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Chemical
Physics
Letters
j o ur na l ho me p ag e :w w w . e l s e v i e r . c o m / l o c a t e / c p l e t t
Thermodynamic
characterization
of
two
layers
of
CO
2
on
a
graphite
surface
T.T.
Trinh
a,
D.
Bedeaux
a,
J.-M.
Simon
b,
S.
Kjelstrup
a,c,∗aDepartmentofChemistry,NorwegianUniversityofScienceandTechnology,Trondheim,Norway
bLaboratoireInterdisciplinaireCarnotdeBourgogne,UMR-6303CNRS-UniversitédeBourgogne,Dijon,France
cDepartmentofProcessandEnergyLaboratory,DelftUniversityofTechnology,Delft,TheNetherlands
a
r
t
i
c
l
e
i
n
f
o
Articlehistory:
Received3July2014
Infinalform8August2014
Availableonline14August2014
a
b
s
t
r
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Wefindbyexaminationofdensityprofilesthatcarbondioxideadsorbsongraphiteintwodistinctlayers. Wereporttheactivitycoefficient,entropyandenthalpyforCO2ineachlayerusingaconvenient
com-putationalmethod,theSmallSystemMethod,therebyextendingthismethodtosurfaces.Thisopensup thepossibilitytostudythermodynamicpropertiesforawiderangeofsurfacephenomena.
©2014TheAuthors.PublishedbyElsevierB.V.ThisisanopenaccessarticleundertheCCBY-NC-ND license(http://creativecommons.org/licenses/by-nc-nd/3.0/).
1. Introduction
Phasetransformations[1],formationsofnanostructures[1,2], metastablephases[3]oragglomerations[4],aswellaschemical reactions[5]areallphenomenawhichbecomespecialatsurfaces. Asurfacecanalsoposeamajorbarriertotransport[6,7]. Thermody-namicdatawillimprovetheunderstandinganddynamicmodeling ofequilibriumandnonequilibriumstates.Butthermodynamicdata forsurfacesarenoteasilyavailablebyexperiments.Withthe intro-ductionoftheSmallSystemMethod[8,9]computationalresults havebecomefeasible.Thismethodhassofarnotbeenusedto studysurfaces.Inthisworkweextendthemethodtoatechnically importantprocess,thephysisorptionofCO2onagraphitesurface.
Graphiticmembranesarepromisingcheapcandidatemembranes forCO2separationpurposes[10].Theprocesscanbewritten:
CO2(g)+graphiteCO2(s) (1)
where (g) means gas phase and (s) means adsorbed gas. The purposeoftheworkistodemonstratehowthermodynamic infor-mationcanbegainedofanadsorbedstateusingthenewsimulation method.Weshallseethatadsorptiontakesplaceintwodistinct thermodynamiclayers,andthatthefillingintothelayerscanbe regardedasatrade-offbetweentheentropiesandenthalpiesfound foreachlayer.
∗ Correspondingauthorat:DepartmentofChemistry,NorwegianUniversityof
ScienceandTechnology,Trondheim,Norway.
E-mailaddresses:trinhthanhthuat@gmail.com(T.T.Trinh),
signe.kjelstrup@ntnu.no(S.Kjelstrup).
2. Methods
The Small System Method [8,9] makes use of the relation betweentheinverseofthermodynamiccorrectionfactorandthe fluctuationinparticlenumberN.Forasurface,therelationis
1 =
N2−N2 N T,,A (2) Fluctuationsaresampledinsmallopensystems(disks) with areaAinsideareservoir.Thereservoiriscreatedasalarge rect-angularboxwithperiodicboundaryconditions.Thetemperature, T,andthechemicalpotential,,inthereservoir arecontrolled. Thethicknessofthesamplingsystemissettothethicknessofthe surface(seebelow).Theareaofthesamplingsystemisvaried, vary-ingtheradiusofthedisk,L.Thesmallestradiususedissosmall thatitallowsonlyonemoleculeinsidethedisk;thelargestradius contains20–30molecules.Theinversethermodynamicfactorisa linearfunctionofthe1/L[11–13]inaparticularrange,tobefound foreachcase:1 = 1 ∞,s
1+B L (3) HereBisasmallsystemspecificconstantandsuperscript∞means thevalueinthethermodynamiclimit.Byextrapolatingthelinear regimetothethermodynamiclimit,weobtainthewantedquantity ∞,s.Lateronweuses=∞,sforsimplicity.Thechemicalpotentialofagasadsorbedtoasurfaceinalayer iis: s i= 0,s i +RTlna s i= 0,s i +RTln s i Cs i C0,si (4) http://dx.doi.org/10.1016/j.cplett.2014.08.026
