ContentslistsavailableatScienceDirect
Applied
Catalysis
B:
Environmental
j ou rna l h o m e p a g e :w w w . e l s e v i e r . c o m / l o c a t e / a p c a t b
Effect
of
Ti(IV)
loading
on
CH
4
oxidation
activity
and
SO
2
tolerance
of
Pd
catalysts
supported
on
silica
SBA-15
and
HMS
A.M.
Venezia
a,∗,
G.
Di
Carlo
b,
L.F.
Liotta
a,
G.
Pantaleo
a,
M.
Kantcheva
caIstitutoperloStudiodeiMaterialiNanostrutturati(ISMN-CNR),viaUgoLaMalfa,153,PalermoI-90146,Italy
bIstitutoperloStudiodeiMaterialiNanostrutturati(ISMN-CNR),viaSalariakm29300,00015MonterotondoStazione,Rome,Italy cDepartmentofChemistry,BilkentUniversity,06800Bilkent,Ankara,Turkey
a
r
t
i
c
l
e
i
n
f
o
Articlehistory: Received4April2011
Receivedinrevisedform3June2011 Accepted11June2011
Available online 17 June 2011 Keywords: Pdcatalyst CH4oxidation TiO2-SBA-15 TiO2-HMS SO2effect
a
b
s
t
r
a
c
t
PuresilicaSBA-15andHMSandcorrespondingTi(IV)modifiedmesoporoussilica,with5and10wt% ofTiO2,werepreparedandusedassupportforpalladium(1wt%)catalysts.Thematerials,analysedby XPS,XRD,BET,NH3-TPDandFT-IRtechniques,weretestedinthetotaloxidationofmethane.The cat-alyticactivitywasmeasuredinleanconditionsatWHSV=60,000mlg−1h−1intheabsenceandpresence of10vol.ppmSO2.Moreover,theeffectofaprolongedreactionagingandsevereSO2poisoningonthe catalyticperformanceofthebestperformingcatalystwasinvestigated.TheadditionofTiO2improved thecatalyticperformanceoftheSBA-15supportedcatalystsbyincreasingthesulfurtoleranceandmost importantlybyfavoringtheregenerationofthecatalystinsubsequentSO2-freeruns.Anopposite behav-iorwasobservedwiththepalladiumsupportedonTi(IV)-modifiedHMSsupportwhichexhibitedlower activityandasubstantialworseningoftheSO2toleranceascomparedtopalladiumsupportedonpure HMS.Onthebasesofthestructuralandchemicalinvestigation,thedifferencesbetweenthetwoseries ofcatalystswereascribedtothedistinctstructuralandacidicpropertiesofthesupports.Inparticular, thegoodperformanceoftheTi(IV)dopedSBA-15supportedcatalystswasduetothecombinationof Ti(IV)structurallyincorporatedintothesilicalatticeandpresentassurfacedispersedTiO2particles.The negativeeffectoftheTi(IV)overtheHMSsupportedcatalystswasrelatedtothehighacidityinducedby themorehomogeneousincorporationofTi(IV)intothesilicastructure.
© 2011 Elsevier B.V. All rights reserved.
1. Introduction
Natural gas, mainly consisting of methane, is increasingly
replacinggasolineordieselasfuelfortransportationvehicles[1,2].
Thereasonforthischangeisthedeclineofthepetroleumreserves
and theloweremission of pollutantsassociated withthe
com-bustionofmethane.Sincethenaturalgasfuelledvehicles(NGV)
typicallyrunatlowtemperature(320–420◦C)theemissionofNOx
islowerandduetothehighH:CratioalsotheproducedCO2 is
lessascomparedtotheotherfueldrivenvehicles[2].Nevertheless
amajorconcernrelatedtotheuseofnaturalgasistheemission
oftheunburnedmethanewhichhasanevenstrongergreenhouse
effectascomparedtotheCO2[3].Sincemethaneisanalmostinert
molecule,itrequireshightemperatureforitscompleteoxidation.
Acrucialstepintheachievementofthetotalcombustionprocess
istheactivationofthefirstC–Hbond[4,5].Eitherhomolyticbond
cleavagewiththeformationofradicals,orheterolyticC–Hbond
cleavageattheacid–basepairofsitesisgenerallyconsidered.In
anycase,inordertoincreasetheefficiencyofthemethane
com-∗ Correspondingauthor.Tel.:+390916809372;fax:+390916809399. E-mailaddresses:venezia@pa.ismn.cnr.it,anna@pa.ismn.cnr.it(A.M.Venezia).
bustionatlowtemperature(below600◦C)itisnecessarytousea
suitablecatalyst.Forthisspecificreaction,twoclassesofcatalysts
arecurrentlyinvestigated,thosebasedontransitionmetaloxides
assolidsolutionoxides[6,7],perovskites[8,9],hexaaluminate[10],
andthosebasedonnoblemetals[11–14].Amongthislatterclass,
Pd-basedcatalystsarethemostactiveforthemethanetotal
oxi-dationatlowtemperatures.Aspointedoutinseveralstudies,their
catalyticactivitydependsstronglyonthenatureofthesupport[12],
onthepalladiumprecursors[15,16]andonthesizeofthePdO
particles[17].Theirmajordrawbackisrepresentedbytheireasy
poisoningbysulfurderivedfromthegasandenginelubricating
oil[11].Accordingtotheliterature,whenasulfatingsupportlike
Al2O3isused,palladiumdeactivatesslowly,duetothe
preferen-tialinteractionofSOxwiththesupport,atvariancewithpalladium
overtheinertSiO2deactivatingquicklybecauseofthedirect
inter-actionbetweenpalladiumandSOx.Nevertheless,theuseofsilica,
intheabsenceofparticlesintering,allowsaneasierregenerationof
thesulfur-poisonedcatalystthroughthethermaldecompositionof
thepalladiumsulfateoccurringattemperatureabove600◦C[1,11].
Recentstudiesinourgrouphaveshownthatbothmethane
conver-sionactivityandsulfurtolerancecouldbeimprovedsubstantially
by using high surface areasilica with specific characteristic of
acidityand morphology. In particular,supportingpalladium on
0926-3373/$–seefrontmatter © 2011 Elsevier B.V. All rights reserved. doi:10.1016/j.apcatb.2011.06.013
mesoporous silica HMS yielded more efficientand more sulfur
resistantcatalystsascomparedtoalowersurfaceareasilica
sup-portedcatalyst[18].Incorporationofapreciseamount(10wt%)
ofTiO2 duringthesol–gelpreparation ofamorphoussilica
pro-ducedanadditionalimprovementofthesulfurtoleranceduring
themethaneoxidation inthepresenceofSO2,stillallowingthe
completecatalystregenerationtypicalofasilicasupport[19,20].
Thepositive behaviorwasattributedtothecombination ofthe
highsurfaceareasupportandthescavengeractionofthesulfating
oxidelikeTiO2.Withinthisframe,thepresentstudyintendsto
fur-therimprovethecatalyticbehaviorofpalladiumfortheoxidation
ofmethanebyusingtitania-dopedsilicamesoporousmaterialsas
catalystsupports.Tothisaimtwoseriesofpalladiumcatalysts
sup-portedonTi(IV)-modifiedHMSandTi(IV)-modifiedSBA-15were
prepared.Inordertocomparewiththeprevioussol–gelprepared
titaniamodifiedsilica[19],Ti(IV)wasincorporatedusingtheone
stepsynthesisinwhichtitaniumprecursorwasaddedduringthe
preparationofthemesoporousmaterials.Toevaluatetheeffectof
thesupportstructureonthePdactivityandstability,analysesby
XPS,XRD,BET,NH3-TPDandFT-IRtechniqueswereperformed.
