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Catalysis
Today
jo u r n al h om epa ge :w w w . e l s e v i e r . c o m / l oc a t e / c a t t o d
SO
x
uptake
and
release
properties
of
TiO
2
/Al
2
O
3
and
BaO/TiO
2
/Al
2
O
3
mixed
oxide
systems
as
NO
x
storage
materials
Göksu
S.
S¸
entürk
a,
Evgeny
I.
Vovk
a,b,
Vladimir
I.
Zaikovskii
b,
Zafer
Say
a,
Aslı
M.
Soylu
a,
Valerii
I.
Bukhtiyarov
b,
Emrah
Ozensoy
a,∗aChemistryDepartment,BilkentUniversity,06800Bilkent,Ankara,Turkey bBoreskovInstituteofCatalysis,630090Novosibirsk,RussianFederation
a
r
t
i
c
l
e
i
n
f
o
Articlehistory:
Received15September2011 Receivedinrevisedform 23November2011 Accepted1December2011 Available online 30 December 2011 Keywords: Al2O3 BaO TiO2 Anatase Sulfurpoisoning DeNOx NOx SOx Sulfation NSR LNT HDS ClausProcess
a
b
s
t
r
a
c
t
Titaniawas used as a promoter toobtain novel materials in the form of TiO2/Al2O3 (Ti/Al)and
BaO/TiO2/Al2O3(Ba/Ti/Al,containing8wt%or20wt%BaO)thatarerelevanttoNOxstoragereduction
(NSR)catalysis.Twodifferentprotocols(P1,P2)wereutilizedinthesynthesis.Ti/Al(P1)manifestsitselfas crystallitesofTiO2on␥-Al2O3,whileTi/Al(P2)revealsanamorphousAlxTiyOzmixedoxide.Thestructures
ofthesynthesizedmaterialswereinvestigatedviaTEM,EDX,BETanalysisandXPSwhilethecatalytic functionality/performanceofthesesupportmaterialsuponSOxandsubsequentNOxadsorptionwere
investigatedwithTPDandinsituFTIRspectroscopy.Ti/Al(P1,P2)revealedahighaffinitytowardsSOx.
OverallthermalstabilitiesoftheadsorbedSOxspeciesandthetotalSOxuptakeoftheBa-freesamples
increaseinthefollowingorder:TiO2(anatase)␥-Al2O3<Ti/Al(P1)<Ti/Al(P2).ThesuperiorSOxuptake
ofTi/Al(P1,P2)supportmaterialscanbetentativelyattributedtotheincreasingspecificsurfacearea uponTiO2promotionand/orthechangesinthesurfaceacidity.PromotionofBaO/Al2O3withTiO2leads
totheattenuationoftheSOxuptakeandasignificantdecreaseinthethermalstabilityoftheadsorbed
SOxspecies.TherelativeSOxadsorptioncapacitiesoftheinvestigatedmaterialscanberankedasfollows:
8Ba/Ti/Al(P1)<8Ba/Ti/Al(P2)<8Ba/Al∼20Ba/Ti/Al(P1)<20Ba/Al<20Ba/Ti/Al(P2).
© 2011 Elsevier B.V. All rights reserved.
1. Introduction
Controllingthesurfacechemistryofmixed-oxidesurfacesisof vitalimportancetodesignnovelcatalyticmaterialswith unprece-dentedfunctionalities.Sulfur poisoningonmetaloxidesurfaces isoneof thefrequentlyobservedsurface deactivation phenom-enainheterogeneouscatalysis.AccumulationofSOxspecies on
metaloxidesurfaceshavebeenverycommonlystudiedinthe liter-atureinrelevancetothree-waycatalysis(TWC),selectivecatalytic reduction(SCR),NOxstoragereduction(NSR),
hydrodesulfuriza-tion(HDS)andothercatalyticprocesses,whereAl2O3isutilizedas
themainsupportmaterial[1–7].Twomajordeactivation phenom-enaareoftenreportedfortheNSRcatalysts.Thefirstrouteinvolves thermaldegradationofthestructuralintegrityofthecatalyst mate-rialduetosolidstatereactionsbetweenthecatalystcomponents
∗ Correspondingauthor.
E-mailaddress:ozensoy@fen.bilkent.edu.tr(E.Ozensoy).
andsinteringwhilethesecondrouteisassociatedwiththesulfur poisoning [8,9].The latterdeactivationphenomenon is particu-larlyachallengingproblem.InNSRapplications,NOx(g)andSOx(g)
adsorbates,competeforthesamebasicadsorptionsitesonoxide surfaces.Consequently,maximizationoftheNOxstorage
capac-ity(NSC)whileminimizingtheirreversibleSOxuptakeoftheNOx
storagesitesimpliescarefuloptimizationofthesurfaceproperties ofthecatalyticsupportmaterialssuchasthesurfacecomposition, acidity,morphologyandspecificsurfacearea(SSA).
SulfurpoisoningofNSRcatalyststypicallyleadstothe forma-tionofalkalineearth/preciousmetalsulfates,sulfitesorsulfides [8]. For a large number of oxide substrates, the stability of some of the common adsorbates increases in the following order:NO2−∼CO32−<NO3−<SO42− [10–15]. Thus, sulfur
effec-tively blocks the catalytic sites for NOx storage and gradually
reducestheoverallNOxstoragecapacityoftheNSRcatalysts[16].
Effortstowardsimprovingthecatalytictoleranceagainstsulfur poisoninganddesigninghighlyactiveandstablenovelcatalysts arevitalfortheglobalizationoftheNSRtechnology[14,15,17–20]. 0920-5861/$–seefrontmatter © 2011 Elsevier B.V. All rights reserved.
Scheme1.SynthesisofTiO2-promotedNOxstoragematerials:P1andP2.
Misonoand Inui[21],Fritzand Pitchon [22]and severalothers [12,13,23–27]reporteddetailedstudiesontheimprovementand thedurabilityenhancementofNSRcatalysts.Thecommercial cat-alystsarealsosuccessfullyusedinlimitedmarketssuchasJapan wherethesulfurcontentofthedieselfuelisrelativelylow(below 10ppm)[28].AccordingtoYamazakietal.,Fewasfoundtodecrease thesulfuruptakeandpromotethedecompositionofBaSO4 [29].
Fansonetal.observedthatFefacilitatedtheformationofabulk nitratespecieswhichweresuggestedtoberesilientagainstsulfur poisoning[30].Kayhanetal.reportedthattheinitialNOxuptake
mechanismandtheratiobetweenthesurfaceandbulkBaOsites weresignificantlyinfluencedbyFeloading[20].
TiO2 containingsupportmaterialswerealsoreportedto
sup-pressthesulfurpoisoning[31,32].Thiseffectwasassociatedwith thesurfaceacidityofTiO2,inhibitingtheadsorptionofacidicSOx
species[33].Decompositiontemperatureofthesulfatesonpure TiO2 isknowntobelowerthanthatof␥-Al2O3[34,35].
Further-more,activesitesonthesulfatedTiO2surfacecanalsobereadily
regeneratedunderreactionconditions[36].Recently,itwasalso reportedthatTiO2sitesonthesupportsurfacecanfunctionas
effi-cientanchoringsitesforBaO,whichmaybeexploitedtoenhance thesurfacedispersionofBaOdomainsandfine-tunethesurface morphology[37].
Inordertocircumventsomeoftheunfavorablepropertiesof pureTiO2suchasthelimitedthermalstability,lowsurfacearea,
andpoormechanicalproperties,itscombinationwithsecondary oxidesareutilizedtodesignnovelsupportmaterialswithenhanced properties.Alongtheselines,␥-Al2O3[14,19,32,36,38–42]and/or
ZrO2[43–45]arepromisingchoicesforthesecondaryoxidesthat
can beused in combination withTiO2. It was reported that if
sulfur-poisonedBa/Pt/Al2O3catalystwasblendedwithnon
sulfur-poisonedPt/TiO2catalyst,sulfurdesorptionfromtheBa/Pt/Al2O3
catalystunderrich conditionsisimproved[14].Furthermore,it wassuggestedthat theinterfacebetweenAl2O3 andTiO2 plays
animportantroleinthesulfate decompositionandthe desorp-tionprocesses[32].Matsumotoandco-workers[14,46]reported thatacombinationofTiO2 andlithium-doped␥-Al2O3 presents
anoptimumsurfaceaciditytowardssulfurpoisoning.The macro-scopicgeometricalstructure ofthe catalytic monolithwasalso foundtobeeffectivein limitingthesizeofthesulfate particles andcontrollingthesulfatedecomposition/desorptiontemperature [47,48].Itwasshownthatsulfatedecompositionisfacilitatedon
thesmallersulfatedomains.Therealsoexistanumberofsurface sciencestudiesonplanarmodelNSRcatalysts[49–53]focusingon thestructureandtheoperationalprinciplesofNSRsystemsatthe molecularlevel.Despitetheestablishedsulfurresistingeffectof TiO2asanadditiveinthecompositionofthePt/Ba/␥-Al2O3
cata-lysts,anumberofcrucialaspectsregardingtheinfluenceofTiO2
ontheinteractionbetweentheNOxstoragecomponentandthe
supportmaterialhavenotyetbeenelucidated.
Thus,inthecurrentwork,wefocusourattentiononthe inter-action ofSOxwiththeTiO2/Al2O3 and BaO/TiO2/Al2O3 surfaces
aswellastheinfluenceofTiO2domainsontheNOxuptakeafter
deactivationbySO2(g)+O2(g).