Here 0,si is thestandard chemical potential, as is the
(dimen-sionless)activityoftheadsorbedphase,Cs isthesurfaceexcess
concentration,andsistheactivitycoefficient.Thestandardstate
is thehypothetical idealstate havings=1 atlayer saturation,
C0,s (giveninparticlesper(nm2)).Theentropyfollowsfromthe
standardrelationSs=−(ds/dT)andtheenthalpyofthelayerfrom
Hs i=
s i+TS
s
i. Weshallfindtheseproperties fortheadsorption
(1).Totalsurfaceexcessconcentrations(adsorptions)aredefined accordingtoGibbs[14,15]
Cs=
∞0
(C(z)−Cg(˛)(z−˛))dz (5)
whereC(z)andCgaretheconcentrationsofadsorbedmolecules
andofmoleculesinthegasphase,respectively.Theintegrationis carriedoutfromtheequimolarsurfaceofgraphite(atz=0)tothe bulkgasphase(z=∞).TheHeavisidefunction,,isbydefinition unitywhentheargumentispositive,andzerowhentheargument isnegative.Fordefinitionoflayerconcentrations,seeSection3.The thermodynamicfactorisalsodefinedby:
s=1+
∂
lns∂
lnCs T,A (6) WecandeterminetheactivitycoefficientbyintegratingEq.(6) fromzeroadsorption,oncethethermodynamicfactorisknown fromtheSmallSystemMethod.Thisgives s 1 dlns= Cs 0 (s−1)dlnCs (7)WhenCs→0,thereisnointeractionbetweenparticles,meaning
thats=1.Wealsohave
s−s=
s s ds=RT Cs Cs sdlnCs (8)meaningthatwecanfindthechemicalpotentialatany adsorp-tionrelativetoareferencestate(indicatedby)fromthisequation. Weshallusethisrelationtodeterminethestandardstate chem-icalpotential0,si byplottingthelefthandsideofEq.(8)versus ln(s
iC s i/C
0,s
i ),extrapolatingtothestatewherethisexpressionis
zero.
3. Simulationdetails
ThesystemconsistedofsheetsofgraphiteandCO2molecules.
Thegraphitewasmadefrom5sheetsof graphenewithoutany defects.We orientedthesheets in theboxsuchthat thesheet surfaceswereperpendiculartothez-axis.Thedistancefromthe graphitesurfacewasmeasuredalongthisaxis,takingthe equimo-larsurfaceofgraphiteaszero.Thegraphitelayerswerefixedin space,stillyieldinggoodresultsforadsorptionanddiffusionofgas onthesurface[16,17].Arigidbodymodel,TraPPE,wasusedfor CO2 [18].TheintermolecularpotentialbetweenCO2–CO2 wasa
shiftedandtruncated12-6Lennard–Jones(LJ)potential[19]with long-rangeCoulombinteractions,whichweredealtwithusingthe Ewaldsummationtechnique[19].TheinteractionbetweenCO2and
theC-atomsofgraphitewassimilarlydescribedbyaLJpotential. Detailsofparametersforthesimulationweregivenearlier[16]. Theyhavebeenconfirmedtoyieldanaccurateadsorptionenergy forCO2ongraphitesurface[16].
Classicalmoleculardynamics(MD)simulationswereperformed usingtheLAMMPSpackage[20].Asnapshotofthesystemisgiven in Figure1,showing graphiteat 500K withCO2 ina relatively
densegasandinanadsorbedstate.Periodicboundaryconditions wereusedforthereservoirinalldirections.Thesimulationwas donewithtime steps of 0.001ps. The initialconfigurationwas
Fig.1.SnapshotshowingCO2inthegasphaseatafluid-likedensityandadsorbed
onagraphitesurfaceat500K.ThenumberofCO2particlesinthesystemwasNCO2=
2800.Thegreenandredcolorsrepresentcarbonandoxygenatoms,respectively.
(Forinterpretationofthereferencestocolorinthisfigurelegend,thereaderis
referredtothewebversionofthisarticle.)
constructedby randomlydistributing CO2 molecules above the
graphitesurface.Thesystemwasstabilizedduring2000psbyruns withconstantNtotVtotTusingNosé–Hooverthermostats[21].
InordertochecktherangeofvalidityofEq.(3),thereservoir sizewasvaried.Thereservoirhastobelargeenoughcomparedto thesamplingsystem.Forahardspheresystem,wefoundthata suitablereservoirhadalength20timesthehardsphereradiusL [12,13].Simulationboxsizesof(a=42 ˚A,b=54 ˚A,c=84 ˚A),(2a,2b, c),and(3a,3b,c)weretested.Thelargestsystemsgaveidentical results,sobox(2a,2b,c)wasused.
