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Logo of nihpaAbout Author manuscriptsSubmit a manuscriptHHS Public Access; Author Manuscript; Accepted for publication in peer reviewed journal;
 
J Phys Chem A. Author manuscript; available in PMC 2010 October 1.
Published in final edited form as:
PMCID: PMC2785229
NIHMSID: NIHMS144561

Kinetics of the Gas-Phase Reaction of OH with Chlorobenzene

Abstract

The kinetics of the reaction of hydroxyl radicals with chlorobenzene was studied experimentally using a pulsed laser photolysis/pulsed laser induced fluorescence technique over a wide range of temperatures, 298-670 K, and at pressures between 13.33 and 39.92 kPa. The bimolecular rate constants demonstrate different behavior at low and high temperatures. At room temperature, T = 298.8±1.5 K, the rate constant is equal to (6.02 ± 0.34)×10-13 cm3 molecule-1 s-1; at high temperatures (474 - 670 K), the rate constant values are significantly lower and have a positive temperature dependence that can be described by an Arrhenius expression k1(T ) = (1.01 ± 0.35)×10-11 exp[(-2490 ± 170 K)/T] cm3 molecule-1 s-1. This behavior is consistent with the low-temperature reaction being dominated by reversible addition and the high-temperature reaction representing abstraction and addition-elimination channels. The potential energy surface of the reaction was studied using quantum chemical methods and a transition state theory model was developed for all reaction channels. The temperature dependences of the high-temperature rate constants obtained in calculations using the method of isodesmic reactions for transition states (IRTS) and the CBS-QB3 method are in very good agreement with experiment, with deviations smaller than the estimated experimental uncertainties. The G3//B3LYP-based calculated rate constants are in disagreement with the experimental values. The IRTS-based model was used to provide modified Arrhenius expressions for the temperature dependences of the rate constant for the abstraction and addition-elimination (Cl replacement) channels of the reaction.

I. Introduction

Understanding the reactions of chlorinated hydrocarbons is an essential component of efficient incineration of hazardous wastes, assessing the environmental effects of open burning of wastes, and developing methods for production of chlorine-containing commoditites. Reaction kinetic modeling of these processes is important to optimizing their efficiency and developing tools to otherwise minimize their impacts on human health and welfare. However, success of such modeling is limited by the lack of fundamental information on the rates and products of a large number of elementary reactions involving chlorinated hydrocarbon species.1

The hydroxyl radical plays a key role in the chemistry of combustion processes, with initial attacks by OH on closed-shell species serving as a source of a large variety of reactive radical intermediates. In this work we report the results of our experimental and computational study of the gas-phase reaction of the hydroxyl radical with chlorobenzene

OH+C6H5Clproducts
(1)

Reaction 1 has previously been studied experimentally.2-5 The only earlier direct determination of the rate constant, that of Wallington et al.,3 focused on the low-temperature range, where addition to the benzene ring is the dominant process. The maximum experimental temperature was 438 K, where the reverse of the addition reaction became dominant, and the abstraction and substitution channels just began to become important. However, only two data points (at 363 K and 438 K) were determined at temperatures where reverse reaction was important. The observed absence of a positive temperature dependence suggests that the experimental temperatures were not sufficiently high for the reversible addition reaction to become unimportant compared to the abstraction and displacement channels. The only study at higher temperature where the addition is completely reversed is that of Mulder and Louw.4 These authors used a relative rates technique to determine the ratio of the rate constant of reaction 1 to that of the reaction of OH with benzene at one temperature, 563 K.

The current experimental study of the kinetics of reaction 1 has been performed over a wide temperature range from 298 K (to compare with the earlier low-temperature studies) to 670 K. The temperature dependence of the rate constant was determined under the high-temperature conditions where the reaction is dominated by H abstraction and Cl displacement channels that are more relevant to combustion conditions. The kinetics and mechanism of reaction 1 were studied computationally, with the results providing recommendations for the temperature dependences of the rate constants of these channels over wide temperature ranges.

