Experimental Study of the Reactions of Br Atoms with Thiirane and Nitrosyl Chloride

Abstract

The kinetics of Br-atom reactions with C₂H₄S and ClNO were studied as a function of temperature at a total pressure of 2 Torr of helium using a discharge–flow system combined with mass spectrometry: Br + C₂H₄S → SBr + C₂H₄ (1) and Br + ClNO →BrCl + NO (2). The rate constant of reaction (1) was determined at T = 340–920 K by absolute measurements under pseudo-first-order conditions, either by monitoring the kinetics of Br-atom or C₂H₄S consumption in excess of C₂H₄S or of Br atoms, respectively, and by using a relative rate method: k₁ = (6.6 ± 0.7) × 10⁻¹¹ exp(−(2946 ± 60)/T) cm³molecule⁻¹s⁻¹ (where the uncertainties represent the precision at the 2σ level, the estimated total uncertainty on k₁ being 15% at all temperatures). The rate coefficient of reaction (2), determined either from the kinetics of the formation of the reaction product, BrCl, or from the decays of Br-atoms in an excess of ClNO, showed non-Arrhenius behavior, being practically independent of temperature below 400 K and increasing significantly at temperatures above 500 K. The measured rate constant is well reproduced by a sum of two exponential functions: k₂ = 1.2 × 10⁻¹¹ exp(−19/T) + 8.0 × 10⁻¹¹ exp(−1734/T) cm³ molecule⁻¹ s⁻¹ (with an estimated overall temperature-independent uncertainty of 15%) at T = 225–960 K.

1. Introduction

The peculiarity of the thiirane reactions with different atoms is that they proceed by desulfurization of C₂H₄S, resulting in almost stoichiometric formation of ethylene and corresponding sulfur-containing radicals. In this regard, these reactions, in addition to their theoretical interest, are of practical importance associated with laboratory studies of gas-phase kinetics, where they can potentially be used to generate various sulfur-containing radicals. Previous work has reported kinetic studies of the reactions of C₂H₄S with hydrogen [1,2,3], oxygen [4,5], sulfur [6,7,8] and chlorine atoms [9,10]. In this paper, we report the results of the first experimental study of the reaction of thiirane with bromine atoms:

Br + C₂H₄S → SBr + C₂H₄            Δ_rH° = (9.18 ± 1.25) kJ mol⁻¹

(1)

The enthalpies of formation used for the calculations of Δ_rH° were the following: Δ_fH(298K) = (111.87 ± 0.12), (82.3 ± 1.0), (52.45 ± 0.13) and 150.9 kJ mol⁻¹ for Br [11], C₂H₄S [12], C₂H₄ [11] and SBr [13], respectively. In contrast to the previously studied reactions of thiirane with different atoms, reaction (1) is endothermic and is expected to proceed with a significant activation energy. The aim of this work was to measure the rate constant of reaction (1) as a function of temperature and to obtain information about the reaction mechanism by detecting the expected reaction product, the SBr radical.

In addition, as a part of this study, the rate constant of the reaction of bromine atoms with ClNO was measured. In fact, this reaction was used in the study of reaction (1) for the detection of Br atoms by mass spectrometry through their chemical conversion to the stable species BrCl and as a reference reaction in the relative measurements of k₁:

Br + ClNO → BrCl + NO

(2)

So far, the reaction rate constant has only been measured in two studies, by Clyne and Cruse [14] at room temperature and by Abbatt et al. [15] in the temperature range (229–424) K. In the present work, we report the measurements of the rate constant in an extended temperature range, T = 225–960 K.

2. Results and Discussion

2.1. Rate Constant of Reaction (1)

2.1.1. Absolute Measurements of k₁: Kinetics of Br Atom Consumption

Br atoms were generated from the microwave discharge in trace amounts of molecular bromine in He (Figure 1). The dissociation of Br₂ was verified by mass spectrometry to be between 50 and 95% (increasing with decreasing Br₂ concentration).