Weperformed2000psrunsinareservoiratthermal equilib-rium,varyingLfrom1.3to20 ˚A,samplingrandomly30disksacross thegraphitesurface.Thetotalnumberofframeswas10000.Hence, thevalueofsforeachLwasobtainedfromthestatisticsof300000
samples[11,13].Thesamplingwasdonefortemperaturesranging from300Kto550K,andforanumberofCO2particlesinthebox,
varyingfrom200to2800(correspondingtoapressurerangeof 1–60barat300K).
4. Resultsanddiscussion
4.1. Adsorptions
Wedescribefirsthowwefindtheadsorptions Cs
1 andC2s for
eachlayer.ThetotaladsorptionisthenCs=Cs
1+C2s.The
adsorp-tion(excessconcentration)ofCO2wasfoundusingtheresultsin
Figure2withthedefinition(5).Thefigureshowsthedensityof CO2 moleculesasafunctionofthedistancetothegraphite
sur-face,andisaquantificationofsnapshotsliketheoneshowedin Figure1.WeobserveinbothfiguresthatCO2canformtwolayers
onthegraphiticsurface.InFigure2,weseealayeraroundthefirst peakwhichextendsfromthegraphitesurfacetoposition␣,while asecondpeakextendsfrom␣to.WerefertotheintegralinEq. (5)duetothefirstpeakasthebottomlayeradsorption,whilethe correspondingintegralrelatedtothesecondpeak,iscalledthetop layeradsorptiononthegraphite.Thepositionofthefirstpeakat 5 ˚Acoversapproximatelyonemolecularlayer,asthelengthofthe moleculeis5.4 ˚A.Thesnapshotshowsthatmostofthecarbon diox-idemoleculesarelyingparalleltothesurface.Thisgivesaheight morelikethediameterofanoxygenion,3.6 ˚A.Athicknessof5 ˚A canbeinterpretedtoincludesomemoleculeswhicharestanding slightlytiltedwithrespecttothesurface,andsuchmoleculescan alsobefoundbyvisualinspectionofFigure1.Itisinterestingthat thepositionofplane␣isalwaysnear5 ˚A,independentofthe tem-perature.Thiscanreflectthatmoleculesareeitherlyingorstanding
Fig.2.ThedensityofCO2moleculesasafunctionofdistancetothesurfaceina
reservoirwithNCO2=2800.Thetemperaturesare500Kand350K.Wedistinguish
betweenthreezones,from0to␣:firstadsorbedlayer,␣to:topadsorbedlayer,
above:gasphase.Thebottomlayerextendstoaround5 ˚A.Thethicknessofthe
toplayerislargerat350Kthanthatat500K.
inthefirstlayer.Theattractiveforcesofthegraphite,notbeingable toreachabovethelayer,seemtobecentralforthislayer.Butthe factthatthetoplayerstartstobefilledbeforethebottomlayeris full,motivatesadivisionofthewholesurfaceintotwolayers.The toplayer,whichextendsfrom␣to,appearsalsoratherdifferent fromthefirst.WeseefromFigure2thatthepositionoftheplane varieswithtemperature,unlikethepositionofplane␣.Forthe sys-temwith2800CO2molecules,issmallerat500Kthanat350K.
Thetoplayeristhusmorediffuse.Fewattractiveforcesareableto keepthemoleculeswithinthissurfacelayer,whenthemolecular kineticenergybecomeslarger.TheadsorptionofCO2ongraphiteis
alwayshigheratlowtemperatureinbothlayers,meaningthatthis kindoftrade-offbetweenkineticandpotentialenergiesappliesto bothlayers.
Wefindthatthebottomlayerhasalwaysmore thanhalfof thetotal adsorption, independentof temperature (not shown). Thefractionislarger,thelowerthetemperatureis,butdoesnot exceed0.9.Thefractiondecreaseswithincreasingtotaladsorption, becausethebottomlayerbecomessaturated,whilethetoplayer keepsgrowing.Fullcoverage(maximumadsorption)ofthe bot-tomlayerisobtainedat300KwithC10,s=12.5(molecules/nm2).
Wethereforechoseasstandardstate,theidealstatewithC10,s= 12.5(molecules/nm2), corresponding to0.31 CO
2 moleculeper
surfacecarbonatom.
