Kinetics of the reactions of ONOO− with small molecules

Viggiano, Albert A.; Midey, Anthony J.; Ehlerding, Anneli

doi:10.1016/j.ijms.2005.12.007

Cited by 11 publications

(18 citation statements)

References 30 publications

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“…The thermochemistry of CO 3 .− has been investigated by ion‐molecule reactions and photodissociation . The most recent photodissociation study of CO 3 .− (Ar n ) by Johnson, Viggiano, and co‐workers, which agrees with quantum chemical calculations, reports a CO 2 −O .− bond dissociation energy of 269±5 kJ mol −1 .

e^{-} + O_{2} + M \to O_{2}^{•}^{-} + M, M = O_{2}, N_{2}, Ar, H_{2} O, etc .

O_{2}^{•}^{-} + O_{3} \to O_{2} + O_{3}^{•}^{-}

O_{3}^{•}^{-} + CO_{2} \to CO_{3}^{•}^{-} + O_{2}

…”

Section: Figuresupporting

confidence: 53%

Electrons Mediate the Gas‐Phase Oxidation of Formic Acid with Ozone

Linde

Tang

Siu

et al. 2016

Chemistry A European J

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Gas-phase reactions of CO3 (.-) with formic acid are studied using Fourier transform ion cyclotron resonance (FT-ICR) mass spectrometry. Signal loss indicates the release of a free electron, with the formation of neutral reaction products. This is corroborated by adding traces of SF6 to the reaction gas, which scavenges 38 % of the electrons. Quantum chemical calculations of the reaction potential energy surface provide a reaction path for the formation of neutral carbon dioxide and water as the thermochemically favored products. From the literature, it is known that free electrons in the troposphere attach to O2 , which in turn transfer the electron to O3 . O3 (.-) reacts with CO2 to form CO3 (.-) . The reaction reported here formally closes the catalytic cycle for the oxidation of formic acid with ozone, catalyzed by free electrons.

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e^{-} + O_{2} + M \to O_{2}^{•}^{-} + M, M = O_{2}, N_{2}, Ar, H_{2} O, etc .

O_{2}^{•}^{-} + O_{3} \to O_{2} + O_{3}^{•}^{-}

O_{3}^{•}^{-} + CO_{2} \to CO_{3}^{•}^{-} + O_{2}

…”

Section: Figuresupporting

confidence: 53%

Electrons Mediate the Gas‐Phase Oxidation of Formic Acid with Ozone

Linde

Tang

Siu

et al. 2016

Chemistry A European J

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“…An example is ONOO À , which is made through the reaction of CO 4 À with NO. 47 Once the ions are thermalized, a neutral reagent is added between 35 and 55 cm from the end of the flow tube and allowed to react with the primary ion. Rate constants are measured by monitoring the exponential decay of the primary ion as a function of the flow rate of the reactant neutral.…”

Section: Methodsmentioning

confidence: 99%

Reexamination of ionospheric chemistry: high temperature kinetics, internal energy dependences, unusual isomers, and corrections

Viggiano

2006

Phys. Chem. Chem. Phys.

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The public reporting burden for this collection of information is estimated to average 1 hour per response, including the time for reviewing instructions, searching existing data sources, gathering and maintaining the data needed, and completing and reviewing the collection of information. Send comments regarding this burden estimate or any other aspect of this collection of information, including suggestions for reducing the burden to Department of Defense, Washington Headquarters Services Directorate for Information Operations and Reports (0704-0188), 1215 Jefferson Davis Highway, Suite 1204, Arlington VA 22202-4302. Respondents should be aware that notwithstanding any other provision of law, no person shall be subject to any penalty for failing to comply with a collection of information if it does not display a currently valid OMB control number. A number of aspects of ionospheric chemistry are revisited. The review discusses in detail only work performed at AFRL, but other work is mentioned. A large portion of the paper discusses measurements of the kinetics of upper ionospheric reactions at very high temperatures, i.e. the upper temperature range has been extended to at least 1400 K and in some cases to 1800 K. These temperatures are high enough to excite vibrations in 02, N 2 , and NO and comparing them to drift tube data allows information on the rotational temperature and vibrational level dependences to be derived. Rotational and translational energy are equivalent in controlling the kinetics in most reactions. Vibrational energy in 02 and N 2 is often found to promote reactivity which is shown to cause ionospheric density depletions. NO vibrations do not significantly affect the reactivity. In a number of cases, detailed calculations accompanied the experimental studies and elucidated details of the mechanisms. Kinetics of two peroxide isomers important in the lower ionospheric have been measured for the first time, i.e. NOOW and ONOO-. Finally, two examples are shown where errors in previous data are corrected. PLEASE DO NOTIntroduction information learned by studying temperature dependences over very wide ranges. The low range can be extended downIn the 1960's and 1970's the ion chemistry of the ionosphere ward in other laboratories by the CRESU and trap techniwas studied extensively and many of the important properties ques4-' 9 While going to lower temperatures helps in elucidated.'-4 However, the measurements did not extend to interpreting mechanisms, it is more important for interstellar all relevant conditions and to all species. Temperature depenchemistry than for ionospheric chemistry. dences were often lacking or extended over only part of the Not only has the ionospheric chemistry been remeasured at pertinent range.s-8 Product state information was only occa-AFRL over wider ranges of temperatures, but information on sionally known.9-1" The maximum temperature studied was how rotational and vibrational energy affects reactivity can below that for which vibrational excitation of N 2 , 02, and ...

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“…These experimental data were expressed in the functional form of power-law temperature dependences shown in Table 10. The same selected ion flow tube was used by Viggiano et al (2006) to measure Surv Geophys the binary rate coefficient for ONOO -ions with NO 2 at 300 K temperature. The uncertainties of the measured rate coefficients were estimated as ± 35 % by Viggiano et al (2006).…”

Section: Chemical Reactions Of Negative Ions With Thermal Electrons Amentioning

confidence: 99%

“…To overcome this uncertainty in EA, it is possible to use EA(CO 3 ) = 2.69 eV in calculations of K XY following the recommendation given by Rienstra-Kiracofe et al (2002). Table 13 shows that only the upper limit value of EA(ONOO) was evaluated by Viggiano et al (2006). At the same time, it follows from Eq.…”

Section: Mutual Neutralization Of Negative and Positive Ionsmentioning

confidence: 99%