2. Experimental
2.1. Supportandcatalystpreparation
ThemesostructuredHMSmaterialwassynthesizedaccording
toapublishedprocedure[21].Basically,HMSwasassembledfrom
4:1molarmixturesoftetraethylorthosilicate(TEOS)(Aldrich)as
theinorganicprecursoranddodecylamine(DDA)(Aldrich)asthe
structure-directingsurfactantin90:10(v/v)water/ethanol.About
49mmolofDDAweredissolvedin50mlofethanoland450mlof
H2O.Tothesurfactantsolution,heatedto60◦C,196mmolofTEOS
wereadded.Thegelmixturewaskeptina closedTeflonvessel
at60◦Cfor20h.Thereactionproductwasfiltered,washedwith
distilledwateranddriedatroomtemperaturefor24h.The
surfac-tantwasremovedbycalcinationinairat500◦Cfor4h.Titanium
containingHMSmaterialsweresynthesizedaccordingtothe
pro-cedurereportedbyTanevetal.[22]usingTi(iso-OC3H7)4(Aldrich)
astitaniumprecursor,andfollowingthesamestepsasabove.The
titaniumprecursor wasaddedin appropriateamounttoyield a
5wt%and10wt%ofTiO2inthefinalmixedoxide.
SBA-15 was synthesized following a procedure described
by Zhao et al. [23]. Accordingly, 8.1g of Pluronic P123
(EO20PO70EO20,Aldrich)wasdissolvedin146.8gdistilledwater
and4.4gof conc.HCl (37%) and stirredover night at35◦C. To
thissolution16gofTEOS(Si(OC2H5)4,Aldrich98%)wasquickly
addedandstirredfor24hat35◦C.Thesuspensionwasannealed
at100◦Cfor24hinclosedpolypropylenebottle.Thesolidproduct
wasfiltered,washedwithwaterandcalcinedat500◦Cfor5hin
air.Similarprocedurewasusedforthesynthesisofthetitanium
containingSBA-15materials.Themaindifferenceconsistedinthe
pre-hydrolysisofTEOSfor5hat35◦Cbeforeaddingappropriate
amountofTi(iso-OC3H7)4 dropbydropundervigorousstirring.
Thetitaniumprecursorwasaddedinappropriateamounttoyield
sampleswith5wt%and10wt%ofTiO2inthefinaloxide.
Attainment of the ordered mesoporous structures was
con-firmed by the SAXS patterns and by the typical type IV N2
adsorption–desorptionisotherms[21,24].
Palladiumwasdepositedbywetimpregnationusingan
aque-oussolutionofpalladiumnitrateintheappropriateamounttoyield
1wt%Pd loadedcatalysts.Thesampleswere calcinedat 500◦C
for4h.Thechemicalcompositionofthesampleswascheckedby
X-rayfluorescenceanalyses.ThesampleswerelabelledPd/HMS,
Pd/TixHMS,Pd/SBA-15andPd/TixSBA-15wherexrepresentedthe
TiO2weightpercentage(wt%).
2.2. Catalystcharacterization
X-raydiffractionpatternsweremeasuredwithaPhilips
verti-calgoniometerusingNi-filteredCuK␣radiation.Aproportional
counterand0.05◦stepsizesin2wereused.Theassignmentofthe
variouscrystallinephaseswasbasedontheJPDSpowder
diffrac-tionfilecards[25].Fromthelinebroadeningofthemainreflection
peaks,usingtheScherrerequation,particlesizesabovethe
detec-tionlimitsof3nmweredetermined[26].
SAXS measurements were performed with BRUKER AXS
NANOSTARwithstepsizesof0.02◦in2.
X-rayfluorescencewasperformedusingtheBrukerS2Ranger
spectrophotometer.
The microstructural properties of thematerials were
deter-minedfromN2adsorption–desorptionisothermsat−196◦Cusing
aSorptomatic1900(CarloErba)instrument.Beforethe
measure-ments,sampleswereheatedinvacuumat250◦Cfor2h.Specific
surfaceareasandporedistributionsofthematerialswereobtained
respectively using the Brunauer–Emmett–Teller (BET) and the
Barret–Joyner–Hatenda(BJH)calculationmethods[24].
TheX-rayphotoelectronspectroscopyanalyseswereperformed
withaVGMicrotechESCA3000Multilab,usingthe
unmonochro-matisedAlK␣source(1486.6eV)runat14kVand15mA.Forthe
individualpeakenergyregions,apassenergyof20eVwasused.
Samplesweremountedwithdouble-sidedadhesivetape.Binding
energieswerereferencedtotheC1sbindingenergyofadventitious
carbonsetat285.1eV.ThesoftwareprovidedbyVGwasusedfor
peakanalysesandforthecalculationoftheatomicconcentrations.
Theprecisiononthebindingenergyandontheatomicpercentage
valueswasrespectively±0.15eVand±10%.
The acidity of the oxide catalysts wasdetermined by
mea-surements oftemperature-programmeddesorptionof ammonia
(NH3-TPD).Thesampleamountof0.1gwasout-gassedina5vol.%
O2/He flow at 500◦C for 1h. This was followed by
ammonia-saturation by flowing 5% NH3/He stream (30ml/min) at room
temperaturefor1h.Afterpurgingwith100ml/minHeflowfor1h
at100◦Candthencoolingdowntoroomtemperature,thecatalyst
washeatedunderHe(30ml/min)inalinearrateof10◦C/minto
950◦Candtheammoniadesorptionwascontinuouslymonitored
bytheTCD.In ordertodeterminethetotalacidityof the
cata-lystfromitsNH3desorptionprofile,theareaunderthecurvewas
integrated.
The type of acidity (Lewis and Brønsted) was investigated
by FT-IR spectroscopy of adsorbed pyridine. The FT-IR spectra
wererecordedusingaBomemHartman&BraunMB-102model
FT-IRspectrometerwith a liquid-nitrogencooled MCTdetector
ata resolution of 4cm−1 (100scans).The self-supportingdiscs
(∼0.013g/cm2)wereactivatedintheIRcellbyheatingfor1hina
vacuumat450◦Candinoxygen(100mbar,passedthroughatrap,
cooledinliquidnitrogen) atthesametemperature,followedby
evacuationfor1hat450◦C.Thepyridine(Sigma–Aldrich)
adsorp-tiontestwascarriedoutbytheadmissionof1.6mbarofthebase
intotheIRcell,leftincontactwiththesamplefor15min.Theexcess
pyridinewasthenevacuatedatroomtemperaturefor15min,
fol-lowedbyadesorptionofthestronglybondedbasefractioninthe
temperaturerange 25–250◦C.Thespectraoftheadsorbed
com-poundswereobtainedbysubtractingthespectraoftheactivated
samplesfromthespectrarecorded.Thesamplespectrawerealso
gas-phasecorrected.
