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 acid-catalyzed demetalation of 1-(tri-n-butylstannyl)-2-phenylethyne. A surprisingly small β-stannyl effect

1996 ◽  
Vol 74 (7) ◽  
pp. 1366-1368 ◽  
Author(s):  
I. Egle ◽  
V. Gabelica ◽  
A.J. Kresge ◽  
T.T. Tidwell
Keyword(s):  
Key Words ◽  
Isotope Effect ◽  
Acid Concentration ◽  
Rate Constant ◽  
Perchloric Acid ◽  
Hydronium Ion ◽  
Stabilizing Effect ◽  
Aromatic Product ◽  
Acid Catalyzed ◽  
The Difference

Rates of conversion of 1-(tri-n-butylstannyl)-2-phenylethyne to phenylethyne in H2O and D2O solutions of perchloric acid were found to be proportional to acid concentration, giving the hydronium ion rate constant [Formula: see text] and the isotope effect [Formula: see text]. The magnitude of this isotope effect suggests that the reaction occurs by rate-determining hydron transfer to the substrate, producing a vinyl carbocation; this carbocation then loses its tributylstannyl group, giving phenylacetylene as the only detectable aromatic product. The hydronium ion rate constant, when compared to the rates of protonation of phenylethyne and 1-(trimethylsilyl)-2-phenylethyne, gives a β-stannyl stabilizing effect of δΔG≠ = 6.6 kcal mol−1 and a differential β-stannyl/β-silyl effect of δΔG≠ = 3.2 kcal mol−1. These stabilizations are very much smaller than previously reported β-stannyl effects. Possible reasons for the difference are suggested. Key words: β-stannyl effect, β-silyl effect, carbocation stabilization, protodemetalation.

The oxidations of DL-atrolactic and 2-hydroxyisobutyric acids by cerium(IV) in sulphuric acid solutions

1970 ◽  
Vol 23 (4) ◽  
pp. 757 ◽  
Author(s):  
VK Grover ◽  
YK Gupta
Keyword(s):  
Complex Formation ◽  
Acid Solution ◽  
Organic Acid ◽  
Sulphuric Acid ◽  
Rate Constant ◽  
Sulphuric Acid Solution ◽  
Acid Solutions ◽  
Rate Law ◽  
Hydroxyisobutyric Acid

Oxidations of DL-atrolactic and 2-hydroxyisobutyric acids by cerium(IV) in sulphuric acid solution occur in accordance with the empirical rate law: (see equation in article) where k1 is a complex rate constant and A is an unspecified constant. Spectrophotometric results suggest complex formation between cerium(1v) and the organic acid, but no kinetic evidence was obtained. Manganese(11) catalyses the reactions. DL-Atrolactic acid is more reactive than 2-hydroxyisobutyric acid. The products of oxidations were acetophenone and acetone respectively.

scholarly journals Leaching of chalcopyrite concentrate by hydrogen peroxide in sulphuric acid solution

Tehnika ◽  
2019 ◽  
Vol 74 (1) ◽  
pp. 66-70 ◽  
Author(s):  
Miroslav Sokić ◽  
Branislav Marković ◽  
Željko Kamberović ◽  
Srđan Stanković
Keyword(s):  
Hydrogen Peroxide ◽  
Acid Solution ◽  
Sulphuric Acid ◽  
Sulphuric Acid Solution ◽  
Chalcopyrite Concentrate

Oxyhalogen-sulfur chemistry — Kinetics and mechanism of the oxidation of cysteamine by acidic iodate and iodine

2006 ◽  
Vol 84 (1) ◽  
pp. 49-57 ◽  
Author(s):  
Alice Chanakira ◽  
Edward Chikwana ◽  
David H Peyton ◽  
Reuben H Simoyi
Keyword(s):  
Acid Concentration ◽  
Rate Constant ◽  
Oxidation Product ◽  
Initial Conditions ◽  
Reaction Dynamics ◽  
Reaction Scheme ◽  
Kinetics And Mechanism ◽  
Sulfur Chemistry ◽  
Bimolecular Rate Constant ◽  
Acidic Conditions

The oxidation of cysteamine by iodate and aqueous iodine has been studied in neutral to mildly acidic conditions. The reaction is relatively slow and is heavily dependent on acid concentration. The reaction dynamics are complex and display clock behavior, transient iodine production, and even oligooscillatory production of iodine, depending upon initial conditions. The oxidation product was the cysteamine dimer (cystamine), with no further oxidation observed past this product. The stoichiometry of the reaction was deduced to be IO3– + 6H2NCH2CH2SH → I– + 3H2NCH2CH2S-SCH2CH2NH2 + 3H2O in excess cysteamine conditions, whereas in excess iodate the stoichiometry of the reaction is 2IO3– + 10H2NCH2CH2SH → I2 + 5H2NCH2CH2S-SCH2CH2NH2 + 6H2O. The stoichiometry of the oxidation of cysteamine by aqueous iodine was deduced to be I2 + 2H2NCH2CH2SH → 2I– + H2NCH2CH2S-SCH2CH2NH2 + 2H+. The bimolecular rate constant for the oxidation of cysteamine by iodine was experimentally evaluated as 2.7 (mol L–1)–1 s–1. The whole reaction scheme was satisfactorily modeled by a network of 14 elementary reactions.Key words: cysteamine, cystamine, Dushman reaction, oligooscillations.

Reduction of chlorothallium(III) complexes by arsenic(III)

1973 ◽  
Vol 26 (10) ◽  
pp. 2115 ◽  
Author(s):  
PD Sharma ◽  
YK Gupta
Keyword(s):  
Ionic Strength ◽  
Acid Solution ◽  
Rate Constant ◽  
Perchloric Acid ◽  
Intermediate Formation ◽  
Chloride Ions ◽  
Hydrogen Ion ◽  
Ion Concentration ◽  
Perchloric Acid Solution ◽  
Hydrogen Ion Concentration

The oxidation of arsenic(III) by thallium(III) in perchloric acid solution is inhibited by chloride ions. The reactivity of various chlorothallium(III) species is in the order Tl3+ > TlCl2+ > TlCl2+ > TlCl3 > TlCl4-. The rate decreases by increasing the hydrogen ion concentration and ionic strength. The redox process occurs by intermediate formation of a complex of thallium(III) and arsenic(III). The rate constant for the reaction between Tl3+ and arsenic(III) calculated from the data of the present investigation compared well with that of the reaction1 in the absence of chloride ions.

The rate of reaction of nitrous acid and 4-aminobenzenesulphonamide in nitric acid

1973 ◽  
Vol 26 (7) ◽  
pp. 1607 ◽  
Author(s):  
PK Bhattacharyya ◽  
RD Saini
Keyword(s):  
Hydrogen Peroxide ◽  
Nitric Acid ◽  
Acid Medium ◽  
Acid Concentration ◽  
Rate Constant ◽  
Nitrous Acid ◽  
Nitric Acid Concentration ◽  
Nitric Acid Medium ◽  
Competitive Reaction ◽  
Rate Of Reaction

On the basis of the competitive reaction of nitrous acid with hydrogen peroxide in nitric acid medium the rate constant of the reaction of 4- aminobenzenesulphonamide with nitrous acid has been determined to be 6.4 l2 mol-2 s-1 at 22�C and has been found to be independent of nitric acid concentration in the range 0.5-2M.

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