2. Experimental
TiO2/Al2O3binaryoxidesupportmaterials(whichwillbe
here-afterreferredasTi/Alinthetext)werepreparedviatwodifferent syntheticprotocolsP1[23,37]andP2[37]whichweredescribed in detail in ourformer reports. These syntheticprotocolswere schematically described in Scheme 1. Briefly, in the first syn-theticprotocol(P1),␥-Al2O3(PURALOX,200m2/g,SASOLGmbH,
Germany)andTiCl4(Fluka,titanium(IV)chloridesolution∼0.1M
in20%hydrochloric acid)wereusedasstartingmaterials.TiCl4
wasdilutedincooleddeionizedwaterundercontinuousstirring atatemperaturebelow333K.Then,␥-Al2O3powderwasslowly
added to theprepared solution. Next, 30vol% NH3 was slowly
addedtothesolutionuntilpH≥9.0wasachievedandagelwas formed.Thiswhite gelwasagedfor 24hunderambient condi-tions,filtered,washedwithdistilledwater,andcalcinedat873K for 2hin air. In thesecond syntheticprotocol (P2), thebinary Ti/Aloxidesupportmaterialwassynthesizedbyasolgelmethod. In this synthetic protocol (P2), titanium and aluminum alkox-ides were used as precursors. First, aluminum-tri-sec-butoxide (97%,Sigma–Aldrich)wasdissolvedinthemixtureof propan-2-ol(99.5+%,Sigma–Aldrich)andacetylacetone(99.3%,Fluka).Then, titanium(IV)isopropoxide(97%,Sigma–Aldrich)wasaddedtothe solutionatroomtemperature. Next,0.5MHNO3 wasgradually
addedtothesolutionin ordertoinitiatethegelformation.The resulting gel was aged for 10 days under ambient conditions, ground, and baked at873Kfor 2hin air. The molefractionof TiO2 (i.e. TiO2=nTiO2/(nTiO2+nAl2O3))intheTiO2/Al2O3binary mixture wasequal to 0.3 (based onthe amounts of Ti and Al
precursorsusedinthesynthesis)inbothofthesyntheticprotocols. BaO/TiO2/␥-Al2O3 (whichwillbehereafterreferred asBa/Ti/Al)
sampleswithdifferentBaloadings(8and20wt%BaO)were syn-thesizedbyconventionalincipientwetnessimpregnationofthe Ti/AlbinaryoxidesupportmaterialswithBa(NO3)2.In the
cur-renttext,sampleswith8and20wt%BaOloadingwillbedenoted as 8Ba/Ti/Al(P1, P2) and 20Ba/Ti/Al(P1, P2), respectively. For a comprehensivediscussionofthestructuralcharacterizationofthe synthesized materials via SEM, EDX, BET, Raman spectroscopy andXRD,theanalysisofthesurfaceacidityoftheTi/Al(P1)and 8/20Ba/Ti/Al(P1)samplesviapyridineadsorption,aswellasNOx
adsorption/releasepropertiesviaFTIRandTPD,readerisreferred toourpreviouslypublishedwork[23,37]whichwillalsobeused frequentlyinthediscussionofthecurrentresults.␥-Al2O3(Puralox,
200m2/g,SASOLGmbH,Germany)usedin(P1)syntheticprotocol
wasalsoutilizedasareferencematerialinsomeexperiments. TEMimageswere obtainedwitha resolution of 0.14nm on a JEM-2010 (200keV) microscopeequipped withan EDX spec-trometerwitha Si (Li) detectorhavinganenergy resolution of 130eV. The analyzed area in a typical EDX measurement was about10×10nm2.ThesamplesfortheTEManalysiswere
pre-paredby dispersing thepowders in anultrasonic ethanol bath andsubsequentdepositionofthesuspensionupona“holey” car-bonfilmsupportedonacopperTEMgrid.XPSdatawererecorded using a SPECS spectrometer with a PHOIBOS-100 hemispheri-calenergyanalyzerandamonochromaticAlK␣X-rayirradiation (h=1486.74eV, 200W). FTIRspectroscopic measurementswere carriedoutintransmissionmodeinabatch-typecatalytic reac-tor[20]coupledtoanFTIRspectrometer(BrukerTensor27)and a quadrupole mass spectrometer(QMS,Stanford Research Sys-tems,RGA200)usedforTPDexperiments.AllFTIRspectrawere acquiredat323K.IntheTPDexperiments,alineartemperature rampwithaheatingrateof12K/minwasutilizedtoheatthe sam-plewithin323–1023K.TheQMSsignalswithm/zequalto18(H2O),
28(N2/CO), 30(NO),34(H2S),32(O2), 44(N2O/CO2), 46(NO2)and
64(SO2)weremonitoredduringtheTPDmeasurements.BETSSA
andporesizedistributionmeasurementswereperformedusinga MicromeriticsTristar3000surfaceareaandporesizeanalyzerby low-temperatureisothermaladsorption–desorptionofN2.
Thesulfurexposureexperimentswereperformedthroughfour differentconsecutivesteps.In thefirstspectralacquisitionstep, the sample was exposed to 0.6Torr of SO2(g)+O2(g) mixture
(SO2:O2=1:10)for1hat323Kand thefirstFTIRspectrum was
obtainedinthepresenceoftheSO2(g)+O2(g)mixtureoverthe
sample.Inthesecondstep,thesamplewasannealedto473Kin thepresenceoftheSO2(g)+O2(g),andaftercoolingto323K,the
secondFTIRspectrumwasacquired.Inthethirdstep,beforethe spectrumacquisition,thesamplewasannealedto673K(inthe presenceofSO2(g)+O2(g)),thencooledto323Kandsuccessively
evacuatedat323Kfor20min(Preactor<1×10−4Torr).Inthefourth
step,thesamplewasflashedto673Kinvacuumandafter cool-ingthesampleto323K,aFTIRspectrumwasobtained.ForNO2
adsorptionexperiments,thefreshsampleswerepre-poisonedby anexposureof0.6TorrofSO2(g)+O2(g)(SO2:O2=1:10)mixture
at323Kandwerefurtherheatedinthegasmixtureat473Kfor 30min.Afterhavingpumpedoutthereactor,poisonedsamplewas exposedto8TorrofNO2(g)at323Kfor20mininordertosaturate
thesurfacewithNOx.ThisisfollowedbytheevacuationandFTIR
spectraacquisitionat323K.
3. Resultsanddiscussion
3.1. TEMcharacterizationofTi/Almaterials
Fig.1representstheTEMmicrographsoftheTi/Al(P1,P2) sam-plesshowingthemorphologyofthesynthesizedsupportmaterials.
EDXanalysisofarea1giveninFig.1a,whichisabundantindarker domains,revealsthepresenceofTiO2andAl2O3containingspecies
withaTi:Alatomicratioequalto70:30.EDXanalysisofthebright domainssuchasarea2inFig.1a,demonstratedthattheseareas exclusivelycontainAl2O3.However,theFourieranalysisofarea2
inFig.1adidnotrevealwell-definedspots,mostlikelyduetothe smallparticlesizesandthedefectivenatureofthesealumina crys-tallites.TheimageinFig.1bshowsahigh-resolutionTEM(HRTEM) micrographofsuchabrightdomain.
ItisvisibleinFig.1athatthedarkerdomainscontainaggregates withsizesofabout10nm.Fig.1cshowsaHRTEMimageofone ofthesedarkerdomains.InterplanarspacingmeasuredonHRTEM micrographsofthesedarkerdomainsareinverygoodagreement withtheanatasephaseofTiO2.FastFourierTransform(FFT)picture
obtainedfromthisimageisalsoshownasaninsetinFig.1cand isingoodagreementwiththereflexesofanatasephase(fileno. 21-1272inPDF-2Database,JCPDS-ICDD).
Fig.1d–fshowsTEMimagesoftheTi/Al(P2)sample.Itisclearly visibleintheseimagesthatthissampledisplaysarather homoge-nousmorphologyexhibitingauniformsponge-likefinestructure whichisduetothemesoporouscharacterofthemixedTixAlyOz
oxidephasethatisabundantinTiOx/AlOxinterfaces.Area1given
in Fig. 1e highlights a characteristic region where this rather homogenousandporousstructureisapparent.Ti:Alelementalratio obtainedfromtheEDXspectrumofarea1inFig.1discloseto 15:85which isinvery goodagreementwiththenominal com-positionexpectedfrom therelative concentrationsof TiandAl precursorsusedin thematerialsynthesis (20:80).On theother hand,EDX elementalanalysisof a lesscharacteristic (minority) regioninFig.1d(labeledasarea2)revealsthepresenceofalmost exclusivelyAl2O3 particles.TheTEMimagegivenin Fig.1eand
HRTEMimagegiveninFig.1fshowthecharacteristicsponge-like structureofTi/Al(P2).FFTimageoftheTEMimagegiveninFig.1f isalsopresentedasaninset.FuzzycharacteroftheFFTimageis inagreementwiththeamorphouscharacteroftheTixAlyOzoxide
phase withsmall anddisorderedAlOxand TiOx domains.
How-ever,the steepintensitychanges near0.45nm fromthecenter showsthat disorderedstructure isprobablyduetothealumina spinelstructure(thisdistancecanbeassociated withd-spacing between(111)closepackedoxygenplanesinthelatticeof␥-Al2O3
(fileno.29-0063inPDF-2Database,JCPDS-ICDD).FFTfiltered pic-ture(Fig.1g)supportsthelackofanorderedcrystallinestructure. TheseobservationsindicatethattheTi/Al(P2)structureismostly composedofa TixAlyOz mixedoxideexhibitinga large
concen-tration ofTiOx/AlOx interfacialsites,while theTi/Al(P1) reveals
aninhomogeneousdistributionoflargerAl2O3andTiO2
agglom-erates witha relativelysmaller concentrationof suchinterface sites.
3.2. Poresizedistribution
BET SSA analysis demonstrates that Ti/Al(P1) and (P2) sam-pleshavesurfaceareavaluesof167.0and393.2m2/g,respectively [37]. SSA values of Ti/Al(P1, P2) support materials as well as 8(20)Ba/Ti/Al(P1,P2) materialsafter thermal treatments within 623–1023Kcanbefoundinoneofourformerreports[37].Thepore sizedistributionsofthesesupportmaterialsmonitoredduringN2
desorptionarepresentedinFig.2.TheTi/Al(P1)sampleshowsa relativelybroadpeakwithanaverageporesizeabout80 ˚Awhichis probablyduetotheconvolutionoftheporesizedistributionsofthe discreteTiO2andAl2O3domains,whileTi/Al(P2)sample
demon-stratesarelativelynarrowdistributionwithanaverageporesizeof 30 ˚A,correspondingtotheTixAlyOzmixedoxidenetwork.Ascanbe
seeninFig.2,theporesizeanalysisisconsistentwiththedissimilar surfacestructuresoftheTi/Al(P1)andTi/Al(P2)supportmaterials.
Fig.1.(a–c)TEMimagesofTi/Al(P1),region1:TiO2-richdomains,region2:␥-Al2O3-richdomains,and(d–g)Ti/Al(P2),region1:sponge-likestructureoftheTiOx AlOx
mixedoxide,region2:(dark)Al2O3domains.EDXspectraobtainedfromselectedregionsarealsogivenasinsets.
3.3. SOxinteractionwithTi/AlandBa/Ti/Almaterials:FTIR
Itshouldbenotedthatthereisnotaclearconsensusonthe vibrationalspectroscopicassignmentsoftheSOxspeciesonmetal
oxides(particularlyonAl2O3)duetotheheavilyconvolutednature
oftheFTIRsignalsoftheadsorbedSOxspecies.Assignmentsofthe
FTIRsignalsforvariousSOxspeciesdiscussedintheliteratureare
summarizedinTable1.