II. Experimental

II.1. Experimental Technique

Absolute rate coefficients for the reaction of hydroxyl radicals with chlorobenzene were measured using the pulsed laser photolysis/pulsed laser induced fluorescence (PLP/PLIF) technique. All experiments were carried out in a slow-flow, heatable quartz reactor (reaction cell) under pseudo-first-order conditions with a large excess of chlorobenzene. A detailed description of the experimental set-up, data acquisition methodology, and data processing has been given in our previous articles.6,7 Therefore, only the details necessary to understand the present measurements are considered here.

Hydroxyl radicals were generated by the 351-nm (XeF excimer) pulsed laser photolysis (the repetition frequency was 10 Hz) dissociation of HONO molecules8,9

HONO+hv(351nm)OH+NO
(2)

This method of the OH generation was applied to eliminate the possible effects of the laser photolysis excitation and dissociation of chlorobenzene on the observed OH decay rates (vide infra).

After the excimer laser pulse, a second pulse at approximately 282 nm from a Nd:YAG-pumped, frequency-doubled, tunable pulsed dye laser induced excitation of the hydroxyl radicals via the A 2Σ+ — X 2Π (1 — 0) transition. Hydroxyl radicals were observed via fluorescence from the (1 — 1) and (0 — 0) bands at 308 — 316 nm.9,10 The fluorescent radiation emitted perpendicular to the plane defined by the two laser beams was detected with a photomultiplier tube, using appropriate filters (308 nm peak transmission) to minimize the contribution of scattered light. The signal from the photomultiplier was amplified and then recorded by a digital oscilloscope. The oscilloscope obtained the integrated voltage averaged for a desired number of the accumulated signals (typically 100 — 200) at a given time delay between the excimer laser and Nd:YAG laser pulses. This time delay was varied to record kinetic information using a digital delay generator. The value, St, received from the integration of the average voltage signal is a sum of two components: the integral from the average LIF signal of OH radicals, SOH, which is proportional to the absolute OH concentration, and the integral from the average scattered light signal, Ssc. Ssc was directly measured in the absence of the hydroxyl radicals in the reactor.

We used four individually controlled flows of N2 or He (main carrier gas flow), H2O/ N2 or He, HONO/ N2 or He, and C6H5Cl/N2 or He to prepare a reaction gas mixture. H2O was transported to the reaction cell by bubbling a flow of N2 or He through water at controlled pressure and temperature in a thermostabilized saturator. HONO was made from the drop-wise addition of a 0.2 M aqueous solution of NaNO2 to a 20% sulfuric acid aqueous solution in a flask or a saturator which were kept in an ice bath (at temperature near 0 °C). The small flow of N2 or He through the flask or the saturator was varied to control the HONO concentration entering the reaction cell. These mixtures were replaced daily.8 Chlorobenzene was accurately, manometrically diluted with nitrogen or helium using a Pyrex vacuum system. To minimize systematic error in chlorobenzene concentration determinations, mixtures of C6H5Cl in N2 or He were prepared with different concentrations of chlorobenzene in the range 0.72 - 0.98 %. All flows were premixed using a delivery system and then directed through the reaction cell. The total flow rate ranged between 5.8 and 9.6 STP cm3 s-1. The total pressure in the reactor was measured with the 100.00 or 1000.0 Torr (1 Torr = 133.322 Pa) capacitance manometers. The reaction gas temperature in the detection zone was monitored with a retractable Chromel-Alumel thermocouple. The maximum total uncertainty in the measurements of the reaction temperatures, T, did not exceed 0.5% of T.6,7

The molecular concentration of chlorobenzene in the detection zone was calculated by means of multiplying the three values: the total concentration derived from the measured total pressure and temperature using the ideal gas law, the molecular partial concentration in the flow carrying chlorobenzene, and the value from the ratio of the flow carrying chlorobenzene to the total gas flow rate.

