Kinetics and Products of the Reactions of Ethyl and n-Propyl Nitrates with OH Radicals

Article abstract of DOI:10.1002/kin.21037

The kinetics of the reactions of ethyl (1) and n-propyl (2) nitrates with OH radicals has been studied using a low-pressure flow tube reactor combined with a quadrupole mass spectrometer. The rate constants of the title reactions were determined under pseudo–first-order conditions from kinetics of OH consumption in high excess of nitrates. The overall rate constants, k₁ = 1.14 × 10^?13 (T/298)^2.45 exp(193/T) and k₂ = 3.00 × 10^?13 (T/298)^2.50 exp(205/T) cm³ molecule^?1 s^?1 (with conservative 15% uncertainty), were determined at a total pressure of 1 Torr of helium over the temperature range (248–500) and (263–500) K, respectively. The yields of the carbonyl compounds, acetaldehyde and propanal, resulting from the abstraction by OH of an α-hydrogen atom in ethyl and n-propyl nitrates, followed by α-substituted alkyl radical decomposition, were determined at T = 300 K to be 0.77 ± 0.12 and 0.22 ± 0.04, respectively.

Full text of DOI:10.1002/kin.21037

Kinetics and Products of
the Reactions of Ethyl and
n-Propyl Nitrates with OH
Radicals
JULIEN MORIN, YURI BEDJANIAN, MANOLIS N. ROMANIAS
Institut de Combustion, Ae´rothermique, Re´activite´ et Environnement (ICARE), CNRS and Universite´ d’Orle´ans, 45071,
Orle´ans Cedex 2, France
Received 8 July 2016; revised 22 August 2016; accepted 25 August 2016
DOI 10.1002/kin.21037
Published online in Wiley Online Library (wileyonlinelibrary.com).
ABSTRACT: The kinetics of the reactions of ethyl (1) and n-propyl (2) nitrates with OH radicals
has been studied using a low-pressure flow tube reactor combined with a quadrupole mass
spectrometer. The rate constants of the title reactions were determined under pseudo–first-
order conditions from kinetics of OH consumption in high excess of nitrates. The overall rate
constants, k1 = 1.14 × 10−13 (T/298)2.45 exp(193/T) and k2 = 3.00 × 10−13 (T/298)2.50 exp(205/T)
cm3 molecule−1 s−1 (with conservative 15% uncertainty), were determined at a total pressure of
1 Torr of helium over the temperature range (248–500) and (263–500) K, respectively. The yields
of the carbonyl compounds, acetaldehyde and propanal, resulting from the abstraction by OH
of an α-hydrogen atom in ethyl and n-propyl nitrates, followed by α-substituted alkyl radical
decomposition, were determined at T = 300 K to be 0.77 0.12 and 0.22 0.04, respectively.
ꢀC
2016 Wiley Periodicals, Inc. Int J Chem Kinet 1–8, 2016
tropospheric lifetime from a few days to a few weeks,
depending on their reactivity toward OH radicals and
photolysis rate [2–5].
In the present work, we report the results of the ex-
perimental investigation of the reactions of ethyl (ENT)
and n-propyl (PNT) nitrates with OH radicals:
INTRODUCTION
Organic nitrates are the intermediates of the atmo-
spheric oxidation of volatile organic compounds in
the presence of nitrogen oxides. They are formed in
the minor (addition) channel of the reaction of per-
oxy radicals with NO and also in the NO3-initiated
oxidation of unsaturated organic compounds [1]. Or-
ganic nitrates are temporary reservoirs of NOx with a
OH + C2H5ONO2 → Products
OH + C3H7ONO2 → Products
(1)
(2)
Correspondence to: Y. Bedjanian; e-mail: yuri.bedjanian@cnrs-
orleans.fr.
Current address of M. N. Romanias; Mines Douai, SAGE,
F-59508, Douai, France.
Previously, the rate constant of reaction (1) was mea-
sured in several absolute [3,6,7] and relative rate stud-
ies [6,8,9]. Currently, there is significant disagree-
ment between the reported data concerning both room
Supporting Information is available in the online issue at
www.wileyonlinelibrary.com.