WeperformedFTIRinvestigationsofSO2(g)adsorptionon
␥-Al2O3.Theresults(datanot shown)are inagreementwiththe
formerinvestigations,revealingtheformationofsurfacesulfites (SO32−)(notethatbulkAl2(SO3)3doesnotexist[60]),withoutany
additionaloxidationtosulfates.
300 250 200 150 100 50 0 0,0 0,5 1,0 1,5 2,0 2,5 3,0 3,5 4,0 Ti/Al (P1) Ti/Al (P2) pore size (Å) pore volume (cm 3/g)
Fig.2.PoresizedistributionplotsforTi/Al(P1)andTi/Al(P2)supportmaterials.
TheadsorptionofSO2(g)+O2(g)onthe␥-Al2O3surfaceat323K
(Fig. 3a, spectrum i) revealsa major broad band at 1073cm−1 aswellasweakerandpoorlydefinedadditionalfeaturesaround 1350,1250,1180and1005cm−1.ThepresenceofSO32−species
areapparentdue totheintense characteristic sulfitefeatureat c.a.1073cm−1(3)andtheshouldersat1049cm−1(3)aswellas
1005cm−1(1)[58–60].Minorfeaturesat1350(3)and1180cm−1
(1)canbeattributedtochemisorbedSO2 onabasic(O2−)
sur-facesites[59,60]whilethefeaturelocatedat1250cm−1 canbe associatedwiththeSO2adsorbedonAl3+Lewisacidsitesand/or
bidentatesulfates[59].AveryminorcontributionfromtheSO2(g)
speciesmayalsobepresentat1130(3),1150(1)and2499cm−1
(1+3,notshown)[60].
As the adsorption temperature increases to 473K (Fig. 3a, spectrumii)the1368,1102signalsbecomemore visiblewhich correspondtothe3 and1 modesofsurfacesulfatesonAl2O3, [60],respectively.Furthermore,theshoulderlocatedat1170cm−1 whichcanbeassociatedwithbulkAl2(SO4)3[56]startstobemore
discernible.Inaddition,arelativelyminorcontributionfrom sul-fatespeciesthatareinteractingwiththesurface–OHgroupswhich revealtypicalsignalsat1290and1080cm−1cannotbeexcluded [58].Increasingthetemperatureto673K(Fig.3a,spectraiiiandiv) resultsinthegrowthofthesurfaceandbulkaluminasulfatesin expenseofthesurfacesulfiteandchemisorbedSO2species.
Theseresultsindicatethatsulfitesareinitiallyformedonthe aluminasurfaceduringtheSO2+O2 adsorptionat323Kwhileat
elevatedtemperatures(473–673K),thesespeciesare converted intorelativelystablesurfacesulfates(SO42−/Al2O3)aswellasbulk
Al2(SO4)3.Theformationofsulfatesonaluminasurfacewas
con-sideredinnumerousformerstudies[56,57,60,68].Typically,SO2
bindstotheacidicsites(i.e.coordinatelyunsaturatedaluminum cations,Al3+)formingphysisorbedSO
2.TheadsorptionofSO2on
thebasicadsorptionsitesisfollowedbyacleavageofanAl Obond onthesurface(primarilyatOHsitesoratexposedoxygenatoms,
Table1
TypicalFTIRsignalsassociatedwithcommonSOxspecies[7,54–67].
Species Symmetry v1(cm−1) v3(cm−1) References
SO2(gas) C2v 1151 1362 [54] SO32−(freeion) C3v 961 1010 [54,55] SO42−(freeion) Td 1104 [54] S O O Al3+ (physisorbed) C2v 1135–1150 1300–1370 [7,55–58] S O O Al
(chemisorbed) C2v 1255(typeI),1189(typeII) [59]
S O O OH Al Cs 1148–1150 1330–1334 [55,59] O S O O Al Al C2v 1140 1320–1326 [55,59,60] S O O Al O C3v 1050–1065 1135 [56,59] S O O O O Al Al Al C3v 1045–1130 1380 [58,61] S O O O O Ti Ti Ti C3v 1005,1045 1370 [61] S O O O O C C (organicsulfates) C2v 1230–1150 1440–1350 [62,63] S O O S O O C2v ∼910 960–1000 S O O Fe O O C2v 1180,968 1375, 1025 [64] (NH4)2SO4 C2v 1090 1390 [65] BaSO4(surface) 1060 1120 [66] Ce(SO4)2(surface) 980 1340–1400 [67] Al2(SO4)3(bulk) 1190 [56] BaSO4(bulk) 1155,1248 [66] Ce(SO4)2(bulk) 1145–1240 [67]
O2−)leadingtotheformationofchemisorbedSO32−.Theoxidation
ofadsorbedSO32−/SO2inoxygenatrelativelyhightemperatures
(673–773K)leadstotheformationofsurfacesulfatespecieswhich arecoordinatedtothemetalcationsoftheoxidesurfacethrough threeoxygenatoms[60].
In order to examine the sulfur accumulation on the TiO2
(anatase) surface, SO2+O2 adsorption experiments were also
performed on TiO2 (Fig. 3b). At 323K (Fig. 3b, spectrum i)
acomplexandaconvolutedgroupofsignalswereobservedwithin 1150–950cm−1whicharelikelytobeassociatedwithSO32−and/or
HSO3− species[60].At473K,thefeatureat1137cm−1 startsto
growtogetherwithanintensefeatureat1350cm−1.In analogy withthesimilarbehaviorobserved fortheAl2O3 surface, these
twobandsareassignedtoweaklyadsorbedmolecularSO2species.
This assignment is also consistent with the attenuationof the 1137cm−1 signalafterevacuationat673K(Fig.3b,spectrumiv).
1000 1100 1200 1300 1400 1049 1005 1350 1250
absorbance (arb.u.)
γ-Al2O3 ii 1368 1170 995 1102 1073 0.05 (a)i
iii
iv
900 1000 1100 1200 1300 1137 0.05ii
i
iii
iv
TiO2 (anatase) (b) 1002 1046 1083 1160 1287 1356 13661000
1100
1200
1300
1400
(c) Ti/Al (P1)wavenumber(cm
-1)
1353 1173 1032 1235 1384i
ii
iii
iv
0.05900
1000
1100
1200
1300
1060 (d) Ti/Al (P2) 1360 1080 1160 1350 1260 0.05i
ii
iii
iv
Fig.3. FTIRspectrafor0.6TorrSO2(g)+O2(g)(SO2:O2=1:10)co-adsorptionon(a)␥-Al2O3,(b)TiO2(anatase),(c)Ti/Al(P1),(d)Ti/Al(P2).(i)After1hexposuretoSO2(g)+O2(g)
at323K(spectrumwasobtainedinthepresenceofthegasmixture),(ii)aftersubsequentflashingofthesampleto473KinSO2(g)+O2(g)mixtureandcoolingto323K
(spec-trumwasobtainedinthepresenceofthegasmixture),(iii)aftersubsequentflashingto673KinSO2(g)+O2(g)mixtureandfurtherevacuationat323K(Preactor<1×10−4Torr),
(iv)aftersubsequentflashingthesampleto673Kinvacuumandcoolingto323K.
Notethatitisdifficulttofollowthefateofthe1350cm−1at ele-vatedtemperaturessincenewbandsstartstogrowinthesame spectralregionat673K.Thefeaturelocatedat1287cm−1together withthe1083cm−1featurecanbeattributedtobidentatesulfates interactingwiththeadsorbedwaterat473–673K[58]and ortho-chelatingbidentatesulfateswhichrevealvibrationalfeaturesina similarrange[64,69].Aftertheevacuationat673K,relatively well-resolvedfeaturesareobservedintheFTIRdata(Fig.3b,spectrum iv).Thusthebandsat1366–1356,1160,1046and1002cm−1are assignedtosurfacesulfatesontheTiO2surfacewhichareformed
aftertheoxidationoftheadsorbedSOxspeciesat673K[61,70]. Fig.3canddshowstheIRspectraoftheTi/Al(P1)andTi/Al(P2) supportmaterialsaftertreatmentinSO2+O2atdifferent
temper-atures(323–673K),followedbyevacuation.TheIRspectradueto
theSO2+O2adsorptiononTi/Al(P1,P2)at323and473K(spectra
iandiiinFig.3candd)exhibitastrongresemblancewherethe mostprominentfeatureisthebroadIRsignalat∼1050cm−1 cor-respondingtosulfitespecies.Themaindifferencebetweenthese twospectraisthepresenceoftheshoulderat1130cm−1forthe Ti/Al(P1) sample which maybe likely due toweakly adsorbed SO2species,similartotheonesthatwereobservedforbothpure
anataseand ␥-alumina surfaces.Increasing the temperatureto 673KinthepresenceofSO2+O2leadstotheformationof
addi-tionalfeaturesassociatedwithsurfacesulfatesat1350–1360and 1160–1175cm−1onbothTi/Al(P1,P2)samples.Hightemperature SO2+O2 exposure alsoseem to triggerthegrowth of the
con-volutedbandat 1230–1260cm−1 on both samples,which may indicatetheformationofbidentatesulfates.Thepresenceofthe
1160–1170cm−1signalinFig.3canddalsosuggeststhepossible formationofbulkAl2(SO4)3species.Ageneralcomparisonofthe
lineshapesoftheFTIRspectragiveninFig.3canddrevealsthat sulfatecontainingsurfacedomainsontheTi/Al(P1)sampleare rela-tivelymoreorderedandwell-crystallizedwithrespecttothatofthe Ti/Al(P2)sample,whichisconsistentwiththesharperandbetter resolvedsulfatebandsvisibleinFig.3c.
Analogous experiments were also performed with Ba con-taining samples. In these studies, conventional 8(20)Ba/Al benchmark samples that do not contain TiO2, were compared
with 8(20)Ba/Ti/Al(P1,P2) samples containing TiO2. After the
introductionofa SO2+O2 mixtureonto the8Ba/Al and 20Ba/Al
samplesat323K(Fig.4aandc,spectrai)amajorbroadbandat 1080cm−1,whichcanbeattributedtosulfitespecies,isobserved. Aftersubsequentheating at473K (intheSO2+O2 gasmixture)
no substantial changes are observed in the case of the 8Ba/Al sample(Fig.3a, spectrumii),while in thecaseof 20Ba/Al,two differentfeaturesat1250and1160cm−1becomeapparent.These featurescanbeassignedtobulkBaSO4[66].Subsequentheating
at673KinSO2+O2mixture(Fig.4a,spectrumiii)andinvacuum
(Fig.4a,spectrumiv)leadstotheappearanceofthebulkBaSO4
bandsforthe8Ba/Alsample.Theadditionalsignalat1350cm−1 is associated with surface sulfates on alumina domains. This bandis morepronouncedforthe8Ba/Alsample, incomparison to the 20Ba/Al surface due to the larger number of exposed alumina sites in the former case as a result of the lower BaO loading.
