Reaction of methanol with chlorate ions in acid solution containing Hg<sup>+2</sup> by NMR

Ernst, William R.; Indu, Bhart; Crump, Brian; Gelbaum, Leslie T.

doi:10.1002/aic.690420518

Cited by 2 publications

(1 citation statement)

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“…Linnivov uses ethanol for creation of supersaturation in solutions allowed to vary strongly the crystallization process conditions. Aqueous solutions of sodium chlorate with methanol are used in chlorine dioxide facilities. They are continuously fed to a vessel that serves as reactor and evaporative crystallizer.…”

Section: Introductionmentioning

confidence: 99%

Densities and Viscosities for Aqueous Solutions of Sodium Chlorate and Potassium Chlorate + Methanol from (288.15 to 318.15) K at 0.1 MPa

Pérez-Durán

Iglesias‐Silva

2019

J. Chem. Eng. Data

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In this work, we present densities and viscosities of aqueous solutions of sodium and potassium chlorate from (288.15 to 318.15) K at molalities from (0.1 to 1) and (0.01 to 0.5) for the aqueous solutions of sodium and potassium chlorate, respectively. Also, densities and viscosities of these aqueous solutions of sodium and potassium chlorate + methanol are measured from (288.15 to 318.15) K at concentration from (0.1 to 1, 0.1 to 0.3) m, respectively. Densities are from a vibrating tube densimeter and viscosities are from a rolling ball microviscosimeter. Ternary mixtures are prepared by adding (1 to 20)% volume of methanol to the aqueous solutions. Apparent molar volumes are calculated from the density measurements. Apparent molar volumes have been correlated using an extended Redlich–Rosenfeld–Meyer equation. The values of the parameters indicate that a stronger interaction of solvent–ions occurs in the potassium chlorate solution than in the sodium chlorate aqueous solutions. The equation correlates the data within an average absolute percentage deviation of 3.7%. Limiting apparent molar volumes for the sodium and potassium chlorate aqueous solution from this work agree within 1.9 cm3/mol with the literature values. Solutions of potassium chlorate show an iso-viscosity behavior at the temperatures and concentrations considered in this work. Also, the Dole-Jones equation correlates the viscosity data within an average absolute percentage deviation of 0.29%.

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Section: Introductionmentioning

confidence: 99%

Densities and Viscosities for Aqueous Solutions of Sodium Chlorate and Potassium Chlorate + Methanol from (288.15 to 318.15) K at 0.1 MPa

Pérez-Durán

Iglesias‐Silva

2019

J. Chem. Eng. Data

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Influence of Mercuric Nitrate on Species and Reactions Related to Chlorine Dioxide Formation

Indu

Hoq

Ernst

1997

Ind. Eng. Chem. Res.

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Mercuric ions influence reactions and intermediates that are involved in forming chlorine dioxide from chlorate ions. Addition of mercuric ions to reaction solutions can aid in understanding the mechanism and kinetics of this system. Mercuric ions do not react with aqueous solutions of chlorine dioxide unless those solutions contain chlorous acid. This unusual effect has enabled us to confirm that chlorous acid is an intermediate in the formation of chlorine dioxide in the methanol−chlorate reaction. This work discusses the effect of mercuric ions on solutions containing various Cl species (chlorine, chlorine dioxide, chlorous acid, and both chlorine dioxide and chlorous acid) and on reactions that involve these same species. The work also explores the methanol−chlorate reaction in the absence of mercuric ions. In the initial stage of the process, chlorine dioxide forms after an induction period, during which an intermediate rapidly forms, maximizes in concentration, and then disappears, and a second intermediate forms and attains a steady-state concentration. We show by several methods, including mercuric ion addition, that the second intermediate is chlorous acid. We have not conclusively identified the first intermediate. The increase and decline in its concentration is accompanied by the development and disappearance of the solution color (yellow). Although the UV absorbance behavior of the system suggests that the intermediate is chlorine, the color of the solution associated with this intermediate is not characteristic of solutions containing chlorine at these concentrations.

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Reaction of methanol with chlorate ions in acid solution containing Hg⁺² by NMR

Abstract: The reaction rate of methanol

Cited by 2 publications

References 18 publications

Densities and Viscosities for Aqueous Solutions of Sodium Chlorate and Potassium Chlorate + Methanol from (288.15 to 318.15) K at 0.1 MPa

Densities and Viscosities for Aqueous Solutions of Sodium Chlorate and Potassium Chlorate + Methanol from (288.15 to 318.15) K at 0.1 MPa

Influence of Mercuric Nitrate on Species and Reactions Related to Chlorine Dioxide Formation

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Reaction of methanol with chlorate ions in acid solution containing Hg+2 by NMR

Abstract: The reaction rate of methanol

Cited by 2 publications

References 18 publications

Densities and Viscosities for Aqueous Solutions of Sodium Chlorate and Potassium Chlorate + Methanol from (288.15 to 318.15) K at 0.1 MPa

Densities and Viscosities for Aqueous Solutions of Sodium Chlorate and Potassium Chlorate + Methanol from (288.15 to 318.15) K at 0.1 MPa

Influence of Mercuric Nitrate on Species and Reactions Related to Chlorine Dioxide Formation

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Reaction of methanol with chlorate ions in acid solution containing Hg⁺² by NMR