Kinetics of chlorine oxide reactions. I. The reaction of oxygen atoms with Cl2O

C G Freeman, L. F. Phillips

Research output: Contribution to journalArticle

Abstract

The reaction has been studied in a fast-flow system, using a mass spectrometer to monitor the partial pressures of reactants and products. The ratio of Cl2O to O consumed was 0.8, with excess Cl2O present in a poisoned system at total pressures near 0.25 torr. The following reaction scheme is proposed to account for the observations: (1) O + Cl2O ? 2ClO; (2) O + ClO ? O2 + Cl; (3) Cl + Cl2O ? Cl2 + ClO; (4) Cl + wall ? 1/2Cl2; (5) 2ClO ? Cl2 + O2, where we find that k1 = (8.3 ± 1.4) × 1012 cm3 mol-1 sec-1 and k2 = k1.

Original languageEnglish
Pages (from-to)3025-3028
Number of pages4
JournalJournal of Physical Chemistry
Volume72
Issue number8
Publication statusPublished - 1968

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Mass spectrometers
Partial pressure
Oxygen
Atoms
Kinetics
chlorosyl

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Freeman, C G ; Phillips, L. F. / Kinetics of chlorine oxide reactions. I. The reaction of oxygen atoms with Cl2O. In: Journal of Physical Chemistry. 1968 ; Vol. 72, No. 8. pp. 3025-3028.
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Kinetics of chlorine oxide reactions. I. The reaction of oxygen atoms with Cl2O. / Freeman, C G; Phillips, L. F.

In: Journal of Physical Chemistry, Vol. 72, No. 8, 1968, p. 3025-3028.

Research output: Contribution to journalArticle

TY - JOUR

T1 - Kinetics of chlorine oxide reactions. I. The reaction of oxygen atoms with Cl2O

AU - Freeman, C G

AU - Phillips, L. F.

PY - 1968

Y1 - 1968

N2 - The reaction has been studied in a fast-flow system, using a mass spectrometer to monitor the partial pressures of reactants and products. The ratio of Cl2O to O consumed was 0.8, with excess Cl2O present in a poisoned system at total pressures near 0.25 torr. The following reaction scheme is proposed to account for the observations: (1) O + Cl2O ? 2ClO; (2) O + ClO ? O2 + Cl; (3) Cl + Cl2O ? Cl2 + ClO; (4) Cl + wall ? 1/2Cl2; (5) 2ClO ? Cl2 + O2, where we find that k1 = (8.3 ± 1.4) × 1012 cm3 mol-1 sec-1 and k2 = k1.

AB - The reaction has been studied in a fast-flow system, using a mass spectrometer to monitor the partial pressures of reactants and products. The ratio of Cl2O to O consumed was 0.8, with excess Cl2O present in a poisoned system at total pressures near 0.25 torr. The following reaction scheme is proposed to account for the observations: (1) O + Cl2O ? 2ClO; (2) O + ClO ? O2 + Cl; (3) Cl + Cl2O ? Cl2 + ClO; (4) Cl + wall ? 1/2Cl2; (5) 2ClO ? Cl2 + O2, where we find that k1 = (8.3 ± 1.4) × 1012 cm3 mol-1 sec-1 and k2 = k1.

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