Thesulfationexperimentsof8Ba/Ti/Al(P1)and20Ba/Ti/Al(P1) samplesarepresentedinFig.4bandd. AfterSO2+O2 exposure
at 323K, a set of broad and overlapping bands appear within 1100–980cm−1indicatingtheformationofvarioussulfitespecies. Interestingly,onlyinsignificantlyminorchangesareobservedfor the8Ba/Ti/Al(P1)sampleevenafterhightemperaturetreatment (Fig. 4b, spectra ii–iv) indicating that the formation of surface aluminum sulfate and bulkBaSO4 species is rather suppressed.
The changes observed for the 20Ba/Ti/Al(P1) sample are more pronounced (Fig. 4d): bulk BaSO4 related features at 1260 and
1160cm−1appearafterheatingat473Kandthesebandsbecome slightlymoreintenseaftersubsequentheatingat673K.Itisclear thatsuppressionofbulk BaSO4 formation byTiO2 promotionis
effectiveforthe8Ba/Ti/Al(P1)samplewhileitislessefficientfor 20Ba/Ti/Al(P1)sample.Wehavereportedinourpreviousstudies thatTiO2domainsfunctionasanchoringsitesforBaOsitesandlimit
thesurfacediffusionofBaOclusters[23,37].Thus,itislikelythat forlowBaOloadings,mostoftheBaOdomainsonthe8Ba/Ti/Al(P1) samplecaneffectivelybindtoTiO2domains,andpreventthe
sin-teringofBaOdomains.Thus,forlowBaOloadings,TiO2domains
canefficientlysuppresstheformationoflargeBaOclusterswhere thermallystablebulkBaSO4canform.Ontheotherhand,forhigher
BaOloadings,asinthecaseof20Ba/Ti/Al(P1),alargerfractionof theBaOdomainsarelocatedonthealuminasurfacewheretheycan diffusefasterandformlarger3DBaOclusterswhichcanenablethe formationofbulkBaSO4 asinthecaseof20Ba/Al(Fig.4c). Itis
worthmentioningthatsimilarexperimentswerealsoperformed on8(20)Ba/Ti/Al(P2)samples(datanotshown)andaqualitatively similarbehavior wasobservedindicatingthesignificanceofthe Ba/TiratiointhepromotionaleffectofTiinSOxuptake.
Inordertoquantitatively comparetheamountofSOxstored
ontheinvestigated surfaces,XPSanalysisofthepoisoned sam-pleswasperformed.Becauseoftherelativelylowsensitivityofthe XPStechniquetowardssulfur,poisoningprocedurewasmodified toobtainabettersignaltonoiseratioandmoreaccurateatomic ratiovalues.Thus,beforetheatomicratiodeterminationbyXPS,the sampleswerepoisonedin10TorrofSOx(SO2:O2=1:10)at673K
for30min.TheshapeoftheFTIRspectrarecordedafterthis poi-soningprocedure(datanotshown)wereinverygoodagreement
withthecorrespondingspectrapresentedinFigs.3and4.Binding energy(BE)ofS2p(168–170eV)XPSsignalindicatedthepresence ofmainlysulfates(i.e.S6+states)onallsamples.Itisworth
men-tioningthatalthoughinsituFTIRdatagiveninFig.4bsuggestthe presenceofmostlysulfitespeciesonthe8Ba/Ti/Al(P1)sample,XPS dataindicatesthepresenceofpredominantlysulfatespecies.This maybeassociatedwiththeexposureofthe8Ba/Ti/Al(P1)sample toatmospherebeforetheXPSanalysisresultingintheoxidation ofsulfitesintosulfates.Fig.5demonstratesthatunderidentical poisoningconditions,Ti/Al(P1,P2)samplesaccumulateupto3–5 timesmoresulfurthan␥-Al2O3.Thisbehaviormightbe
originat-ingfromthelargerSSAof theTi/Almaterialsincomparison to ␥-Al2O3aswellasthedecreasingnumberoftotalLewisacidsites
inmixedTi/Aloxides.ThelessacidicTi/Almixedoxidesurfaces candemonstrateahigheraffinitytowardsacidicSOx.Theacidityof
TiO2 Al2O3mixedoxidesaswellas␥-Al2O3hasbeeninvestigated
inpreviousstudies[23,71]bypyridineadsorption.Itwassuggested thatadditionofTiO2toAl2O3introducessomemediumstrength
Lewisacidsites,[23]howeveritwasdemonstratedinanotherstudy thatthetotalamountofLewisacidsitesisdecreasedby30%for TiO2 Al2O3incomparisontopurealumina[71].
Analysis of Fig. 5 also reveals that for an identical mass of eachmaterial(i.e.20mg),8Ba/Ti/Al(P1,P2)samplesaccumulate alesserquantityofsulfurthanthe8Ba/Alsample,demonstrating thefavorablepromotionaleffectofTionlimitingsulfur accumula-tion.Furthermore,8Ba/Ti/Al(P2)sampleseemstostoremoreSOx
(perunitsampleweight)thanthe8Ba/Ti/Al(P1)samplewhichcan beexplainedbythelargerSSAoftheformermaterial(185cm2/g
vs.150cm2/g,respectively)[37].However,itisimportantto
men-tion that the promotion of 8Ba/Al sample with TiO2 favorably
decreasesthetotalSOxuptake(perunitsampleweight)
regard-lessofthepreparationmethod(i.e.P1orP2)(notethattheSSA ofthefresh8Ba/Al sampleis185cm2/g[20]).Thistrendis
par-tiallyreversedwhentheBaOloadingisincreasedto20wt%.Fig.5 revealsthatalthough20Ba/Ti/Al(P1)sample(SSA=79cm2/g[37])
storesalesserquantityofSOx(perunitsampleweight)thanthat
of20Ba/Alsample(SSA=126cm2/g[20]);20Ba/Ti/Al(P2)sample
(SSA=173cm2/g[37])storesagreatertotalamountofSO x.These
resultssuggestthatforhigherBaOloadings,thepromotionaleffect ofTiO2isweaker.BesidestheseSSAtrends,thisobservationmay
alsoarisefromthefactthatnotalloftheBaOdomainsarelocated ontheTiO2sitesforhighBaOloadingsandalargefractionofthe
BaOdomainsdirectlyinteractwiththeunderlyingaluminasitesas inthecaseof20Ba/Alsystem.
3.4. InfluenceofSOxpoisoningontheNOxadsorption
NOxadsorptiononfreshTi/Al(P1,P2)andfresh8(20)Ba/Ti/Al(P1,
P2)samplesviaFTIRtechniqueandthecorrespondingassignments oftheobservedvibrationalbandswerethoroughlydiscussedinone ofourrecentreports[37]andthuswillnotbereiteratedhere.In thelightofthesepreviousstudies,similarNOxadsorption
experi-mentswerealsoperformedonthesulfur-poisonedmaterialsand theresultswereanalyzed.
Fig.6a comparestheNOxuptake characteristicsof thefresh
and poisoned ␥-Al2O3 surface at 323K.After the saturationof
thefresh␥-Al2O3 surfacewithNO2(g),vibrationalfeatures
asso-ciatedwithdifferenttypesofnitratespecieswereobserved.These nitratespeciesadsorbedon␥-Al2O3wereintheformofbridged
(1258,1628cm−1),bidentate(1300,1604cm−1)andmonodentate nitrates(1300, 1564cm−1)[37,72].Additionally,theweakband locatedat∼1958cm−1 thatwasformedafterNOxadsorptionon
thepoisonedsurfaceisassociatedwiththeadsorbedNO+and/or
weaklyadsorbedN2O3[73].Thepoisoningofthe␥-Al2O3surface
bySO2+O2decreasestheintensitiesofthenitratesignals,
1000 1100 1200 1300 1400 1043 1350 1250
absorbance (arb.u.)
8Ba/Al ii 1160 995 1080 0.05 (a)i
iii
iv
900 1000 1100 1200 1300 1250 0.05ii
i
iii
iv
8Ba/Ti/Al (P1) (b) 995 1046 1100 1160 1350 1000 1100 1200 1300 1400 1080 (c) 20Ba/Alwavenumber (cm
-1)
1350 1160 1040 1250i
ii
iii
iv
0.05 900 1000 1100 1200 1300 980 1120 1046 (d) 20Ba/Ti/Al (P1) 1100 1160 1350 1260 0.05i
ii
iii
iv
Fig.4.FTIRspectrafor0.6TorrSO2(g)+O2(g)(SO2:O2=1:10)co-adsorptionon(a)8Ba/Al,(b)8Ba/Ti/Al(P1),(c)20Ba/Al,(d)20Ba/Ti/Al(P1).(i)After1hexposureto
SO2(g)+O2(g)at323K(spectrumwasobtainedinthepresenceofthegasmixture),(ii)aftersubsequentflashingofthesampleto473KinSO2(g)+O2(g)mixtureand
coolingto323K(spectrumwasobtainedinthepresenceofthegasmixture),(iii)aftersubsequentflashingto673KinSO2(g)+O2(g)mixtureandfurtherevacuationat323K
(Preactor<1×10−4Torr),(iv)aftersubsequentflashingthesampleto673Kinvacuumandcoolingto323K.
inFig.6athatSOxpoisoningdecreasestherelativeratioof
mon-odentateandbidentatenitrates(1300cm−1)tothebridgednitrates (1258cm−1).Thisobservationsuggeststhatsulfatespeciesonthe ␥-Al2O3surfacesuppresstheformationofalltypesofnitrates,
par-ticularlythemonodentateandbidentatenitratesbyoccupyingthe correspondingadsorptionsites.
Theappearanceofthebandsat1375and1100cm−1inFig.6a forthepoisonedsampleindicatestheformationofsurfacesulfates. Althoughsulfateformationonthe␥-Al2O3surfaceintheabsence
ofNOxspecies(Fig.3a)requiresarelativelyhightemperature(i.e.