Two chemical conversion methods were used to detect Br atoms. In the first, Br atoms were converted to BrCl by reaction (2) with excess ClNO ([ClNO] = (1–2) × 10¹⁴ molecule cm⁻³) prior to introduction into the mass spectrometer (Figure 1) and detected at m/z = 114/116 (BrCl⁺):

k₂ = 1.2 × 10⁻¹¹ exp(−19/T) + 8.0 × 10⁻¹¹ exp(−1734/T) cm³ molecule⁻¹ s⁻¹ (T = 225–960 K, this work). The second method used the reaction of Br atoms with excess I₂ ([I₂] = (2–3) × 10¹³ molecule cm⁻³), converting the Br atoms to IBr, followed by mass spectrometric detection of the IBr⁺ ion at m/z = 206/208:

Br + I₂ → IBr + Br

(3)

k₃ = (1.20 ± 0.15) × 10⁻¹⁰ cm³ molecule⁻¹ s⁻¹ (T = 298 K) [16]. To our knowledge, only the room temperature value of k₃ is available in the literature. However, the rate constant of reaction 3 is not expected to be strongly temperature dependent, given the very high value of k₃ at T = 298 K.

The rate constant of reaction (1) was determined under pseudo-first-order conditions from the kinetics of Br-atom ([Br]₀ = (1.0–2.5) × 10¹¹ molecule cm⁻³) consumption monitored under an excess concentration of C₂H₄S (

Table 1. Summary of the measurements of the rate constant of reaction (1).

T (K)	[Excess Reactant] a	k1 b	Method c
340	2.82–23.6	0.115	AM/Br (ClBr) kinetics
370	0.48–8.31	0.252	AM/Br (ClBr) kinetics
415	0.70–12.4	0.476	AM/Br (ClBr) kinetics
425	1.16–15.5	0.654	AM/Br (ClBr) kinetics
455	0.44–11.0	1.05	AM/Br (IBr) kinetics
470	0.57–12.5	1.18	AM/Br (ClBr) kinetics
500	0.12–1.87	1.93	AM/C2H4S kinetics
505	0.79–6.50	1.90	AM/Br (ClBr) kinetics
535	0.40–6.02	2.77	AM/Br (ClBr) kinetics
535	0.46–9.32	2.40	AM/Br (ClBr) kinetics
585	0.13–1.24	4.35	AM/C2H4S kinetics
625	0.10–3.45	6.18	AM/Br (ClBr) kinetics
625	0.34–6.32	6.06	AM/Br (ClBr) kinetics
660	0.07–0.69	8.77	AM/C2H4S kinetics
700	0.14–2.01	9.56	AM/Br (IBr) kinetics
720	0.19–3.60	10.7	AM/Br (ClBr) kinetics
720		11.7	RRM
735	0.14–1.15	11.9	AM/C2H4S kinetics
760	0.14–1.40	12.6	AM/Br (ClBr) kinetics
805	0.07–1.29	16.2	AM/Br (ClBr) kinetics
857		22.0	RRM
863	0.10–1.73	21.1	AM/Br (ClBr) kinetics
920	0.09–1.65	27.8	AM/Br (ClBr) kinetics

^a units of 10¹⁴ molecule cm⁻³. ^b units of 10⁻¹³ cm³molecule⁻¹s⁻¹; statistical 2σ uncertainty is (2–3)%, total estimated uncertainty on k₁ is 15% and 20% for absolute and relative measurements, respectively. ^c AM/Br (ClBr) and AM/Br (IBr): absolute measurements of k₁ from Br kinetics in an excess of C₂H₄S with Br detection as ClBr and IBr (see text), respectively; AM/C₂H₄S kinetics: absolute measurements of k₁ from kinetics of C₂H₄S in an excess of Br atom; RRM: relative rate method.

).