4.2. Thethermodynamiccorrectionfactor
Resultsfortheinversethermodynamicfactor(s)−1were
plot-tedversus 1/L for the top and bottom layers separateand for theircombination (notshown).Thecurvesapproached unityas expected,when1/Lwasincreased.Thisisthesmallsystemlimit, whichhasatmostoneparticleinthesamplingsystem.Inorderto findthethermodynamiclimitvalue,weappliedlinearregression topointsintheinterval0.1<1/L<0.4andextrapolatedthelineto largeL.Theregionusedforextrapolationcoincidedwiththeregion foundearlier[11,13].
Thethermodynamiclimitvalueoftheinversethermodynamic correctionfactor(s)−1wasplottedasafunctionoftheadsorption
ineachsinglelayer,andinthecombinedlayers,forall temper-atures.AtypicalexampleisshowninFigure3forT=500K.The bottomlayerhadalwaysthesmallest(s)−1,whilethetotallayer
hadthebiggestvalueof(s)−1.Wefoundthat(s)−1decreased
more or less linearly with the adsorption. The results for the
Fig.3.Thermodynamiclimitvaluesfor(s)−1inthetop,bottomandtotalCO2layer
ongraphiteat500K.Astraightlineisfittedtotheresultsandforcedthrough1on
they-axis.
bottomlayerandthetwolayerscombined(thetotal layer) fol-lowedthestraightlinenicely,whilethescatterofresultsaround thelinedrawnforthetoplayerwaslarger.
Allcurvesmustextrapolatetoathermodynamiccorrection fac-torequal1,whentheadsorptiongoestozero.Thiswasfoundthe relationbetween(s)−1ofthetotallayerandthetotaladsorption
wasquitelinear.Theobservedlineardependenciesmeanthatthe inversethermodynamicfactorofthetotallayer,canbefoundby addingcontributionsfromthebottomandtoplayers.
4.3. Theactivitycoefficientsforcarbondioxideinthesurfaces Asetoftypicalactivitycoefficients,obtainedat500KfromEq. (7),areshowninFigure4.Thecoefficientsapproach1asexpected atlowdensity,somewithmorenoisethanothers.Theincreasein thecoefficientforthebottomlayerislargerthanforthetoplayer andthereforelargerthanforthetotallayer.Thisreflectsthatthe moleculesarefurtherapartinthetoplayerthaninthefirst,making repulsiveforceslessrelevantinthetopthaninthebottomlayer. Themoleculesdonotadsorb,unless thesurfacebindingenergy canovercometherepulsion,however.Thetotallayeractivity coef-ficientwasexpressedasafunctionoftotalsurfaceadsorptionat differenttemperatures,witharegressioncoefficient0.99orbetter: s
i =1+aCis+b(Cis) 2
(9)
Fig.4.Activitycoefficientofbottom,topandtotallayerasafunctionofthelayer
Table1
ParametersthatdescribethetotallayeractivitycoefficientintheempiricalEq.(9).
Theregressioncoefficientwas0.99orbetter.
T(K) b a 300 0.0060 0.0005 350 0.0059 0.0054 400 0.0055 0.0066 450 0.0059 0.0233 500 0.0057 0.0320 550 0.0067 0.0216
Fig.5. ChemicalpotentialofCO2onagraphitesurfaceasafunctionofln(sCs/C0,s)
atdifferenttemperatures.ThestraightlineisfittedtoEq.(4).
ParametersaandbaregiveninTable1.Theseresultsmaybe usefulforthermodynamicmodelingofthetotalCO2adsorbedona
graphitesurface(Fig.5).
4.4. Thechemicalpotentialofthesurfaceadsorbedgas
Thechemical potentialof theadsorbed staterelative tothe chemicalpotentialatthelowestadsorptionwasfoundfromEq. (8). The chemical potential difference for the total layer was plotted vs the right hand side for the different temperatures used.UsingtherelevantactivitycoefficientandC10,s=C20,s=C0,s=
12.5molecules/(nm2), we next used Eq. (4) to plot the same
data.Theslope ofthelinear fit gaveRTas expectedwithgood accuracy.Thestandardstatevalue,0,s,wasfoundforeach
tem-peraturefromthiscurvesettinglns i(C
s i/C
0,s
i )=0. Forthetotal
layer,weobtained0,s(T0)=−7.6kJ/molat298K.Thetemperature
variationofthechemicalpotentialwasusedtofindthestandard entropy S0,s=10.6J(molK). It was constant in the temperature
intervalused.Thestandardenthalpyat298Kwasthencalculated toH0,s=−4.4kJ/mol.Dataforthetotalandseparatelayersaregiven
inTable2.