ꢀC
2016 Wiley Periodicals, Inc.

2
MORIN ET AL.
temperature value of k1 (roughly a factor of three
spread) and its temperature dependence. For example,
Nielsen et al. [6] and Shallcross et al. [7] have reported
negative (E/R = –716 K) and positive (E/R = 699
K) temperature dependence of k1, respectively, in the
temperature range 298–373 K. One absolute [6] and
three relative rate measurements [6,8–10] are available
for the rate constant of OH + PNT reaction; however,
temperature dependence of the rate constant has been
investigated in only one study and in a rather narrow
temperature range T = 298–368 K [6].
[12–14], was employed at low temperatures (248–
355 K). The second reactor (Fig. 1S, in the Support-
ing Information), which was recently developed for
high-temperature kinetic studies (up to T = 1000 K),
consisted of a Quartz tube with an electrical heater
and water-cooled extremities [15]. Temperature in the
reactor was measured with a K-type thermocouple po-
sitioned in the middle of the reactor in contact with
its outer surface. The axial temperature gradient along
the flow tube measured with a thermocouple inserted
in the reactor through the movable injector was found
to be less than 1% [15].
Abstraction of an α-hydrogen atoms in organic ni-
trates by OH radicals leads to the formation of an α-
substituted alkyl radicals:
OH radicals were generated in the fast reaction of
hydrogen atoms with NO2, H atoms being produced in
a microwave discharge of H2/He mixture:
OH + CH3CH2ONO2 → CH3C•HONO2 + H2O
H + NO2 → OH + NO
(3)
(1a)
NO2 was always used in excess over H atoms. OH
radicals were detected as HOBr+ (m/z = 96/98) after
scavenging by an excess of Br2 ([Br2] ࣈ 5 × 1013
molecule cm−3, added at the end of the reactor, 5 cm
upstream of the sampling cone) via reaction:
OH + CH3CH2ONO2 → CH3CH2C•HONO2 + H2O
(2a)
These radicals are known to be unstable, dissociating
spontaneously without an energetic barrier to form a
carbonyl compound and NO2 [11]:
OH + Br2 → HOBr + Br
(4)
CH3C•HONO2 → CH3CHO + NO2
This method for OH detection was preferred to the
direct detection of these radicals at m/z = 17 (OH+)
due to significant background signal at this mass. Simi-
larly, the chemical conversion of OH to HOBr was used
for the measurements of the absolute concentrations of
the radicals: [OH] = [HOBr] = ꢀ[Br2], i.e. concen-
trations of OH were determined from the consumed
fraction of [Br2]. [Br2] was determined from the mea-
sured flow rate of known Br2/He mixtures. The possi-
ble influence of secondary chemistry on this method of
HOBr detection and their absolute calibration proce-
dure was discussed in details in previous papers from
this group [12,13].
ENT and PNT were introduced into the flow re-
actor from a 10-L flask containing nitrate–He mix-
ture or by passing helium through a thermostated
glass bubbler containing liquid nitrate and were de-
tected by mass spectrometry at their fragment peaks at
m/z = 76 (CH2ONO2+), which were much more in-
tense than the parent ones (m/z = 91 and 105, re-
spectively). All other species were detected at their
parent peaks: m/z = 44 (acetaldehyde, CH3CHO+), 58
(propanal, C2H5CHO+), 160 (Br2+), 96/98 (HOBr+),
46 (NO2+). The absolute concentrations of the ni-
trates as well as of other stable species in the reactor
were calculated from their flow rates obtained from the
measurements of the pressure drop of mixtures of the
species with helium in calibrated volume flasks.
CH3CH2C•HONO2 → CH3CH2CHO + NO2
In this respect, the measurements of the yield of corre-
sponding carbonyl compound provide the information
on the extent of H-atom abstraction from α carbon. In
the present paper, we report the measurements of the
temperature dependence of k1 and k2 in an extended
temperature range (248–500) K and the yields of the
carbonyl compounds (at T = 300 K), acetaldehyde and
propanal, resulting from α-hydrogen atoms abstraction
by OH in ENT and PNT, respectively.
