The oxidation of chlorine ions under the joint action of ozone and permanganate ions

The oxidation of chlorine ions in the system O₃ + MnO ₄ ^? + H⁺ + Cl^? with the formation of Cl₂ in the gas phase was studied. The phenomenon of transfer catalysis of the reaction between O₃ and Cl^? by the MnO ₄ ^? ion was observed (the products of the reduction of MnO ₄ ^? by the chlorine ion are oxidized by ozone to recover MnO ₄ ^? ). The rate of the formation of Cl₂ in the O₃ + MnO ₄ ^? + H⁺ + Cl^? system was higher than the sum of the corresponding rates in the oxidation of Cl^? by O₃ and MnO ₄ ^? separately. A scheme explaining the trends observed experimentally for the formation of Cl₂ and changes in MnO ₄ ^? concentration was suggested. The formation of MnO ₄ ^? in the oxidation of Mn³⁺ with ozone in acid media was studied.     

Kinetic salt effects in the reaction of permanganate ions with iodide ions in concentrated electrolyte solutions

The oxidation of iodide ion by permanganate ion has been studied in several electrolyte solutions over the concentration range (0–6M). The observed kinetic salt effect may be interpreted as arising as a result of ionsolvent interactions. This salt effect is additive for different salts. Support for these conclusions comes from an examination of the activity coefficients of species estimated from the treatment given by Pitzer. It has also been shown that the species relevant in terms of kinetic control are unassociated.     

The chemical passivation of copper in ammonia solutions containing chlorine ions

It was shown that the CuCl layers deposited on copper chemically and electrochemically from copper-ammonia solutions were different. The layer formed chemically was loose, and that formed on the anode, dense. During multilayer copper passivation, the chemically deposited CuCl layer interfered with the formation of electrochemical CuCl and Cu₂O layers.     

The reaction between solid lead and chlorine gas

When lead reacts with a chlorine atmosphere the reaction rate shows a logarithmic rate law followed by a parabolic one. Both reaction rates can be explained by assuming that electron holes in the reaction product are rate-determining. In the beginning, the reaction of holes with lead (I) ions on lead ion lattice sites in PbCl₂ is the rate-determining step; later, the transport of holes by diffusion through the growing PbCl₂ layer becomes rate-determining.An oxide layer on the lead before chlorination retards the reaction, while, on the contrary, traces of oxygen in the chlorine gas accelerate the reaction. Both phenomena can be explained by assuming that a mixed compound PbO_1?xCl_2x is formed. It is concluded that the presence of impurities in the system may influence the reaction rate drastically.     

Umetric determination of persulphate in sulphuric acid solutions by permanganate

The determination of persulphate in a ca. 12.5 N sulphuric acid solution by direct titration with permanganate is described. The results are satisfactory but the conditions are critical.     

Luminescence kinetics and association equilibria of lanthanide ions in aqueous solutions

Luminescence life time measurement can be used under certain conditions to determine the thermodynamic constants of complex formation between the luminescent (central ion) and ligand. The basic equations correlating the life time and the equilibria constants were derived for two cases: the time for establishing the thermodynamic equilibrium is much shorter than the life time of the excited state of the central ion; and the time for establishing the equilibrium and the life time are of the same order of magnitude.     

Symmetry of chloronium ions from ionic reaction of chlorine, chlorine monofluoride gas, and chlorine monofluoride complex with terminal alkenes

Ionic chlorination of 1H,1H,7H-perfluorohept-1-ene (2) and heptafluoropropyl trifluorovinyl ether (4) with chlorine monofluoride (ClF) gas in aprotic solvent; and alkenes 2, 1H-perfluorohept-1-ene (3E), and 4 with chlorine (Cl₂) in protic solvent were investigated. Regiochemical data from SN₂-like ring-opening of the intermediate was used to predict the symmetry of the chloronium ion. The chloronium ions from perfluorohydroalkene 2 with two terminal hydrogens were found to be unsymmetrical with positive charge localized on the terminal carbon. However, reaction of ClF_(g) with 3E containing a single terminal fluorine atom gave data suggesting a symmetrical chloronium ion. Alkene 4 contains a heptafluoropropyl ether group that stabilizes positive charge on the number-2 carbon and it is reactive enough to give products with the sluggish ClF complex generated in situ. Reactive eletrophiles ClF_(g), Cl_2(g), or the less reactive ClF complex, give an unsymmetrical chloromium ion with charge localized on the internal number-2 carbon.     

