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Eprints ID : 14529
To link to this article : DOI : 10.1016/j.apcatb.2015.07.019
URL :
http://dx.doi.org/10.1016/j.apcatb.2015.07.019
To cite this version : Faure, Benjamin and Alphonse, Pierre
Co–Mn-oxide spinel catalysts for CO and propane oxidation at mild
temperature. (2016) Applied Catalysis B: Environmental, vol. 180. pp.
715-725. ISSN 0926-3373
Any correspondance concerning this service should be sent to the repository
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Co–Mn-oxide
spinel
catalysts
for
CO
and
propane
oxidation
at
mild
temperature
Benjamin
Faure
faure.benjamin.n@gmail.com,
Pierre
Alphonse
∗CIRIMAT-UPS,UniversitédeToulouse,118routedeNarbonne31062Toulousecedex09,France
Keywords: Mixedoxalate Cobaltitespinel Totaloxidation Propane VOCsremoval
a
b
s
t
r
a
c
t
CoxMn3−xO4oxides(0≤x≤3)werepreparedbycontrolleddecompositionofmixedoxalatesnear200◦C,
followedbyacalcinationat300◦C.Theseoxidesareamorphousforx<0.9.Forhighercobaltfractionthey
haveacubicspinelstructureandtheircrystallitesizegrowswiththecobaltfraction.Thesematerials havealargesurfacearea;thehighestvalues,exceeding250m2/g,wereobtainedforx≈2.Thespinel
oxidesexhibitanoutstandingcatalyticactivityforpropaneoxidationatmildtemperature(20–200◦C).
TheyarealsoactiveforCOoxidationatambienttemperature.Thishighactivitywascorrelatedbothwith thesurfaceareaandthecobaltconcentration.ThemostefficientmaterialisCo2,3Mn0,7O4,whichhasa
betteractivitythancobaltoxidecatalystsreportedintheliterature.
1. Introduction
Catalyticoxidationisaveryeffectivemethodfortheabatement oflowconcentrationsofVolatileOrganicCompounds(VOCs). Cur-rently,themostactivecatalystsaresupportednoblemetals[1–3]. Howeverthesecatalystsareveryexpensiveandtheiractivitycanbe stronglyinhibitedbyCO[4],waterorchloride[5].Forlow tempera-tureapplications,likeVOCsremovalinindoorair,preciousmetals canbereplacedbytransitionmetaloxides[6].Especiallyspinel cobaltoxide(Co3O4)wasreportedtobethebestcatalystforthe
totaloxidationofCO[7]andhydrocarbons[6,8].Spineloxides,with thegeneralformulaAB2O4,containcationsitesofdifferent
coordi-nation(tetrahedralandoctahedral)withtheoxideanionsarranged in a cubicclose-packed lattice.Partialsubstitution of cobaltby manganesegivesmixedCo–Mnspineloxides,whichcanbebetter catalyststhanCo3O4fortheoxidationofVOCs[9–11].
Mostoftenthecatalystsreportedintheliteratureare synthe-sizedathightemperature(>500◦C).Thisrequirement,unavoidable
for automotive catalytic converters, becomes useless for VOCs abatementatmildtemperature(<300◦C).Actuallyitisexpected
thatmetastablenanocrystalline oxides,withverylargeporosity andsurfacearea,willbehighlyactivecatalysts.Thiskindof mate-rialscanbeeasilyobtainedbythermaldecomposition ofmetal oxalates.Indeedaclosecontrolofthedecompositionallows
prepar-∗ Correspondingauthor.
E-mailaddress:alphonse@chimie.ups-tlse.fr(P.Alphonse).
ing mixed oxides with very high surface area (300–500m2/g)
[12,13].Moreoverthiseasyandinexpensivemethodisalsovery convenienttoobtainmixedoxides[14].
Thegoalofthisstudywasthesynthesisoflargesurfacearea CoxMn3−xO4 oxides (0≤x≤ 3) by controlled decomposition of
mixedoxalates and theevaluationof thecatalytic performance of these metastable materialsfor the total oxidation of carbon monoxideandpropaneatmildtemperature(20–200◦C).Carbon
monoxideisproducedinlargeamountbytransportation,industrial anddomesticactivities.Itisextremelytoxicandcatalytic oxida-tionintoCO2 constitutesthebestsolutionforCO removalfrom
indoorair[7].Thuslowcost,preciousmetalfreecatalysts, work-ingatroomtemperaturearehighlydemanded.Propaneislargely usedasdomesticandindustrialfuel.Besidesitisalsothethirdmost commonmotorvehiclefuelintheworldbehindgasolineandDiesel fuel.Ontheotherhanditisgenerallyadmittedthatalkanesarethe leastreactiveamongVOCsandacatalystabletoremovepropaneat mildtemperaturesisexpectedtobeactiveforotherVOCsaswell.