2.3. Catalyticactivity
Methaneoxidation catalytictests wereperformedusinga U
shapedquartzreactorwithaninnerdiameterof12mm,electrically
heatedinafurnace.Thecatalystpowder(sievedfractionbetween
thermalgradients,anditwasplacedonaporousquartzdisk.The
reactiontemperaturewasmeasuredbyaK-typethermocouplein
contactwiththecatalyticbedlong12mm.Priortothecatalytic
testing,thesamplesweretreated“insitu”underflowingO2(5vol.%
inHe,50ml/min)at350◦Cfor0.5handunderHeduringcooling
at200◦C.Thestandardreagentgasmixture,consistingof0.3vol.%
ofCH4+2.4vol.%O2 inHe,wasledoverthecatalyst(50mg)ata
flowrateof50ml/min(STP),equivalenttoaweighthourlyspace
velocity(WHSV)of60,000mlg−1h−1.Activitiesweremeasuredby
increasingthetemperaturefrom200◦Cto600◦C(bystepsof50◦C,
holdtime45min).Theinletandoutletgascompositionswere
anal-ysedbyonlinemassquadrupole(ThermostarTM,Balzers),inorder
tofollowtheevolutionofallthespecies,CH4,CO,CO2,H2,H2O,
O2.Moreover,theconcentrationsofCO,CO2andCH4specieswere
checkedbyIRanalysers(ABBUras14,Uras26),calibratedinthe
range0–3000ppmforCO,0–10,000ppmforCO2and0–30,000ppm
forCH4.ThereactionproductsofmethaneoxidationwereCO2and
H2O.NoCOwasdetectedintheoverallrangeoftemperature.
Car-bonbalancewascloseto±5%inallthecatalytictests.Experiments
ofmethaneoxidationinthepresenceofSO2wereperformedby
co-feeding10vol.ppmofSO2.Betweenconsecutiverunsthesample
wascooleddowninHeatmosphere.
3. Resultsanddiscussion
3.1. Characterization
3.1.1. N2adsorption–desorptionanalyses
TheN2adsorptionanddesorptionisothermsofthepuresilica
supportsandofthetitaniadopedonesareshowninFig.1.The
Fig.1. Nitrogenadsorption–desorptionisothermsofpureandTi(IV)dopedHMS andSBA-15supports.
Table1
TexturalandstructuraldataofpureandTi(IV)-modifiedSBA-15andHMSsupports.
Sample Sa(m2/g) d pb(nm) Vpc(cm3/g) a0d dwe(nm) HMS 824 3.2 0.99 4.6 1.4 Ti5HMS 845 2.5 1.33 4.5 2.0 Ti10HMS 728 2.6 1.00 4.3 1.7 SBA-15 838 7.7 0.99 11.3 3.6 Ti5SBA-15 912 7.1 1.35 11.3 4.2 Ti10SBA 841 7.1 0.96 11.0 3.9
aTheBETsurfaceareavalueswerecalculatedintherange0.05–0.2p/p0. bThemeanporediameterdeterminedusingtheBJHmodelfromN
2
adsorp-tion/desorptionisotherms.
c Theporevolumedeterminedconsideringtherangep/p0from0.1untilto0.98. dUnitcellparametercalculatedasa
0=2d100√3withd100beingtheplanedistance
computedaccordingtotheBragg’slaw(=2dsin).a0correspondstothedistance
betweenthepores.
eThewallthicknesscalculatedasd w=a0−dp.
isotherms areoftype IV,withhysteresisloopscharacteristicof
mesoporouscompounds.AccordingtotheIUPACclassification,the
hysteresisloopsoftheSBA-15andHMScanbeclassifiedasH1and
H3types,respectively[24].Asalreadyreportedinliterature,the
hysteresisloopsoftheSBA-15andTixSBA-15supportsarelarger
andtypicallyofthepresenceofmesopores[27].Incontrast,the
hysteresisloopsofHMSandTixHMSareratherflatandextended
overa largerange ofrelativepressures,indicating thepresence
ofbothframeworkmesoporosityandinterparticlemacroporosity
[27].ThetexturalpropertiesaresummarisedinTable1.TheBET
surfaceareasoftheHMSandSBA-15supportsaresimilarandquite
large.Bothsupportsareslightlyaffectedbythepresenceoftitania.
Asa functionofthetitanialoadingthesurfaceareasdo not
fol-lowanycleartrend,onthecontrary,theporediametersdecrease.
Asexpected,theaverageporediametersoftheSBA-15seriesare
morethandoublethoseoftheHMSseries.
3.1.2. SAXS
The SAXSpatterns of thetwo series of supports are shown
in Fig. 2. The correspondingunit cellparameters (a0), and the
wallthickness(dw)areprovidedinTable1.Theunitcell
param-eterswerecalculatedasa0=2d100√3,assumingahexagonalunit
cellforbothseriesofsupports.Thewallthicknesswasestimated
bysubtractingfroma0 theporediametersobtainedfromtheN2
physisorptionmeasurements.TheSAXScurvesoftheHMS
sam-plesarecharacterizedbyonemainbroadpeak,ataround2≈2◦
correspondingtoaunitcellparametersof≈4.4nmattributedto
abi-dimensionalhexagonalstructure[21].Theinsertionof
tita-niuminHMSresultedinaprogressivelossofthislong-rangeorder
andin aslightdecreaseoftheunitcellparameter.Onthe
con-trarySBA-15exhibitsthreemainreflectionpeaksindexedas(100),
(110)and(200)typicalofamoreorderedmaterial,withaunitcell
parameterof≈11.3nm.Theinsertionoftitaniadoesnotchange
sig-nificantlytheoriginalhexagonalstructurebut,inaccordwiththe
decreasedpeakintensity,slightlycausesadeteriorationofthelong
rangeorder.AsshowninTable1,aslightdecreaseoftheunitcell
parametersisobservedforthetitaniacontainingsupportsand
cor-respondinglyanincreaseoftheframeworkwallthickness,toalarge
extentintheHMSseries.Thiseffectwouldconfirmacertaindegree
oftitaniaincorporationinthestructureofthesilica[28,29].The
Table2
AcidpropertiesofthesupportsasdeterminedbyTPD-NH3intherange50–500◦C.
Sample T(◦C) VNH3(mlg−1)
HMS 114 1.4
Ti10HMS 157 7.8
SBA-15 118 2.0
Fig.2. SAXSCurvesofpureandTi(IV)dopedHMSandSBA-15supports.
subsequentimpregnationofpalladiumleavesunchangedtheSAXS
patterns(notshowninhereforbrevity)ofbothseriesofsupports.
3.1.3. TPD-NH3
Thechange of acidityupon insertion of titania was
investi-gatedbytemperatureprogrammeddesorptionofammonia.The
techniqueprovidedinformationonthetotalacidityofthesolids,
includingbothBrønstedandLewisacidityandaccountingforthe
differentstrengthandnumberofacidsites.TheTPDpatternsofthe
pureandofthe10wt%TiO2dopedmesoporoussilicasareshown
inFig.3.TheresultsaresummarisedinTable2,intermsof
tem-peratureofNH3desorptionandvolumesofdesorbedNH3.Forboth
typesofmesoporousmaterialsonlythefirstpeakwasconsidered.