The kinetics of the reaction between magnesium and EBT

The kinetics of the reaction between Mg²⁺ and Eriochrome-Black-T (EBT) has been investigated in the pH range between 7.05 and 9.0, in the presence of 12% ethanol. The reaction is found to consist of two parallel paths, one involving the tervalent unprotonated ligand, and one its monoprotonated form. The rate constant for the unprotonated ligand has a “normal” value, whereas that for the protonated form is much lower. The numerical value of the rate constant for the unprotonated ligand obtained from results at a magnesium concentration of 10^?3M and a pH up to 9.0 is, however, inconsistent with that obtained from results at [Mg²⁺] = (1 to 4) × 10^?3M and pH up to 8.1. This can be explained, at least partially, if we assume the intermediate MgHD to lose its proton not only to H₂O, but also to other bases present in the solution.     

The electrochemistry of gold in acid aqueous solutions containing chloride ions

Results obtained with differently prepared gold electrodes in acid solutions containing chloride ion at temperatures ranging from 22 to 65°C are reported. Potentiostatic techniques and rotating disc electrodes were employed. The anodic dissolution, the onset of passivity and the cathodic deposition of the metal are investigated under different experimental conditions. The anodic dissolution of Au is discussed in terms of possible reaction mechanisms involving the participation of different adsorbed species. The onset of passivation is related to the depletion of chloride ion at the reaction interface. The experimental voltammograms can be reporduced by means of an equation which considers the diffusion of chloride ion, the activation polarization related to the dissolution of Au and the establishment of passivity.     

The kinetics of the gas-phase reaction between ozone and alkenes

The rate law ? d[O₃]/ dt = k₁[A][O₃] + k₃[A][O₃]²/ (k₄ + k₅[O₂]) has been found to obtain for the reaction of ozone with allene and with 1,2-butadiene. We now find that this rate law also applies to the reaction of ozone with ethylene and presumably with all lower alkenes. This generalizes the inhibiting effect of oxygen and accounts for the simplifed rate law found in the presence of excess oxygen. Oxygen itself is a product of the ozone–ethylene reaction, and we find that as [O₃]₀ increases, the (O₂ formed)/(O₃ used) ratio approaches 1.5. Values of k₁, k₃/k₅ for ethylene are compared with those for allene, 1,3-butadiene, and propene. A generalized mechanism is postulated for the reaction of ozone with alkenes involving a chain sequence that produces oxygen and which accounts for the observed rate law. A specific mechanism is postulated for the reaction of O₃ with ethylene, and the thermochemistry of the chain sequence is examined in detail.     

Decomposition of reaction networks: the initial phase of the permanganate/oxalic acid reaction

The determination of all chemical reaction networks composed of elementary reactions for a given net chemical reaction is one of the fundamental problems in chemistry, since the decomposition elucidates the reaction mechanism. It is essential in a wide range of applications: from the derivation of rate laws in physical chemistry to the design of large-scale reactors in process engineering where presence of unexpected side products can disturb operation. As an example we consider the well-known permanganate/oxalic acid reaction. We characterize all intermediate substances that can in principle act (auto-)catalytic, list all possible additional intermediate substances that would suffice to start the reaction without assuming presence of any autocatalyst. In particular, we propose for the first time a minimal network in which the well-known autocatalyst Mn²⁺ is produced. To derive our results we present an automatic method to determine whether a net chemical reaction can be explained by some reaction network with a given list of intermediate substances, how to generate all such networks, and how to suggest more intermediate substances if no network with the initially given substances exists.     