673K),sulfateformationcanreadilyoccurbyexposingthealumina surfacetoSO2(g)+O2(g)at473KfollowedbyNO2(g)exposureat
323K.Itisapparentthat,NOxspeciesfunctionasefficientoxidizing
agentsintheoxidationoftheSO2 and SO32−tosulfatesonthe
␥-Al2O3surface.Thefollowingreactionpathwayscanbesuggested
fortheinteractionbetweensurfaceSOxspeciesandtheadsorbed
NOxspecieson␥-Al2O3:
I:
SO32−(ads)+NO2(ads,g)→ SO42−(ads)+NO(g) (1)
SO32−(ads)+2NO2(ads,g) →SO42−(ads)+N2O3(ads) (2)
N2O3(ads)→ NO2−(ads)+NO+(ads) (3)
II:
3NO2(g)+O2−(s)→2NO3−(ads)+NO(g) (4)
Fig.5. Relativesulfurcontent(i.e.percentileofsulfuratomsonthesurfacewith respecttoallotheratoms)oftheinvestigatedsamplesaftersulfurpoisoning(as describedinthetext)determinedbyexsituXPSanalysis.
NO2−(ads)+NO2(ads,g) →NO3−(ads)+NO(g) (6)
NO2−(ads)+2NO2(ads,g) →NO3−(ads)+N2O3(ads) (7)
PathwayIsuggeststhatthesulfitespeciesonthe␥-Al2O3surface
thatareformedintheprocessofpoisoningcanbedirectlyoxidized tosulfateswiththehelpofNO2(g)orweaklyadsorbedmolecular
NO2.Ontheotherhand,pathwayIIproposesanalternativeroute
forthesulfateformation,wheresurfacenitratespeciesfacilitate theoxidationofsurfacesulfites(orweaklyadsorbedmolecularSO2
species).Inthislatterroute,duringthesulfateformation,nitrates areconsumed at theexpense ofnitrite and NO(NO+)or N
2O3
generation.Theobservationof1958cm−1featureintheFTIR spec-trumcorrespondingtothepoisonedsampleinFig.6a,which is notpresentinthecorrespondingspectrumforthefreshsample, supportstheformationofN2O3/NO+(reactions(2)and(7)).Itis
difficulttoassesswhichofthesetwopathwaysisfavoredonthe surfaceunderthecurrentexperimentalconditions.However,by takingintoaccountthefacileformationofnitratespeciesonthe ␥-Al2O3surface,itcanbearguedthatpathwayIImaypresumably
beoccurringmorereadilythanpathwayI.
Fig. 6b, presents analogous poisoning and subsequent NOx
uptakeexperimentsconductedonpureTiO2(anatase).TheLewis
acidsitesontheanatasesurfacerevealfourandfive-coordinated Ti4+ions(refereedas␣andsites,respectively)where␣-Lewis
acid sites (with two oxygen vacancies) favor bidentate (1578 andshoulder at∼1220cm−1)and bridge(1627 and1236cm−1) nitrateformationwhilethe-sites(Ti4+withoneoxygenvacancy)
favortheformationofmonodentatenitrates(groupoffeaturesat 1550–1500cm−1andpeakat1282cm−1)[37,74–77].SimilarFTIR signals,thoughwithreducedintensitiesofallNOxvibrational
sig-nalsarealsoobservedforthepoisonedanatasesamplemarkedin redinFig.6b.Thepoisonedanatasesamplealsoshowssome addi-tionalbandsat1359and1030–1070cm−1thatareassociatedwith thesulfiteandsulfatespecies.
SimilarexperimentswerealsoperformedonTi/Al(P1,P2) sur-facesasshowninFig.6candd.ItisreadilyseenthattheNOxuptake
issuppressedbySOxpoisoningonbothsurfaces.ItisvisibleinFig.6
thattheextentofthenitratesignalsuppressionismorepronounced forTi/Al(P1,P2)samplesincomparisonwithpure␥-Al2O3andTiO2.
ThisresultisinagreementwiththeXPSdatagiveninFig.5, indi-catingasignificantlyhigheraffinityofTi/Al(P1,P2)towardsSOx
thanthatofpure␥-Al2O3.Sucha behaviorcanbeexplainedby
anincrease intheSSAvalues and adecreasein thetotal num-berofLewisacidsitesuponTiO2promotion.Asimilarinteresting
behaviorwasalsoreportedintheliteratureforTiO2–ZrO2mixed
oxidesystems.Forinstance,itisknownthatpureTiO2(anatase)or
pureZrO2 (monoclinic/tetragonal)haveverylimitedNOxstorage
capacities[78].Ontheotherhand,whenthesetwodifferenttypes
ofoxidesarecombinedtoobtainanamorphousTiO2–ZrO2mixed
oxide,NOxstoragecapacitycanbeimprovedbymorethananorder
ofmagnitude,whichwasattributedtotheformationofnewLewis basicsitesattheTiO2–ZrO2hetero-junctions[78].Inanalogywith
theseobservations,Ti/Al(P1,P2)surfacesmayalsocontainnewand strongSOxadsorptionsites,whicharenotpresentoneitherpure
TiO2or␥-Al2O3surfaces.
WhentherelativepoisoningofTi/Al(P1)iscompared tothat ofTi/Al(P2) (Fig.6cand d),itis visiblethatnitratefeaturesare suppressedtoalesserextentonTi/Al(P2),althoughtheintensities ofsulfatefeatures(1360and1100cm−1)arestrongeronTi/Al(P2) (Fig.5d).Thisobservationsuggeststhattheporousanddisordered surfacemorphologyoftheTi/Al(P2)sampleresultsinalarger over-allSOxuptake,howeverduetoitslargesurfacearea(SSAoffresh
Ti/Al(P1)and Ti/Al(P2)are167and393m2/g,respectively [37]),
Ti/Al(P2)surfacestillpossessesalargernumberofNOxbindingsites
withrespecttoTi/Al(P1).Ontheotherhand,suchacomparison basedsolelyonIRintensitiesshouldbeconsideredwithcaution, astheIRabsorptioncross-sectionsofadsorbednitratespecieswith dissimilaradsorptionconfigurationscanbesignificantlydifferent, whichmayrenderadirectIRintensitycomparisonrelatively inac-curate.
Fig. 7 compares the NOx adsorption properties of
8(20)Ba/Ti/Al(P1, P2), samples before and after SOx
adsorp-tion at323K.The FTIRresultscorrespondingtotheadsorption of NO2 onthefreshsampleswerealready discussed elsewhere [37].Briefly,uponNO2 adsorption,thefreshsamplesurfacesare
characterized by adsorption bands due to the presence of the bulk(ionic)Ba-nitrateslocatedat∼1320,∼1440and∼1480cm−1, surface (bidentate) Ba-nitrate features located at 1585, 1565, 1300cm−1andadditionalnitratebandsat1583and∼1630cm−1 thatareassociated withnitratesadsorbedontheTiO2 domains
havingbidentateandbridgedconfigurations.AfterSOxpoisoning
ofthesampleswithSO2+O2at473K,itisclearlyvisiblethatthe
NOx storage capacities decrease significantly. Additionally, the
presenceofminorbandsat∼1150and∼1245cm−1 impliesthe existenceofsulfatespeciesonallofthesamples.Formationof sul-fatespeciesonallofthesamplesaftersubsequentNO2adsorption
at 323Kdemonstrates theefficient oxidizingcapability of NO2
whichcanreadilyoxidizesulfitespeciesthatareformedduring the SO2+O2 exposure. It is worth mentioning that the similar
experimentsperformedon8(20)Ba/Alsamples(datanotshown) revealedqualitativelysimilarresultsindicatingthesuppressionof NOxuptakeuponsulfurpoisoning.
3.5. ThermalstabilityoftheadsorbedNOxspeciesonthe
sulfur-poisonedmaterials
In order to have a betterunderstanding of theinfluence of SO2+O2 treatmenton thethermal stability and thedesorption
propertiesoftheNOxspecies,TPDexperimentswerepreformed. Fig.8showstheNOxdesorptionprofilesfromthefreshandSOx
poisoned␥-Al2O3andTiO2(anatase)benchmarksamples.For
clar-ity,onlythem/z=30,m/z=32andm/z=46desorptionchannelsare shown.Forthefreshaluminasurface,twomajorNOandNO2
des-orptionfeaturesareobserved,thatisingoodagreementwiththe literaturedata[20,79].ThefirstNOxdesorptionfeatureat387K
is associated withthe desorption of monodentate nitrates and weaklyboundN2O3and/orNO+specieswhichdesorbintheform
ofNO2andNO(almostwithoutO2).Thesecondmajordesorption
bandhasitsmaximumat625Kandisassociatedwiththe desorp-tion/decompositionofbridgedandbidentatenitrateswhichyield agreaterNO2desorptionsignalalongwithNOandO2[20,79].
TheSO2-poisoning ofthealuminasurfacehasastrong
influ-enceontheNOxdesorptionfeatures.AsitisseeninFig.8b,sulfur
1000 1200 1400 1600 1800 2000 2200
absorbance (arb.u.)
γ-Al2O3 (a) 1958 1628 1604 1375 1300 1259 1102 10411003 Fresh sample 1564 0.2 Poisoned sample 1200 1400 1600 1800 2000 TiO2 (anatase) (b) Poisoned Sample Fresh Sample 1627 1578 1550 1359 1282 1236 1070 1028 0.2 1000 1200 1400 1600 1800 2000 2200 (c) Ti/Al (P1)wavenumber (cm
-1)
Fresh Sample Poisoned Sample 1631 1580 1294 1258 1040 0.2 1200 1400 1600 1800 2000 (d) Ti/Al (P2) Fresh Sample Poisoned Sample 1640 1584 1237 1212 1100 1360 1040 0.2Fig.6. FTIRspectramonitoredafterNO2adsorptionat323Konfresh(blackspectra)andpoisoned(redspectra)(a)␥-Al2O3,(b)TiO2(anatase),(c)Ti/Al(P1),(d)Ti/Al(P2)
samples.Poisoningwasperformedbyexposingthesamplesto0.6TorrSO2(g)+O2(g)(SO2:O2=1:10)at323K,followedbyheatinginthegaseousmixtureat473Kfor30min
andafinalevacuationat323K(Preactor<1×10−3Torr).NOxuptakewasperformedbyexposingthesamplesto8TorrofNO2(g)at323Kfor20min,followedbyevacuation
to<1×10−3Torr.Allspectrawereacquiredinvacuumat323K.(Forinterpretationofthereferencestocolorinthisfigurelegend,thereaderisreferredtothewebversion
ofthisarticle.)
species.Forthepoisonedsample,themajorfeaturearound380K (associatedwiththemonodentatenitratesorweaklyboundN2O3
desorption)appearstoalargerextentthandesorptionof biden-tate/bridgednitrateat675K.Thisfindingisalsoconsistentwiththe FTIRresultsobtainedforNO2adsorptiononthesulfated␥-Al2O3
surface,yieldingthebandcorrespondingtoadsorbedNO+/N 2O3
speciesat 1958cm−1 (Fig.6a).Relativelylower intensityofthe 1958cm−1 band(Fig.5a)incomparisontotheotherNOxbands
couldbeassociatedwithitslowIRabsorptioncross-section.Thus, SOx species seem tocompete withthe nitratespecies for
sur-faceadsorptionsites.Furthermore,inthepresenceofSOxspecies,
stronglyadsorbednitratesarepartiallyconsumedandconverted intoweaklyboundN2O3(reactions(2)and(7))orNO+ (reaction (3))whilesomeofthesulfitesandchemisorbedSO2speciesare
con-vertedintosulfatesthroughreactionssimilartotheonesproposed above(pathwayII).