Indeedtheotherfeature,consistingofabroadpeakobservedonly
inthe SBA-15samples,wasdue to theevolution of water and
organicmaterials,asdetectedbythequadrupolemeasurements,
andthereforenotincludedintheacidityevaluation.Accordingto
thepatternsandtothevalueslistedinTable2,itisevidentthatthe
insertionofTi(IV)inHMScausedasubstantialincreaseofacidity
intermsofboth,strengthandnumberofacidsites.Onthecontrary
theadditionoftitaniuminSBA-15producedonlyalimitedacidity
changes.
3.1.4. XRDanalyses
Inordertoidentifythecrystallinephasespresentinthesamples
theX-raydiffractionanalysesof thesupportedpalladium
cata-lystswereperformed.InFig.4thecorrespondingdiffractograms
areshownalongwiththediffractionlinesofthereferencephases,
anataseTiO2andPdO.TheXRDpatternsshowabroaddiffraction
bandbetween20◦and30◦2attributedtotheamorphouspartof
thesubstrate.CharacteristicPdOpeaksarepresentinthepatterns
Fig.3. TPD-NH3patternsintherange50–500◦Cofthemesoporoussupports.
ofbothseriesofsamples.Theanatasephaseisvisibleinthe
Ti(IV)-dopedSBA-15samples,butnotintheTi(IV)–dopedHMSseries.
Theanatasephasewasalsoobservedinasimilarlyprepared
Ti-SBA-15materialcontaining2.5at%Ti.DRSUV–visspectraofthis
samplepresentedanabsorptionbandaround334nmduetoTi4+
inoctahedralcoordinationtypicaloftheanatase[30].Generally
speaking,preparationof ion-dopedSBA-15bydirect
incorpora-tionduringthesynthesisofthemesoporousoxideisratherdifficult
duetothestrongacidicmedia[31].Indeed,understronglyacidic
conditions(pH<1)free titaniumspeciessuchasTi4+exist only
incationicformandthusarenotabletoentertheframeworkof
SBA-15[32].Thegraftingprocedureusingseveraltypesoftitanium
precursorsallowsinsertingonlyabout6at%oftitaniumrelativeto
siliconintoSBA-15matrix.Highertitanialoadings,8–10at%asin
thepresentcase(usedSi/Tiratiosof25and12),wouldproduce
anatasecrystallites ofTiO2 [33].Inthepresentwork,thedirect
synthesisprocedureadoptedforthepureSBA-15was
intention-allyused,aimingtoinvestigatetheeffectofTiO2eitherformedas
aggregatesandalsoasstructuralmodifier.ByapplyingtheScherrer
equationtothelinewidthofthemainreflectionpeaks,the
diam-etersofthePdOandTiO2 particlesinthedifferentsampleswere
estimated.ThecorrespondingcalculatedvaluesarelistedinTable3.
TiO2particlesizeof8nmwereobtainedfortheSBA-15supported
catalysts,whereasPdOparticlesizesof6–7nmwereobtainedfor
allthesamples,includedalsotheHMSsupportedones.
3.1.5. XPSanalyses
Informationonthe chemical stateand the surface chemical
compositionofthepalladiumsamples,beforethecatalytictests,
Fig.4.XRDpatternsofSBA-15andHMSsupportedpalladiumcatalystswithand withoutTi(IV).ThepatternsofpureanataseTiO2andPdOoxidesareshownas
references.
Table3
XRDderivedPdOandTiO2particlediametersinthefreshsamples.
Sample dPdO(nm) dTiO2(nm)
Pd/SBA-15 6 – Pd/Ti5SBA-15 6 8 Pd/Ti10SBA-15 7 8 Pd/HMS 7 – Pd/Ti5HMS 6 n.d.a Pd/Ti10HMS 6 n.d.a an.d.=notdetectable.
2p3/2andtheO1sbindingenergiesarecompiledalongwiththe
XPS-derivedatomicratiosTi/SiandPd/(Ti+Si).Thepalladium3d
photoelectronspectraarecharacterizedbythePd3d5/2binding
energyof337.2eV±0.2eV.ThevalueistypicalofPd4+asinPdO
2.
Fig.5. Ti2pphotoelectronspectraofPdcatalystssupportedon10wt%TiO2doped
mesoporoussilicas.
Thisoxidehasbeenalreadyreportedforsimilarsamples[19,34].
Itsformationmaybeattainedbyoxygenincorporation intothe
PdOcrystallatticeduringcalcination[34].TheTi2pspectraofthe
10wt%Ti(IV)dopedcatalystsareshowninFig.5.Theyare
char-acterizedbythetwospin-orbitcomponents,Ti2p3/2andTi2p1/2,
5.7eVapart.Thethirdcomponentat≈462.5eV±0.5eVincluded
inthefittedspectraisattributabletoacontributionfromtheO1s
lineexcitedbytheAlKlineofthenon-monochromatized
radi-ation(h=69.7eV)[31].ThebindingenergyoftheTi2p3/2 in
thepureTiO2oxidesis458.9eVtypicalofaTi4+species[30,35].In
accordwithapreviousstudy[19],largervaluesofTi2p3/2binding
energyareobservedforthetitaniaincorporatedsilicas.The
chem-icalshifts,withrespecttothepureTiO2value,rangefrom1.6eVin
theHMSseriesto0.5eVfortheSBA-15series.Twocontributions
mayberesponsibleforsuchsignificantshift,a“finalstate”andan
“initialstateeffect”.Astotheformereffect,itgenerallyaccountsfor
theTi2p3/2chemicalshiftwhenmovingfromPd/TixSitoPd/TiO2
[36]. It originatesfrom theextraatomic relaxationenergy [37]
whichisrelatedtothepolarizabilityoftheoxidecarrier.Theless
mobiletheelectronsare,asinSiO2,thesmalleristherelaxation
energyandthereforethelargeristhemeasuredbindingenergyof
thephotoelectrons.Thiseffect,relatedtotheelectricalpropertyof
thematerial,wouldproduceanalogousshiftinthetwotypesof
mesoporoussilicasupportedsamples,thereforeitcouldaccount
forpartofthetotalshift.Thesecondeffect,socalled“initialstate”
effect,discussedalreadyforaseriesofTiO2-graftedSiO2[35,38]and
responsibleforalargeshiftbetweenthetwoseriesofsamples,may
Table4
XPSbindingenergiesandXPS-derivedatomicratiosofthefreshcatalysts.
Sample Pd3d5/2(eV) Ti2p3/2(eV) O1sa(eV) Ti/Sib Pd/(Ti+Si)
Pd/HMS 337.4 533.6 0.02 Pd/Ti5HMS 337.3 460.5 533.4(97%) 0.02 (0.04) 0.02 530.6(3%) Pd/Ti10HMS 337.4 460.3 533.4(94%) 0.04 (0.08) 0.02 530.9(6%) Pd/SBA 337.2 533.4 0.02 Pd/Ti5SBA-15 337.0 459.3 533.5(90%) 0.06(0.04) 0.02 530.6(10%) Pd/Ti10SBA-15 337.0 459.4 533.5(85%) 0.08 (0.08) 0.02 530.8(15%)
aThevaluesinparenthesesrepresenttheatomicpercentagesoftheoxygenchemicalcomponents. bThevaluesinparenthesesrepresentthenominalatomicratios.