EXPERIMENTAL
The gas-phase reactions of OH radicals with alkyl ni-
trates were studied at 1 Torr total pressure of helium
over the temperature range 248−500 K. Experiments
were carried out in a discharge flow tube under lami-
nar flow conditions. Modulated molecular beam mass
spectrometer was used to monitor the reactants and
reaction products in the gas phase. Depending on the
temperature range, we have used two different flow re-
actors. The first one, thermostated Pyrex tube (45 cm
length and 2.4 cm i.d.) covered with halocarbon wax
International Journal of Chemical Kinetics DOI 10.1002/kin.21037

KINETICS OF REACTIONS OF ETHYL AND n-PROPYL NITRATES WITH OH RADICALS
3
The nitrates were synthesized in the laboratory via
slow mixing of 5 mL of the corresponding alcohol with
20 mL mixture of H2SO4:HNO3 (1:1) kept at tem-
perature <5°C [16]. After neutralization of the final
solution with water, the supernatant layer was sepa-
rated and mixed with anhydrous magnesium sulfate
to remove remaining water. Finally, the solution was
filtered to retrieve the liquid nitrate. The synthesized ni-
trates were degassed before use. Gas chromatographic
analysis of the nitrates has shown that impurities were
less than 0.1%. The purities and origin of other gases
used were as follows: He > 99.9995% (Alphagaz,
France) was passed through liquid nitrogen traps; H2 >
99.998% (Alphagaz, France); Br2 > 99.99% (Aldrich,
France); NO2 > 99% (Alphagaz, France); acetalde-
hyde > 99.5% (Sigma-Aldrich, France); propanal >
97.0% (Sigma-Aldrich, France).
RESULTS AND DISCUSSION
Rate Constants of Reactions (1) and (2)
The measurements of the rate constants were carried
out under pseudo–first-order conditions in high excess
of nitrates over OH radicals. The initial concentration
of OH radicals was nearly 5 × 1011 molecule cm−3
.
The ranges of the concentrations of nitrates are shown
in Tables I and II. The flow velocity in the reactor
was in the range (660–1660) cm s−1. Examples of the
Table I Summary of the Measurements of the Rate Constant of the Reaction OH + Ethyl Nitrate
c
[C2H5ONO2]
k1
T (K)
Reactor Surfacea
Number of Kineticsb
(1014 molecule cm−3
)
(10−13 cm3 molecule−1s−1
)
248
263
283
298
300
320
340
353
355
388
443
473
500
HW
HW
HW
HW
HW
HW
HW
Q
HW
Q
Q
Q
Q
7
7
6
9
6
6
7
6
6
6
6
7
6
1.1–9.1
0.4–7.4
0.9–8.4
0.2–5.7
0.8–8.1
1.6–9.2
1.3–8.7
0.2–2.7
0.8–7.0
0.4–3.0
0.3–2.9
0.2–2.3
0.3–2.9
1.54
1.74
1.98
2.22
2.15
2.52
2.68
3.09
2.96
3.57
4.56
5.27
5.97
aHW: halocarbon wax, Q: quartz.
bNumber of OH decays recorded.
cEstimated uncertainty on k1 is nearly 15%.
Table II Summary of the Measurements of the Rate Constant of the Reaction OH + n-Propyl nitrate
c)
[C3H7ONO2]
k2
T (K)
Reactor Surfacea
Number of Kineticsb
(1014 molecule cm−3
)
(10−13 cm3 molecule−1s−1
)
263
276
288
298
300
320
340
355
389
415
455
500
HW
HW
HW
HW
HW
HW
HW
HW
Q
6
6
6
7
6
6
6
6
7
7
9
8
0.4–3.0
0.6–4.0
0.5–3.0
0.2–2.3
0.3–2.4
0.4–2.7
0.5–3.2
0.5–3.2
0.2–1.2
0.2–2.3
0.2–1.5
0.2–1.9
4.85
5.18
5.74
6.09
5.80
6.94
7.19
8.13
9.93
11.32
13.78
16.26
Q
Q
Q
aHW: halocarbon wax, Q: quartz.
bNumber of OH decays recorded.
cEstimated uncertainty on k2 is nearly 15%.