Consumption of the excess reactant, C₂H₄S, was negligible due to its high excess over Br atoms. Figure 2 shows examples of exponential decays of Br atoms in the presence of different concentrations of thiirane in the reactor: [Br] = [Br]₀ × exp(−k₁′ × t), where k₁′ = k₁ × [C₂H₄S] + k_w is a pseudo-first order rate constant and k_w is the rate of heterogeneous loss of Br atoms.

Examples of second-order plots observed at different temperatures are shown in Figure 3. All data in Figure 3 were measured with Br detected as BrCl after its chemical conversion in reaction (2).

Similar quality data were obtained when Br was detected by conversion to IBr in reaction (3) (Figure 4). All pseudo-first order rate constants, k₁′, were corrected for axial and radial diffusion of Br atoms [17]: k₁′(corrected) = k₁′ × (1 + D_effk₁′/v²), where D_eff = D + r²v²/48D (D is the diffusion coefficient of Br in He calculated as D₀ = 480 × (T/298)^1.85 Torr cm⁻² s⁻¹ [18], v is a linear flow velocity and r is the reactor radius). The corrections were typically a few percent.

The rate constants of the reaction (1), obtained from a linear least-squares fit of the k₁′ data as a function of [C₂H₄S], are given in Table 1. Good agreement can be observed between the results obtained with two methods of Br-atom detection, using chemical conversion of Br to BrCl and IBr in reactions (2) and (3), respectively.

SBr was directly detected by mass spectrometry as the product of reaction (1) at m/z = 111/113 (SBr⁺). The addition of I₂ at the end of the reactor (Figure 1) resulted in the appearance of mass spectrometric signals at m/z = 238/240 (ISBr⁺) and m/z = 159 (IS⁺) (ISBr fragment), indicating the occurrence of the reaction SBr + I₂ → ISBr + I, leading to the formation of ISBr. Although the absolute concentrations of SBr were not measured, judging from the relative mass spectrometric signals, the SBr formation channel is the main and, probably, the only reaction channel under the experimental conditions of the study. Attempts to detect HBr as another potential reaction product showed that its yield was less than 3% at T = 920 K, the highest temperature of the study.

The thermal decomposition of thiirane under the experimental conditions of the study was rather slow, at least without any noticeable effect on the C₂H₄S concentration along the reaction zone. An indirect indicator of the C₂H₄S decomposition was the formation of S₂ (detected at m/z = 64 (S₂⁺), ~0.3% of the C₂H₄S signal intensity in experiments at T = 920 K), most likely, in the reaction sequence:

C₂H₄S + M → C₂H₄ + S + M

(4)

S + C₂H₄S → S₂ + C₂H₄

(5)

Secondary reactions leading to additional consumption or reproduction of Br atoms in the chemical system used with potential impact on k₁ measurements can be discussed. First, the influence of the secondary reaction of Br atoms with C₂H₄ formed in reaction (1) can be neglected due to the low initial concentrations of Br atoms used in the kinetic measurements (and hence the low concentration of the reaction product C₂H₄). For the same reason, the potential consumption of Br in the reaction with SBr and Br reproduction in the reverse reaction of SBr with C₂H₄ should not have a significant effect on the k₁ measurements. Other potential candidates for reproducing Br atoms include the reactions of SBr:

SBr + Br₂ → Br + SBr₂

(6)

SBr + SBr → 2Br + S₂

(7)

SBr + SBr → Br + SSBr

(8)

To the best of our knowledge, there is a paucity of data in the literature on the rate constants of these reactions. However, their significant influence on the present measurements can be ruled out based on general considerations. Thus, a significant effect of reaction (6) on Br kinetics under experimental conditions is unlikely given very low Br₂ concentrations (≤3 × 10¹⁰ molecule cm⁻³) in the reactor. Reaction (7) is endothermic by 50.5 kJ mol⁻¹ [11,13]. There are no thermochemical arguments (the enthalpy of SSBr formation is unknown) to exclude the occurrence of reaction (8) in our experiments. However, even if reaction (8) occurs, its impact should be limited given the low initial concentrations of Br atoms (and hence SBr) used in the kinetic measurements.