Fig.6. O1sphotoelectronspectraofPdcatalystssupportedon10wt%TiO2doped
mesoporoussilicas.
reflecttheoccurrenceintheTi(IV)-dopedsamplesofanintimate
associationofTiO2andSiO2,producingTi–O–SibondswhereTi4+
occupiestetrahedralcoordinationsitessimilartoSiinSiO2 [39].
Sincetitaniumismoreelectropositivethansilicon,theincreaseof
thepositivechargeonthetitaniumcenterofaTi–O–Sibondas
com-paredtoTi–O–Ti,woulddetermineanincreaseoftheTi2pbinding
energy.ThelargershiftobservedintheHMSderivedsamplesisin
accordwiththeXRDresults,suggestingabettertitaniadispersion
inthesesamplesascomparedtotheSBA-15samples.TheO1score
levelspectraofthemixedoxidesupportedcatalystsareshownin
Fig.6andthecorrespondingbindingenergiesarelistedinTable4.
TheO1sspectrawerefittedwithtwocomponents,ahighbinding
energyoneat≈533.5eV±0.1eVassignedtoSiO2andalow
bind-ingenergyfeatureat530.7eV±0.2eVclosertothevaluereported
forTiO2[39].Itisworthnoticingthattherelativeintensityofthe
lowenergypeakwithrespecttothehighenergypeakis
signifi-cantlyhigherinthePdTi10SBA-15ascomparedtothePdTi10HMS.
Thisdifferencereflectslargersurfaceamountofoxygen
interact-ingwithtitaniumandthereforelargeramountofsegregatedTiO2
atthesurfaceofthePdTi10SBA-15sample.AsshowninTable4,the
experimentalTi/Siatomicratioincreaseswithincreasingloadings
ofTiO2,asexpectedfromthenominalratiosgiveninparentheses.
Itisworthnoticingthelargervaluesofthisratioobtainedforthe
titaniadopedSBA-15samplesascomparedtothecorresponding
titaniadopedHMSsamples.Inaccordwiththeoxygenresults,this
againindicatesapreferentialsurfacesegregationoftitaniuminthe
SBA-15supportedcatalysts.ThePd/(Ti+Si)atomicratioslistedin
Table4arethesameforallsamplesand,aspredictablebecause
oftheadoptedimpregnationprocedure,theyarelargerthanthe
theoreticalvalueof∼0.006.
3.1.6. FT-IR
InFig.7theFT-IRspectraintheOHstretchingregionofthe
activatedHMSandSBA-15samplesarecomparedwiththespectra
of Pd-free and Pd-loaded 10% titania-doped mesoporous
com-posites.ThespectraofHMS andSBA-15exhibitasharpbandat
3744cm−1,assigned toisolated Si–OHspecies[40]. Thedoping
ofHMSwith10wt%TiO2 resultsina shiftoftheOHstretching
vibrationtowardlowerwavenumbersandappearanceofadistinct
shoulderatapproximately3690cm−1.Thedepositionofpalladium
causesdisappearanceoftheabsorptionsat3734and3690cm−1
and regeneration of thesignal at 3744cm−1. This leads tothe
conclusionthattheformertwobandscanbeascribedtotitanol
groupsthatserveasanchoringsitesofthepalladiumspecies.The
Fig.7.FT-IRspectraofthesamplesintheOHstretchingregion.
Pd-freeand Pd-loadedTi10SBA-15 sample spectradisplay very
strongabsorptionintheOHstretchingregionandtheintensities
ofthecorrespondingbandsareoff-scale.Thisindicatesthatthe
OHgroupsinducedbythemodificationofSBA-15withtitaniaare
Fig.8. (a)FT-IRspectrainthe1700–1400cm−1 regionoftheTi10HMSsample
recordedafteradsorptionofpyat25◦Candsubsequentdesorptionatvarious
tem-peratures.(L,Lewisacidity;B,Brønstedacidity;andH,hydrogenbondedpy)(b) FT-IRspectrainthe1700–1400cm−1regionofTi10SBA-15samplerecordedafter adsorptionofpyat25◦Candsubsequentdesorptionatvarioustemperatures.(L,
Fig.9.(a)FT-IRspectrainthe1700–1400cm−1regionofthePd/Ti10HMSsample
recordedafteradsorptionofpyat25◦Candsubsequentdesorptionatvarious tem-peratures.(L,Lewisacidity;B,Brønstedacidity;andH,hydrogenbondedpy)(b) FT-IRspectrainthe1700–1400cm−1regionofthePd/Ti10SBA-15samplerecorded
afteradsorptionofpyat25◦Candsubsequentdesorptionatvarioustemperatures.
(L,Lewisacidity;B,Brønstedacidity;andH,hydrogenbondedpy.)
associatedwiththeTiO2 phase whichis inagreementwiththe
XRDandXPSresultsshowinganatasecrystallitesatthesurfaceof
SBA-15.Theshoulderat∼3715cm−1,visibleinthespectraofboth
Ti-containingsupportsisassignedtoterminalTi–OHgroups[41].
Thebroadbandat∼3560cm−1inthespectraofTi10SBA-15and
Pd/Ti10SBA-15samplesisattributedtoH-bondedsilanol/titanol
groups[40].ThisabsorptionisabsentinthespectraofTi10HMS
andPd/Ti10HMSsamples.Thediscrepancyisprobablyrelatedto
somestructuraldifferencesbetweenthetwomesoporoussilicas.
In ordertodiscriminate theBrønstedand theLewis acidity,
theadsorptionofpyridine(py)hasbeenstudiedovertheTi-free
andTi-containingsupports,andforthePdcatalysts.Thespectra
obtaineduponroom-temperatureadsorptionofthebasefollowed
byevacuationatvarioustemperaturesareshowninFigs.8and9for
theTi-dopedsupportsandforthePdcatalystsrespectively.Allthe
spectraincludingthoseoftheTi-freesupports(notshowninhere)
exhibitedbandsat1598and1446cm−1duetonon-acidicsilanols
andcorrespondingtopymoleculesweaklyperturbedbyH-bonding
withthesurfaceOH-groups[29,42–44].Inaddition,aweak
absorp-tionat1626cm−1frompyridiniumiononacidicBrønstedsiteswas
observedalsoinbothTi-freesupports[28,42–44].However,the
protonatedbasewasweaklyboundand disappearedduringthe
evacuationat100◦C.ThedopingoftheHMSandSBA-15supports
bytitaniacaused significantchangesin thespectraofadsorbed
py.AsshowninFig.8,thebandsat1603and1462cm−1present
onlyintheTi-dopedsamplesareattributedtothe8aand19b
ringvibrations,respectively,ofpymoleculescoordinatedtostrong
Lewisacidsites,whilethebandat1584cm−1revealsthepresence
ofweakLewisacidsites[28,42–44].Byevacuationatdifferent
tem-peratures,theintensitiesofthebandsofpycoordinatedtoLewis
acidsites decreasesconsiderably. Smallamount of coordinated
pyremainsafterdegassingat250◦Candpressureof∼10−3mbar.