Fig.8canddshowstheTPDprofilesforNOxdesorptionfrom
freshandSOxpoisonedTiO2(anatase)samples.FreshTiO2sample
presentsaweakshoulderat455Kandtwobroadfeatureslocated at610and900KinNOdesorptioncurve.Inthelightoftheformer studies[74–77]theshoulderat455Kcanberelatedto molecu-larlyboundNO2 speciesandmonodentatenitrates.Thebandat
1000 1200 1400 1600 1800 2000 2200 8Ba/Ti/Al (P2) 8Ba/Ti/Al (P1)
absorbance (arb.u.)
(a) 1630 1440 1310 1240 1150 1040 Fresh sample 1570 0.2 Poisoned sample 1200 1400 1600 1800 2000 1450 (b) Poisoned Sample Fresh Sample 1635 1580 1485 13051260 1150 1040 0.2 1000 1200 1400 1600 1800 2000 2200 1040 1440 20Ba/Ti/Al (P1) (c)wavenumber (cm
-1)
Fresh Sample Poisoned Sample 1630 1570 1320 1250 1150 0.2 1200 1400 1600 1800 2000 1320 1440 1570 1630 20Ba/Ti/Al (P2) (d) Fresh Sample Poisoned Sample 1250 1155 1040 0.2Fig.7.FTIRspectramonitoredafterNO2adsorptionat323Konfresh(blackspectra)andpoisoned(redspectra)(a)8Ba/Ti/Al(P1),(b)8Ba/Ti/Al(P2),(c)20Ba/Ti/Al(P1),(d)
20Ba/Ti/Al(P2)samples.Poisoningwasperformedbyexposingto0.6TorrSO2(g)+O2(g)(SO2:O2=1:10)at323K,followedbyheatinginthegaseousmixtureat473Kfor
30minandafinalevacuationat323K(Preactor<1×10−3Torr).NOxuptakewasperformedbyexposingthesamplesto8TorrofNO2(g)at323Kfor20min,followedby
evacuation.Allspectrawereacquiredinvacuumat323K.(Forinterpretationofthereferencestocolorinthisfigurelegend,thereaderisreferredtothewebversionofthis article.)
610Kisattributedtothedesorption/decompositionofthebridged andbidentatenitrates.Thehightemperaturedesorptionfeatureat 900Kcanbeattributedtothedesorptionofstronglyboundnitrates. Itisknown[23]thatphasetransitionfrombulkanatasetobulk rutilestartsatT>800K.ThereforethestrongNOxdesorption
sig-nalat900KinFig.8ccouldbeassociatedwiththedrasticdecrease inthesurfaceareaofTiO2asaresultofthephasetransitionfrom
anatasetotherutilephase.Notethatduringtheactivationofthe freshandpoisonedanatasesurfacesbeforetheTPDexperiments, TiO2sampleswerenotexposedtotemperatureshigherthan623K
inordertopreservetheanatasephasepuritythus,theactivation wasperformedviaO2(g)ratherthanNO2(g).
The poisoned TiO2 sample shows an additional minor
des-orption feature at 345K (Fig. 8d). We attribute this feature to thedesorptionofweaklyadsorbedN2O3/NO+ (desorptionoccurs
mainlyintheformofNO+NO2).Thedesorptionfeatureat450Kis
associatedwithweaklyadsorbedmolecularspeciesand/orwith monodentatenitrates. TPDprofileof thepoisoned TiO2 sample
(Fig.8d)revealsa decreasein the450K desorptionsignalwith respecttothatofthefreshsample(Fig.8c)inagreementwiththe FTIRdata(Fig.6b)indicatinga suppressionofthemonodentate nitratesignalsat1550and1282cm−1 uponpoisoning.Themain desorptionbandforthepoisonedTiO2sampleoccursat615K
1000 900 800 700 600 500 400
QMS intensity (arb.u.)
γ-Al2O3 fresh (a)
NO2 O2 NO 385 620
1x10-6
1000 900 800 700 600 500 400 γ-Al2O3 poisoned (b) 675 630 NO NO2 O21x10-6
380 1000 900 800 700 600 500 400 x4TiO2 (anatase) fresh (c)
Temperature (K)
NO2 O2 x4 NO1x10-6
455 610 900 900 800 700 600 500 400TiO2 (anatase) poisoned (d)
x4 x4 NO2 NO O2 345 450 615 545 805
1x10-6
Fig.8.TPDprofilesobtainedfromfreshandpoisoned(aandb)␥-Al2O3,(candd)TiO2(anatase)samplesaftersaturationwith8TorrNO2(g)at323Kfor20min.Black,blue
andredcurvescorrespondtom/z=30(NO),m/z=32(O2)andm/z=46(NO2)signals,respectively.Poisoningwasperformedbyexposingthesamplesto0.6TorrSO2(g)+O2(g)
(SO2:O2=1:10)at323K,followedbyheatinginthisgaseousmixtureat473Kfor30minandafinalevacuationat323K.(Forinterpretationofthereferencestocolorinthis
figurelegend,thereaderisreferredtothewebversionofthisarticle.)
theformofbridged/bidentatenitrates.Animportantaspectofthe poisonedanataseTPDprofileisthelackofastrongdesorption sig-nalatT>800KsuggestingtheblockingofthestrongNOxadsorption
sitesbysulfates.
Fig.9aandbpresentstheNOxdesorptionprofilesoffreshand
poisonedTi/Al(P1)samples.Takingintoconsiderationthesurface morphologyofthefreshTi/Al(P1)sample,whichiscomposedof rel-ativelyorderedandwell-crystallizedAl2O3andTiO2domains,the
lowtemperaturepeaksofNOandNO2desorptionat355and395K
canbeattributedtodesorptionofweaklyadsorbedN2O3 (NO+)
and/ormonodentatenitratesonthealuminadomains.Desorption ofbridgedandbidentatenitratesoccursintheformofNO2+O2
at625Kwhilethe780Kdesorptionsignalisobservedintheform ofNO+O2.Thedesorptionsignalat625KinFig.9amayoriginate
frombothaluminaandtitaniadomainsofTi/Al(P1)sincesimilar featuresexistintheTPDprofilesofpureTiO2andAl2O3samples
(Fig.8aandc).Ontheotherhand,themajordesorptionsignalin Fig.9aappearingat780Kwithashoulderat870Khasasignificantly higherdesorptiontemperaturethananyofthepureAl2O3
desorp-tionfeatures.Thus,the870KfeatureinFig.9acanbeattributedto thedecompositionofstronglyboundnitratesontheTiO2domains
orontheperipheraladsorptionsiteswhicharelocatedatthe inter-facebetweenTiO2andAl2O3domains.Itisimportanttomention
thattheoriginofthisdesorptionfeatureisprobablyquitedifferent thanthe900KdesorptionsignalinFig.8cwhichisobservedfor pureanatase.Ourprevious[23,37]XRD,Ramanspectroscopyand BETanalysisresultsindicatethatonTi/Al(P1,P2)surfaces,anatase torutileand␥-Al2O3→␣-Al2O3phasetransformationphenomena
1000 900 800 700 600 500 400
QMS intensity (arb.u.)
Ti/Al (P1) fresh (a)
NO NO2 O2 780 870 625 355 395
1x10-6
x4 x4 1000 900 800 700 600 500 400 Ti/Al (P1) poisoned (b) x4 x4 370 720 630 NO O2 NO21x10-6
1000 900 800 700 600 500 400 885 Ti/Al (P2) fresh (c)Temperature (K)
x4 x4 NO O2 NO2 370 645 745 815 9201x10-6
1000 900 800 700 600 500 400 NO O2 NO2 x4 x4 Ti/Al (P2) poisoned (d) 440 560 640 8501x10-6
Fig.9. TPDprofilesobtainedfromfreshandpoisoned(aandb)Ti/Al(P1),(candd)Ti/Al(P2)samplessaturatedwith8TorrNO2(g)at323Kfor20min.Black,blueand
redcurvescorrespondtom/z=30(NO),m/z=32(O2)andm/z=46(NO2)signals,respectively.Poisoningwasperformedbyexposingthesamplesto0.6TorrSO2(g)+O2(g)
(SO2:O2=1:10)at323K,followedbyheatinginthisgaseousmixtureat473Kfor30minandafinalevacuationat323K.(Forinterpretationofthereferencestocolorinthis
figurelegend,thereaderisreferredtothewebversionofthisarticle.)
occuronlyattemperatureshigherthan1073K.Accordingly,onlya moderatedecreaseinthespecificsurfaceareavaluesareobserved atT≤900K.Thus,itisunlikelythatthe870KfeatureinFig.9aisdue toanatasetorutileor␥-Al2O3→␣-Al2O3phasetransitionsorany
otherassociateddrasticattenuationinthesurfaceareaofthe sam-ples.AnotherinterestingaspectoftheTPDdatagiveninFig.9isthe relativelylowintensityoftheO2desorptionsignalsincomparison
withthatoftheNOdesorptionsignals.Onepossibleexplanation forthisobservationisthat,duringthevacuumannealingand acti-vationoftheTi/Al(P1,P2)samplesinsidetheIR-TPDcell,someof thesurfaceTiO2domainsmaybepartiallyreduced.Thesereduced
TiO2surfacedomainscontainingoxygendefectsarehealedbythe
oxygenspeciesthataregeneratedduringthedecompositionofthe nitratespeciesinthecourseoftheTPDexperiments.