2. Experimental
2.1. Synthesisofoxides
2.1.1. Preparationofmixedoxalates
MixedoxalatesCox/3Mn(3−x)/3C2O4.2H2Owereprecipitatedat
roomtemperaturebyquickintroductionofanaqueoussolution ofcobaltandmanganesenitrates(200mL;0.2M)intoanaqueous solution of ammonium oxalate (200mL; 0.22M) under vigor-http://dx.doi.org/10.1016/j.apcatb.2015.07.019
ousstirring.After30min,theprecipitatewasfiltered,thoroughly washedwithdeionizedwateranddriedinairat70◦C.
2.1.2. Thermaldecompositionofoxalates
Thethermaldecompositionofoxalateswascarriedoutina ver-ticaltubularfixed-bedflowreactorunderatmosphericpressure. Theinternaldiameterofreactorwas1cm.Theflowrateoftheinlet gas(4%O2inAr)was100cm3/min.Theoutletgascompositionwas
followedusingamassspectrometer(HPR20-QICfromHiden Ana-lytical).ThetemperatureofthereactingsolidwasrecordedbyaK
thermocouplepositionedinsidethepowderedsample.Thissetup allowedcontrollingboth thetemperatureofthereacting mate-rialandthecompositionoftheatmosphere.Thetemperaturewas increasedat2.5◦C/minuntilCO
2emissionwasdetected;fromthen
thedecompositionwasdoneinisothermalconditions.For exam-ple,inthecaseofmanganeseoxalatethistemperaturewasabout 210◦C.WhenCO
2emissionwasover,toensureatotal
decompo-sition,eveninthecoreofparticles,thepartialpressureofO2was
augmentedgraduallyto20%;thenthetemperaturewasincreased at5◦C/minupto300◦Candmaintainedtothisvaluefor1h.
2.2. Thermalanalysis(TGA-DSC)
Thethermaldecompositionofoxalateswasstudiedby thermo-gravimetricanalysis(TGA)anddifferentialscanningcalorimetry (DSC),usinga constantheatingrate(5◦C/min),ona TGA-DSC-1
Mettler–Toledodevicein thetemperaturerange30–600◦C. The
flowinggaswasamixture20%O2inAr.About5mgofoxalate
pow-derwereplacedina40mLaluminiumpanandthereferencewas anemptyaluminiumpan.
2.3. PowderX-raydiffraction(PXRD)
ThecrystalstructurewasinvestigatedviapowderX-ray diffrac-tion.Datawascollected,atroomtemperature,withaBrukerAXS D4–2 diffractometer,in theBragg–Brentanogeometry,using filteredCuKaradiationandagraphitesecondary-beam monochro-mator.Diffractionintensitiesweremeasuredbyscanningfrom20 to80◦(2)withastepsizeof0.02◦(2).
Aquantitativeestimationofthelatticeparametersand peak broadeningwasaccomplishedbyprofilefittingofthewholeXRD patternsusingtheFullprofsoftware[15].Thepeakprofileswere modeledbyThompson-Cox-Hastings[16]pseudo-Voigtfunctions. The parameters refined were zero shift (2), background, cell parametersandpeakshape.Thesizeandstraincontributiontothe integralbreadthofeachreflectionwerecalculatedbythesoftware. Theinstrumentalbroadeningcontributionwasevaluatedbyusing ana-aluminasample(NISTStandardReferenceMaterial1976b).
Thestructuralchangesversustemperaturewerefollowedby HighTemperatureX-rayDiffraction(HTXRD)withaBrukerAXSD8 diffractometer(usingNi-filteredCuKaradiation)equippedwith ahightemperaturechamber AntonPaarHTK1200N. Diffraction intensitieswererecordedinsyntheticairflow(20%O2inN2),at
fixedtemperature,every10◦C,intherange100–500◦C.The
heat-ingratebetweeneach stepwas10◦C/min.Thetime neededto
recordeachpatternwasabout15min.
2.4. Specificsurfacearea,poresizedistribution
Specificsurfaceareaandporesizedistributionwerecalculated fromnitrogenadsorption-desorptionisothermscollectedat77K, usinganadsorptionanalyzer(MicromeriticsTristarII3020).The specificsurfaceareaswerecomputedfromadsorptionisotherms, usingtheBrunauer–Emmett–Teller(BET)method[17].Thepore sizedistributions(PSD)werecomputedfromdesorptionisotherms
bytheNLDFTmethod[18](withQuantachromeAutosorb-1 soft-wareusingsilicaequilibriumtransitionkernelat77K,basedona cylindricalporemodel).
Porevolume(Vpore)wascalculatedfromtheadsorbedvolume
atarelativepressureof0.995(Vsat)by:
Vpore=
N2gasdensity
N2liq.densityVsat
=0.00155Vsat
Priortoanalysis,toremovethespeciesadsorbedonthesurface, theoxalatesamples(about0.5g)weredegassedfor16hat70◦C
whereastheoxidesamples(about0.1g)weredegassedfor16hat 90◦C(finalpressure<10−3Pa).
