Untersuchungen in der ?Gro�en Bonner Kugel?

Groth, W.; Becker, K. H.; Comşa, George; Elzer, A.; Fink, E.H.; Jud, W.; Kley, D.; Schurath, U.; Thran, D.

doi:10.1007/bf00623126

Cited by 9 publications

(5 citation statements)

References 11 publications

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“…The low-pressure reactor used for the rate constant measurements has been described in previous publications [9,10]. It consists of a 220-m3 stainless steel sphere which can be evacuated below torr by oil diffusion pumps.…”

Section: Methodsmentioning

confidence: 99%

The rate constant of NO + O₃ → NO₂ + O₂ in the temperature range of 283–443 K

Lippmann

Jesser

Schurath

1980

Int J of Chemical Kinetics

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The reaction NO + 0 3 -NO2 + 0 2 has been studied in a 220-m3 spherical stainless steel reactor under stopped-flow conditions below 0.1 mtorr total pressure. Under the conditions used, the mixing time of the reactants was negligible compared with the chemical reaction time. The pseudo-first-order decay of the chemiluminescence owing to the reaction of ozone with a large excess of nitric oxide was measured with an infrared sensitive photomultiplier. One hundred twenty-nine decays a t 18 different temperatures in the range of 283-443 K were evaluated. A weighted least-squares fit to the Arrhenius equation yielded k = (4.3 f 0.6) X exp[-(1598 f 50)/T] cm3/molecule sec (two standard deviations in brackets). The Arrhenius plot showed no curvature within experimental accuracy. Comparison with recent results of Birks and co-workers, however, suggests that a nonlinear fit, as proposed by these authors, is more appropriate over an extended temperature range.

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Section: Methodsmentioning

confidence: 99%

The rate constant of NO + O₃ → NO₂ + O₂ in the temperature range of 283–443 K

Lippmann

Jesser

Schurath

1980

Int J of Chemical Kinetics

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“…We wish to report some 02(1Ag) quenching rate constants obtained from experiments in a 220-m3 stainless steel sphere. The reactor, as well as the experimental method, has been described in previous publications (2, 3). Briefly, 02(1Ag) was generated by passing a stream of high-purity oxygen (Air Liquide A 48) through a microwave discharge.…”

mentioning

confidence: 99%

“…The decay can either be observed directly by measuring the infrared atmospheric band 02(1Ag -3 ?_) at 1.27 µ using a lead sulfide detector, or indirectly by measuring the intensity of the atmospheric band 02(1Ag+ -*• 32g~) at 7620 A, which decays twice as fast as the infrared atmospheric band, with an infrared sensitive photomultiplier. Both methods have been used in this laboratory and found compatible (2, 3).…”

mentioning

confidence: 99%

Quenching of singlet molecular oxygen by some atmospheric pollutants

Penzhorn¹,

Guesten²,

Schurath³

et al. 1974

Environ. Sci. Technol.

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Room temperature rate constants for the deactivation of singlet molecular oxygen (^(cflAg) by SO2, H2S, CH3SH, CH3COCH3, CH2O, ambient air, and dry synthetic air were measured in a 220-m3 low-pressure reactor under static conditions. Emission at 7620 Á from 02(h12g+), which is continuously produced from the energy pooling reaction 202(1Ag) -Ü2(12g+) + 02(3 ß_), was taken as a relative measure of the 02(1Ag) concentration in the system. The compounds deactivate singlet oxygen at rates comparable to or lower than ground state molecular oxygen. The rate constants for deactivation by CH3SH, dry air, and ambient air are critically compared with literature values. It is concluded that singlet oxygen does not contribute to the atmospheric conversion of the trace gases investigated.

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“…The chamber was built between 1966-68 by W. Groth upon the initiative of P. Harteck. The facility was operated by K. H. Becker, E. Fink, D. Kley and U. Schurath (Groth et al, 1972).…”

Section: Reactionsmentioning

confidence: 99%

“…A large chamber, known as the "Große Bonner Kugel" (Groth et al, 1972), was built in Bonn between 1966and 1968; its conception was initiated by Groth and Harteck to study air glow reactions at the low pressures prevailing in the upper atmosphere. Afterwards, the chamber was also used to study reactions of tropospheric interest, but the knowledge of tropospheric chemistry at that time was very basic.…”

Section: Introductionmentioning

confidence: 99%

Overview on the Development of Chambers for the Study of Atmospheric Chemical Processes

Becker

Nato Science Series: IV: Earth and Environmental Science

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Indoor chambers without light sources, or irradiated by black lamps or solar simulators. Year of Building LaboratoriesDescription Application Groth et al., Bonn dark chamber 220 m 3 , stainless steel (high vacuum) without light sources, for low pressure studies Pitts et al., Riverside 6 m 3 , evacuable, thermostated, FEP coated aluminium photooxidant and kinetic studies Niki et al., Dearborn 150 l Pyrex kinetic and mechanistic studies Akimoto et al., Tsukuba 6 m 3 evacuable, thermostated, FEP coated aluminium photooxidant studies Winer et al., Los Angeles 6 m 3 evacuable, thermostated, FEP coated aluminium photooxidant studies Becker et al., Wuppertal 420 l Duran glass, evacuable, thermostated -50 to +50 ºC gas phase studies Joshi et al.

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Untersuchungen in der ?Gro�en Bonner Kugel?

Cited by 9 publications

References 11 publications

The rate constant of NO + O₃ → NO₂ + O₂ in the temperature range of 283–443 K

The rate constant of NO + O₃ → NO₂ + O₂ in the temperature range of 283–443 K

Quenching of singlet molecular oxygen by some atmospheric pollutants

Overview on the Development of Chambers for the Study of Atmospheric Chemical Processes

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Untersuchungen in der ?Gro�en Bonner Kugel?

Cited by 9 publications

References 11 publications

The rate constant of NO + O3 → NO2 + O2 in the temperature range of 283–443 K

The rate constant of NO + O3 → NO2 + O2 in the temperature range of 283–443 K

Quenching of singlet molecular oxygen by some atmospheric pollutants

Overview on the Development of Chambers for the Study of Atmospheric Chemical Processes

Contact Info

Product

Resources

About

The rate constant of NO + O₃ → NO₂ + O₂ in the temperature range of 283–443 K

The rate constant of NO + O₃ → NO₂ + O₂ in the temperature range of 283–443 K