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

C G Freeman; L. F. Phillips

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

C G Freeman, L. F. Phillips

School of Engineering & Physical Sciences

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20 Citations (Scopus)

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 language	English
Pages (from-to)	3025-3028
Number of pages	4
Journal	Journal of Physical Chemistry
Volume	72
Issue number	8
Publication status	Published - 1968

Cite this

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title = "Kinetics of chlorine oxide reactions. I. The reaction of oxygen atoms with Cl2O",

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.",

author = "Freeman, {C G} and Phillips, {L. F.}",

year = "1968",

language = "English",

volume = "72",

pages = "3025--3028",

journal = "Journal of Physical Chemistry",

issn = "0022-3654",

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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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M3 - Article

SN - 0022-3654

VL - 72

SP - 3025

EP - 3028

JO - Journal of Physical Chemistry

JF - Journal of Physical Chemistry

IS - 8

ER -

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

Abstract

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