2.1.2. Absolute Measurements of k₁: Kinetics of C₂H₄S Consumption

Although potential secondary chemistry appears to have a limited impact on the measurements of k₁, to be more confident of its minor role we performed experiments in which k₁ was determined from C₂H₄S decays ([C₂H₄S]₀ = (2–5) × 10¹¹ molecule cm⁻³) monitored in excess of Br atoms (Table 1). Examples of the concentration vs. time profiles of thiirane observed at T = 735 K with different concentrations of Br atoms are shown in Figure 5: [C₂H₄S] = [C₂H₄S]₀ × exp(−k₁′ × t), where k₁′ = k₁ × [Br] is the pseudo-first order rate constant and [Br] corresponds to the average Br-atom concentration along the reaction zone. In fact, the Br-atom consumption was insignificant and was mainly due to the heterogeneous loss of the atoms (k_w < 10 s⁻¹). The Br atoms consumed in the reaction with C₂H₄S were, at least, partially reproduced in reaction (6) between SBr, the product of reaction (1), and Br₂ still present in the reactor as a precursor of the Br atoms (incomplete dissociation in the microwave discharge).

The second-order plots observed in this series of experiments at different temperatures are shown in Figure 6. The corresponding values of k₁ derived from linear least squares fit of these data at each temperature are given in Table 1.

2.1.3. Relative Measurements of k₁

In addition to the absolute measurements, at two temperatures, the rate constant of reaction (1) was measured relative to that of the reaction of Br atoms with ClNO (reaction (2)). The experiments consisted of measuring the yield of BrCl as a function of the [C₂H₄S]/[ClNO] ratio after complete consumption of [Br]₀ (≈3 × 10¹¹ molecule cm⁻³) in the reaction with a mixture of C₂H₄S and ClNO ([C₂H₄S] = (0.16–3.37) × 10¹⁴ and (0.15–5.41) × 10¹⁴ molecule cm⁻³, ([ClNO] ≈ 1 × 10¹³ and 2.3 × 10¹³ molecule cm⁻³ at T = 720 and 860 K, respectively):

$$\left[\mathrm{BrCl}\right]={\displaystyle \frac{k_2\left[\mathrm{ClNO}\right]}{k_2\left[\mathrm{ClNO}\right]+k_1\left[{\mathrm{C}}_2{\mathrm{H}}_4\mathrm{S}\right]+k_w}}\times {\left[\mathrm{Br}\right]}_0$$

(9)

Transforming this expression, we obtain:

$${\displaystyle \frac{{\left[\mathrm{Br}\right]}_0}{\left[\mathrm{B}\mathrm{r}\mathrm{C}\mathrm{l}\right]}}-1={\displaystyle \frac{k_1\left[{\mathrm{C}}_2{\mathrm{H}}_4\mathrm{S}\right]}{k_2\left[\mathrm{C}\mathrm{l}\mathrm{N}\mathrm{O}\right]}}+{\displaystyle \frac{k_{\mathrm{w}}}{k_2\left[\mathrm{C}\mathrm{l}\mathrm{N}\mathrm{O}\right]}}$$

(10)

At a constant concentration of ClNO, the second term in Equation (10) is constant, and the k₁/k₂ ratio can be determined as the slope of the linear dependence of ([Br]₀/[BrCl] − 1) on the [C₂H₄S]/[ClNO] ratio. The initial concentration of Br atoms, [Br]₀, could be expressed in terms of the BrCl signal by titration of Br in reaction with ClNO in the absence of C₂H₄S in the reactor ([Br]₀ = [BrCl]₀), thus avoiding the measurement of absolute Br and BrCl concentrations. The observed experimental data are shown in Figure 7. The final values of k₁, calculated using the ratios of k₁ to k₂ determined from the slopes of the straight lines in Figure 7 and k₂ measured in the present work (see below), are given in Table 1.