2.5. Electronmicroscopy
Transmission electron microscopy analyses were performed withaJeolJEM-1400operatingat80kV.Sampleswereprepared byputtingadropofanethanolsuspensionofparticlesona carbon-coatedcoppergrid.
Scanningelectronmicroscopyanalyseswereperformedwitha SEMFEGFEIQuanta-250at20kV.Thesampleswerepreparedby puttingadropofanethanolsuspensionofparticlesonanaluminum sampleholder.Beforeanalysis,thesampleswerecoveredwitha thinlayer(5nm)ofPtbysputtercoating.
2.6. ChemicalanalysisbyX-rayfluorescence
Theelementalcompositionwasdeterminedonpowder sam-plesbyX-rayfluorescencewithaBrukerS2Rangerworkingwitha maximumvoltageof50kVandacurrentof2mA.
2.7. Catalytictests
Theactivitiesofcatalystsweretested forCO andC3H8 total
oxidation.Thesetestswereperformed,atambientpressure,ina tubularfixedbedflowglassreactor(internaldiameter=6mm).The catalystmasswasalwayscloseto0.05g.Thecatalystpowderwas packedinthetubegivinga2–3mmbedlength.Thevolumetric flowratewas1.63mLs−1givingacontacttimeof0.03s.Thesizeof
catalystparticleswasabout10mm.Thereactoroperatesat differ-entialconditionsonlyforpropaneoxidation,atmildtemperatures (conversion<10%).Thereactantsweredosedbymassflow con-trollers (Brooks5850).The catalysttemperaturewascontrolled byaK-typethermocouplepositionedinsidethecatalystbed.For COoxidationthetemperaturerangewas30–200◦Candtheinlet
gascompositionwas0.8%CO+20%O2inAr.ForC3H8 oxidation
thetemperaturerangewas30–300◦Candtheinletgas
composi-tionwas0.4%C3H8+20%O2 inAr.Thecatalysttemperaturewas
increasedataheatingrateof200◦C/h.Thegasphasecomposition
duringthetestswasmonitoredbymassspectrometry(HPR20-QIC fromHidenAnalytical).BeforetheCOoxidationtest,thecatalysts werefirstpretreatedwith20%O2inArfor60minat200◦C.The
C3H8oxidationtestwasdoneafterCOtestwithoutany
pretreat-ment.
3. Resultsanddiscussion
3.1. Characterizationofoxalateprecursors 3.1.1. XRD
TheXRDpattern(Fig.1)ofmanganeseoxalatecorrespondsto themonoclinicstructurewiththespacegroupC2/c(PDF# 00-025-0544)whereascobaltoxalatehastheorthorhombicstructurewith thespacegroupCccm(PDF#00-025-0250).Thestructureofmixed Co–Mnoxalatesdependsontheirmanganesecontent.Foroxalates containingmoreMnthanCo,patternmatchingwiththemonoclinic
Fig.1. ExamplesofXRDpatternsofCox/3Mn(3−x)/3C2O4.2H2OaftertheprofilefittingwiththeFULLPROFsoftware[15].Theupperpatternswereindexedforthemonoclinic structure(PDF#00-025-0544)whereasthelowerpatternswereindexedfortheorthorhombicstructure(PDF#00-025-0250).
Table1
StructureparametersofCox/3Mn(3−x)/3C2O4.2H2Odeterminedbyprofilefittingof XRDpatternswithFULLPROFsoftware[15].Disthecrystallitesize.
x Spacegroup a(nm) b(nm) c(nm) ˇ(◦) D(nm) 0 C2/c 1.200 0.565 0.998 128.3 52 0.6 C2/c 1.197 0.561 0.996 128.2 55 0.9 C2/c 1.194 0.557 0.996 128.1 51 1.6 Cccm 1.192 0.550 1.556 90 15 2.0 Cccm 1.188 0.545 1.557 90 17 2.3 Cccm 1.191 0.546 1.564 90 21 3 Cccm 1.187 0.542 1.557 90 32
structuregives abetteragreementwhereas,whenCoequalsor exceedsMn,abestfitisobtainedwithorthorhombicstructure.The latticeparametersandthecrystallitesizearereportedinTable1. BothaandblatticeparametersdecreasewhentheproportionofCo increasesindicatingthatthesmallerCo2+ions(r=89pmHS)
sub-stituteforthelargerMn2+ions(r=97pmHS).Thecrystallitesize
isconstant,atabout50nm,forthemonoclinicstructureanddrops near20nmwhenthestructurebecomesorthorhombic.However thecrystallitesizeofcobaltoxalateislarger,atabout30nm,than thatofCo-richmixedoxalates.