Thisindicatesthatthesamplesarecharacterizedbyamoderate
Lewisacidity.ThespectraoftheTi10HMStakenbetween50and
250◦C(Fig.8a)containasplitbroadbandwithmaximaat1648
and1628cm−1whichisattributedtothe8aand8bvibrations
of protonatedpy indicatingthe presenceof Brønstedacidsites
[28,42–44].Itshouldbenotedthatthebandataround1540cm−1
thatcorrespondstothe19bvibrationofpyadsorbedonBrønsted
acidsitesisnotobserved.Thereasonforthiscouldbethelow
con-centrationofsurfacehydroxylswithacidicprotons.However,the
absorptionsat1648and1628cm−1areclearlyvisibleinallofthe
spectratakeninthe50–200◦Ctemperaturerangewhichconfirm
thepresenceofcertainamountofweakBrønsted acidityin the
Ti10HMSsample.Pyridiniumionvibrationsat1646and1628cm−1
arenotobservedintheTi10SBA-15sample(Fig.8b)indicatingthe
absenceofBrønstedacidity.Thereforeforthismaterial,theband
at1476cm−1 (whichcanbeassignedtopycoordinatedtoboth
BrønstedandLewisacidsites)isrelatedonlytoLewisacidsites.
Severalmodelshavebeenproposedtoexplaintheappearanceof
acidsitesinamixedoxide.Themostacceptedoneisthemodel
byTanabeassumingthattheextrachargegeneratedbyintimately
mixingtwooxidesproducesacidicsitesofBrønstedorLewis
char-acterdependingonthesignofthischarge[45,46].Negativecharge,
balanced by association withprotons, generatesBrønsted sites
whereaspositivechargegeneratesLewissites.Applyingthismodel
tothecaseofthemixedtitaniaandsilicaoxideintheexcessofsilica,
followingtherulesofthemodel,thechargeexcessatthetitanium
cationwouldbenegative,thereforeproducingBrønstedacidsites.
Theeffectivenessofthemodelimpliesarelationshipbetweenthe
molecularhomogeneityandtheacidsitedensity.Then,the
pres-enceofBrønstedacidsitesontheHMSsamplesmayreflectabetter
Si/Tistructuralhomogeneity.Theresultwouldbeinaccordwith
theabsenceofanatasephaseintheXRDpatternsandalsowiththe
largerTi2pchemicalshiftandthelowerintensityofthelowenergy
O1scomponentobservedintheXPspectraoftheHMSsamples.
ThespectraofpyridineadsorbedonthePdpromotedsamples
aregiveninFig.9.ThecomparisonwiththespectraofFig.8
indi-catesthattheincorporationofpalladiumintothesupportslowers
theamountofLewisacidsites,especially inthePd/Ti10SBA-15
sample. Moreover,theabsorptionbandin the1675–1620cm−1
rangeofthespectrumofthePd/Ti10HMScatalyst(Fig.9a),assigned
topyridinecoordinatedtoBrønstedacidsites,becomesbroaderand
strongerthanthatofthesupport.Thissuggeststhatthepromotion
ofTi10HMSwithPdgeneratesadditionalBrønstedacidityandas
aresult,thetotalsurfaceacidityofthePd-containingTi10HMSis
higherthanthatofthePd-freesample.
In order to get preliminarymechanistic information on the
oxidation of methane and look for the formation of
interme-diate species, in situ FT-IR experiments were performed. The
spectra of the palladium catalysts, during 15min of exposure
to a gas mixture containing 15mbar CH4 and 85mbar O2 at
the various temperatures, were collected. The spectra for the
Pd/Ti10HMS andPd/Ti10SBA-15are shown inFig.10.The
pos-itiveabsorptioninthe3690–2700cm−1 rangeindicatesthatthe
amountofH-bondedhydroxylshasincreasedasaresultofwater
formation. The bands at 1635–1627 and 1534–1545cm−1 are
attributedtoadsorbedcarbonatespeciesmostlikelycoordinated
toTisites[15,43]whicharetheintermediatesforproducingCO2.
Inspiteoftheclosesimilaritybetweenthespectraofthetwo
sam-ples,itisworthnoticingthelargerintensityofthepeaksrelated
Fig.10.FT-IRspectrarecordedduringtheexposureofthePd/10Ti-HMSandPd/10Ti-SBA-15catalyststoamixtureof15mbarCH4+85mbarO2atvarioustemperatures.
spectrumofPd/Ti10HMSsampleascomparedtothesamepeaks
inthespectrum of Pd/Ti10SBA-15sample.No otheradsorption
speciesrelatedtotheactivatedmethaneweredetected.The
pres-enceofadsorbedformatespecies(HCOO−),withtypicalbandsat
3000–2700cm−1(C–Handcombinationsoffundamental
frequen-cies)and at1600–1550cm−1 (as C–O),as intermediatesofthe
reaction,couldnotbeexcluded[15,47].Thegasphasespectra(not
shownhere) indicatedformation ofCO2 withpeak observedat
2350cm−1.
3.2. CatalyticactivitywithSO2-freeandSO2-containingreactant
mixtures
Inordertocomparethecatalyticperformanceofthecatalysts,
T50values(correspondingtotemperaturesof50%CH4conversion)
offirstandsecondrunsperformedsequentiallyusingdifferent
con-ditionsarelistedinTable5alongwiththeArrheniusparameters.
Firstcyclesonthefreshsampleswereperformedwithpure
reac-tantmixtureandwithSO2containingmixture.Then,inorderto
checkforthermal instabilityand for possibleresidual
contami-nanteffects,secondrunswereperformedonsamplesagedupon
exposuretothepurereactantmixturefor16hat600◦C.Likewise,
aimingtorecoverthecatalystactivityafterthefirstruninthe
pres-enceofthepoisoningSO2,asecondcyclewasperformedusingSO2
–freereagents.
ByinspectionofTable5,judging fromthevalues oftheT50,
thefreshPd/HMSappearsslightlymoreactiveascomparedtothe
Pd/SBA-15.Quiteinterestingthelongexposuretothereactantsat
600◦C,withsomeexceptions,determinesanoveralldecreaseof
theT50valueswhichcouldbeattributedtotheremovalofsome
residualorganicprecursors.Asexpectedandinaccordwith
pre-viousresultsobtainedwithpalladiumsupportedonamorphous
titaniamodifiedsilica[19],thepresenceof10ppmofSO2 inthe
reactantmixturedeactivatesthecatalystsbycausingasubstantial
increaseoftheT50withrespecttothecycleswithoutSO2.Within
thesedataitisworthnotingthedifferentbehaviorofthecatalysts
supportedonsilicaHMSandsilicaSBA-15.Theeffectofthesupport
modificationbytitaniaappearstobestronglyrelatedtothetype
ofthesupport.InthecaseofSBA-15,anincreaseoftitanium
con-centrationimprovestheactivity(lowerT50).Onthecontrary,inthe
caseoftheHMScatalyststheadditionoftitaniuminthesupportis
detrimentalsinceitproducesanincreaseoftheT50.Onepossible
explanationforthesurprisingbehavioroftheHMScatalystcould
bethestrongsupportaciditywhichhindersthepreferential
reac-tionoftheSOxwiththesupport,beneficialforthepalladiumactive
sites.ConsideringthesecondcycleaftertheSO2exposure,the
activ-ityimprovesinallthesamples,asalreadyreportedforpalladium
catalystssupportedonhighsurfaceareasilica[18,19].Theeffect
oftitaniaonthecatalyticperformanceisshowninFigs.11and12,
whereselectedplotsofmethaneconversionasafunctionof
tem-peraturearegivenrespectivelyfortheHMSandtheSBA-15series
ofsupportedPdcatalysts.Thecurvesrefertoafirstcyclewiththe
SO2inthereactantmixtureandtothesubsequentcyclewiththe
SO2freereactantmixture.