The chemicals utilized in this work had the following specified minimum purities (and were supplied by): N2, 99.999% (Capitol Welders Supply Co.); He, 99.999% (Capitol Welders Supply Co.); H2O, A.C.S. reagent grade (Sigma-Aldrich); H2SO4, 95-98% aqueous solution, A.C.S. reagent grade (Sigma-Aldrich); NaNO2, 99.5%, super free-flowing (Sigma-Aldrich); C6H5Cl, 99.99%, CHROMASOLVR, for HPLC (Sigma-Aldrich). Chlorobenzene was purified by vacuum distillations prior to use. The chemical purities of this sample was examined by GC/MS (Agilent Technologies 6890N Gas Chromatography System/5973 Mass Selective Detector). After purification by vacuum distillation, the purity of the sample of chlorobenzene exceeded the specifications provided by Sigma-Aldrich and was at least 99.996%. The GC/MS analysis revealed the presence of benzene in the sample of chlorobenzene as the main impurity at level less than 0.0036% and only trace levels of others impurities. These small concentrations had a negligible effect on the observed OH decay rates.

II.2. Reaction Rate Measurements and Data Processing

All experiments measuring the bimolecular rate coefficients for the reaction of OH with C6H5Cl were performed under pseudo-first-order kinetics conditions with a large excess of chlorobenzene with respect to the initial concentration of the hydroxyl radical, [OH]0, ranging approximately from 8×1010 to 7×1011 molecule cm-3 in the detection zone. The initial concentrations of OH radicals were estimated in way similar to that previously described.8 Accurate knowledge of the initial OH radical concentration is not needed to determine the bimolecular rate coefficients because all experiments were performed under pseudo-first-order conditions with a large excess of chlorobenzene. The estimated OH radical detection limit, defined by unity signal-to-noise ratio at 150 accumulated signals, was found to range from 1×108 to 6×108 molecule cm-3 depending on experimental conditions.

A typical set of relative OH concentration temporal profiles (a set of experiments) are depicted in Figure 1 as a plot of ln(SOH) = ln(St - Ssc) versus time delays, t. Water vapor was always added to the reaction mixtures at concentrations that were varied from 1.5×1015 to 1.4×1016 molecule cm-3 from set to set of experiments. This was done to ensure that the rotational and vibrational equilibration of OH radicals to the Boltzmann distribution proceeded sufficiently fast to have a negligible effect on the measured rate coefficients.11 Furthermore, over the entire experimental temperature range, temporal profiles of the formation of OH (X 2Π, ν = 0) under typical experimental conditions in the absence of chlorobenzene were also obtained. Prompt OH (X 2Π, ν = 0) formation was observed that was always much faster ( at least 4 times) than the initial detection time delays, t0, in all relative OH concentration decays used in the rate constant determinations. This indicates that the rotational and vibrational equilibration of OH radicals to the Boltzmann distribution proceeded fast enough to be neglected at the time delays tt0 that would have otherwise led to non-prompt OH (X 2Π, ν = 0) formation.

Figure 1
Examples of relative OH concentration temporal profiles obtained under the following experimental conditions: nitrogen buffer gas; temperature T = 665 K; total pressure P = 26.72 kPa (200.4 Torr); [H2O] = 1.1×1016 molecule cm-3; [HONO] ≈ ...

Each set of experiments was analyzed assuming pseudo-first-order kinetics behavior of the hydroxyl radical decay to determine bimolecular rate coefficients of the OH + C6H5Cl reaction:

ln(SOH)=ln(StSsc)=constantkt
(I)

where the effective first-order rate coefficient, k’, is given by

k=k1[C6H5Cl]+k0
(II)

Here, k1 is the bimolecular rate coefficient of the reaction OH + C6H5Cl, [C6H5Cl] is the molecular concentration of chlorobenzene; and k0 is the effective first-order rate coefficient of the hydroxyl radical decay due to OH reaction with HONO, possible OH reactions with background impurities in the buffer gas, H2O, and HONO, and OH diffusion and flow out of the detection zone (OH background loss). The effective first-order rate coefficient values, k’, were derived from linear least-squares fits of the experimental values ln(SOH) to equation I. These least-squares fits and all next least-squares fits in the present work were performed with no weighting of the data points.

Examples of effective first-order rate coefficient dependencies on molecular chlorobenzene concentration are presented in Figure 2. We determined the bimolecular rate coefficient, k1, from the slope of the least-squares straight line drawn through the k’ versus [C6H5Cl] data points including the (0, k0) point, where k0 was derived from the OH temporal profile directly measured at zero concentration of the molecular substrate.

