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Chemical Physics Letters
j o ur na l ho me p ag e :w w w . e l s e v i e r . c o m / l o c a t e / c p l e t t
An experimental and theoretical study on the kinetic isotope effect of C 2 H 6 and C 2 D 6 reaction with OH
Fethi Khaled
a, Binod Raj Giri
a,∗, Milán Sz ˝ori
b, Béla Viskolcz
c, Aamir Farooq
a,∗aCleanCombustionResearchCenter,DivisionofPhysicalSciencesandEngineering,KingAbdullahUniversityofScienceandTechnology(KAUST), 23955-6900Thuwal,SaudiArabia
bDepartmentofChemicalInformatics,FacultyofEducation,UniversityofSzeged,Boldogasszonysgt.6,H-6725Szeged,Hungary
cInstituteofChemistry,FacultyofMaterialsScienceandEngineering,UniversityofMiskolc,Hungary
a r t i c l e i n f o
Articlehistory:
Received18September2015 Infinalform23October2015 Availableonline30October2015
a b s t r a c t
Wereportexperimentalandtheoreticalresultsforthedeuteratedkineticisotopeeffect(DKIE)ofthe reactionofOHwithethane(C2H6)anddeuteratedethane(C2D6).Thereactionswereinvestigatedbehind reflectedshockwavesover800–1350KbymonitoringOHradicalsnear306.69nmusinglaserabsorp- tion.Inaddition,highlevelCCSD(T)/cc-pV(T,Q)Z//MP2/cc-pVTZquantumchemicalandstatisticalrate theorycalculationswereperformedwhichagreedverywellwiththeexperimentalfindings.Theresults reportedhereinprovidethefirstexperimentalevidencethatDKIEasymptotestoavalueof1.4athigh temperatures.
©2015ElsevierB.V.Allrightsreserved.
1. Introduction
Smallalkanes(<C5)constitutealmostallofthecompositionof naturalandliquefiedpetroleumgas(LPG),whereaslargerstraight orbranchedalkanes(≥C5)aretheprimaryconstituentsofgaso- line,dieselandaviationfuels[1–4].Hydrogenabstractionreactions fromalkanesbyhydroxylradicals(OH+RH→R+H2O)arethepri- maryoxidationpathwaysofthesefuelsatcombustionconditions.
Accuratemodelingofcombustionkineticsrequirespreciseknowl- edgeoftotalandsite-specificratecoefficientsoverawiderangeof temperaturesandpressures.Aconventionalwaytoderiveoverall andsite-specificratecoefficientsistostartfromsmallmolecules and then usegroup additivity approximationsto estimaterate coefficientsforlongchainmolecules.Variousapproximationshave beenusedin theliterature, suchasthe Next-Nearest-Neighbor (NNN)[5,6]andStructureActivityRelationship(SAR)[7].Tullyetal.
[8–13]pioneeredtheuseofdeuteriumforthestudyofdeuterium kineticisotopeeffect(DKIE)toelucidaterulesforthecalculation ofsite-specificratesofH-abstractionfromavarietyofhydrocar- bonmolecules.Thismethodologyhas,forexample,beenusedto discernthebranchingratiosofthetwocompetingchannelsduring thereactionofpropane(C3H8)withOHatlowtemperatures[10]
andhightemperatures[14].Recently,Badraetal.[15]published
∗Correspondingauthors.
E-mailaddresses:binod.giri@kaust.edu.sa(B.R.Giri),aamir.farooq@kaust.edu.sa (A.Farooq).