Inordertogetinformationontheactivesitevariation,dueto
theoxideTiO2and/ortotheSO2poisoning,theapparentactivation
energiesweredeterminedforthedifferentcatalyticruns.
Neglect-ingtheeffectofsmallamountsofwaterformedintheprocess,the
integralequationofafirstorderreactionwithrespecttomethane
andpseudo-zeroorderwithrespecttooxygenwasusedforthe
calculationof thereaction rateconstants k [18,48].Then, from
Fig.11.MethaneconversionasafunctionoftemperatureoverHMSandTi(IV) promotedHMSPdcatalystsfordifferentcyclesindifferentconditions.
Table5
ValuesofT50(◦C)andArrheniusparametersa,activationenergy(Eact)andpreexponentialfactorA(s−1)ofthecatalysts,forthedifferentreactioncycles.
Sample 1stcycle 2ndcycleafter16hat600◦C 1stcyclewithSO2 2ndcycle
T50(◦C) Eact(kJ/mol) lnA T50(◦C) Eact(kJ/mol) lnA T50(◦C) Eact(kJ/mol) lnA T50(◦C) Eact(kJ/mol) lnA
Pd/SBA-15 341 77 17 346 71 16 405 125 25 395 85 18
Pd/Ti5SBA-15 302 78 19 308 73 17 383 90 19 325 77 18
Pd/Ti10SBA-15 304 76 20 282 67 21 334 79 18 292 75 18
PdHMS 322 79 18 289 76 18 382 120 24 359 81 18
Pd/Ti5HMS 344 97 21 334 69 16 407 85 18 375 72 16
PdTi10HMSb n.a. n.a. 422 81 16 383 73 14
aE
actandAarecalculatedfromtheArrheniusplotinthetemperaturerange250–350◦C. bn.a.indicatesthatthetestsforthissamplewerenotperformed.
theArrheniusplotofln(k)versus1/T,inthetemperaturerangeof
250–350◦Ccorrespondingtoconversionsrangingbetween10%and
80%,theactivationenergiesEactandthepre-exponentialfactorsA
oftheArrheniusequation,k=Aexp(−Eact/RT),werecalculatedand
listedalsoinTable5.Withsomeexceptions,thevaluesofthe
activa-tionenergiesarebetween70and85kJ/mol,whichareclosetothose
reportedpreviouslyforsimilarcatalystsforthesametemperature
range[19].Acarefulinspectionofthetablegivesinterestinghints
aboutthestructuralchangesuponthechemicalreactions.Although
mostofthevariationsarewithintheexperimentalerror(±10%),
somesystematicchangesareenvisagedwhichcanberelatedto
structuralmodificationduetothereaction.Afterathermal
treat-mentat600◦Cfor16h,alowervalueoftheactivationenergyis
observed,correspondinginsomecasestoanenhancementofthe
activity(lowerT50).Asreportedbefore,thepresenceofSO2inthe
reactantmixturecausesanincreaseoftheactivationenergy,quite
remarkableinthesampleswithoutTiO2inthesupport[18].Then,
forallthesamples,thesubsequentcycleaftertheSO2exposureis
characterizedbyloweractivationenergyandbyapartialrecovery
oftheactivity.Theactivityiscompletelyregainedinthecaseofthe
TipromotedSBAsupportedcatalysts,butonlypartiallyrecovered
inthepureSBA-15,HMSandTi-dopedHMSsupportedcatalysts.
Theincreaseoftheactivationenergyduringtheruninthe
pres-enceofSO2confirmedtheearlierideathatsulfurdeactivationwas
relatedtotheformationofacompositespeciesofloweractivity,
likePdO–SO3,quitelabileandeasilydecomposingattemperature
≥450◦C[18,19].
3.3. Stability,deactivationandstructuralchangesof
Pd/Ti10SBA-15
Themostinterestingsample,thePdTi10SBA-15exhibitingthe
lowestT50duringthecyclewithSO2andduringthesecondcycles,
Fig.12.MethaneconversionasafunctionoftemperatureoverSBA-15andTi(IV) promotedSBA-15Pdcatalystsfordifferentcyclesindifferentconditions.
Fig.13.CH4conversionasafunctionoftemperatureoverPd/Ti10SBA-15for
differ-entcyclesindifferentconditions.
wasselectedforaseriesofconsecutivecyclesinordertotestits
stability, deactivationand activityrecovery.Particularly, aftera
firstcyclewiththeSO2 containingreagentsand asecondcycle
withSO2-freereagents,thesampleunderwentanovernight
treat-mentinflowing10vol.ppmofSO2inHeat350◦Cataflowrateof
50ml/min.Afterthistreatmentthreemorecycleswiththepure
reagentswere performed.Alltherelated conversioncurvesare
given in Fig.13including alsothetwo curves (I cycleSO2 and
IIcycle)givenalreadyinFig.2.Thecorrespondingvalues ofT50
and Arrheniusparametersare listedinTable6. Forthesake of
claritysomeofthevaluesareduplicatedfromTable5.A
remark-ableincreaseoftheT50isobservedafterthenighttreatmentwith
SO2.Atthesametime,anincreaseoftheactivationenergyupto
114kJ/molisobtained.Inthefollowing4thand5thcycles,the
activ-ityiscompletelyrecovered.Itisremarkablethatthefinalvalues
oftheactivationenergies(95–94kJ/mol),althoughdecreasedwith
respecttothevalueobtainedaftertheseveredeactivation,donot
reachthelowestvalueof67kJ/molobtainedforthesecondcycle.
Thesignificantdifference,wellabovetheexperimentalerror,could
reflectsomestructuralchangesoftheactivesiteand,aslongasthe
Table6
ValuesofT50 (◦C)andArrheniusparametersa,activationenergy(Eact)and
pre-exponentialfactorA(s−1)ofthePd/Ti10SBA-15catalystforthedifferentreaction
cycles.
Reactioncycle T50(◦C)Eact(kJ/mol)lnA
1stcycle 304 76 20
2ndcycleafter16hexposuretothereactionmixtureat600◦282C 67 21
1stCycleSO2 334 79 18
2ndcycleSO2-free 292 75 18
3rdcycleafterovernightSO2treat. 375 114 23
4thcycle 287 95 22
5thcycle 286 94 22
aE
act andAarecalculatedfromtheArrheniusplotinthetemperaturerange 250–350◦C.
Table7
XRDderivedPdOandTiO2particlediametersandXPPd3d5/2bindingenergyandTi/SiandPd/(Ti+Si)atomicratiosinspentcatalysts.
Sample dPdO(nm) dTiO2(nm) Pd3d5/2(eV) Ti/Si Pd/(Ti+Si)
PdTi10SBA-15after5thcycleincludingSO2nighttreat. 18 7 337.0 0.08 0.005
PdTi10SBA-15after4daysreactionat600◦C 16 8 337.3 0.07 0.005
finalactivityisconcerned,iswellcompensatedbyanincreaseof
thepre-exponentialfactor.Onthesamesamplebutona
differ-entbatchastabilitytestwasperformedbyrunningacatalytictest
afterexposingthesampletothepurereagentmixturefor4days
at600◦C.Asrevealedbytheconversioncurve(notgiveninhere),
matchingexactlythecurveofthesecondcycle,(Table6secondrow
data)nochangeinthecatalyticperformanceoccurred.