2.1.4. Temperature Dependence of k₁

The results of all measurements of the rate constant of the reaction (1) are displayed in Figure 8.

A very good agreement can be observed between the values of k₁ measured with the relative and two absolute measurement methods. The combined uncertainty on the absolute measurements of k₁ was estimated to be ≤15% by adding in quadrature statistical error (≤3%) and those on the measurements of the absolute concentration of C₂H₄S (Br) (~10%), flows (3%), pressure (2%) and temperature (1%).

The observed temperature dependence of k₁ can be described by the following Arrhenius expression:

k₁ = (6.6 ± 0.7) × 10⁻¹¹ exp(−(2946 ± 60)/T) cm³molecule⁻¹s⁻¹

in the temperature range from 340 to 920 K and with 2σ uncertainties representing the precision of the fit. It can be noted that the experimentally determined activation energy (≈24.5 kJ mol⁻¹) significantly exceeds the endothermicity of the reaction (≈9.2 kJ mol⁻¹), which obviously indicates that reaction (1) proceeds through a transition state located well above the energy of the reaction products. Consequently, the reverse addition–elimination reaction of SBr radicals with C₂H₄ is expected to proceed with a significant activation energy.

2.2. Rate Constant of Reaction (2)

2.2.1. Kinetics of Br Atom Consumption

In this series of experiments, the rate constant of reaction (2) was determined under pseudo-first order conditions by monitoring the kinetics of Br-atom consumption in excess of ClNO. Br atoms were converted to IBr prior to sampling in the mass spectrometer and were detected at m/z = 206/208 (Figure 9). As expected, exponential [Br] decays were observed, [Br] = [Br]₀ × exp(−k₂′ × t), where [Br] and [Br]₀ ([Br]₀ = (1.0–2.5) × 10¹¹ molecule cm⁻³) are the time-dependent and initial concentrations of Br atoms, respectively, and k₂′ = k₂ × [ClNO] + k_w. The pseudo-first-order rate constants were determined from an exponential fit to the Br atom consumption kinetics. Diffusion corrections applied to k₂′ were <10%. The consumption of excess reactant, ClNO, in reaction (2), although insignificant (<10%), was taken into account. At the highest temperature of the study, T = 960 K, a slow thermal decomposition of ClNO (within a few %) was observed, as evidenced by the formation of Cl₂ as a result of two consecutive reactions:

ClNO + M → Cl + NO + M

(11)

Cl + ClNO → Cl₂ + NO

(12)

This process did not affect the Br-atom kinetics; appropriate corrections were made to the ClNO concentration.

Examples of the dependence of the pseudo-first order rate constant, k₂′, on the concentration of ClNO at different temperatures are shown in Figure 10. The values of k₂ at different temperatures, obtained by linear least squares fitting of kinetic data similar to those shown in Figure 10, are given in

Table 2. Summary of the measurements of the rate constant of reaction (2).

T (K)	[ClNO] a	k1 b	Reactor Surface c	Method d
225	0.12–2.52	1.31	HW	BrCl kinetics
245	0.16–2.83	1.30	HW	BrCl kinetics
265	0.27–2.68	1.28	HW	BrCl kinetics
280	0.27–3.26	1.31	HW	Br kinetics
297	0.16–2.95	1.30	HW	BrCl kinetics
300	0.24–3.00	1.27	Q	Br kinetics
320	0.17–3.23	1.28	HW	Br kinetics
340	0.19–3.39	1.30	Q	Br kinetics
360	0.10–4.08	1.28	Q	Br kinetics
390	0.30–2.67	1.39	Q	Br kinetics
420	0.14–3.69	1.38	Q	Br kinetics
460	0.22–2.44	1.47	Q	Br kinetics
500	0.34–6.32	1.50	Q	Br kinetics
560	0.14–2.62	1.58	Q	Br kinetics
630	0.14–2.01	1.73	Q	Br kinetics
660	0.16–1.24	1.76	Q	BrCl kinetics
710	0.11–1.87	1.91	Q	Br kinetics
780	0.09–1.41	2.12	Q	Br kinetics
860	0.10–1.35	2.29	Q	Br kinetics
960	0.10–1.44	2.52	Q	Br kinetics

