Thermodynamics of solution of SO2(g) in water and of aqueous sulfur dioxide solutions

Goldberg, Robert N.; Parker, V. B.

doi:10.6028/jres.090.024

Cited by 101 publications

(58 citation statements)

References 29 publications

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“…(4,18) It may be seen that values quoted by Perry (2) are too high. Figure 5 and 6 compare our results at T = 298.15 K with experimental values (5,(19)(20)(21) and correlations (4,13,18) over a large molality range (up to 1 mol·kg −1 ). In dilute aqueous solutions, the experimental results of Johnstone and Leppla (5) agree very well with our calculated values.…”

Section: Resultsmentioning

confidence: 87%

“…Despite numerous investigations, (7)(8)(9)(10)(11)(12) there still exists disagreement on the value of the equilibrium constant for this reaction; the recommended values at T = 298.15 K being 0.0139 (8,10,11,13) and 0.0172. (7,9,12) To check which of these values is thermodynamically more consistent and to get more insight into the system, the concentration of the aqueous sulphur dioxide SO 2 (aq) was determined by analysing the liquid phase and using a simple thermodynamic model based on established thermodynamic data and the Debye-Hu¨ckel equation for the activity coefficients.…”

Section: Introductionmentioning

confidence: 99%

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Spectrophotometric measurement of the vapour-liquid equilibria of (sulphur dioxide + water)

Siddiqi¹,

Krissmann²,

Peters-Gerth³

et al. 1996

The Journal of Chemical Thermodynamics

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Section: Resultsmentioning

confidence: 87%

Section: Introductionmentioning

confidence: 99%

Spectrophotometric measurement of the vapour-liquid equilibria of (sulphur dioxide + water)

Siddiqi¹,

Krissmann²,

Peters-Gerth³

et al. 1996

The Journal of Chemical Thermodynamics

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“…To interpret the pH dependence of the oxidation rates mechanistically, it is necessary to have reliable dissociation constants for the dissociation of H2SO3 and solubilities of SO2 in aqueous solutions. Reliable thermodynamic constants, (Ki), are available for the dissociation of H2SO3 and the solubility for SO 2 SO2 (g) = SO2 (aq) Ko, SO2 + H20 = H ++ HSO3 K1, HSO~ = H + + SO~-K 2 in pure water (Goldberg and Parker, 1985).…”

Section: Introductionmentioning

confidence: 99%

The solubility of SO2 and the dissociation of H2SO3 in NaCl solutions

et al. 1989

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The pK~ and pK~ of H2SO 3 have been determined in NaCI solutions as a function of ionic strength (0.1 to 6 m) and temperature (5 and 25 °C). The extrapolated values in water were found to be in good agreement with literature data. The experimental results have been used to determine the Pitzer interaction parameters for SO2, HSO~ and SOl-in NaC1 solutions. The resultant parameters for NaHSO3 and Na2SO 3 were found to be in reasonable agreement with the values for NaHSO4 and Na2SO 4. It, thus, seems reasonable to assume that the interactions of Mg 2÷ and Ca 2+ with HSO 3 and SO~-can be estimated from the values with HSO~ and SO]-until experimental values are available. Measurements ofpK~ and pK~ in artificial seawater were found to be in good agreement with the calculated values using the derived Pitzer parameters. It is, thus, possible to make reasonable estimates of the activity coefficients of HSO~ and SO32-ions and pK~ and pK~ for the ionization of H 2 SO 3 in marine aerosols.

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“…The values of the thermodynamic equilibrium constants for these equations were calculated using data reported by Goldberg and Parker 22 (eqs 5 and 6) and by Brewer 23 (eqs 7 and 8). Together with the equilibrium equations relative to eqs 5-8, the stoichiometric equations for total sulfite and sulfate concentrations and the electroneutrality equation were considered.…”

Section: Resultsmentioning

confidence: 99%

Sulfite Oxidation Catalyzed by Cobalt Ions in Flue Gas Desulfurization Processes

Karatza

Prisciandaro

Lancia

et al. 2010

Journal of the Air & Waste Management Association

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This paper presents an experimental study of calcium bisulfite oxidation, a key step in the wet limestonegypsum flue gas desulfurization (FGD) process, in the presence of catalysts (e.g., cobalt ions and a mixture of ferrous and cobalt ions). A fundamental approach is followed, by reproducing a simplified synthetic FGD liquor in which both catalyst ions, alone or mixed together, are present. A laboratory-scale apparatus is used, in which sulfurous solution is contacted with a gas phase at a fixed oxygen partial pressure (21.3 kPa) and at different temperature levels (25, 45, and 55°C). The experimental results are analyzed using the theory of gas-liquid mass transfer with chemical reaction, showing that the slow reaction regime is explored and the transition from the kinetic to the diffusional subregime is identified. The experimental results are compared with those obtained in the presence of other catalytic species (manganese and ferrous ions), showing that cobalt is effective in catalyzing the oxidation of calcium bisulfite to sulfate, but to a minor extent with respect to iron and manganese.

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Thermodynamics of solution of SO2(g) in water and of aqueous sulfur dioxide solutions

Cited by 101 publications

References 29 publications

Spectrophotometric measurement of the vapour-liquid equilibria of (sulphur dioxide + water)

Spectrophotometric measurement of the vapour-liquid equilibria of (sulphur dioxide + water)

The solubility of SO2 and the dissociation of H2SO3 in NaCl solutions

Sulfite Oxidation Catalyzed by Cobalt Ions in Flue Gas Desulfurization Processes

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