experimentalresultsanddetailed kineticanalysisontheappli- cationofDKIEtoextractbranchingratiosofthethreecompeting channelsduringthereactionofpropene(C3H6)withOHradicalsat hightemperatures[15].TheimportanceofDKIEofsmallmolecules suchasethane,ethyleneand acetyleneinthedetermination of branchingratiosoflongerchainalkanes,alkenesandalkynesis demonstratedtherein[15].Theaimofthecurrentworkistoextend low-temperature(290–800K)DKIEdataofethane[9]tohightem- peratures(800–1350K)usingratecoefficientmeasurementsofthe reactionofethaneanddeuteratedethanewithOHradicals:
C2H6+OH →C2H5+H2O (R1)
C2D6+OH→ C2D5+HDO (R2)
These resultswill be helpful in elucidating thecompetition ofdifferentH-abstractionchannelsduringthereactionoflarger alkaneswithOHradicals.Moreover,acloserlookintothedatabase fortheratecoefficientsofR1revealsthatthereareonlythreedirect high-temperature(T>950K)measurementsavailableintheliter- ature[16–18].Muchoftheearlierstudiesarelimitedtonearroom temperatures[9,16,17,19–23];andingeneraltheyshowexcellent agreementtoeachotherwithinoveralluncertaintiesof±20%at 298K[19].Surprisingly,therearenotmanyreportsoftheoretical rateconstantestimationsusingtheelectronicstructuremethods otherthantwostudiesfromKrasnoperovandMichael[18] and MelissasandTruhlar[24].ThelateremployedPMP2//MP2/adj2- cc-pVTZleveloftheorytocomputethepotentialenergysurface forthereactionofethanewithOHradicals.Theycomputedthe http://dx.doi.org/10.1016/j.cplett.2015.10.057
0009-2614/©2015ElsevierB.V.Allrightsreserved.
rateconstantsusingabinitioandcanonicalvariationaltransition statetheorycalculationswithsmallcurvaturetunnelingcorrec- tions.Theircalculatedvalueswerefoundtoagreewellwiththe experimentswithinafactorof2.3overawiderangeoftemper- atures.KrasnoperovandMichael[18]usedB3LYP/6-31G*levelof theorytomapoutthepotentialenergysurfaceforethane+OHreac- tion.Theyhadtoadjustthebarrierheightto10.2kJ/molandone ofthelowbendingmodewastakenas250cm−1toachievegood matchwiththeavailableexperimentaldataover140≤T/K≤1600. Theyfurthersuggestedthata highleveltheoryshouldbeused tostudythereactionbetweenethane and OH.Asfor R2,there isonlyoneexperimentalstudyfromTullyetal.[9]atrelatively lowtemperaturesandnotheoreticalreportsarefoundinlitera- ture.ThecurrentworkthusaimstoreportthetheoreticalDKIEfor ethane/d-ethane+OHreactionusinghigh-levelquantumchemical andstatisticalratetheorycalculations.
2. Experimentalsetup
Thelow-pressureshocktubefacility (LPST)atKingAbdullah UniversityofScienceandTechnology(KAUST)wasusedtoconduct allexperimentspresentedhere.Asthedetailsofourexperimental facilitycouldbefoundelsewhere[25],onlyabriefdescriptionis providedhere.TheLPSThas9mlongdriveranddrivensections withaninnerdiameterof14.2cm.Thelengthofthedriversection ismodifiabledependingontherequiredtesttime.Opticalwin- dowswereinstalledatthesidewalllocation,20mmfromtheend walloftheshocktube.Shocktubewaspumpeddowntolessthan 10−5mbarusingturbo-molecularpumppriortoeachexperiment toensurehighpurityoftheshocktube.Theshocktubewasfound tohavealeakrateof<1×10−6mbar/min.Allexperimentsreported herewereconductedbehindreflectedshockwaves,andthecon- ditions(T5,P5)werecalculatedbymeasuringtheincidentshock speedandusingRankine–Hugoniotshock-jumprelations[26,27]
embeddedintheFroshcode[28].
Hydroxylradicalswereproducedbyrapidthermaldecompo- sitionoftert-butylhydroperoxide(TBHP),whichisknowntobe acleanthermolyticsourceofOHradicalsandhadbeenvalidated inmanyearlierstudies[25,29,30].Hydroxylradicalsweremea- suredbyusingthewell-characterizedR1(5)absorptionlineinthe (0,0)bandoftheA2+←X2OHtransitionnear306.7nm.Mea- suredabsorbancetime-historywasconvertedtoOHconcentration time-historyusingtheBeer–Lambertlaw.A70% TBHPin water solutionwasobtainedfromSigmaAldrich.Ethane(99.99%),argon (99.999%),andhelium(99.999%)werepurchasedfromAHGases.
