroslav Majer
Keyword(s):  
Aqueous Solutions ◽  
Phase Transfer ◽  
Heterogeneous Reaction ◽  
Qualitative Model ◽  
Kinetic Effect ◽  
Tetraalkylammonium Salts ◽  
Reaction Conditions ◽  
Kinetics Of Oxidation ◽  
Kinetics Of ◽  
Heterogeneous Reaction Conditions

The kinetics of oxidation of alkenes by thallic sulphate in aqueous solutions, involving the two reaction steps-the hydroxythallation and the dethallation - was studied, and the effect of salts on the kinetics was examined; this made it possible to specify more precisely the reaction mechanism and to suggest a qualitative model of the reaction coordinate. It was found that in homogeneous as well as in heterogeneous reaction conditions, the reaction can be accelerated appreciably by adding tetraalkylammonium salts. These salts not only operate as catalysts of the phase transfer, but also exert a significant kinetic effect, which can be explained with a simplification in terms of a stabilization of the transition state of the reaction.

Kinetics of oxidation of aliphatic alcohols by ozone in aqueous solutions

1999 ◽  
Vol 68 (2) ◽  
pp. 257-263 ◽  
Author(s):  
A. Ya. Gerchikov ◽  
Yu. S. Zimin ◽  
N. V. Trukhanova ◽  
V. N. Evgrafov
Keyword(s):  
Aqueous Solutions ◽  
Aliphatic Alcohols ◽  
Kinetics Of Oxidation ◽  
Kinetics Of

Kinetics of oxidation of ponceau 4R in aqueous solutions by Fenton and photo-Fenton processes

2011 ◽  
Vol 105 (2) ◽  
pp. 293-306 ◽  
Author(s):  
Cristina Benincá ◽  
Patrício Peralta-Zamora ◽  
Ronaldo Cardoso Camargo ◽  
Célia Regina Granhen Tavares ◽  
Everton Fernando Zanoelo ◽  
...  
Keyword(s):  
Aqueous Solutions ◽  
Kinetics Of Oxidation ◽  
Ponceau 4R ◽  
Kinetics Of

KINETICS OF THE OXIDATION OF URANIUM (IV) BY IRON (III) IN AQUEOUS SOLUTIONS OF PERCHLORIC ACID

1955 ◽  
Vol 33 (12) ◽  
pp. 1780-1791 ◽  
Author(s):  
R. H. Betts
Keyword(s):  
Electron Transfer ◽  
Ionic Strength ◽  
Aqueous Solutions ◽  
Perchloric Acid ◽  
Rate Constants ◽  
Kcal Mole ◽  
Kinetics Of Oxidation ◽  
Temperature Coefficients ◽  
Kinetics Of ◽  
Rate Controlling Step

The kinetics of oxidation of uranium (IV) by iron (III) in aqueous solutions of perchloric acid have been investigated at four temperatures between 3.1 °C. and 24.8 °C. The reaction was followed by measurement of the amount of ferrous ion formed. For the conditions (H+) = 0.1–1.0 M, ionic strength = 1.02, (FeIII) = 10−4–10−5 M, and (UIV) = 10−4–10−5 M, the observed rate law is d(Fe2+)/dt = −2d(UIV)/dt[Formula: see text]K1 and K2 are the first hydrolysis constants for Fe3+ and U4+, respectively, and K′ and K″ are pseudo rate constants. At 24.8 °C., K′ = 2.98 sec.−1, and K″ = 10.6 mole liter−1 sec−1. The corresponding temperature coefficients are ΔH′ = 22.5 kcal./mole and ΔH″ = 24.2 kcal./mole. The kinetics of the process are consistent with a mechanism which involves, as a rate-controlling step, electron transfer between hydrolyzed ions.

scholarly journals 1,4-Dioxane Degradation Using Persulfate Ion and Ag(I) Ion

2017 ◽  
Vol 57 (2) ◽  
Author(s):  
Rosa María Felix-Navarro ◽  
Wai Lin Shui ◽  
Arturo Zizumbo-López ◽  
Sergio Pérez-Sicairos ◽  
Edgar Alonso Reynoso-Soto ◽  
...  
Keyword(s):  
Sulfuric Acid ◽  
Aqueous Solutions ◽  
Reaction Rate ◽  
Experimental Results ◽  
Kinetics Of Oxidation ◽  
Decay Model ◽  
Increasing Temperature ◽  
Kinetics Of

The kinetics of oxidation of 1,4-dioxane by persulfate ion with Ag+ in aqueous solutions at various temperatures and concentrations of S<sub>2</sub>O<sub>8</sub><sup>2-</sup>, Ag<sup>+</sup> and H<sub>2</sub>SO<sub>4</sub>, were investigated. Experimental results indicate that 1,4-dioxane degradation follows a pseudo-firstorder decay model and that reaction rate significantly accelerate by increasing temperature and concentration of oxidant, sulfuric acid and Ag<sup>+</sup> ions up to 0.46 mM; for the range from 0.46-0.70 mM of Ag<sup>+</sup> ions the reaction rate remains constant and at higher concentrations the reaction rate decreases. It was possible to degrade approximately 100% of 1,4-dioxane in less than one hour with the following conditions: [Ag<sup>+</sup>] = 0.46 mM, H<sub>2</sub>SO<sub>4</sub>] = 0.30 M and from a concentration of 25 mM Na<sub>2</sub>SO<sub>4</sub>.

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