^a Units of 10¹³ molecule cm⁻³. ^b units of 10⁻¹¹ cm³molecule⁻¹s⁻¹; statistical 2σ uncertainty is (2–3)%, total estimated uncertainty on k₁ is 15%. ^c HW: halocarbon wax; Q: quartz. ^d Br kinetics: k₁ determined from kinetics of Br consumption; BrCl kinetics: k₁ determined from kinetics of BrCl production.

.

2.2.2. Kinetics of BrCl Production

At low temperatures, the detection of Br atoms by their conversion to IBr was difficult due to I₂ condensation. For this reason, the reaction rate constant was determined from the kinetics of the formation of the reaction product, BrCl, monitored in an I₂-free system under experimental conditions similar to those used above in the study of Br kinetics. The kinetics of the reaction product can be approximated by the following expression: [BrCl] = [Br]₀ − [Br]₀ × exp(−k₂′t) where k₂′ ≈ k₂ × [ClNO], provided that k_w << k₂ × [ClNO]. The latter condition is satisfied at least at high ClNO concentrations, given that k_w < 10 s⁻¹. A rearrangement of this expression gives [BrCl]_∞ − [BrCl] = [BrCl]_∞ × exp(−k₂′t), where [BrCl]_∞ = [Br]₀ was determined by titration of bromine atoms with high concentrations of ClNO. In experiments, the kinetics of [BrCl] growth was monitored and [BrCl]_∞ − [BrCl] was plotted as a function of time, yielding the values of k₂′. Examples of the dependence of the pseudo-first order rate constant, k₂′ ≈ k₂ × [ClNO], on ClNO concentration are shown in Figure 11. The slopes of the straight lines in Figure 11 provide the values of k₂ at corresponding temperatures. All k₂ data determined within this experimental approach are shown in Table 2.

2.2.3. Temperature Dependence of k₂

The results of the previous and current measurements of k₂ are shown in Figure 12.

Abbatt et al. [15] measured the rate constant of reaction (2) as a function of temperature (T = 225–425 K) in a discharge flow reactor using resonance fluorescence technique to detect Br atoms. The results obtained by these authors for k₂ are in excellent agreement with the present measurements (Figure 12). The room temperature value of k₂ = (1.0 ± 0.2) × 10⁻¹¹ cm³ molecule⁻¹s⁻¹ reported by Clyne and Cruse [14] is somewhat lower, but agrees with the present data within the reported uncertainties.

The present measurements, carried out over an extended temperature range, revealed a curved temperature dependence of the rate constant: k₂, which is practically independent of temperature below 400 K, increases significantly at temperatures above 500 K. The solid line in Figure 12 represents a fit of the present experimental k₂-values to the sum of two exponential functions:

k₂ = 1.2 × 10⁻¹¹ exp(−19/T) + 8.0 × 10⁻¹¹ exp(−1734/T) cm³ molecule⁻¹ s⁻¹

This expression reproduces all experimental data to within 3% and is recommended from the present work for the rate constant of reaction (2) in the temperature range T = (225–960) K with conservative independent of temperature uncertainty of 15%. The experimental data can also be described with temperature independent k₂ = (1.3 ± 0.2) × 10⁻¹¹ cm³ molecule⁻¹ s⁻¹ at T = (225–340) K and modified Arrhenius expression of k₂ = 6.33 × 10⁻¹⁶ × (T)^1.47exp(455/T) cm³ molecule⁻¹ s⁻¹ (uncertainty of 15%) at T = 340–960 K.