Ethane-d6 (98%) was obtained from CDN Isotopes Inc. Several reflected-shockexperimentswereconductedforeachfuel(C2H6
andC2D6)andtheconcentrationsofreactants(fuel,TBHP)were chosenbasedonsensitivityanalysestoachievepseudo-first-order kinetics.
3. Quantumchemicalcalculations
Molecularand transitionstategeometrieswereoptimizedat theMP2/cc-pVTZleveloftheory[31–33]applyingthe‘tight’con- vergencecriterionoftheGaussian09programpackage[34].The MP2/cc-pVTZharmonicvibrationalwavenumbersofthemolecules and transition states were scaled by a factor of 0.95 adopted fromCCCBDBdatabase[35].Similartopreviousworks[36–38], theaccuratedescriptionoftheelectronicstructureswasapprox- imatedbyextrapolationschemes.WhileFellerextrapolation[39]
was utilized for HF energies (using cc-pVXZ basis sets, where X=D,TandQ[31]),Helgakerextrapolation[40]forCCSD(T)cor- relation energies [41] was applied with cc-pVTZ and cc-pVQZ basis sets. Sum of these extrapolated energies manifested in
100 50
0 -5 -4 -3 -2 -1 0
C2H6 + OH => C2H5 + H2O
TBHP => TBUTOXY + OH
CH3COCH3 + OH => H2O + CH2CO + CH3 CH3 + OH => CH2* + H2O
C2H6 (+M) => 2CH3 (+M) CH3 + OH (+M) => CH3OH (+M)
OH sensitivit y
t (µµs)
Figure1.HydroxylsensitivityforC2H6+OHreactionat1106Kand1.38atm.OH sensitivityisdefinedasSOH=(∂XOH/∂ki)×(ki/XOH),whereXOHisthelocalOH-mole fractionandkiistherateconstantfortheithreaction.Initialmixturecomposition:
342ppmethane,22.4ppmTBHP(70ppmwater)dilutedinargon.
CCSD(T)/cc-pV(T,Q)Z//MP2/cc-pVTZleveloftheorywhichischo- sentoestablishhigh-levelabinitiodescriptionofthezero-point correctedrelativeenergies(E0)forbothisotopologues(C2H6and C2D6).
The rateconstantsfor ethane+OH and ethane-d6+OH were calculatedusingcanonicaltransitionstatetheory(CTST)withthe molecularparametersfromourabinitiocalculations.IntheseCTST calculations,allspecieswereassumedtobeintheelectronicground stateexceptOH,forwhichtheelectronicpartitionfunctionwascal- culatedwithaspinorbitsplittingof139.7cm−1[42].Onelowlying bendingmodecorrespondingtoC-Crotationinthereactantsand twoofthelowfrequencytorsionalmodesofthetransitionstates correspondingtoC CandOHrotationsweretreatedashindered rotorswithinPitzer–Gwinn[43]approximations.Ratecalculations werecarriedoutusingChemRatecode[44].
4. Resultsanddiscussion
The JetSurf 1.0 mechanism [45] is used asthe basemecha- nismand tert-butylhydroperoxide(TBHP)chemistryfromPang et.al[46]isaddedtothebasemechanismtosimulateOH-time histories.Sensitivityanalysiswasperformedtoexploretherole ofsecondaryreactionsthatmightaffectOHconcentrationtime- profileinourexperimentalconditions.AscanbeseeninFigure1, thesecondarychemistryhasnegligiblecontributiontoOH-decay profile.Measurements forR1 werecarried outin thetempera- turerangeof847–1285Kusingamixtureof342ppmofethane with22.4ppmTBHPdilutedinargon,whereasthemeasurements ofR2rangedfrom805to1345Kusingamixtureof310ppmof ethane-d6with22.2ppmTBHPdilutedinargon.Toensurepseudo- firstorderkinetics,theconcentrationofTBHPwasalwayskeptat least10timessmallerthanthatofethaneorethane-d6.Therate coefficientsofreactionsR1andR2areobtainedbyfittingthesimu- latedOHtimeprofilestotheexperimentalOHtime-profileswhile varyingtherateconstantofthetargetreactioninthekineticmech- anism.RepresentativeexperimentalandmodeledOHprofilesin additiontotheeffectof20%deviationfromthebestfitforethane andethane-d6areshowninFigures2and3,respectively.Measured valuesoftheratecoefficientsalongwithexperimentalconditions arecompiledinTables1and2.OurdataareplottedinFigure4 along withthepreviouslow-temperaturedatafromTullyetal.