Figure 2
Examples of experimentally obtained k’ versus [C6H5Cl] dependences.

II.3. Experimental Results

The kinetics study of the gas-phase OH radical reaction with C6H5Cl was performed over the temperature range of 298 — 670 K and at pressures between 13.33 and 39.92 kPa. The conditions and results of the experiments used to determine the values of the absolute bimolecular rate coefficients for reaction 1 are compiled in Table 1.

TABLE 1
Conditions and Results of Experiments on the Reaction of Hydroxyl Radicals with Chlorobenzene

The initial concentration of hydroxyl radicals was varied from experimental set to set by changing the photolysis laser intensity or the concentration of HONO over wide ranges: 26 - 64 mJ pulse-1 cm-2 and 1013 - 6×1013 molecule cm-3, respectively. The measured rate coefficients demonstrate no correlation with pressure and initial concentration of OH radicals within the experimental ranges. The fact that the rate coefficients are independent of the initial OH radical concentration indicates the absence of any influence from potential secondary reactions on the kinetics of OH radical decay due to the low values of [OH]0 in the detection zone ([OH]0 ≈ (8 - 70)×1010 molecule cm-3). There was no correlation between the measured rate coefficients and the photolysis laser intensity within the experimental range. This fact allows one to consider the possible effects of the reaction between OH and the products of laser photolysis of C6H5Cl on the rate coefficient measurements as negligible in our experiments. At the highest temperatures in this study, the absence of any potential influence from thermal decomposition of chlorobenzene and HONO on the final results was verified by measuring the bimolecular rate coefficients at different bulk flow velocities and reaction pressures that varied by factors 1.3 and 1.5, respectively.

We could not measure the absolute bimolecular rate coefficient for the reaction of OH with C6H5Cl in the temperature range ~ 350 - 450 K because non-exponential OH decays were observed under these experimental conditions. Similar behavior was observed in previous works3,12 for the OH reactions with benzene and halogenated benzene. The explanation is as follows. At room temperature and lower, the addition channels probably dominate the reaction of hydroxyl radical with chlorobenzene, resulting in formation of three different C6H5ClOH isomers as the main products. These radicals are stabilized by buffer gas and do not decompose at the time of detection. At temperatures between ~ 350 and 450 K, decomposition of C6H5ClOH becomes important on the time scale of the experiments and relaxation to equilibrium in the reversible addition process results in non-exponential OH decay profiles. At temperatures above ~ 450K and pressures above ~ 100 Torr of nitrogen, the addition channels are completely reversed and thus provide practically no contribution to OH decay.

In the temperature range of 474 - 670 K the kinetics of the OH decays followed the pseudo-first-order law and the derived bimolecular rate coefficients from our experimental data did not correlate with reaction pressure. The bimolecular rate coefficients for the OH + C6H5Cl reaction determined in our study are plotted along with those from the earlier studies2-4 in Figure 3. The k1(T) rate coefficient data set for reaction 1 exhibits a positive temperature dependence in the temperature range of 474 - 670 K. The linear least-squares fit of this data set to the Arrhenius expression yields the following expression for the bimolecular rate constant temperature dependence:

k1(T)=(1.01±0.35)×1011exp[(2490±170K)T]cm3molecule1s1(474670K)
(III)

This Arrhenius expression reproduces the experimental data very well, with the maximum and the average square deviations being only 7.5% and 4.4%, respectively.

Figure 3
Temperature dependence of the bimolecular rate coefficient for the reaction of OH with C6H5Cl displayed in Arrhenius coordinates. Symbols represent the experimental data from several groups. Filled circles, results of the current study; open circles, ...

III. Potential Energy Surface and Transition-State Theory Model of the OH + C6H5Cl reaction

III.1. Potential Energy Surface

The potential energy surface (PES) of reaction 1 was studied using quantum chemical approaches. The density functional BH&HLYP13,14 method with the aug-cc-pVDZ basis set15 was used for the optimization of molecular structures and calculation of vibrational frequencies. The version of the BH&HLYP functional implemented in Gaussian 0316 was used, which, as described in the Gaussian manual, is different from that reported in the literature13. Energies of the transition states relative to the reactants were calculated using the IRTS method17,18 (Isodesmic Reactions for Transition States) using the prototype reactions

OH+C6H6H2O+C6H5
(3a)

and

OH+C6H6C6H6OH
(3b)

as the reference reactions. BH&HLYP/aug-cc-pVDZ-level energy values were used for the IRTS calculations.