International Journal of Chemical Kinetics DOI 10.1002/kin.21037

4
MORIN ET AL.
exponential decays of OH in reaction (2) are shown in
Fig. 1. Figures 2 and 3 show examples of the depen-
dencies of the pseudo–first-order rate constants, k1ꢁ =
k1[ENT] + kw and k2ꢁ = k2[PNT] + kw, on concen-
tration of the corresponding nitrate. kw represents the
rate of OH decay in the absence of nitrate in the reac-
tor. It was measured in separate experiments and did
not show appreciable dependence on temperature be-
ing rather dependent on the state (treatment history) of
the reactor. All the measured values of k1ꢁ and k2ꢁ were
Figure 3 Example of pseudo–first-order plots obtained
from OH decay kinetics in excess of n-propyl nitrate.
corrected for axial and radial diffusion of OH [17]. The
diffusion coefficient of OH in He was calculated using
the following expression: D0 = 640 × (T/298)1.85 Torr
cm2 s−1 [18,19]. Corrections were generally less than
10%; however, in a few kinetic runs they were some-
what higher (up to 19%). The slopes of the straight
lines in Figs. 2 and 3 provide the values of k1 and k2 at
respective temperatures. The intercepts were generally
somewhat higher (however in agreement in the range
of the experimental uncertainty) than the correspond-
ing OH loss rate measured in the absence of nitrates
in the reactor (examples of the measured values of kw
are shown in Fig. 2 for T = 263 and 355 K only for
reason of clarity). The measured values of kw were not
included in the analysis of the data in Figs. 2 and 3, as
the reactor surface may behave differently in the pres-
ence of nitrates. Anyway, the use of kw in the analysis
has very limited impact on the slopes of the straight
lines (within 3%), because (i) the intercepts are very
close to the measured values of kw, (ii) kw is much
lower than the maximum values of k1ꢁ and k2ꢁ, and (iii)
the range of nitrate concentrations used is quite wide.
All the results obtained for k1 and k2 at different tem-
peratures are shown in Tables I and II, respectively.
The lowest temperature in the rate constant measure-
ments (for both reactors used) was limited by impact of
the heterogeneous chemistry which was manifested in
an anomalous increase of the measured rate constant
with decreasing temperature. Highest temperature of
the study (500 K) was limited by thermal decomposi-
tion of the nitrates.
Figure 1 Examples of the exponential decays of OH in
reaction with PNT: T = 500 K.
Figure 2 Example of pseudo–first-order plots obtained
from OH decay kinetics in excess of ethyl nitrate.
International Journal of Chemical Kinetics DOI 10.1002/kin.21037

KINETICS OF REACTIONS OF ETHYL AND n-PROPYL NITRATES WITH OH RADICALS
5
The possible impact on the measurements of the
rate constants of secondary chemistry was explored in
separate series of experiments, where the reaction rate
was measured as a function of initial concentration of
OH. Figure 2S (in the Supporting Information) shows
the results of the measurements of k2ꢁ at a fixed concen-
tration of PNT (1.0 × 1014 molecule cm−3) and OH
estimated to be nearly 15%, including statistical error
(within a few percent) and those on the measurements
of the flows (5%), pressure (2%), temperature (1%),
and the absolute concentrations of the nitrates (ꢀ10%).
Both rate constants increase with temperature, how-
ever deviate from a simple Arrhenius behavior. The
experimental data were fitted with three-parameter ex-
pression, leading to the following results for k1 and
k2:
varied in the range (0.4–4.4) × 1012 molecule cm−3
.
Independence of k2ꢁ of the initial concentration of OH
for [OH]0 < 1012 molecule cm−3 indicates the negligi-
ble contribution of the secondary chemistry to the OH
loss under experimental conditions of the study ([OH]0
ࣈ 5 × 1011 molecule cm−3). Similar picture was also
observed in the case of OH reaction with ENT.
Temperature dependences of k1 and k2 are shown
in Figs. 4 and 5, respectively. The combined uncer-
tainty on the measurements of the rate constants was
k1 = 1.14 × 10−13 (T /298)2.45
× exp (193/T) cm3 molecule−1 s−1
(T = 248–500 K)
k2 = 3.00 × 10−13 (T /298)2.50
× exp (250/T) cm3 molecule−1 s−1
(T = 263–500 K)
with conservative 15% uncertainty.