AfterpoisoningoftheTi/Al(P1)sample,desorptionoftheweakly adsorbed NOx species at < 400K proceedsmainly in the form
of NO2 (Fig. 9b). One can also see that NO2 desorption peak
at625–630Kissignificantlydiminished.Furthermore,themost prominentNOxdesorptionfeatureshiftstoalowertemperature
by60Kand islocatedat720Kfor thepoisonedTi/Al(P1) sam-ple.Thisis accompaniedbythealmostcomplete disappearance ofthehightemperatureNOdesorptionsignalat870K.Itisclear that thepresenceofsulfiteand sulfate speciesontheTi/Al(P1) surfaceleadstotheblockingofthestrongNOxbindingsitesand
inhibitstheformationofstronglyboundnitrates.Inaddition,SOx
accumulationonthesurfacealsodestabilizesthenitratespecies whichareboundtointermediate-strengthNOxadsorptionsiteson
1000
900
800
700
600
500
400
QMS intensity (arb.u.)
8Ba/Ti/Al (P1) fresh (a)
NO NO2 O2 780 930 390
1x10-6
1000
900
800
700
600
500
400
8Ba/Ti/Al (P1) poisoned (b) 360 760 640 NO O2 NO21x10-6
1000
900
800
700
600
500
400
x4 20Ba/Ti/Al (P1) fresh (c)Temperature (K)
NO O2 NO2 380 710 800 9301x10-6
1000
900
800
700
600
500
400
370 770 20Ba/Ti/Al (P1) poisoned NO O2 NO2 (d) 490 640 6901x10-6
Fig.10.TPDprofilesobtainedfromfreshandpoisoned(aandb)8Ba/Ti/Al(P1),(candd)20Ba/Ti/Al(P1)samplessaturatedwith8TorrNO2(g)at323Kfor20min.Black,blue
andredcurvescorrespondtom/z=30(NO),m/z=32(O2)andm/z=46(NO2)signals,respectively.Poisoningwasperformedbyexposingthesamplesto0.6TorrSO2(g)+O2(g)
(SO2:O2=1:10)at323K,followedbyheatinginthisgaseousmixtureat473Kfor30minandafinalevacuationat323K.(Forinterpretationofthereferencestocolorinthis
figurelegend,thereaderisreferredtothewebversionofthisarticle.)
TheTPDprofileoffreshTi/Al(P2)(Fig.9c)demonstratesminor NOandNO2desorptionpeaksat370KandsomebroadNO,NO2and
O2desorptionfeaturesthatappearbetween645–745K.These
fea-turescanbeattributedtotheNOxdesorptionfromAl2O3domains [37]oftheTi/Al(P2)surface.Thissamplealsorevealsa NO des-orptionsignalat900–920Kwhichcanbeassociatedwithstrongly boundbidentateorbridgingnitratesadsorbedonthedisordered anddefective bindingsites of theporousTixAlyOz mixedoxide
surface.
Afterpoisoning (Fig. 9d) the Ti/Al(P2) sample, the presence of sulfates inhibits the adsorption of NOx species particularly
on the weak (T<550K) and strong (T>870K) NOx binding
sites, while influencing the intermediate-strength NOx binding
sites (550K<T<870K) to a lesser extent. Thus, formation of weaklybound(N2O3/NO+/NO2)aswellasstronglybound
biden-tate/bridgingnitratesaresignificantlysuppressedafterpoisoning. Alongtheselines,themainNOandNO2 desorptionfeaturesare
alsoshiftedtolowertemperaturesafterSOxpoisoningindicating
thedestabilizationoftheadsorbednitrates.
SimilarTPDexperimentswerealsoperformedonBa contain-ingBa/Ti/Al systemsand therepresentativedatacorresponding tosomeoftheseexperimentsarepresentedbelow.TheNOx
des-orptionfeaturesfromthefresh 8Ba/Ti/Al(P1)sampleupon NO2
adsorptionat323KarepresentedinFig.10a.Thedominant fea-tureat 930Kis associated withthe decomposition of thebulk Ba-nitrates onthelargeBaO clusterswhich are locatedonthe
agglomeratedTiO2 particles[23].Thelow-temperaturefeatures
areattributedtotheconvolutionofsignalsoriginatingfromthe decompositionofnitratesonlargeTiO2crystallites(780K)andthe
decompositionofthesurface(bidentate)nitratesonBa-domains (650–700K)[23].
Thepoisoningof8Ba/Ti/Al(P1)samplewithSOxat323K,prior
to the NO2 adsorption increases the desorption signal of the
weaklyadsorbedspecies(Fig.10b)asobservedinthecaseofthe correspondingsupportmaterialTi/Al(P1).TheprominentNOx
des-orptionbandobservedforthepoisonedsampleislocatedat760K, witha shoulderat 640K.Thehightemperaturedesorption fea-tureat930Kisnotdetectedforthepoisoned8Ba/Ti/Al(P1)sample, suggestingtheinteractionoftheSOxspecieswiththelargerBaO
clustersandsuppressionoftheformationofthermallystablebulk nitratespeciesbyblockingthesurfacesitesandlimitingthe diffu-sionofnitratesintothesubsurfaceoftheBaOclusters.Unlikethe freshsample,poisonedsampleyieldsmorepronouncedNOx
des-orptionfeaturesat∼640KassociatedwithsurfaceBaOandTiO2
sitesratherthanbulkBaO.Furthermore,it isworthmentioning thatthedesorption/decompositionofthestoredNOxiscompleted
atca.900Kforthepoisoned8Ba/Ti/Al(P1)samplewhichclearly emphasizesthedestabilizationeffectofthesulfatesonthestored nitratespecies.
TPDdatagiven in Fig.10c andd for the20Ba/Ti/Al(P1)also demonstratethesuppressionofthehigh-temperaturedesorption signal located at 900–950K after sulfur poisoning. Concomi-tantly,medium-temperatureNOdesorptionsignalat600–800K which is associated with nitrates on well-dispersed titania domainsaswellasnitratesonaluminasitesis alsosuppressed to a certain extent. Suppression of the bulk Ba(NO3)2
forma-tion upon sulfur poisoning was also observed in similar TPD experiments(datanotshown)performedwith8(20)Ba/Ti/Al(P2) samples.
3.6. ThermalstabilityoftheadsorbedSOxspecies
DuringTPDexperimentsgiveninsection3.5,whichwere per-formedafterthesaturationofSOx-poisonedsurfaceswithNO2,
desorptionofSO2(m/z=64)wasalsomonitoredinaparallel
fash-iontotheNOxdesorptionchannels.ItisworthmentioningthatSO2
wastheonlysignificantSOxspeciesdesorbingfromthe
investi-gatedsurfacesinadditiontoaveryminoramountofH2S(m/z=34)
specieswhoseintensitywasatleast20-foldsmallerthanthatof SO2.TheSO2 andH2SdesorptionchannelsoftheseTPD
experi-mentsarepresentedinFig.11.
ThegeneralcharacteristicsoftheSOxdesorptionfromtheTiO2
(anatase)surface(Fig.11)revealrelativelyunstableSOxspecies
thatdesorbat452Kasabroadpeak(duetoSO32−and/orweakly
boundmolecularSO2).At760K,anintenseSO2desorptionsignal
isvisible.ThisdrasticSO2 evolutionataratherlowtemperature
(i.e.760K)couldbeassociatedwiththedecompositionofsulfates asaresultoftheanatasetorutilephase transitionandthe col-lapseoftheporousanatasestructuretoformthelow-surfacearea rutilepolymorph.For␥-Al2O3,twomajordesorptionsignalsare
observedintheSO2desorptiontrace.Thefirstdesorption
maxi-mumappearsat510KandisprobablyassociatedwithSO32−and/or
weaklyboundmolecularSO2.Thesecondandthemostprominent
desorptionsignalstartstoappearatT>900Kandrevealsalarge desorptionsignalwhosedesorptionmaximumisbeyondthe ulti-matetemperaturelimit(i.e.ca.1020K)thatcanbereachedinthe currentTPDexperimentalsetup.ThishightemperatureSO2
des-orptionsignalisattributedtothestronglyboundsurfaceand/or bulksulfatesonalumina[80].
TheSO2 desorptionprofileofthepoisonedTi/Al(P1)(Fig.11)
surfaceappearsastwoconvolutedbutdistinguishablelow temper-aturefeaturesat480and542Kaswellasahightemperaturefeature
whichbarelystartstoappearat900K(whosedesorptionmaximum islikelylocatedatT1020K).Comparisonofthelow-temperature bands arising from theTi/Al(P1) surface withthe ␥-Al2O3 and
TiO2referencematerials,indicatesthatthe480Kfeatureismost
likely associatedwiththedesorptionfromTiO2 domains,while
the542Kfeature isassociated withthedesorption fromAl2O3
domains.Inthelowtemperatureregion,SO2desorptionprobably
takesplacefromboth␥-Al2O3 andTiO2 domainswhilethehigh
temperaturedesorptionfeatureappearingatT>1000Kcouldbe relatedtothesulfatedesorptionfromthe␥-Al2O3domainsorfrom
theTiO2 Al2O3hetero-junction(interface)sites.Themost
impor-tantaspectoftheSO2desorptionsignalfromtheTi/Al(P1)sample
is thatthestrongly boundsulfatespecies desorbata tempera-turehigherthanthatofthe␥-Al2O3surface.TheSO2desorption
profileoftheTi/Al(P2)sample(Fig.11d)demonstratesabroad des-orptionsignalwithin400–800Kwithamaximumat590K.This broadpeakcanbeenvisionedasaconvolutionofallofthe low-temperatureSO2 desorptionfeaturesthatareobservedforTiO2,
Al2O3andTi/Al(P1)whichisinlinewiththepoorlydefinedandthe
amorphoussurfacestructureoftheTi/Al(P2)samples.Itis impor-tanttomentionthattheSO2desorptionfeaturesforTi/Al(P2)in
theintermediatetemperatureregion(400–800K)appearhigher than that ofTi/Al(P1). Thisobservationindicatesthat the ther-malstabilityofSOxspeciesontheTi/Al(P2)surfaceishigherthan
thatofTi/Al(P1).ApparentlyTi/Al(P2)samplealsopresentsa high-temperatureSO2 signalwhich startstoevolveat T>970Kwith
adesorptionmaximumlocatedatT1020K.Initialtake-offfor this high-temperaturedesorption featurealsostartsat ahigher temperaturethanthecorrespondingfeatureforTi/Al(P1) consis-tent with the higher stability of SOx species on Ti/Al(P2). The
SOxdesorptionprofilesofalloftheBa-containingsampleswere
rathersimilartoeachother(Fig.11),presentingalow-temperature SO2desorptionsignalwithabroadlineshapewithin400–700K.