In addition, two composite high-level single-point energy methods were used for the calculation of energy barriers and enthalpies of reactions: CBS-QB319,20 and G3//B3LYP.21 All PES calculations lead to the same qualitative conclusions regarding the mechanism of reaction 1; energy values quoted in the text henceforth are those obtained in the IRTS calculations for transition states and in CBS-QB3 calculations for stable species. These energies include vibrational zero point energies unless stated otherwise. The results of the PES study are summarized in Table 2 and Figure 4 and the detailed information is given in the Supporting Information (Table 1S). The Gaussian 03 program16 was used in all potential energy surface (PES) calculations.

Figure 4
Potential energy surface of reaction 1. Energies of transition states are those obtained in IRTS calculations. Energies of stable species were obtained using the CBS-QB3 method.
Table 2
Energies of Reactants, Products, and Stationary Points on the PES of Reaction 1 Obtained in Quantum Chemical Calculations.a

The mechanism of reaction 1 is qualitatively similar to that of reactions 3a and 3b (refs 22, 23 and references cited therein). The pathways leading to C6H4Cl + H2O products are those of H atom abstraction:

OH+C6H5ClH2O+2C6H4Cl
(1a)
OH+C6H5ClH2O+3C6H4Cl
(1b)
OH+C6H5ClH2O+4C6H4Cl
(1c)

Addition of OH to the ring leads to formation of several isomers of the C6H5ClOH adduct:

OH+C6H5Cl2C6H5ClOH
(1d)
OH+C6H5Cl3C6H5ClOH
(1e)
OH+C6H5Cl4C6H5ClOH
(1f)

Reaction 1, like that of OH with benzene, is dominated by addition at low temperatures. Addition is reversed at temperatures above ~ 400 K, and high-temperature reaction is that of H-abstraction. An important difference from the OH + C6H6 reaction is that addition of OH to the ring in the alpha position to chlorine results in substitution:

OH+C6H5Cl(1C6H5ClOH)C6H5OHClCl+C6H5OH
(1g)

The unstable adduct 1-C6H5ClOH, presented in parentheses in the equation of reaction 1g, has a very low barrier for transformation to the C6H5OH···Cl complex (the BH&HLYP-aug-cc-pVDZ level of calculations yields a barrier of 0.4 kJ mol-1 without ZPE and -0.2 with ZPE). This adduct does not exist as a PES minimum if B3LYP method is used for structure optimization with smaller basis sets, such as CBSB7 and 6-31G(d) used in the CBS-QB3 and G3//B3LYP methods, as confirmed by relaxed C-Cl distance scans. For the C6H5OH···Cl complex, the large energy difference (~ 76 kJ mol-1) between the “entrance” and the “exit” transition states makes stabilization highly unlikely. Thus, channel 1g is considered as a substitution channel with the reaction bottleneck located at the PES saddle point for OH addition to the ring.

The reaction paths of channels (1d - 1g) proceed through a shallow van der Waals minimum (weakly bound OH···C6H5Cl complex) on the reactant side, followed by addition energy barriers. The structure of the OH···C6H5Cl complex is similar to that found for the OH + C6H6 reaction, with OH oriented perpendicular to the benzene ring and H atom of the hydroxyl radical oriented toward the ring. Application of the IRTS method to the reaction of addition of OH to benzene ring is somewhat problematic because the barrier for addition, if any, is very low. Application of transition state theory for such reactions generally requires the use of variational formalism, which, in turn, requires the knowledge of the potential energy surface over an extended range of reaction coordinate. Nevertheless, an attempt was made to use the IRTS technique for the addition reaction channels 1d - 1f and the addition-elimination channel 1g using the prototype reaction 3b as the reference reaction. The energy barrier value for the reference reaction of 1.13 kJ mol-1 was obtained in fitting the calculated rate constants to the experimental data of Tully et al.12 at 250 K and 298 K, which are in agreement with the results of other direct determinations3,24,25 of the rate constant of reaction 3 in this temperature range and thus were taken as representative of these data. The resultant values of the addition energy barriers for channels 1d - 1f resulting in formation of adducts are low and similar in values, ranging from 0.8 to 3.7 kJ mol-1. The addition barrier for the reaction channel 1g is significantly higher, 14.1 kJ mol-1.

