Cloud chamber studies of dark transformations of sulfur dioxide in cloud droplets

Stehle, R.; Gertler, Alan W.; Katz, U.; Lamb, Dennis; Miller, David F.

doi:10.1016/0004-6981(81)90264-x

Cited by 19 publications

(9 citation statements)

References 12 publications

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“…No detectable effect was observed using high concentrations of NaC1 aerosol. This is in agreement with previous studies such as Junge and Ryan (1958) or Steele et al (1981). In the presence of CuC12 aerosol SO2(g) may be removed by both the catalytic S(IV) oxidation and the reduction of Cu(II) to Cu(I) in the liquid phase (Cheng et al, 1971 ;Dasgupta et al, 1979):…”

Section: The Table Belowsupporting

confidence: 92%

Study of metal aerosol systems as a sink for atmospheric SO2

Berresheim

Jaeschke

1986

J Atmos Chem

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The chemical removal of SO 2 in the presence of different aerosol systems has been investigated in laboratory experiments using a dynamic flow reactor. The aerosols consisted of wetted particles containing one of the following substances: MnC12, Mn(NO3)2, MnSO4, CuCI2, Cu(NO3)2, CuSO4, FeC13, NaCI. The SO2 removal rate R was measured as a function of the SO2 gas phase concentration (SO 2)g, the spatial metal concentration CMe , and the relative humidity rH in the reactor. A first-order dependence with regard to (SO 2)g was observed for each type of aerosol. For the Mn(II) and Cu(II) aerosols R was found to be a non-linear function of CMe except for MnSO a and Cu(NO 3)2 particles. The removal rate showed a significant increase with the relative humidity particularly when rH was close to the deliquescence point of the wetted particles. Among the Mn(II) and Cu(II) aerosols investigated Mn(NO3) 2 was found to be most efficient for the chemical removal of SO 2 at atmospheric background conditions, especially in haze and fog droplets. The results further indicate that the catalytic oxidation of S(IV) in such aerosol systems may be as efficient as its oxidation by H20 2 in cloud water.

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Section: The Table Belowsupporting

confidence: 92%

Study of metal aerosol systems as a sink for atmospheric SO2

Berresheim

Jaeschke

1986

J Atmos Chem

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“…That this scatter may be significant has been pointed out in the preceding section and is illustrated by the shaded area in Fig. 1, which represents the range of values measured by Steele et al (20). The lines shown in Fig.…”

Section: Kineticssupporting

confidence: 51%

“…Most of the experimental studies of the aqueous reaction between S0 2 and 0 2 have been carried out in bulk solutions, although use has also been made of heterogeneous gas/liquid and droplet systems (7,14,16,20). The reaction has been studied over a wide range of S(IV) concentrations (10~7 to 10" l M) in buffered and unbuffered solutions, and using a variety of techniques to monitor the progress of the reaction.…”

Section: Experimental Studiesmentioning

confidence: 99%

“…Their results obtained using this "purified" water show up to a twentyfold variation in the characteristic oxidation time at identical experimental conditions, which puts in question their purification technique. In fact, most authors find wide variability of results whatever the water quality, and scatter of an order of magnitude is common in the reported studies (16,20). On the other hand, other authors have been quite selective when deciding which particular results to present (42).…”

Section: Experimental Studiesmentioning

confidence: 99%

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On the discrepancy between reported studies of the uncaialysed aqueous oxidation of SO₂by O₂

Radojević

1984

Environmental Technology Letters

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The uncatalysed aqueous oxidation of S0 2 is a reaction with diverse applications, and it has long been the subject of considerable controversy. The extensive literature on this reaction is critically reviewed and the results of kinetic studies are presented in tabular form. A number of factors which may be responsible for the discrepancy between reported experiments are discussed, and of these the pH and the purity of experimental solutions appear to be the most important. The following rate equation is proposed for predicting atmospheric oxidation rates via this reaction:The mechanism appears to be of little consequence in the conversion of atmospheric SO 2 .

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“…The 6.7 m 3 , Desert Research Institute Dynamic Cloud Chamber was described by Steele et al (1981), who performed experiments with the oxidation of SO 2 in droplets formed on a range of CCN, without the addition of extra oxidants such as O 3 . The same chamber was then used by Miller et al (1986) to perform experiments with the addition of O 3 .…”

Section: Introductionmentioning

confidence: 99%

Aqueous phase oxidation of sulphur dioxide by ozone in cloud droplets

et al. 2016

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Abstract. The growth of aerosol due to the aqueous phase oxidation of sulfur dioxide by ozone was measured in laboratory-generated clouds created in the Cosmics Leaving OUtdoor Droplets (CLOUD) chamber at the European Organization for Nuclear Research (CERN). Experiments were performed at 10 and − 10 • C, on acidic (sulfuric acid) and on partially to fully neutralised (ammonium sulfate) seed aerosol. Clouds were generated by performing an adiabatic expansion -pressurising the chamber to 220 hPa above atmospheric pressure, and then rapidly releasing the excess pressure, resulting in a cooling, condensation of water on the aerosol and a cloud lifetime of approximately 6 min. A model was developed to compare the observed aerosol growth with that predicted using oxidation rate constants previously measured in bulk solutions. The model captured the measured aerosol growth very well for experiments performed at 10 and −10 • C, indicating that, in contrast to some previous studies, the oxidation rates of SO 2 in a dispersed aqueous system can be well represented by using accepted rate constants, based on bulk measurements. To the best of our knowledge, these are the first laboratory-based measurements of aqueous phase oxidation in a dispersed, supercooled population of droplets. The measurements are therefore important in confirming that the extrapolation of currently accepted reaction rate constants to temperatures below 0 • C is correct.

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Cloud chamber studies of dark transformations of sulfur dioxide in cloud droplets

Cited by 19 publications

References 12 publications

Study of metal aerosol systems as a sink for atmospheric SO2

Study of metal aerosol systems as a sink for atmospheric SO2

On the discrepancy between reported studies of the uncaialysed aqueous oxidation of SO₂by O₂

Aqueous phase oxidation of sulphur dioxide by ozone in cloud droplets

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Cloud chamber studies of dark transformations of sulfur dioxide in cloud droplets

Cited by 19 publications

References 12 publications

Study of metal aerosol systems as a sink for atmospheric SO2

Study of metal aerosol systems as a sink for atmospheric SO2

On the discrepancy between reported studies of the uncaialysed aqueous oxidation of SO2by O2

Aqueous phase oxidation of sulphur dioxide by ozone in cloud droplets

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On the discrepancy between reported studies of the uncaialysed aqueous oxidation of SO₂by O₂