Inordertocheckthattheresultsfortheseparatelayerswere internallyconsistent,weexpressedthechemicalpotentialsofthe topandbottomlayersofCO2 byEq.(2).Atequilibrium,wehave
s
1=s2,wherethesubscriptdenoteslayernumber.Byintroducing
expression(2)intothisequilibriumcondition,weobtained
Cs 1 Cs 2 =
s 2 s 1 e(0,s2 − 0,s 1 )/RT (10)
By plotting the left hand side versus the ratio of activity coefficients,fittingtheplottoastraightline,wecalculated0,s2 − 0,s1 fromtheslopeasafunctionoftemperature.Thedifferencein thestandardchemicalpotentialswasconsistentwiththedifference obtainedfromthedatainTable2.
Thethermodynamicdatathatwehavedeterminedforthetotal layerofadsorbedgas,arereasonable.Thestandardchemical poten-tialandtheenthalpyarebothnegative,indicatingthatadsorption is favorable in the standard state,in spite of a largereduction in the entropy from the gas phase tothe surface, a reduction whichislargerthanthatfromthegastotheliquidstate.Wehave furthermoreseenthatwecandistinguishbetweentwoseparate thermodynamically defined layersof carbondioxidewithin the wholelayeronthegraphitesurface.Eachlayerhasitsown ther-modynamicproperties.WeseefromTable2,thatthebottomlayer entropyisrelativelysmallcompared tothegasentropyofCO2.
Infactitcancomparetothecarbonentropyinagraphitelattice. ThenegativeentropydifferencerepresentedbytheorderingofCO2
whenitisadsorbedmustbeovercomebyarelativelylargeenthalpy foradsorptionintothelayer.Thetoplayerentropyislargerthan theentropyofthebottomlayer.Itisnotgas-like,butfourtimes higherthanthatofthebottomlayervalue.Thislayercantherefore bestabilizedwithasmallerenthalpy.Thetotallayerpropertiescan besaidtomaskthepropertiesofthesinglelayers,asthetotallayer hasstandardentropyclosertothetoplayer,andanenthalpymore likethebottomlayer.Informationoftheseparatelayersobtained fromthesimulationwillthereforeaddinsighttothesystem.Such insightcannotbeeasilyobtainedbyexperiments,asitisdifficult todistinguishbetweenthelayersinanadsorptionexperiment.It ishoweverrathersimpletocompareanexperimentallyobtained adsorptionisothermtotheadsorptionisothermderivedherefor thetotaladsorption.
5. Conclusion
WehaveshownthatarecentlydevelopedSmallSystemMethod canbeusedtocalculateaconsistentsetofthermodynamicdatafor surfacesfromoneMolecularDynamicssimulation.Forcarbon diox-ideadsorbedtographite,wedeterminedthechemicalpotential, theactivitycoefficient,theentropyandenthalpydirectly.Closer inspectionofdensityprofilesrevealedthatwecanspeakoftwo, notonelayerofadsorbedgas.Thethermodynamicanalysesreveal adistinctionbetweenthelayers.Thegashaslargerentropyinthe topthaninthebottomlayer,ismoremobileinthislayer.Thetwo layersareinequilibriumwithoneanother,meaningthata lower-ingoftheentropycantakeplace,iftheenthalpycancompensate forthechangeinentropywhenatopparticlemovestothebottom layer.Suchinformationisinvaluableinthemodelingand expla-nationofsurfaceprocesses.Extensionstoothersurfacesshouldbe straightforward.
Table2
ThermodynamicdataforstandardstateadsorptionofcarbondioxideatagraphitesurfaceatT=298K.Theuncertaintyinthedeterminationsisontheaverage3%.
Correspondingvaluesforgraphiteandcarbondioxidegasarealsogiven.
T=298K Totallayer(thiswork) Bottomlayer(thiswork) Toplayer(thiswork) Graphitea CO2gasa
0,s i (kJ/mol) −7.6 −9.8 −5.1 – – S0,s i (J/molK) 10.6 4.1 13.7 5.74 213.78 H0,s i (kJ/mol) −4.4 −8.6 −1.0 1.05 9.36
Acknowledgments
TheauthorsacknowledgeTheResearchCouncilofNorwayRCN projectno209337andTheFacultyofNaturalScienceand Technol-ogy,NorwegianUniversityofScienceandTechnology(NTNU)for financialsupport.ThecalculationpowerisgrantedbyThe Norwe-gianMetacenterforComputationalScience(NOTUR).ETHZürichis thankedforguestprofessorshipstoSKandDB.
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