Previously, the rate constant of reaction (1) was
measured in two room temperature [8,9] and three tem-
perature dependence studies [3,6,7]. All these data are
shown in Fig. 4. Current recommendations for k1 [2,20]
are based on the experimental data from the most ex-
tensive study of reaction (1) by Talukdar et al. [3] who
also observed the curvature of the Arrhenius plot and
fitted the rate constant data to a sum of two exponen-
tials:
k1 = 3.68 × 10−13 (−1077/T)
+ 5.32 × 10−14 exp (126/T) cm3 molecule−1 s−1
Figure 4 Summary of the measurements of the rate con-
stant of the reaction OH + ethyl nitrate. Colored dashed
lines show the temperature dependence of the rate constant
reported in the respective studies.
over the temperature range 223–394 K. One can note
that the experimental data of Talukdar et al. [3] and
those from the present study (fitted to a three-parameter
expression) exhibit identical temperature dependence
(Fig. 4), the absolute values of k1 from the present
study being systematically higher by 10–15%. In this
respect, the expression for k1 obtained in the present
work with somewhat reduced A-factor seems to be a
good compromise between the results of two studies
(black solid line in Fig. 4) and can be recommended
for use over the temperature range 220–500 K:
k1 = 1.05 × 10−13 (T /298)2.45
× exp (193/T) cm3 molecule−1 s−1
It can be noted that the experiments of Talukdar
et al. [3] were carried out at total pressure of 50–300
Torr with different buffer gases (He, N2, SF6), whereas
Figure 5 Summary of the measurements of the rate con-
stant of the reaction OH + n-propyl nitrate.
International Journal of Chemical Kinetics DOI 10.1002/kin.21037

6
MORIN ET AL.
the data from the present study were obtained at nearly
1 Torr pressure of helium. Good agreement between
the results of two studies supports the conclusion of
Talukdar et al. [3] that addition of OH to the alkyl
nitrate is unlikely, reaction is a bimolecular one and
proceeds via abstraction of an H atom from the alkyl
group.
For reaction OH + PNT, three relative [6,8,10] and
one absolute rate [6] measurements are available in the
literature (Fig. 5). Temperature dependence of k2 was
explored in only one study: The Arrhenius expression
k2 = 5.3 × 10−13 exp(140 144/T) cm3 molecule−1
s−1 was reported in the temperature range T = 298–
368 K [6]. On the absolute basis, all the previous
data are in a reasonable agreement with those from
the present work obtained in an extended temper-
ature range. The similarity of the results obtained
in previous studies in 1 atm of air and present
data at 1 Torr total pressure of He seems to in-
dicate that rate constant of reaction (2) is pressure
independent.
Figure 6 Example of kinetics of OH consumption and ac-
etaldehyde formation in reaction of OH radicals with ethyl
nitrate: T = 300 K; [ENT] = 5.0 × 1014 molecule cm−3
.
Reaction Products
In this study, we have determined at T = 300 K the
yield of the carbonyl compounds, acetaldehyde and
propanal, resulting from the abstraction by OH of an α-
hydrogen atom in ethyl and n-propyl nitrates, followed
by α-substituted alkyl radical decomposition. Exam-
ples of the kinetics of the product formation along
with the kinetics of OH consumption are shown in
Fig. 6 and 3S (in the Supporting Information). Solid
and dashed lines in the figures represent the simula-
tion of the experimental profiles of OH (exponential
function) and reaction product, respectively. Tempo-
ral profiles of products are fitted with the following
equation:
kꢁ − kwꢁ
ꢁ
[Product] = a ×
× [OH]0(1 − e−k t
)
kꢁ
where α is the product yield, kꢁ and kw are the first-order
rate constants of OH consumption in the presence and
in the absence (heterogeneous loss) of nitrate in the
reactor, respectively. α was the only fitting parame-
ter. The values of α obtained from the best fit to the
acetaldehyde profile in Fig. 6 and propanal profile in
Fig. 3S (in the Supporting Information) were 0.76 and
0.23, respectively.