3.1.2. Scanningelectronmicroscopy
TheSEMimagesforseveralcompositionsareshowninFig.2. Theparticlemorphologychangesaccordingtothechemical
com-Table2
BETsurfacearea(SBET)andporevolume(Vpore)ofCox/3Mn(3−x)/3C2O4.2H2O deter-minedfromN2adsorptionisothermsat77K.
x SBET(m2/g) CBET Vpore(cm3/g)
0 26±2 130 0.095±0.008 0.6 2.4±0.2 120 0.010±0.001 0.9 4.0±0.3 130 0.030±0.002 1.6 5.0±0.4 150 0.062±0.005 2.0 4.4±0.3 110 0.044±0.003 2.3 6.0±0.5 160 0.074±0.005 3 4.0±0.3 170 0.024±0.002
position.Theparticlesofmanganeserichoxalates(upperimages) areveryirregularinsizeandshapewhereastheparticlesofcobalt richoxalatesaremoreuniform.Theseparticlesareatleasttentimes largerthanthecrystallitesizedeterminedfromXRD.For2≤x<3 theparticlesaggregateinball-shapedunits(lowerleftimage).We didnotobservesuchaggregatesforcobaltoxalate,whichgivesrod likeparticles(lowerrightimage).
3.1.3. Specificsurfaceareaandporevolume
TheBETsurfacearea(SBET)andporevolume(Vpore)ofoxalates
arereportedinTable2.Thesurfaceareasofallthecompounds con-tainingcobaltaresimilar,intherange4–6m2/g.Theyareatleast5
timeslowerthanthesurfaceareaofmanganeseoxalatewhichhas alsothelargestporevolume.Forthisoxalatewesuspectedthatthe
Fig.2. SEMimagesofsomeoxalates.
degassingprocedure(16hat70◦Cinvacuum)inducedthe
begin-ningofdehydrationbecausetheonsettemperatureofdehydration waslowerthanformixedoxalates(seeSection3.2.1). Neverthe-lessdoublingtheevacuationtimedidnotchangesignificantlythe texturalproperties.
3.2. Decompositionofoxalateprecursors 3.2.1. Thermalanalysisofoxalatedecomposition
TheTGA-DSCanalysiscurvesforseveralcompositionsare plot-tedin Fig.3.The decomposition occursin two main separated stages:below200◦Ctheendothermicdehydrationgivingthe
anhy-drousoxalate,followed bythe exothermicdecomposition near 300◦C. Foran oxalatecontaining2H
2Opermole,themassloss
duetodehydrationmustdecreaseslightlyfrom20.1%forx=0to 19.7%forx=3.Weobtaintheexpectedvalueformanganeseoxalate whereasthemasslossisonly19%forcobaltoxalate,indicatinga numberofwatermoleculesslightlylessthan2.Besides,forcobalt oxalate,theendothermicdehydrationpeakhasasmallshoulder ontherightsideequivalenttoabout10%ofthewholearea.This peakisalwayspresentwhateverthemassofsampleanalyzedor theheatingrate.Itcouldbetheindicationthatwehaveamixture betweentheorthorhombicformandasmallamountofthe mono-clinicpolymorphwiththespacegroupC2/c(PDF#00-025-0251) notdetectedontheXRDpatterns.
Thermaldecompositionoftransitionmetaloxalateshydrates hasbeenstudiedfor manyyears [19–33].It wasobserved that the decomposition product for these oxalates depends on the reducibilityofthemetalliccationinvolved[23,25,32].Withcations
presentingalowreducibility,likeMn2+,thedecompositionleads
tothemetaloxidefollowingthereaction:
MnC2O4→MnO+CO+CO21H= 151kJ/mol (1)
WhereasformorereduciblecationslikeCo2+thedecomposition
producesthemetal:
CoC2O4→ Co+2CO2H= 94kJ/mol (2)
Howeverinair,CoisoxidizedinCo3O4:
3Co+2O2→ Co3O41H=−891kJ/mol (3)
SimilarlyMnOwillbealsooxidizedinair.Accordingtothe reac-tionconditionstheproductwasreportedasMn3O4[34],Mn2O3
[22,35],MnO2[26]oramorphousMnOx[36].
Moreoverthemanganeseorcobaltoxidesformedareknownto begoodcatalystsfortheCOoxidation[7]:
CO+1/2O2→ CO21H= −283kJ/mol (4) Therefore,sincetheseoxidationreactionsareveryexothermic, theoveralldecompositionreactionislargelyexothermictoo.
Theeffectofcobaltfractiononsomecharacteristicsofmixed oxalatedehydrationanddecompositionisillustratedinFig.4.Four featuresarefollowed,theonsettemperatureofdehydration(Ti),
thewidthofthedecompositionpeak(in◦C),theenthalpyof
dehy-drationand theenthalpyof decomposition.The upper-leftplot shows thattheTi ofmixed oxalatesis closetotheTi ofcobalt
oxalate(130◦C) whereas thedehydration ofMn oxalatebegins
atleast30◦Cbelow.Thelower-leftplotshowsthattheenthalpy
Fig.3.TGA-DSCcurvesforsomeoxalates.
about520J/g(95kJ/moloxalate);onlytheenthalpyobservedfor manganeseoxalateisslightlylower.Thisvalueisveryclosetothe enthalpyreportedbyMaciejewskietal.[30].