The abstraction energy barriers (channels 1a - 1c) are higher than those of addition and range from 17.3 to 21.0 kJ mol-1. Following the approach of Seta et al,23 PES of anharmonic bending motions in these transition states (in-plane and out-of-plane C-H-O angles in the C···H···OH structure) were scanned with all other geometric parameters fixed at the optimized values. The obtained potential energy profiles were used in transition state theory calculations of the rate constants (see below).

The IRTS formalism17,18 requires knowledge of a rate constant of a reference reaction, in which the chemical transformation taking place and the structure of the transition state are similar to those of the reaction being studied. For example, a reference reaction for the abstraction channels 1a - 1c should have a transition state with the C···H···OH structure, i.e., it should be another reaction of abstraction of a hydrogen atom by the OH radical. Reaction 3a was consequently selected as the reference reaction for channels 1a - 1c. The rate constant of this reaction has been determined as a function of temperature in the 621 - 1709 K temperature range,12,23,26 with good agreement between the results of three groups. The PES of reaction 3a was studied using the BH&HLYP/aug-cc-pVDZ method-basis set combination. The rate constants for the reference reaction were calculated using transition state theory and the energy barrier was adjusted to reproduce the experimental k3a(T) temperature dependence (see below for the details of the transition state theory calculations). The resultant energy barrier is E3a = 14.73 kJ mol-1. The energy barriers for reaction channels 1a - 1c were obtained by adding to E3a the 0 K enthalpy ΔH(ISO) of the isodesmic reactions

C6H5Cl+C6H5HOH=C6H6+xC6H4ClHOH+ΔH(ISO)
(4)

where x = 2 - 4. The resultant values of the energy barriers are presented in Table 2 and Figure 4.

III.2. Rate Constant Calculations

Rate constants of reaction channels 1a - 1g were calculated using transition state theory.27 A tunneling correction was included for the abstraction channels (1a - 1c) using the Eckart formula28 within the barrier-width method.29-31 The values of the barrier width parameter were obtained in fitting the energy profiles in the vicinity of the PES saddle points obtained by following the intrinsic reaction coordinate32,33 with the Eckart function.28 Properties of the reactants, products, and transition states were obtained in quantum chemical calculations performed at the BH&HLYP/aug-cc-pVDZ level, except for OH and H2O, for which experimental properties were used. The energy barriers were determined in IRTS, CBS-QB3, or G3//B3LYP calculations, as described above.

In transition state theory calculations, partition functions of all species involved were obtained using the approximation of harmonic oscillators and free or hindered rotors, except for the two significantly non-harmonic degrees of freedom in the abstraction transition states. These degree of freedom correspond to bending of the C···H···OH structures. Calculation of the partition functions of these bending modes was performed using the method of Seta et al.23 Potential energy and reduced moments of inertia were obtained as functions of the wagging and rocking angles and the energy levels were calculated by numeric solution of the Schrödinger equation using the FGH1D program.34 Reduced moments of inertia for these degrees of freedom as well as for torsional motions were calculated using the formulas of Pitzer and Gwinn;35,36 partition functions of torsions were calculated using the Pitzer-Gwinn approximation.35

In the IRTS method, the energy barriers for the reference reactions (3a and 3b) were fitted to reproduce the experimental12,23,26 rate constant data. The resultant calculated temperature dependences of the rate constants are compared with the experimental values in Figure 1S in the Supporting information.