The bulk of the experiments on the determination
of the yields of acetaldehyde and propanal in reactions
(1) and (2) consisted of the monitoring of the con-
sumed [OH] and [CH3CHO] (or [C2H5CHO]) formed
at a fixed reaction time of ࣈ 10 ms. Initial concen-
ꢁ
Figure 7 Concentration of acetaldehyde formed in reaction
(1) as a function of the consumed concentration of OH.
trations of the reactants were largely varied: [OH] =
(0.3–2.7) × 1012, [ENT] = (1.8–10.1) × 1014, and
[PNT] = (0.6–5.4) × 1014 molecule cm−3. The exper-
imental data are shown in Figs. 7 and 8. The slopes of
the straight lines in Figs. 7 and 8 provide the yields of
acetaldehyde and propanal in reactions (1) and (2) at
T = 300 K: 0.77
0.12 and 0.22
tively. The estimated nearly 15% uncertainty on the
0.04, respec-
International Journal of Chemical Kinetics DOI 10.1002/kin.21037

KINETICS OF REACTIONS OF ETHYL AND n-PROPYL NITRATES WITH OH RADICALS
7
Atmospheric Implications
The tropospheric lifetimes of ENT and PNT, with re-
spect to their loss in reaction with OH only, calculated
using the measured rate constants (at T = 298 K) and
a 24 h average concentration of the OH radical of 106
molecules cm−3 are 52.6 and 19.2 days, respectively.
The tropospheric lifetimes of these nitrates with re-
spect to their photodissociation reported by Clemit-
shaw et al. [5] for summer conditions are between 3
and 17 days depending on altitude (0–10 km) and lati-
tude (0–60°N). Comparison of these data indicates that
although photolysis is the dominant atmospheric sink
of the nitrates, relative contribution of OH reactions is
appreciable even for small less reactive nitrates.
CONCLUSIONS
Figure 8 Concentration of propanal formed in reaction (2)
In this work, we investigated the kinetics and products
of the reaction of OH radicals with ethyl and n-propyl
nitrates. The reaction rate constants were measured at
T = (248–500) K and, for both reactions, the Arrhe-
nius plots were found to exhibit substantial curvature.
Acetaldehyde and propanal were directly detected as
products of the OH reactions with ENT and PNT for
the first time. Their yields measured at T = 300 K,
0.77 0.12 and 0.22 0.04, respectively, correspond
to the branching ratios for the α-hydrogen atom ab-
straction pathway of the reactions of OH with ENT
and PNT and are in good quantitative agreement with
SAR predictions.
as a function of the consumed concentration of OH.
measurements arises mainly from the combined errors
on the measurements of the absolute concentrations of
OH and corresponding reaction product.
Acetaldehyde and propanal result from the decom-
position of α-substituted alkyl radicals formed upon
initial abstraction by OH of an α-hydrogen atom in
ethyl and n-propyl nitrates, respectively. Their yields
can be considered as the branching ratios for an α-
hydrogen atom abstraction pathway of the respective
reactions:
This study was supported by French National Research
Agency (ANR) through project ONCEM (ANR-12-BS06-
0017-02). J. M. is very grateful for his PhD grant
from CAPRYSSES project (ANR-11-LABX-006-01) funded
by ANR through the PIA (Programme d’Investissement
d’Avenir).
k1a/k1 = 0.77 0.12
k2a/k2 = 0.22 0.04
It can be noted that these values are in good agreement
with those estimated within structure–activity relation-
ship (SAR) [21], 0.77 and 0.24 (calculated with sub-
stituent factor F(–O–NO2) = 0.1) [22], for the extent of
H-atom abstraction from α carbon in ethyl and n-propyl
nitrate, respectively. However, the total rate constants
of the reactions of OH with ENT and PNT calculated
within SAR are lower than the experimental values
by a factor of 1.8 and 1.3 respectively. Currently, we
continue the experimental studies of the kinetics and
products of the OH reactions with other alkyl nitrates
and hope that the gathered kinetic information will al-
low to refine the substituent factors for the –ONO2
containing groups used in the calculations of the rate
constants.