[9] andthree-parameter Arrheniusexpression (k1=2.68×10−18 (T/K)2.224 exp(−373K/T)cm−3molecule−1s−1±13%)obtainedby Krasnoperov and Michael [18] from fitting the entire database
60 40
20 0
0 5 10 15
20 experimental data
kbest fit=1.4× 10-11cm3 molecule-1 s-1 0.8 × kbest fit
1.2 × kbest fit
OH Mole Fraction (ppm)
t (µµs)
Figure2.Hydroxylmolefractionprofileforethane+OHreactionatT=1106K, P=1.38atm.Themixturecompositionwas342ppmethane,22.4ppmTBHP(70ppm water)inargon.Thebest-fittotheexperimentalprofilealongwith±20%perturba- tionsarealsoshown.
80 60
40 20
0 0 5 10 15 20
experimental data
kbest fit= 1.0 × 10-12cm3 molecule-1 s-1 0.8 × kbest fit
1.2 × kbest fit
OH Mole Fraction (ppm)
t (µµs)
Figure3.Hydroxylmolefractionprofileforethane-d6+OHreactionatexperi- mentalconditionsofT=1133K,P=1.44atm,310ppmethane-d6,22.2ppmTBHP (80ppmwater)dilutedinargon.Alsopresentedarethebest-fitsimulatedprofile andperturbationsof±20%.
Table1
MeasuredratecoefficientsofreactionR1(ethane+OH).
Temperature Pressure k1
(K) (atm) (cm3molecule−1s−1)
847 1.68 6.81×10−12
925 1.6 8.93×10−12
970 1.46 1.06×10−11
1034 1.4 1.23×10−11
1106 1.38 1.39×10−11
1142 1.31 1.54×10−11
1275 1.31 1.94×10−11
1277 1.08 2.08×10−11
1285 1.21 1.96×10−11
for ethane+OH reaction over 138–1367K. As can be seen, the three-parameterexpression[18]underpredictsourmeasuredrate coefficientsforR1bya meandeviationof20%.AsforR2,there arenoliteraturedataavailabletocomparewithinthetempera- turerangeofourstudy.Thebestfitofourexperimentaldataalong withlowtemperatureliteraturedataforR1andR2resultedinto
Table2
MeasuredratecoefficientofreactionR2(d-ethane+OH).
Temperature Pressure k2
(K) (atm) (cm3molecule−1s−1)
805 1.68 3.09×10−12
875 1.63 4.47×10−12
943 1.56 5.73×10−12
997 1.34 7.40×10−12
1030 1.62 8.25×10−12
1133 1.44 1.00×10−11
1190 1.44 1.14×10−11
1240 1.28 1.30×10−11
1254 1.42 1.32×10−11
1345 1.37 1.60×10−11
0.8 1.2 1.6 2.0 2.4 2.8 3.2 3.6 1E-13
1E-12 1E-11 1E-10
k (cm3 molecule-1 s-1 )
1000 K / T
Figure4. Comparisonofthecalculatedratecoefficientswiththeexperimentaldata.
( )thisworkforC2H6+OHreaction;( )Tullyetal.[9]forC2H6+OHreaction;( ) thisworkforC2D6+OH;( )Tullyetal.[9]forC2D6+OHreaction.Blueandredlines representtheresultsofourabinitio/CTSTcalculationsforC2H6andC2D6reactions withOHradicals,respectively.Solidlinesrepresentthecalculatedratecoefficients withouttunnelingcorrections,whereasthebrokenlinesincorporateWignertun- nelingcorrection.Dottedlinesaretheresultsfromfittingtheentiredatabasefor C2H6+OHreactionovertheT-rangesof138–1367KobtainedbyKrasnoperovand Michael[18].
