The aqueous oxidation of elemental mercury by ozone
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Mercury
Elemental mercury
Atmospheric chemistry
Aqueous two-phase system
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Micellar solutions
Cationic polymerization
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Elemental mercury can exist at sites undergoing decontamination and decommissioning operations from instruments containing mercury, mercury vacuum pumps, chemical operations, electrical components, and pharmaceutical production. Elemental mercury has been known to be a severe health hazard. Recent studies, utilizing more sensitive methods, are able to detect subclinical effects from mercury exposure at lower concentrations than in past studies. Precautions must be taken if elemental mercury may be present in the workplace.
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Mercury poisoning in children is rare but may have devastating health consequences when exposure is unrecognized. Mercury occurs in three forms: elemental, inorganic, and organic. Elemental mercury (Hg0) vapor may volatilize following an accidental spill and may be readily absorbed from the lungs. The following case study describes how the poison center, health department, physicians, and others worked together to treat a family with long-term exposure to elemental mercury vapor in the home. Identification and prevention of this type of exposure in the community are discussed.
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The kinetics and mechanism of the Ag (I) ion catalyzed reaction of levofloxacin (LFC) by free available chlorine (FAC) during water chlorination processes was investigated for the first time between the pH values 4.2 and 8.2. The pH dependent second order rate constants were found to decrease with increase in pH. (e.g. Apparent second order rate constant for Ag (I) catalyzed reaction, k”app = 114.40 dm−3 mol−1sec at pH 4.2 and k”app.= 8.72 dm−3 mol−1sec at pH 8.2 and at 25±0.2°C). The reaction rates revealed that Ag (I) catalyzed reaction was about six-fold faster than the uncatalyzed reaction. The products of the reaction were determined by Liquid chromatography and high resolution mass spectrometry. The reaction proceeds via formation of intermediate complex between Ag (I) ion and levofloxacin, then HOCl reacts with the complex to form chlorinated product. The effect of catalyst, effect of initially added product, effect dielectric constant and effect ionic strength on the rate of reaction was also studied. The effect of temperature on the rate of the reaction was studied at four different temperatures and rate constants were found to increase with increase in temperature and the thermodynamic activation parameters Ea, ΔH#, ΔS# and ΔG# were evaluated for the reaction and discussed.
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Abstract The reaction rate of the alkaline hydrolysis of ethyl acetate was studied by means of a continuous measurement of the electric conductivity change. The second-order rate constant decreased as the reaction proceeded. The decrease was evident when the initial concentrations of the ester and the base were close together. The initial rate constant at 25°C was measured as 0.1120 1./mol./sec. and the activation energy was 11.56 kcal./mol., values agreed well with those of previous studies. From the standpoint of the electronic theory of organic chemistry, Day and Ingold proposed a sequential reaction mechanism passing through an addition complex. The results of the approximate calculations to the pseudo-first-order reaction and the analog-computation of the exact models coincided with the experimental results. The difference in the activation energies of the forward and reverse reaction rates was calculated from the experimental data. At lower temperatures this reverse reaction rate was small, and the overall reaction rate was approximated as a pure second-order reaction. Other probable reasons for the rate constant decrease were also discussed.
Alkaline hydrolysis
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Reversible reaction
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From the catalystic dechlorination rates of trichloroethylene with four types of iron particle determined by the static method, it was confirmed that the reaction rates of these particles can be expressed as a pseudo-first-order reaction and that α-Fe · Fe3O4 composite nanoparticles showed the highest reaction rate. As determined by static method, the “specific” reaction rate constants of iron nano- and microparticles tended to remain at certain values. Whereas they tended to decrease when the load of the particles increased. The reaction rate and “specific” reaction rate constants of iron nano- and microparticles decreased when the initial TCE concentration was high increased. The reaction rate constants of iron nanoparticles decreased markedly at a low pH and they increased at a high pH. However, the reaction rate constants of iron microparticles hardly depended on pH.
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