BIBLIOGRAPHY
1. Finlayson-Pitts, B. J.; Pitts, J. N. J. Chemistry of the Up-
per and Lower Atmosphere: Theory, Experiments and
Applications; Academic Press: San Diego, CA 2000.
2. Atkinson, R.; Baulch, D. L.; Cox, R. A.; Crowley, J.
N.; Hampson, R. F.; Hynes, R. G.; Jenkin, M. E.; Rossi,
M. J.; Troe, J. Atmos Chem Phys 2006, 6, 3625–4055.
3. Talukdar, R. K.; Herndon, S. C.; Burkholder, J. B.;
Roberts, J. M.; Ravishankara, A. R. J Chem Soc, Faraday
Trans 1997, 93, 2787–2796.
4. Talukdar, R. K.; Burkholder, J. B.; Hunter, M.; Gilles,
M. K.; Roberts, J. M.; Ravishankara, A. R. J Chem Soc,
Faraday Trans 1997, 93, 2797–2805.
International Journal of Chemical Kinetics DOI 10.1002/kin.21037

8
MORIN ET AL.
5. Clemitshaw, K. C.; Williams, J.; Rattigan, O. V.;
Shallcross, D. E.; Law, K. S.; Anthony Cox, R. J Pho-
tochem Photobiol A 1997, 102, 117–126.
6. Nielsen, O. J.; Sidebottom, H. W.; Donlon, M.; Treacy,
J. Chem Phys Lett 1991, 178, 163–170.
7. Shallcross, D. E.; Biggs, P.; Canosa-Mas, C. E.;
Clemitshaw, K. C.; Harrison, M. G.; Reyes Lopez
Alanon, M.; Pyle, J. A.; Vipond, A.; Wayne, R. P. J
Chem Soc, Faraday Trans 1997, 93, 2807–2811.
8. Kerr, J. A.; Stocker, D. J Atmos Chem 1986, 4, 253–262.
9. Kakesu, M.; Bandow, H.; Takenaka, N.; Maeda, Y.;
Washida, N. Int J Chem Kinet 1997, 29, 933–941.
10. Atkinson, R.; Aschmann, S. M. Int J Chem Kinet 1989,
21, 1123–1129.
11. Vereecken, L. Chem Phys Lett 2008, 466, 127–130.
12. Bedjanian, Y.; Le Bras, G.; Poulet, G. J Phys Chem A
1999, 103, 7017–7025.
15. Morin, J.; Romanias, M. N.; Bedjanian, Y. Int J Chem
Kinet 2015, 47, 629–637.
16. Boschan, R.; Merrow, R. T.; van Dolah, R. W. Chem
Rev 1955, 55, 485–510.
17. Kaufman, F. J Phys Chem 1984, 88, 4909–4917.
18. Bedjanian, Y.; Nguyen, M. L.; Le Bras, G. Atmos Env-
iron 2010, 44, 1754–1760.
19. Ivanov, A. V.; Trakhtenberg, S.; Bertram, A. K.;
Gershenzon, Y. M.; Molina, M. J. J Phys Chem A 2007,
111, 1632–1637.
20. Burkholder, J. B.; S. P. S.; Abbatt, J.; Barker, J. R.;
Huie, R. E.; Kolb, C. E.; Kurylo, M. J.; Orkin, V. L.;
Wilmouth, D. M.; Wine, P. H. Chemical Kinetics and
Photochemical Data for Use in Atmospheric Studies,
Evaluation No. 18; JPL Publication 15-10, Jet Propul-
sion Laboratory: Pasadena, CA, 2015. Avaialbela at
http://jpldataeval.jpl.nasa.gov. Accessed July 7, 2016.
21. Kwok, E. S. C.; Atkinson, R. Atmos Environ 1995, 29,
1685–1695.
13. Bedjanian, Y.; Le Bras, G.; Poulet, G. Int J Chem Kinet
1999, 31, 698–704.
14. Romanias, M. N.; Morin, J.; Bedjanian, Y. Int J Chem
Kinet 2015, 47, 42–49.
22. Atkinson, R. Int J Chem Kinet 1987, 19, 799–
828.
International Journal of Chemical Kinetics DOI 10.1002/kin.21037