thefollowingthreeparameterArrheniusexpressions (inunitof cm3molecule−1s−1):
k1(T)=1.02×10−17T2.083exp
−522.2KT
(290−1290K) (1) k2(T)=5.48×10−17T1.866exp
−1138.2KT
(290−1350K) (2) Ourcalculatedenergyprofileofthereactionofethaneisotopo- logueswithOHisshowninFigure5.Theabinitioreactionenergy forethane(−75.9kJmol−1)agreeswithintheuncertainty(1.70kJ mol−1)oftheexperimentalvalue(−76.01kJmol−1)calculatedfrom thedataavailableintheCCBDBdatabase.Ourabinitiobarrierheight forR1isfoundtobe9.3kJmol−1whichisconsistentwiththeearlier reportof9.75kJmol−1fromMelissasandTruhlar[24].Thesecom- parisonssuggestthattheenergiescalculatedinthecurrentworkfor thedeuteratedspeciesarealsohighlyaccurate.Thebarrierheight forR2iscalculatedtobe13.3kJmol−1.Basedontheenergyprofile displayedinFigure5andmolecularparameterslistedinTable3, weperformedCTSTcalculationsthatarefoundtoreproduceour experimentaldataverywell(seeFigures4and6).However,the calculationsunderpredictexperimentalratecoefficientsforboth R1andR2inthelow-temperatureregion.Thissubtlediscrepancy maybeattributedtothetunnelingeffect.AscanbeseeninFigure4, thequantumtunnelingeffectislesspronouncedforR1asopposed toR2.Thisisexpectedasthereactionswithsmallbarrierscon- tributelesstothequantummechanicaltunneling().Tunneling
Figure5. Potentialenergy surface (includingzero-point energies) for the H- abstractionreactionofethaneandethane-d6withOHradicals;energiesarerelative tothereactantenergies.
()wascomputedusingWignerformulathatrequiresimaginary frequency(=/)correspondingtothereactioncoordinateandthe thresholdenergy(E0)asgivenby:
=1− 1 24
h=/ kbT 21+RT E0
(3) AfterincorporatingWignertunnelingcorrection,thetheoretical ratecoefficients(dashedlines,Figure4)forR2showedexcellent agreementwithexperimentaldataover theentiretemperature range.ButforR1,thetunnelingcorrectionappearstobequantita- tivelylessreliableatlowtemperatures.Thecalculatedrateswere overestimatedbyroughlyafactoroftwointhelow-temperature region.AsimilarbehaviorwasreportedbyMelissasandTruhlar [24]whereWignertunnelingcorrectionresultedinanoverestima- tionoftheratecoefficientsbyafactorof2.3at300K.Thetunneling correction,however,isnearlynegligibleinourexperimentalcon- ditions.Moreover,thecontributionoftunnelingisexpectedtobe cancelledouttothelargepartwhencalculating theratioofthe ratecoefficients(k1/k2).Fromtheresultsofabinitioandtransition statetheorycalculations, theratioof thetunneling-uncorrected ratecoefficientsofreactionsR1andR2,i.e.,DKIE,canbeexpressed overthetemperaturerangeof290–1400K:
k1
k2
(T)=(0.38±0.10)exp
−(3046±70)K T
+(1.02±0.05) exp
(527.5±0.2)KT
(4)
Thebestfit of experimentaldata(this workandTully etal.
[9])yieldsthefollowingexpressionforDKIEovertheTrangeof
1400 1200 1000 800 600 0 400
2 4 6 8
k1/k2
T (K) 1.4
Figure 6.Comparison of the experimental and theoretical DKIE of ethane (H/D)+OH.(—)experimentalresultsfromthisworkandTullyetal.[9];( )cal- culatedvaluesfromourabinitio/CTSTmethods.(......)ahorizontallineshowing DKIE=1.4.
293–1350K:
k1
k2
(T)=(0.5±0.10)exp
−(2607±356)K T
+(0.9±0.1) exp
(526±1)KT
(5)
BoththeexperimentalandcalculatedvaluesforDKIEaredis- playedinFigure6.Ascanbeseen,thecalculatedandexperimental DKIEvaluesexhibitgoodagreementovertheentiretemperature range.OurcalculatedvalueforDKIEat290Kis6.4whichiscloseto thatreported(4.61±0.56)byTullyetal.[9].At850K,wemeasured aDKIEvalueof1.67whichagreesverywellwiththeextrapolated valueof1.72fromtheworkofTullyetal.[9].Ourexperimentally determinedDKIEasymptotestoavalueof1.4athightemperatures (T>1200K).