A fast mixing flow system: The kinetics of carbonic acid dehydration in aqueous acid solutions between 20 and 40°c

A simple and inexpensive optical stopped-flow apparatus which includes a springpowered driving system and a very efficient two-stage mixer is described. The total dead-time is less than 2.5 ms. The apparatus has been tested by studying the kinetics of carbon dioxide formation from hydrogencarbonate on mixing with hydrochloric acid, at pH 3–5 and 20–40°C. The average rate constants found for this process are 15.4, 25.1, 42.7, 70.3 and 110.7 s^-1 at 20°, 25°, 30°, 35° and 40°C, respectively. The calculated activation energy is 17950 cal mol^-1. The values are compared with earlier data.     

Cathodic electrochemiluminescence of metal ions in acid fluoride solutions

The conditions for exciting the cathodic electrochemiluminescence (ECL) of mercury-like ions and manganese in dilute HF solutions at aluminum and magnesium electrodes are described. ECL spectra are measured. It is shown that Mn(II) can be determined with a detection limit of 10^?7 M.     

Uptake and reaction kinetics of acetone, 2-butanone, 2,4-pentanedione, and acetaldehyde in sulfuric acid solutions

This work presents a study of the uptake of acetone, 2-butanone (methyl ethyl ketone), 2,4-pentanedione, and acetaldehyde by sulfuric acid solutions with an aim at understanding the reactivity of carbonyl compounds present in the atmosphere toward acidic aerosols. Experiments were performed in a rotating wetted-wall reactor coupled to a mass spectrometer at room temperature (298 +/- 3 K) with 0-96 wt % H(2)SO(4) solutions. For all compounds, a reactive uptake was observed at high acidity (>or=64 wt % H(2)SO(4)). The corresponding reactions were found to follow a second-order kinetics, and their rate constants, k (M(-1) s(-1)) were found to increase exponentially with acidity. These rate constants and their variations with acid concentration were in good agreement with the kinetic behavior of acid-catalyzed aldol condensation reported in the organic chemical literature, except for 2,4-pentanedione. The results of this work suggest that aldol condensation should be too slow to account for the enhanced organic aerosol mass observed in smog chamber studies and should have an even smaller contribution under atmospheric conditions. The rate constants of other compounds, such as large aldehydes, remain however to be measured. However, in order to contribute significantly to organic aerosol formation, a liquid phase reaction would have to result in an uptake coefficient of the order of 10(-2).     

Atmospheric chemistry of cyclohexanone: UV spectrum and kinetics of reaction with chlorine atoms

Absolute and relative rate techniques were used to study the reactivity of Cl atoms with cyclohexanone in 6 Torr of argon or 800–950 Torr of N₂ at 295 ± 2 K. The absolute rate experiments gave k(Cl + cyclohexanone) = (1.88 ± 0.38) × 10^?10, whereas the relative rate experiments gave k(Cl + cyclohexanone) = (1.66 ± 0.26) × 10^?10 cm³ molecule^?1 s^?1. Cyclohexanone has a broad UV absorption band with a maximum cross section of (4.0 ± 0.3) × 10^?20 cm² molecule^?1 near 285 nm. The results are discussed with respect to the literature data. © 2008 Wiley Periodicals, Inc. Int J Chem Kinet 40: 223–229, 2008     

Organic acid solutions in the chromatography of inorganic ions

Summary We present a study of the chromatographic behaviour of sixty ions on thin layers of cellulose, employing as eluents aqueous solutions of tartrate, at various molarities (from 0.1 to 1.0 mol dm^–3 and pH values (from 2.0 to 10.0 obtained with aqueous ammonia). The ions migrate, whether they are complexed with the tartrate or not, with high R_F values and are not influenced by variation of the tartrate concentration. The pH variations, owing to the formation of partial hydrolysis or precipitation products or possibly ammonia complexes, have a greater effect on the rate of ion migration and cause a decrease in the R_F values. We show interesting separations obtained with these eluents.This work has been in part supported by C.N.R. of Italy