Weobservedthattheonsettemperatureofdecomposition aug-mentslinearly withthe cobalt content of oxalates, goingfrom 230◦C for manganese oxalate to255◦C for cobalt oxalate.The
upper-rightplotshowsthatthewidthofthedecompositionpeak, whichislinkedtotherateofthereaction,markedlydecreaseswhen theproportionofcobaltincreases.Neverthelesstheenthalpyof decomposition,estimatedbyintegrationoftheexothermicpeak, doesnotrisemuchwiththecobaltfractionasshownbythe lower-rightplot.Thisis confirmedby theredlinein this plot,which correspondstothe valuescalculated fromthermodynamicdata (1fH◦298)[37,38]assumingtheformationofanidealsolidsolution
havingthespinelstructure(cf.§3.2.2).Thereforewethinkthatthe increaseofthedecompositionratewiththeproportionofcobalt couldbeexplainedbytheveryhighreactivityofmetalcobaltin oxygencontainingatmospheres.Thustoavoidatemperature over-shoot,leadingtoafastgrowthofcrystallites,thedecompositionof cobalt-richoxalatesshallbeperformedinisothermalconditionand lowoxygenpartialpressure.
3.2.2. HT-XRDofoxalatedecomposition
Thethermaldecompositionoftheoxalateswasalsofollowed byHT-XRD.Thesampleswereheatedbystepof10◦Cat5◦C/min.
Takingintoaccountthetimerequiredtorecordeachpattern,the heatingrateontheaveragewasabout0.5◦C/min.Thus,compared
withTGA-DSCforwhichtheheatingratewas5◦C/min,apeakshift
towardlowertemperaturecanbeexpected.
TherelevantXRDpatternsforseveralcompositionsareplotted inFig.5.Theupper-leftchartcorrespondstomanganeseoxalate.
Thefirstpattern,recordedat150◦C,correspondstotheanhydrous
oxalatewhichhasanorthorhombicstructurewiththespacegroup Pmna(PDF#00-032-0646).Thisanhydrousoxalatedecomposes from230◦Ctogiveanamorphousphasewhichcrystallizesonlyat
400◦CincubicMn
2O3(bixbyite)withthespacegroupIa3(PDF#
00-041-1442).Thistransformationgivesasmallexothermalpeak togetherwithaslightmasslossat450◦ContheTGA-DSCplot(see
Fig.3,x=0).
The upper-right plot corresponds to the mixed oxalate Co0.2Mn0.8C2O4.2H2O(xCo=0.6).Theanhydrousoxalatepatternis
observedfrom140◦C.Likeformanganeseoxalate,thisanhydrous
oxalatedecomposesfrom220◦Ctogiveanamorphousphasewhich
crystallizesat450◦Cinatetragonallydeformedspinel(spacegroup
I41/amd)likeMn3O4(hausmannite,PDF#00-024-0734).Mn3O4
isa “normal”spinelbecauseallMn3+cationsarelocatedin the
octahedralsites,givingthecationdistributionMn2+[Mn3+] 2O4[39].
Bordeneuveetal.[40],fromneutrondiffractiondatarecordedon CoxMn3-xO4ceramics,showedthat,forx<1,thesubstitutionoccurs
onlyinthetetrahedralsitewhereCo2+replacesMn2+.
Thedeformationofthecubicspinelstructureiscorrelatedwith adistortionofthecoordinationoctahedronaroundMn3+,usually
interpretedasaconsequenceofthecooperativeJahn–Tellereffect
[41].
The lattice parameters of hausmannite are a=0.576nm and
c=0.944nm[41].Profilematching(usingFullProfsoftware[15]) gives a=0.575nm and c=0.938nm for the pattern recorded at 450◦Canda=0.576nmandc=0.938nmforthepatternrecordedat
500◦C.Thelowercvalueinoursamplescouldoriginatefrom
par-tialoxidationofMn3+intonon-distortingMn4+intheoctahedral
sitesbecause,inhausmannitestructure,thecoordination octahe-dronaroundMn3+areelongatedapproximatelyparallelto[001].
Fig.4.EffectofcobaltfractionontheonsettemperatureofdehydrationTi(upper-left),thewidthofthedecompositionpeak(upper-right),theenthalpyofdehydration (lower-left)andtheenthalpyofdecomposition(lower-right).
Profilematchingalsoprovidesanestimationofthecrystallitesize
D;wefoundD=12nmfor450◦CandD=14nmfor500◦C.