In the previous work [19], a non-Arrhenius curved temperature dependence was observed for the rate constant of the ClNO reaction with OH radicals. The reaction was shown to proceed via two competing pathways with comparable branching ratios: Cl-atom abstraction,

OH + ClNO → HOCl + NO

(13)

and the exchange reaction (14), which probably proceeds by an addition–elimination mechanism,

OH + ClNO → Cl + HONO

(14)

Interestingly, a non-Arrhenius behavior (increasing upward curvature of the reaction rate constant with temperature) was observed for both reaction channels.

For the reaction of Br atoms with ClNO, the second possible channel is too endothermic [11] to compete with the BrCl forming pathway under the experimental conditions of the study:

Br + ClNO → Cl + BrNO         Δ_rH° = 37.3 kJ mol⁻¹

(15)

At this stage, it is difficult to clearly explain the observed curvature of the temperature dependence of k₂. One possible reason is the complex nature of reaction (2), including direct Cl-atom abstraction by the Br-atom and the Br addition–BrCl elimination mechanism.

3. Materials and Methods

All measurements were performed at a total helium pressure of approximately 2 Torr using a discharge flow reactor and a modulated molecular beam mass spectrometer with electron impact ionization operating at 30 eV energy.^1,4 The reaction time was determined by the position of the tip of the movable injector relative to the sampling cone of the mass spectrometer (Figure 1 and Figure 9) and by the linear flow velocity in the reactor ((750–2520) and (1780–2650) cm s⁻¹ for the study of reactions (1) and (2), respectively). The chemical composition of the reactive system in the reactor was monitored by sampling the gas-phase molecules from the flow reactor and detecting them with the mass spectrometer. Two flow reactors were used to provide an extended temperature range for kinetic measurements. The high-temperature reactor consisted of an electrically heated quartz tube (45 cm long and 2.5 cm i.d.) with water-cooled attachments (Figure 1) [20]. Water cooling was necessary to prevent overheating of the mass spectrometer sampling cone (Pyrex) and the main reactor vacuum connections. The temperature in the reactor was measured with a K-type thermocouple positioned in the middle of the reactor in contact with its outer surface [20]. The second flow reactor used at low temperatures consisted of a Pyrex tube (45 cm long and 2.4 cm i.d., coated with halocarbon wax) with a jacket for the circulation of a thermostated liquid (ethanol) (Figure 9).

Gas mixtures were prepared in 10 L glass cylinders by adding helium to a known amount (pressure) of compounds up to a total pressure of 1 atmosphere. Absolute concentrations of Br atoms, generated in a microwave discharge of Br₂/He mixtures, were determined by measuring the dissociated fraction of Br₂ (Δ[Br₂]) and/or the concentration of ClNO consumed (Δ[ClNO]) upon titration of Br atoms in the reaction (2): [Br] = [BrCl] = 2Δ[Br₂] = Δ[ClNO]. The results of the two calibration methods (by Br₂ and ClNO) were in agreement within 5%. The absolute concentrations of C₂H₄S, ClNO and Br₂ in the reactor were calculated from their flow rates obtained from pressure drop measurements in their mixtures in He (≈5%, 20% and 10%, respectively) stored in calibrated volumes.

The purities of the gases used were as follows: He > 99.999% (Alphagaz, Air Liquide France Industrie, Paris, France); Br₂ > 99.99% (Aldrich, St. Louis, MO, USA); F₂, 5% in helium (Alphagaz); C₂H₄S (Merck, Merck SA, Lyon, France), 98%. ClNO was synthesized in the laboratory using a mixture of Cl₂ and NO [21]. The content of Cl₂ and NO impurities in ClNO was estimated to be less than 1 and 2%, respectively.