Thisisfollowedbyahigh-temperatureSO2 desorptionsignalat
T>1000K,whichwasabovethetemperaturewindowaccessible withthecurrentlyusedTPDexperimentalsetup.Thus,although thecurrentTPDexperimentscannotdiscriminatetherelative ther-malstabilitiesofthestronglyboundSOxspecies,FTIRtechnique
canprovide valuableinsights regardingthis point, asdescribed below.
Fig.12showsaninterestingsetofFTIRdatademonstratingthe thermalregeneration capabilitiesoftheTiO2-promotedsamples
aftersulfurpoisoning.TheseseriesofFTIRspectrawereobtained onsampleswhichareinitiallypoisonedwithSO2+O2at323Kand
thensuccessivelysaturatedwithNO2at323Kandfinally
evacu-atedinvacuumat1023K.Afterthehigh-temperatureevacuation, all ofthe adsorbedNOx species werefoundto desorbfrom all
oftheinvestigatedsurfaces.Howeversomeofthethermally sta-bleadsorbedSOxspeciesstillexistonthesamplesurfaces,even
afterthethermal regenerationtreatmentat1023K.Considering thedatacorrespondingtothe8Ba/Al and 20Ba/Alconventional benchmarksamplesinFig.12,itisapparentthatthese conven-tional NOx storage materials still possess a significant amount
of stable surface aluminum sulfates(1360 and 1125cm−1)and bulkBaSO4(1258and1160cm−1)evenafterthermalregeneration
treatmentat1023K.Inotherwords,theeffectofsulfur poison-ingisrelativelysevereandirreversibleonconventionalTiO2-free
materials, leading to extremely stable SOx species that cannot
bereadilyremoved evenafter evacuationatelevated tempera-tures.
On theother hand,TiO2-promotedsamples given in Fig.12
show a much better thermal regeneration behavior, revealing significantlysmallerintensitiescorrespondingtotheSOx
vibra-tional features after evacuation at 1023K. This is particularly validfor8Ba/Ti/Al(P1,P2)and20Ba/Ti/Al(P1)samples.Combining theseresultswiththerelativetotalSOxuptakedatapresentedin
1000 900 800 700 600 500 400 γ-Al2O3 poisoned
QMS intensity (arb.u.)
(a) x20 SO2 H2S 510 6901x10-7
1000 900 800 700 600 500 400TiO2 (anatase) poisoned (b)
x20 H2S SO2 760 775 450
1x10-7
1000 900 800 700 600 500 400 Ti/Al (P1) poisoned (c)Temperature (K)
x20 480 540 720 SO2 H2S1x10-7
1000 900 800 700 600 500 400 Ti/Al (P2) poisoned (d) x20 580 850 SO2 H2S 7601x10-7
Fig.11.SO2desorptionprofilesinTPDexperimentsfor␥-Al2O3,TiO2,Ti/Al(P1andP2),sampleswhichwereinitiallypoisonedwith0.6TorrSO2(g)+O2(g)(SO2:O2=1:10)at
473Kfor30minandthenevacuatedandsuccessivelytreatedwith8TorrNO2(g)at323Kfor20min(seetextfordetails).
Fig.5,it isclearthat 8Ba/Ti/Al(P1,P2)and 20Ba/Ti/Al(P1) sam-plesnotonlyaccumulate asmalleramountof SOxspecies than
theconventional8(20)Ba/Almaterialsuponsulfurpoisoning,but theyalso significantlydestabilizetheadsorbedSOx species and
facilitatetheireffectivethermalregeneration/removalviasimple annealingat 1023Kwithout anadditional reducing agentsuch asCO,H2 orhydrocarbons.Itis alsoimportant tomentionthat
thethermalregenerationtemperaturethatisusedinthecurrent work (i.e. 1023K) is close to temperatures used in such ther-malSOxremovaltreatmentsinrealisticexhaustemissionsystems
(e.g. 750◦C). It is worth mentioning that the current findings arein verygood agreementwiththerecent transientresponse measurement(TRM)studies[81]performedonnano-structured Pt/BaO/TiO2/Al2O3 NSR catalystsreporting thatTiO2 promotion
facilitates both the SOx removal and the catalyst regeneration
underoperationalconditionswhileenhancingthetotalNOx
stor-agecapacity. Ascanbeseen inFig.5,20Ba/Ti/Al(P2)sample is theonly sample which wasfound tostore a larger amountof SOxincomparisontoitsTiO2-freecounterpart(i.e.20Ba/Al).
How-everthe thermal regeneration ofthis sample (Fig.12b) reveals a slightly better SOx removal behavior than the 20Ba/Al case,
indicatingthepositiveinfluenceofTiO2-promotiononthe
destabi-lizationoftheSOxspecies.Itisworthmentioningthatwehave
alsoattemptedtoquantitativelyanalyzetheremaining amount ofsulfurspeciesafterthethermalregenerationstepviaXPSand EDX.HoweverthesulfursignalsinXPSandEDXafterthe regen-eration step were below the analytical detection limits for all samples.
1000 1100 1200 1300 1400 1500 20BaAl 20BaTiAl P1
absorbance( a.u.)
1362 1308 1241 1164 1127 1037 0.1 1184 1117 1084 1044 1248 1125 1088 1042 20BaTiAl P2 (b) 1000 1100 1200 1300 1400 1500 1216 8BaTiAlP2 8BaTiAlP1 x2 8BaAlwavenumber (cm
-1)
wavenumber (cm
-1)
absorbance( a.u.)
1360 1258 1160 1125 1045 x2 0.1 1307 1380 (a)Fig.12.FTIRspectrademonstratingthethermalregenerationcapabilitiesof(a)8Ba/Al,8Ba/Ti/Al(P1),8Ba/Ti/Al(P2)and(b)20Ba/Al,20Ba/Ti/Al(P1),20Ba/Ti/Al(P2)samples aftersulfurpoisoning.Spectrawereobtainedat323Kinvacuumafterinitialsulfurpoisoningwith0.6TorrSO2(g)+O2(g)(SO2:O2=1:10)at323K,followedbyheatinginthis
gaseousmixtureat473Kfor30minandasubsequentevacuationat323K;followedby8TorrNO2(g)adsorptionat323Kfor20minandafinalevacuationstepinvacuum
at1023K.
4. Conclusions
Inthecurrentwork,wehaveinvestigatedthestructural prop-ertiesandchemicalbehaviorofTiO2-promotedbinaryandternary
mixedoxidesystemsthatareparticularlyrelevanttoNSRcatalytic applications.Asystematic approach wasfollowed in whichthe structuralandchemicalbehavioroftheTi/Al(P1,P2)binaryoxide supportmaterialswereinitiallyanalyzedinacomparative fash-ionwithsimpleconventionalsupportmaterialssuchas␥-Al2O3
andTiO2(anatase).Inthelightoftheseinitialstudies,more
com-plex8(20)Ba/Ti/Al(P1,P2)ternaryoxideNOxstoragematerialswere
investigated.Someoftheimportantfindingsofthecurrentstudies canbesummarizedasfollows:
(a)SurfacestructureandthemorphologyoftheTiO2 Al2O3mixed
oxide systems strongly depend on the synthesis protocols. Ti/Al(P1)systemiscomprisedofrelativelyorderedand inho-mogeneouslydistributedTiO2(anatase)crystalliteson␥-Al2O3
domainswhileTi/Al(P2)systemcontainsanamorphousanda highlyporousTixAlyOzstructure.
(b) SOxadsorptiononalloftheinvestigatedsamplesleadstoa
decreaseintheNOxstoragecapacityduetotheblockingofthe
NOxadsorptionsitesbysulfiteandsulfatespecies.
(c) Ti/Al(P1, P2) systems present a higher SOx storage
capac-ity(per unit sample weight) and a higherthermal stability fortheadsorbedSOx speciesthan thatof both␥-Al2O3 and
TiO2 (anatase)surfaces,whileTi/Al(P2)systemdemonstrates
higher affinity towardsSOx than Ti/Al(P1) system. Thiscan
beexplainedbytherelativelyhigherSSAoftheTi/Al(P1,P2) systems(betterdispersionofTiO2 domainson␥-Al2O3 with
respecttobulkanatase)aswellasthedecreaseinthetotal num-berofLewisacidsitesandthepresenceofnewadsorptionsites duetoTiO2promotion.
(d)Typically, TiO2-promoted NOx storage materials (e.g.
8(20)Ba/Ti/Al(P1)and8Ba/Ti/Al(P2))accumulatelessSOx(per
unit sampleweight) than TiO2-freeconventional 8(20)Ba/Al
samples under identical poisoning conditions. Furthermore the(P1)samplesaccumulatelessSOxthan(P2)sampleswhich
canbeassociatedwithbothlowerSSAofthe(P1)samplesand theirdifferentsurfacemorphology.
(e)TiO2-promoted 8(20)Ba/Ti/Al(P1, P2) NOx storage materials
werefoundtoexhibit superiorthermalregeneration behav-ior after sulfur poisoning in comparison to conventional 8(20)Ba/Almaterials.AdsorbedSOxspecieswereobservedto
besignificantlydestabilizeduponTiO2promotionandthus
cor-respondingsulfateandsulfitespeciescanreadilyberemoved fromthe surfaceby simple annealing in vacuumat 1023K, in theabsence of an additional reducing agent suchas H2,
COorhydrocarbons.Thisbehaviorcanbeattributedto well-dispersedBaOunitsonTiO2domainsandthesuppressionof
theformationofbulkBaSO4clusters.Theseresultssuggestthat
TiO2-promotionmightbeapromisingstrategyforenhancing
thesulfurtoleranceofNSRsystemswhichresultsinnotonlythe suppressionoftheSOxaccumulationonthecatalystsurface,but
alsoimprovementofthethermalregenerationcapabilityofthe sulfur-poisonedcatalystandpreventionofirreversiblesulfur uptakeunderoperationalconditions.
Acknowledgement
Authorsgratefullyacknowledgethefinancialsupportfromthe Scientific and Technical Research Council of Turkey (TUBITAK) (ProjectCode: 108M379). E.O.also acknowledgessupport from TurkishAcademyofSciences(TUBA)forthe“OutstandingYoung Investigator” grant.E.V.,V.Z.and V.B.acknowledgeRFBR (Rus-sia)#09-03-91225-CTаand#10-03-00596-а,forfinancialsupport. AuthorsalsothankMargaritaKantchevaforfruitfuldiscussionsand ErmanBenguforhishelpwiththeXPSexperimentsandTEMdata analysis.