Itisworthnoticingthatthecrystallizationobservedat450◦C
isassociatedwithasmallmasslossonTGcurvebut,unlike man-ganeseoxalate,givesnodetectablethermalevent(Fig3,x=0.6). Thiscouldbeanindicationthat,inthis case,thecrystallization involvesonlylittlechangeinthestructuralarrangementofatoms, becausetheamorphousstatehasaproto-spinelstructureasitwas previouslyassumedfornickelmanganitespinelspreparedbylow temperaturedecompositionofmixedoxalates[42].
The lower-left plot corresponds to the mixed oxalate Co0.3Mn0.7C2O4.2H2O (x=0.9). The dehydration occurs above
130◦C giving a compound with a XRD pattern similar to the
monocliniccobaltoxalatewiththespacegroupP21/n(PDF# 00-037-0719). This compound decomposes at 240◦C generating a
poorlycrystallinephasecorrespondingtothecubicspinel(space groupFd-3m).Then,from350◦C,thisphaseisprogressively
con-vertedinthetetragonalspinel.Profilematchinggivesa=0.574nm,
c=0.930nmandD=16nmforthepatternrecordedat500◦C.
Thecriticalconcentrationof distortingMn3+required inthe
octahedralsitestotriggertheJahn–Tellereffectisabout55%[41]. Thusthetransientformationofthecubicspinelcouldbeexplained bythepartialoxidation,aftertheoxalatedecomposition,ofmore than45% of Mn3+ into non-distorting Mn4+
. From 350◦C Mn4+
cationsarereducedinMn3+inducingtheprogressiveconversion
inthetetragonalspinel.
Inthecaseofcobaltoxalate(lower-rightplot)thedehydration occursabove140◦C,givingthemonocliniccobaltoxalate(PDF#
00-037-0719),which startstodecomposeat230◦C toyieldthe
cubicspinelCo3O4(spacegroupFd-3m,PDF#00-042-1467).
Pro-filematching,forthepatternrecordedat300◦C,givesa=0.809nm
andD=12nm.
3.3. Characterizationofoxidesusedascatalysts 3.3.1. XRD
Whatever the decomposition temperature of oxalates, the oxidesusedascatalystswereheatedinairat300◦Cfor1h.The
crystal structure, latticeparameter and crystallite sizeof these materialsarereportedinTable3.Asshownintheprevious sec-tion,theoxidesforwhichx<0.9areamorphous.TheXRDpattern ofCo0.9Mn2.1O4showsverybroadlinescorrespondingtoacubic
spinelcompoundbutisistoopoorlycrystallizedtoevaluateitscell parameterandcrystallitesize.Forx>0.9alltheproductshavea cubicspinelstructure.Thecellparametersofthemixedoxidesare slightlylargerthanthecellparameterofCo3O4.Neutrondiffraction
dataonceramicsshowedthat,for1<x<2,thetetrahedralsitesare fullyoccupiedbyCo2+andthesubstitutionnowoccursin
octahe-dralsiteswhereMn3+isreplacedbothbyCo2+andCo3+bearing
inmindthateachCo2+alsoimpliestheoxidationofoneMn3+in
Mn4+topreservetheglobalelectroneutrality[40].BecauseCo2+
Fig.5. XRDpatternsrecordedatincreasingtemperatureduringthedecompositionofoxalatesinair.
thanLSCo3+ions(55pm)itisexpectedthatthecellparameterof
mixedoxidesbelargerthanthatofCo3O4.Thebiggestcell
param-eterisobservedforx=2probablybecausethisoxidecontainsthe largestamountofCo2+.Furthermoretheincreaseofcobaltcontent
isassociatedwithasignificantgrowthofthecrystallite.
3.3.2. Electronmicroscopy
Atmediummagnification,theSEMimagesofoxalatesbefore and after decomposition are similar as shown in the case of Co2.3Mn0.7O4 in Fig.6(left andcenter images). Thus, despitea
masslosscloseto60%,whenthereactionconditionsallows
con-Table3
Microstructuralandtexturalpropertiesofmixedoxides(CoxMn3−xO4)obtainedafterheatinginairat300◦C.StructuralparameterswasdeterminedbyprofilefittingofXRD patternswithFULLPROFsoftware[15];Disthecrystallitesize.BETsurfacearea(SBET)andporevolume(Vpore)werecalculatedfromN2adsorptionisothermsat77K.The valuesofSBETandVporearetheaverageofseveralmeasurements.
x Structure a(nm) D(nm) SBET(m2/g) CBET Vpore(cm3/g)
0 Amorphous 90±5 110 0.16±0.01 0.6 Amorphous 100±10 140 0.21±0.02 0.9 Cubicspinel 230±20 160 0.28±0.03 1.6 Cubicspinel 8.11 6 270±30 50 0.33±0.04 2.0 Cubicspinel 8.12 7 260±30 40 0.48±0.05 2.3 Cubicspinel 8.10 9 220±20 35 0.29±0.03 3 Cubicspinel 8.09 16 60±5 50 0.27±0.01
Fig.6.SEMimagesofCo0.77Mn0.23C2O4.2H2Ooxalate(leftimage)andCo2.3Mn0.7O4oxide(middleimage).TEMmicrographofCo2.3Mn0.7O4oxide(rightimage).
trollingthedecompositionrate,theexternalshapeoftheoxalate particlesiskept.Itispossibleonthecentralmicrographytomake outmanycracksindicatingthattheoxideparticlesarehighly frac-turedbuttheporosityismoreeasilyevidencedontheTEMimage whichclearlyshowsthevoidbetweencrystallites(rightimage). Thecrystallitesizeisin goodagreementwiththesizeobtained fromXRD.