The calculated rate constant temperature dependences are compared with the experimental rate constants in Figure 5, where k(T) plots for individual channels of reaction 1, as well as that of the overall reaction, are presented. As can be seen from the plot, the model reproduces the experimental k1(T) dependence very well over the 474 - 670 K temperature range. The average deviation from the experiment is 6%, lower than the 8% average statistical uncertainty of the experimental values and comparable to the estimated 5% systematic uncertainty of the experiment (Table 1). The agreement at room temperature is somewhat poorer, with the calculated k1(298K) = 4.65×10-13 cm3 molecule-1 s-1, 23% lower than the average experimental value of (6.02 ± 0.34)×10-13 cm3 molecule-1 s-1. Calculated rate constant values at individual temperatures are given in the Supporting Information (Table 2S).

Figure 5
Comparison of the experimental and calculated temperature dependences of the rate constants of reaction 1. Symbols: experimental values of the current study (filled black circles), Wallington et al3 (open circles, low temperatures), Mulder and Louw4 (open ...

Use of the CBS-QB3 energies for the transition states also results in very good agreement with the experiment at high temperature (average deviation is also less than the experimental uncertainty). The room temperature CBS-QB3-based calculated rate constant is 3.54×10-13 cm3 molecule-1 s-1 which is 41% lower than the experimental value. The rate constants for individual abstraction channels obtained using the CBS-QB3 energies agree with the IRTS values within 25% over the experimental temperature range. However, the larger value for the barrier of the addition-elimination channel 1g obtained using the CBS-QB3 method results in a more significant difference in the rate constants: the IRTS and the CBS-QB3 values of k1g(T) differ by factors of 2.4 - 3.5 over the same temperature range. G3//B3LYP energy barriers are higher than those obtained in IRTS and CBS-QB3 calculations, with larger differences obtained for the addition and addition elimination channels. As a result, the G3//B3LYP based rate constants are lower than the experimental values by a factor of two in the high-temperature range and by two orders of magnitude at room temperature. The temperature dependences of the rate constants calculated using the CBS-QB3 and the G3//B3LYP energies are presented in Tables 3S and 4S and Figures 2S and 3S in the Supporting information.

Rate constants for the abstraction (1a - 1c) and addition-elimination (1g) channels were calculated using the IRTS energies over wide ranges of temperatures. The resultant k(T) dependences can be represented with the following modified Arrhenius expressions:

k1a=1.69×1020T2.64exp(1513KT)cm3molecule1s1(5003000K)
(IV)
k1a=3.64×1031T6.01exp(+320KT)cm3molecule1s1(200600K)
(V)
k1b=3.39×1020T2.59exp(1046KT)cm3molecule1s1(5003000K)
(VI)
k1b=5.17×1027T4.74exp(+140KT)cm3molecule1s1(200600K)
(VII)
k1c=1.89×1020T2.54exp(1080KT)cm3molecule1s1(5003000K)
(VIII)
k1c=1.10×1027T4.83exp(+177KT)cm3molecule1s1(200600K)
(IX)
k1g=3.09×1019T2.10exp(1867KT)cm3molecule1s1(2003000K)
(X)

Since the differences between the overall calculated rate constants and the experimental values are well within the uncertainties of the experiments, equations IV - X can be used for the purpose of extrapolation of the experimental results to temperatures outside the experimental range.

IV. Discussion

The current study provides the first determination of the rate constant of reaction 1 as a function of temperature in the high-temperature range, where the addition channels (1d - 1f) are reversed and the overall reaction is dominated by the abstraction (1a - 1c) and substitution (addition-elimination, 1g) channels. Rate constants were obtained in direct experiments over the 474 - 670 K range. In addition, the room-temperature rate constant (primarily addition) was determined. The results are in agreement with earlier studies where such comparison can be made (Figure 3). The room-temperature rate constant determined in the current work coincides with the directly obtained values of Wallington et al.3 and the relative-rates result of Edney et al.2 The high-temperature results are in very good agreement with the relative-rate single temperature (563 K) determination of Mulder and Louw.4 The study of Wallington et al.3 covered the temperature range of 226 - 438 K; three of the five data points were obtained at low temperatures and two data points are at 363 K and 438 K. The two higher-temperature rate constant values are approximately a factor of three lower than those at the low-temperatures, indicating that addition is mostly reversed. However, it seems likely that the addition channels and the corresponding reverse reactions regenerating OH through the decomposition of the adducts still influenced the kinetics of OH decay because the reported rate constant values indicate either absence of temperature dependence or a slightly negative dependence. These values are also approximately an order of magnitude higher than extrapolation of our high-temperature Arrhenius dependence to lower temperatures would suggest (Figure 3).