The high-temperature asympoting behavior of DKIE can be exploredusingtheoreticalmethods.FromArrheniustheory,DKIE canbewrittenas:
k1
k2
(T)= A1
A2
exp
Ea
RT
(6) whereAisthepre-exponentialfactorandthesubscriptsidentify thecorrespondingreactions;Ea=Ea(D)−Ea(H)isthedifference intheactivationenergiesoftheisotopes.AsTapproachesinfin- ity,k1/k2≈A1/A2.TheratioofA1andA2 canbeapproximatedby takingtheratioofimaginaryfrequenciesofthetransitionstates (1=//2=/)[47].Using 1=/ =1303cm−1 and 2=/ =1003cm−1 (seeTable3),DKIE(k1/k2)comesouttobe1.3.Ontheotherhand,ab Table3
Rotationalconstants(A,B,andC)andharmonicfrequencies(i)ofthestationarypointscalculatedattheMP2/cc-pVTZleveloftheory.Frequenciesarescaledby0.95.
Frequenciescorrespondingtothetorsionalmodesareshowninbold.
Species A,B,C
(GHz)
i
(cm−1)
C2H6 79.26966
19.81782(2)
3045(2),3025.5(2),2951.7,2950.3,1437.7(2),1437.3(2),1358.9,1331.0, 1166.8(2),990.3,785(2),308.5
C2D6 39.66530
13.70550(2)
2254.5(2),2242(2),2127.4,2116.6,1135.5,1041.8(2),1026(2),1017.4,929.1 (2),822.8,567.4(2),218.4
TS 26.33548
4.80059 4.28371
1303i,3621.5,3073.8,3047.0,3032.1,2992.8,2949.2,1432.6,1427.5,1412.7, 1342.1,1311.6,1266.5,1196.0,1154.4,1019.5,974.6,809.9,786.1,630.4, 160.1,114.6,373.3,51.2
TS-d6 17.78627
4.22738 3.74362
1003i,3621.4,2280.3,2258.9,2244.1,2174.0,2120.2,1138.6,1035.8,1026.2, 1017.8,991.5,959.7,937.9,900.4,888.9,846.0,673.2,567.7,537.5,120.8, 101.5,267.5,49.5
initio/CTSTcalculationspredictthatDKIEasymptotesto1.5athigh temperatures.Thesevaluesarequiteclosetotheexperimentally determinedDKIEof1.4.
5. Conclusions
The deuterated kinetic isotope effect (DKIE) for the reac- tionofethaneand ethane-d6 withOHradicalswasdetermined experimentallybetween800and1350K.Additionally,highlevel CCSD(T)/cc-pV(T,Q)Z//MP2/cc-pVTZquantumchemicalandstatis- ticalratetheorycalculationswereperformedtocalculatetheDKIE over290–1400K.Thetheoreticaland experimentalDKIEvalues are found to agree well over the entire temperature range of 290–1350K.Our ab initio/CTSTcalculations predictedthatDKIE asymptotesto1.5athightemperatureswhichisonly7%largerthan theDKIEvaluedeterminedexperimentallyinthecurrentwork.This workreports,toourknowledge,thefirstexperimentalevidence thatDKIEasymptotesto1.4athightemperatures.
Acknowledgments
WewouldliketoacknowledgethefundingsupportfromSaudi AramcoundertheFUELCOMprogramandbyKingAbdullahUni- versityofScienceandTechnology(KAUST).Dr.Sz ˝oriisaMagyary Zoltánfellow supportedbyStateof Hungary andtheEuropean Union,financedbytheEuropeanSocialFundintheframeworkof TÁMOP4.2.4.A/2-11-1-2012-0001“NationalExcellenceProgram”
under the respective grant number of A2-MZPD-12-0139. This workwassupportedbytheJánosBolyaiResearchScholarshipof theHungarianAcademyofSciences(BO/00113/15/7).
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