Inordertocheckforstructuralmodification,thetwoaged
sam-pleswereanalysedbySAXS,XRDandXPStechniques.According
totheSAXSpatterns(notshownhere) theSBA-15mesoporous
structureoftheagedcatalystswasmaintained.TheXRDpatterns
ofthefreshsampleandthecorrespondingpatternsofthe
sam-pleafter5cyclesincludingtheSO2overnighttreatment(referto
Table6)andthesampleafterthelongrunof4daysat600◦Care
comparedinFig.14.ThepatternscontaintheTiO2anatasepeaks
andthePdOrelatedpeaks.ThecalculatedTiO2andPdOparticles
sizearegiveninTable7.ItisworthnoticingthatwhereastheTiO2
particlesmaintainthesamesize,thePdOparticlesizedrastically
increasesafterthelongrunwiththepurereagentmixturesand
alsoafterfivecyclesincludingtheovernightexposuretotheSO2at
350◦C.TheincreaseofthePdOparticlesizeuponsimilarsequence
ofreactioncycleswasalsoobservedrecentlywithapalladium
cat-alystsupportedonamorphousTi10SiO2[20].Itshouldbepointed
outthattheXRDtechniqueidentifiesthelargerparticles,whereas
smallparticlesizes,belowthelimitof3nm,arenotdetected.Then,
inordertoultimatelyconfirmthedecreaseofpalladium
disper-sion,XPSanalysesofthesamples,afterseveralcyclesincluding
theovernightSO2exposureandafterthestabilitytests,were
per-formed.TheXPSresultsofthespentsamplesarelistedinTable7.
Ascomparedtothecorrespondingvaluesofthefreshsample,as
giveninTable4,nosignificantchangesinthepalladiumbinding
energyand intheTi/Siatomic ratioareobserved.Howeverthe
smallervaluesofthePd/(Ti+Si)atomicratiosascomparedtothe
freshsampleareinaccordwiththeenlargementofthePdO
par-ticlesizerevealedbytheXRD.Itisworthnoticingthatinspiteof
thisseriouspalladiumsinteringthecatalyticactivityofthe
cata-lystwasmaintained.Arecentstudyonpalladiumsupportedon
silicaSBA-15,modifiedbyceriaandbyzirconia,reportedaloss
ofactivity, upon a severedeactivation test, for catalysts
show-Fig.14.XRDpatternsofPdTi10SBA-15catalystasfresh,after5thcycleincluding overnightSO2treatmentat350◦Candafterfourdaysofcatalyticreactionat600◦C
(longrun).
inggoodPdOparticlestability[13].Theconclusionofthework
wasthatthelossofcatalystactivityduringreactionwasnot
nec-essarilyrelated tothesinteringof theactivesitesbutratherto
thevariationoftheoxygenstoragecapacityandoxygenmobility
strictlyrelatedtothesupportproperties.It isacceptedthat
Pd-catalysedcombustionofmethaneoccursthrougharedoxorMars
vanKrevelenmechanism[17,49].Accordingly,duringthisreaction
PdOislocallyreducedtoPdbymethane,producingH2OandCO2,
andthenPdisreoxidisedbyoxygen.Althoughtheactivespecies
isconsideredPdO,itiswidelyrecognizedthatmetallicPdplays
theimportantrole in decomposingandactivatingthemethane
molecule[3,15,50].Therefore,theefficiencyoftheallprocessis
relatedtotheredoxpropertiesofthecatalystandtotheoxygen
mobility[17].Inthepresentcase,themaintenanceofthe
activ-ity,inspiteofthesignificantpalladiumoxidesintering,couldbe
attributedtothegoodinteractionbetweensurfacetitaniaand
sil-ica.Such interaction,asreportedin previouspapers,favorsthe
formationof Ti–O–Silinkageswithanincrease oftheoxidizing
potentialoftheTi(IV)cations[38,51].Theincreaseofthispotential
wouldenhancetheoxygenmobilityattheinterfacebetweenthe
Ti–O–Siunitsandthepalladiumparticles[38,49].Onthisaccount,
thestabilityofthePd/Ti10SBA-15catalyst,observedafteralong
lasting reactionat 600◦C and afterseveralcyclesincludingthe
overnightSO2 exposure,islikelyrelatedtotheoxygenmobility
whichallowsthereoxidationofthePdtoPdO.Inthepresenceof
asupportmetal—interaction,theincreaseofthePdOparticlesize
afterthelongreactionisnotdetrimental.Indeed,aninverseparticle
sizestructuresensitivityofthepalladiumcatalysedmethane
com-bustionwasclaimed,relatedtothehighstabilityofthesmallPdO
particlesinteractingwiththesupportandnotbeingeasilyreduced
[13,50].
4. Conclusion
Theeffectoftheadditionoftitaniatodifferentmesoporoussilica
oxidesonthemethaneoxidationactivityofsupportedpalladium
wasfoundtodependonthetypeofmesostructuredmaterial.The
additionof10wt%ofTiO2tothesilicaSBA-15,improvedthe
cat-alyticperformanceofthesupportedpalladiumcatalysts,intermsof
betteractivityandbettersulfurtoleranceascomparedtopalladium
overpureSBA-15support.Thisresultconfirmedthepositiveeffect
playedbytitania,actingasSO2scavenger,onPdcatalystssupported
onamorphoussilica[19].Oppositebehaviorwasobservedwiththe
HMSsamples.InthiscaseadditionofTiO2producedpoorer
cata-lystsintermsofloweractivityandlowerSO2tolerance.According
tothestructuralandmorphologicalanalyses,thetwoseriesof
cat-alystshadsimilarpalladiumdispersionandsimilarsurfaceareabut
differentTiO2distribution.InthecaseoftheHMS,Ti(IV)ionswere
homogeneouslydistributedintothesilicaframework,whereasa
mixtureofframeworkTi(IV)andsurfacesegregatedTiO2anatase
particleswaspresentintheSBA-15.Duetothemoreuniform
dis-tributionofTi(IV)intothesilicamatrix,asubstantialincreaseof
thetotalacidity,inparticularoftheBrønstedtype,developedin
theTixHMSsupportascomparedtotheSBA-15.Moreover,through
theinsituFT-IR,moreadsorbedwaterandcarbonatespecieswere
observedonthePd/Ti10HMSascomparedtothePd/Ti10SBA-15.
Onthebasesoftheseevidences,theformationofastrongeracidity
andthepresenceofBrønstedsiteswereresponsibleforthe
HMSsupportedPdcatalysts.Indeed,thestrongerwateradsorption
overtheacidicsupportwouldinhibitthecatalyticmethane
oxida-tionfavoringformationofthelessactivePd(OH)2andalsoblocking
theactive sites through surface diffusion.The large amountof
adsorbedcarbonatespecies,detectedinthePd/Ti10HMScatalyst
bytheinsituFTIRanalysesat350◦C,couldhavealsocontributed
to the deactivation of the catalysts. Furthermore, the creation
ofthestrongeracidity,byhinderingthepreferentialreactionof
theSOx withthesupport,nullified thescavenger action ofthe
titania.
Acknowledgements
This research hasbeen performed in theframework of the
D36/003/06COSTprogramandaNATOgrantESP.CLG.No.984160.
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