Comparison of the results of the computational study results of reaction 1 with the experimental results demonstrated a very good agreement between the calculated and the experimental rate constants in the high-temperature region, with the differences being less than the uncertainties of the experimental values (Figure 5). The observed agreement serves as an additional confirmation of the high accuracy of the IRTS method.17,18 At the same time, the agreement at room temperatures is poorer, with 23% difference between the experimental and the calculated rate constant values. Also, the calculated low-temperature rate constants have a weak positive temperature dependence while the experimental results of Wallington et al. in the 226 - 296 K range suggest absence of temperature dependence within the data scatter. As was mentioned above, application of the IRTS method to the addition reaction channels is expected to be problematic because of the very low, if any, barrier for addition. Thus, poorer agreement with the experiment is not surprising. At the same time, it is worth mentioning that the 23% disagreement at room temperature corresponds to a 0.65 kJ mol-1 error in the energy barrier, which is rather small for a computation-based method.

Use of the CBS-QB3 energy barriers also results in very good agreement between the calculated and the experimental high-temperature rate constants. The resultant k(T) dependence differs very little from the IRTS-based one and thus is not presented in Figure 5 to avoid plot congestion; instead, CBS-QB3 rate constants are presented in a graph and a table in the Supporting information (Figure 2S and Table 2S). The rate constants for the individual reaction channels 1a - 1c obtained in CBS-QB3 based calculations (with BH&HLYP/aug-cc-pVDZ vibrational frequencies) differ from those obtained in IRTS calculations by only 6%, 22%, and 17%, respectively, over the experimental temperature range. The difference between the rate constants for the addition-elimination channel 1g obtained in the CBS-QB3-based and IRTS calculations is significantly larger: a factor of 2.9, on average, over the same temperature range, reflecting the 4.9 kJ mol-1 difference in the energy barrier values between these two methods.

One unfortunate consequence of the imperfect agreement of the IRTS-based calculated rate constant at room temperature with experiment is the unknown uncertainty of the energy barrier for the reaction channel 1g, that of addition-elimination, or substitution of Cl in chlorobenzene for OH. The barrier of 1.13 kJ mol-1 was derived for the reference reaction 3b within the IRTS method from the analysis of the low-temperature addition rate constant data.12 The low value indicates that variational transition state theory is more appropriate for modeling this addition reaction. However, the barrier for reaction 1g is relatively large (19 kJ mol-1), which means that the location of the dynamic saddle point on the PES is fixed and variational effects in application of transition state theory, if any, can be expected to be much smaller than in the case of the reference reaction. This difference in the degree of variational effects between the reference reaction and the reaction being studied can be expected to result in the uncertainty in the IRST energy barrier for reaction channel 1g that is larger than the above value of 0.65 kJ mol-1 derived from the analysis of the room-temperature rate constant values. Based on these considerations, we can recommend an estimated uncertainty of +3/-7 kJ mol-1 for the energy barrier of the reaction channel 1g (the average coincides with the difference between the CBS-QB3 and the IRTS values). When used with equation X for the rate constant, this energy barrier uncertainty translates into the uncertainties in the rate constants equal to factors of 17/3.4 at 298 K, 5.4/2.1 at 500 K, 2.3/1.4 at 1000 K, 1.5/1.2 at 2000K, and 1.3/1.1 at 3000 K (the first number refers to the factor for increasing the rate constant value and the second to that for decreasing it). Alternatively, one can choose to use the CBS-QB3 based temperature dependence of the channel 1g rate constant

k1g(CBSQB3)=3.09×1019T2.10exp(1279KT)cm3molecule1s1(2003000K)
(XI)

with the +8/-2 kJ mol-1 uncertainty in the activation energy.

Supplementary Material

1_si_001

Acknowledgment

This research was partially supported by NIEHS grant RO1ES015450 and the LSU Patrick F. Taylor Chair. The authors would like to thank Dr. J. N. Crowley, Dr. S. M. Lomnicki, and Dr. V. L. Orkin for helpful discussion and advice.

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