3.3.3. Specificsurfacearea,porevolumeandporesize distribution(PSD)
TheBETspecificsurfaceareas(SBET)andtheporevolume(Vpore)
ofthematerialsheatedat300◦C,calculatedfromtheN
2
adsorp-tionisotherms,arereportedinTable3.Inthecaseofmixedoxides, weobservethatSBETisstronglydependentofthedecomposition
conditionssothat,forseveralpreparationsdoneinsimilar condi-tions,SBETcandifferbyabout20%.Monometallicandamorphous
oxideshavethelowestsurfaceandporevolume.ThehighestSBETis
obtainedforx≈2;abovethisvaluetheincreaseofcobaltcontentis associatedwithadiminutionofthesurfaceareaandporevolume. Thehighsurfaceareaandporosityofoxidesstronglycontrast withthelowtexturalpropertiesmeasuredonoxalates(seeTable2). Thislargeinterfaceiscreatedbecausethereisalmostno shrink-ageoftheoxalateparticlesinducedbythebigmasslossoccurring duringdecompositionprocess.
Somerepresentativeisothermsand theirassociatedPSD, cal-culatedusingNLDFTmethod,areplottedinFig.7.Theporosityof thesematerialspansawiderange,frommicroporestomacropores; howevertheirPSDvariesconsiderablyaccordingtothecobalt frac-tion.Theapproximatecorrelationbetweenthecrystallitesizeand thepositionofthemainpeakofPSDletssupposethatthe meso-porescorrespondtotheinter-crystallitespaces.Theporesinthe macroporerangeareprobablyduetotheinter-granularporosity correspondingforexampletothevoidbetweentheparticles.
3.4. Catalyticactivity
Thecatalyticactivityofthemonometallicand mixedoxides, forCOandC3H8totaloxidation,ispresentedinFig.8.These
mea-surementswerenotdoneatsteadystatebutwithadynamicramp rateoftemperature(200◦C/h)andon-linemonitoringusingmass
spectrometry.For COoxidation,toreachthemaximumactivity, thecatalystswereheated ina drygasflow (20%O2 inAr).For
propaneoxidationthispre-treatmentwasnotrequiredtoobtain optimumactivity.WedetectedonlyCO2 andH2Oasproductsof
oxidationandthecarbonbalancewascloseto100%within2%.All thecatalystsweretestedoverthetemperaturerange(20tests). SomerepresentativeCO(left)andC3H8(right)conversioncurves
versustemperature(light-offcurves)areshownontheupperplots ofFig.8.Wenoticedthatthesameoxalatedecomposedinwhat
Fig.7.N2adsorption-desorptionisothermsandtheirassociatedporesize distribu-tion(PSD)calculatedusingNLDFTmethod[18].
seemstobethesameconditionscouldproducetwocatalysts hav-ingsignificantdifferencesinactivity.Thisisillustratedinthelower chartswheretheconversionobservedat60◦CforCO (left)and
200◦CforC
3H8 (right)areplotted versustheamountofcobalt.
Despitethescatteringoftheresults,theeffectofthesubstitutionof manganesebycobaltseemsrathersimilarforbothreactions. Espe-ciallyweobservethat,forx<0.9,thesubstitutiondoesnotchange theactivitywhereasforx=0.9theactivityisclearlybetter(about3 times).BesidesCo3O4hasaloweractivitythanCo2.3Mn0.7O4which
seemstobethebestcomposition.
The boost of activity for x=0.9 is associated with a strong increaseofSBETwhichrisesfrom100to230m2/g.Inanattempt
todissociatetheeffectofspecificareafromtheinfluenceofcobalt concentration,wecalculated,fromtheconversionrateandSBET,
theintrinsicactivity,Ai,definedasthenumberofreactantmmoles convertedpersecondandperm2ofcatalyst.Thisintrinsic
activ-ity,plottedagainstthecobaltfraction,isshowninFig.9.Inthe caseofCOoxidationAidoesnotappeartobedirectlydependentof
activ-Fig.8. ExamplesoftheCO(upper-left)andC3H8(upper-right)conversioncurvesversustemperature(light-offcurves).Effectofcobaltfractionontheconversionobserved at60◦CforCO(lower-left)and200◦CforC
3H8(lower-right).
Figure10.CO(left)andpropane(right)conversionwithtimeonstreamforCo2.3Mn0.7O4catalyst.
