A kinetic study of the oxidation of N(III) by ClO2− in aqueous acidic media

1980 ◽  
Vol 58 (2) ◽  
pp. 159-163 ◽  
Author(s):  
Samir S. Emeish ◽  
Keith E. Howlett
Keyword(s):  
Kinetic Study ◽  
Rate Equation ◽  
Nitrous Acid ◽  
Hypochlorous Acid ◽  
Chloride Ion ◽  
Acidic Media ◽  
Kinetics Of

Kinetics of the reaction between nitrous acid and chlorite have been studied spectrophotometrically. The rate equation involves terms [HNO2]1.5 and [ClO2−]0.5, and both an uncatalysed and a chloride ion-catalysed path have been identified. A mechanism involving peroxonitrite and hypochlorous acid as intermediates is shown to be consistent with the observations.

The oxidation of uranium(IV) ions by nitrous acid in 30% tri-butyl phosphate

2004 ◽  
Vol 92 (7) ◽  
Author(s):  
V. S. Koltunov ◽  
Robin J. Taylor ◽  
V. I. Marchenko ◽  
O. A. Savilova ◽  
K. N. Dvoeglazov
Keyword(s):  
Rate Equation ◽  
Nitrous Acid ◽  
Kinetics Of

SummaryThe kinetics of the oxidation of U(IV) ions by nitrous acid in a 30% TBP solution have been determined. The rate equation was found to be:-d[U(IV)]/dwhere,

N-Chlorination of secondary amides. I. Kinetics of N-chlorination of N-methyl acetamide

1969 ◽  
Vol 47 (14) ◽  
pp. 2561-2567 ◽  
Author(s):  
M. Wayman ◽  
E. W. C. W. Thomm
Keyword(s):  
Rate Constants ◽  
Reaction Rate ◽  
Hypochlorous Acid ◽  
Chloride Ion ◽  
Active Species ◽  
Ion Concentration ◽  
Kcal Mole ◽  
Ph Range ◽  
Kinetics Of ◽  
Secondary Amides

The rate of N-chlorination of N-methyl acetamide has been studied in acetate buffered hypochlorous acid solutions. The reaction rate is dependent upon pH, chloride ion concentration, and acetic acid concentration. The results fit the following rate expression[Formula: see text]The observed rate constant, kobs, has three components[Formula: see text]The results suggest that the active chlorinating species in the pH range 3.0–6.0 are HOCl, Cl2, and CH3COOCl, in order of increasing reactivity. The values of the corresponding rate constants at 25 °C are [Formula: see text], and [Formula: see text] l mole−1 min−1, the last two rate constants being related to k2 and k3 through the respective equilibrium constants.At temperatures near room temperature, the N-chlorination reaction has an apparent activation energy of 14 kcal/mole when Cl2 is the active species, and 5 kcal/mole when CH3COOCl is the chlorinating agent.

Kinetics of catalytic reduction of nitrogen oxide by carbon monoxide on CuO/Al2O3 catalyst

1983 ◽  
Vol 48 (11) ◽  
pp. 3202-3208 ◽  
Author(s):  
Zdeněk Musil ◽  
Vladimír Pour
Keyword(s):  
Carbon Monoxide ◽  
Nitrogen Oxide ◽  
Rate Equation ◽  
Catalytic Reduction ◽  
Zero Order ◽  
Spectroscopic Measurements ◽  
First Order ◽  
Ir Spectroscopic ◽  
Kinetics Of ◽  
Al2o3 Catalyst

The kinetics of the reduction of nitrogen oxide by carbon monoxide on CuO/Al2O3 catalyst (8.36 mass % CuO) were determined at temperatures between 413 and 473 K. The reaction was found to be first order in NO and zero order in CO. The observed kinetics are consistent with a rate equation derived from a mechanism proposed on the basis of IR spectroscopic measurements.

A kinetic study on the action of rubber oxidation inhibitors—III. Kinetics of inhibited oxidation

1964 ◽  
Vol 6 (6) ◽  
pp. 1208-1215
Author(s):  
Kh.S. Bagdasar'yan ◽  
R.I. Milyutinskaya
Keyword(s):  
Kinetic Study ◽  
Inhibited Oxidation ◽  
Oxidation Inhibitors ◽  
Kinetics Of

A Kinetic Study of the Thermal Isomerization of and Related Complexes

1975 ◽  
Vol 53 (12) ◽  
pp. 1735-1738 ◽  
Author(s):  
William R. Cullen ◽  
Frank L. Hou
Keyword(s):  
Kinetic Study ◽  
Thermal Isomerization ◽  
Isomerization Reaction ◽  
Kinetics Of

The kinetics of the unimolecular isomerization reaction[Formula: see text]have been studied. The ΔH≠ values in kcal mol−1 are 36.8 ± 2.0 (M = M′ = Mn ), 46.8 ± 0.5 (M = M′ = Re ), 39.2 ± 2.8 (M = Mn, M′ = Re ). The mechanism of the rearrangement is discussed.

Kinetics of oxygen reduction reaction at electrochemically fabricated tin-palladium bimetallic electrocatalyst in acidic media

2010 ◽  
Vol 56 (1) ◽  
pp. 285-290 ◽  
Author(s):  
Md. Rezwan Miah ◽  
Jahangir Masud ◽  
Takeo Ohsaka
Keyword(s):  
Oxygen Reduction Reaction ◽  
Oxygen Reduction ◽  
Reduction Reaction ◽  
Acidic Media ◽  
Kinetics Of

The kinetics of the decarboxylation of β-resorcylic acid in catechol

1976 ◽  
Vol 29 (2) ◽  
pp. 443 ◽  
Author(s):  
MA Haleem ◽  
MA Hakeem
Keyword(s):  
Rate Equation ◽  
Kinetic Data ◽  
Reaction Rate ◽  
Complex Mechanism ◽  
First Order ◽  
Absolute Reaction Rate ◽  
First Time ◽  
Kinetics Of ◽  
Absolute Reaction ◽  
Reaction Rate Equation

Kinetic data are reported for the decarboxylation of β-resorcylic acid in resorcinol and catechol for the first time. The reaction is first order. The observation supports the view that the decomposition proceeds through an intermediate complex mechanism. The parameters of the absolute reaction rate equation are calculated.

ChemInform Abstract: DETRITIATION KINETICS OF ACETOPHENONES IN HIGHLY ACIDIC MEDIA

1977 ◽  
Vol 8 (8) ◽  
pp. no-no
Author(s):  
D. W. EARLS
Keyword(s):  
Acidic Media ◽  
Kinetics Of
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