Table4
Comparisonofcatalystactivityforpropaneoxidationat200◦C.
Ref. Catalyst Catalystmass(g) Flowrate(cm3/min) InletC
3H8concentration(%) %C3H8conv.at175◦C Activityat175◦C(mmols−1g−1)
[49] Co3O4 0.25 50 0.80 21 0.25
[50] 4%Au/Co3O4 0.25 50 0.80 32 0.38
[51] Co3O4 0.05 98 0.37 5 0.27
thiswork Co2,3Mn0,7O4 0.05 98 0.37 8 0.43
ityisobservedforhighercobaltcontent.Forpropaneoxidation,a similarcorrelationbetweenAiandcobaltfractionisobservedfor x>1.5.Belowx=1.5,thecorrelationislessclear.
Severalworkshavedemonstratedthattheoctahedralsitesare almost exclusivelyexposed at the surface of the spinel oxides
[43–45].Moreoverit wasalsoshown thatthe catalyticactivity ofcobaltoxideswasduetoCo3+ionsinoctahedralsites[45,46].
Hence,forlowcobaltcontent,itisexpectedthatthecatalytic activ-itydoesnotchangemuchbecausethesubstitutionoccursonlyin theinactivetetrahedralsiteswhereCo2+replacesMn2+.Whenthe
tetrahedralsitesarefullyoccupiedbyCo2+(x>1)thesubstitution
occursinoctahedralsitescreatingactiveCo3+ions[40].
Theapparentactivationenergyforpropaneoxidationwas deter-minedfromArrheniusplotsintheconversionrange0–10%.Except formanganeseoxide,itwasfoundalmostconstantat60±10kJ/mol whateverthecobaltconcentration.ForMnOxtheactivationenergy
isslightlyhigherat75±10kJ/mol.
InthecaseoftheCOoxidationtheconversionistoohightoallow thecalculationofactivationenergy.
Forthebestcatalyst(Co2.3Mn0.7O4)wefollowedtheeffectofthe
oxalatedecompositiontemperature(intherange220–300◦C)on
thecatalyticactivityforpropaneoxidation.Althoughthevariations inactivitywereofthesameorderofmagnitudeasthedifferences betweenreplicatesitseemsthattheoptimumdecomposition tem-peratureis280◦C.
Thelong-termstabilityoftheconversionwastestedwiththe bestcatalyst(Co2.3Mn0.7O4).TheleftplotofFig.10showsthatthe
COconversiondecreasesbyabout8%duringthefirsthalfofthe test.Thenitseemstoremainstableuntiltheendofthetest. Unex-pectedlyweobservedvariationsoftemperatureassociatedwith variationsofconversion.Wecouldnotdetermineifitwasthe tem-peraturechangethatinducedconversionchangeortheconverse. Asregardspropaneoxidation,therightplotofFig.10indicatesthat theconversionwasstableformorethan14hat160◦C.
Tocomparethecatalyticactivityofourmaterialswiththedata reportedintheliteraturewecalculatedthespecificactivitydefined asthenumberofreactantmmolesconvertedpersecondandper gramofcatalyst.
AsitwasdemonstratedthatCOconversionwasstrongly depen-dentupontheamountofwaterintheinletgas[46–48]welimited ourcomparisontopropaneoxidation.Thiscomparisonrevealed (Table4)thatCo2.3Mn0.7O4activitywasmorethan50%higherthan
thatofCo3O4catalystsfoundinthemostrecentpublicationsand
wassimilartocatalystsforwhichpreciousmetalhavebeenadded toenhancetheactivity.
4. Conclusion
Cobalt-manganesemixedoxalatedihydratescrystallizeinthe monoclinicstructurewhenthecobaltfractionis lowerthan0.5 andinorthorhombicstructureotherwise.Thecontrolled decom-positionoftheseoxalatesnear200◦C,followedbyacalcinationat
300◦C,stronglyrestrainstheshrinkageofparticlesandthe
crys-tallitesintering,producingmixedoxidesCoxMn3−xO4withavery
largesurfacearea.Forx<0.9thesematerialsareamorphous.For
x≥0.9theyhaveacubicspinelstructureandtheircrystallitesize increaseswiththecobaltfraction.
Thesespineloxidesexhibitanoutstandingcatalyticactivityfor propaneoxidation.TheyarealsoactiveforCOoxidationevenat ambienttemperature.Thishighactivityiscorrelated both with the surface area and the cobalt concentration. For manganese oxide the apparent activation energy for propane oxidation is 75±10kJ/molwhereasitis60±10kJ/molandnearlyindependent ofcobaltfractionfortheothercatalysts.Themostefficientmaterial isCo2,3Mn0,7O4,whichhasanactivitymorethan50%higherthan
thebestCo3O4catalystsreportedintheliterature.
Acknowledgments
ThisworkwasfinanciallysupportedbytheDGEandtheRegional CouncilofMidi-PyrénéesintheframeworkoftheSOFTAIRproject.
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