Folge,
Transport
of
Carbon
in
Nonisothermal
Low Pressure
Nitrogen
Plasma
By
S. Veprek
Institute ofInorganic Chemistry,
University
ofZürich Rämistrasse76, Zürich, SwitzerlandWith 3figures (Received January 29, 1973)
Zusammenfassung
Kohlenstoffkonnte mit Stickstoff in einem nichtisothermen
Niederdruck-plasma einer
Hochfrequenzentladung
transportiert werden. Der Transporterfolgte
inRichtung
abnehmenderPlasmaenergie
beiTranslationstemperaturen
vonetwa1000°C.Eine Diskussion der
Elementarprozesse
und einVergleichmittheoretischen
Vorstellungen
liefert tiefere Einblicke in dieVorgänge
bei derchemischenVerdampfungund
Abscheidung
fester StoffeunterdenBedingungen
einesnicht isothermenPlasmas.Abstract
Carbon has been
transported
withnitrogen
ina nonisothermallow-pressure
plasmaofa
highfrequency discharge.
Thetransportproceedsin the direction ofdecreasing plasma energy at a translational temperature of about 1000°C.
A discussion of
elementary
processes anda comparisonwiththeory
leadsto adeeper insight
intothe processes of chemicalevaporationanddepositionofsolids under nonisothermal plasmaconditions.1. Introduction
Chemical
transport
reactions1 are well known methods for thegrowth
ofcrystals
and thin films from the gasphase.
The use ofnonisothermal
plasma*
makestransport
possible
also insystems
in* For further information about this kind of
plasma
see 2 and referencesmentioned there.
1H. Schäfer, Chemische
Transportreaktionen, Verlag
Chemie,Weinheim/
S. Veprek
which it is otherwise hindered
kinetically
orthermodynamically
(without
aplasma).
In an earlierpaper2
we have demonstrated thekineticeffect ofa weak
discharge
by
thetransport
ofcarbonaccording
to the Boudouard's reaction and the
thermodynamic
effect of anintense
highfrequency low-pressure discharge
insystems
which arestrongly
exothermic without theplasma (such
asTiN/Cfa, AIN/Cl23
and
C/H2, C/O22).
In this paper we shall show how a nonisothermalplasma having
ahigh
energy content can shift chemicalequilibrium
of a
strongly
endothermic reaction in such a way that chemicaltransport
becomespossible
at atemperature
ofthe solid at which itwould be
quite impossible
underthermodynamical equilibrium
con-ditions. The
system
carbon-nitrogen
seems to be very suitable for this purpose in view of itssimplicity,
sufficientknowledge
of theelementary
processes involved and thepossibility
of acomparison
with
transport
in othersystems
likecarbon-hydrogen
andcarbon-oxygen2.
Several results of this
study
have beenalready
mentioned in ourprevious papers2-4.
In thisarticle,
a shortdescription
of theexperi-ments
along
with a discussion ofelementary
processes in thesystem
under consideration will be
given.
The
carbon-nitrogen
system
has been studied underplasma
con-ditone
by
a numberof authors5-18. Because ofinsufficient information 2 S.Veprek, Second Int. Conf.VapourGrowth &Epitaxy,
Jerusalem 1972,J.Cryst. Growth 17 (1972) 101.
3 S.Veprek, C. Brendeland H. Schäfer,J. Cryst. Growth 9 (1971) 266. 4 S.Veprek,J. chem.
Physics
57 (1972) 952.5M.Möhren,
Compt.
Rend. (Paris)48(1859) 342.6Modern Aspects of
Graphite Technology,
ed. L.Blackman, Academic Press, London 1970.7 F. K.McTaggart, Plasma Chemistry in Electrical
Discharges,
Elsevier,Amsterdam 1967.
8A. Wright and C. Winkler,Active
Nitrogen,
AcademicPress,New York1968.
9R. Baddour and R.Timmins, The
Application
of Plasmas to ChemicalProcessing,
M.I.T. Press,Cambridge
(Massachusetts) 1967.10G. Glocker and S. Lind, The
Electrochemistry
of Gases and otherDielectrics,J.
Wiley,
New York 1939.11C. Fink andD.Wroughton,Trans, electrochem. Soc. 88 (1945)25. 12H.Goldstein, J.
physic.
Chem. 68 (1964) 39.13H.v.Wartenberg, . anorg. Chem. 52 (1907) 299.
"C. Stokes and W.Knipe,Ind.
Engng.
Chem. 52 (1960) 287.isT.Wallis,Ann. Chem. 345 (1906) 353.
about the
experimental
conditions(basic
plasma
parameters)
acom-parison
of differentexperiments
is difficult orquite
impossible
inmost cases. There are two
important
kinds ofexperiments
which have to bedistinguished:
Experiments
in ahigh
temperature
plasma
(arc-discharge, plasma jet)
and in a "cold"plasma (glow-
andhigh-frequency low-pressure discharge).
Thepresent
paper deals witha nonisothermal
low-pressure plasma
of an intensehighfrequency
discharge.
Itwillbe
shown,
that,
when the inner energy of theplasma
reachesa value of about 100
kcal/mole
and the translationaltemperature
liesclose to 1000°
C,
thetransport
of carbon takesplace
in the direction of lowerplasma
energy, 2 ->(see
sect.3).
Under theseconditions,
the energy in the translational
(and
also rotational andvibrational)
degrees
of freedom ofheavy particles
(about
5kcal/mole)
is much lower than the energy in the electronical ones(about
100kcal/mole).
Therefore,
the usual chemicalthermodynamics
as well as the linearirreversible
thermodynamics
are not valid here. Also thegeneral
thermodynamic theory
ofstability
cannotbe used in itspresent
form19asthe
assumption
of localequilibrium
is violatedalready
in individualmolecules.
Only
asimple
statistical model of chemical reaction undernonisothermal
plasma
conditions4 can be used forprediction
ofchemical
transport
today.
2.
Experiments
The
experimental
arrangement
isschematically
shown inFig.
1. Thehighfrequency discharge
takesplace
between theouterelectrodes 2 and 2' in a silica tube 1(inner
diameter R = 37mm).
Thehigh-frequency
output
ofgenerator
3(type
Philips
PH1202/00)
may beadjusted
between 0 and 1.2kW at thefrequency
of 80MHz. The h.f. current is measuredby
aspecial
amperemeter
14. The gas flowand the total pressure in the
discharge
tube areadjustable by
meansofneedlevalve
5,
vacuumvalve 6 androtary
oilpump 4. Thepressurein tube 1 is measured
by
McLeod- and oil-manometers 7. Coldtrap
8prevents
apenetration
of oil- and mercury-vapour into theplasma.
Pure
nitrogen
with a total oxygen- and water-traces below 0.5ppmhas been usedin all
experiments.
« M.Berthelot,
Compt.
Rend. (Paris) 95 (1882) 955; 145 (1907) 354. 18 K.Peters,Naturwissenschaften 19 (1931) 402.19P. Glansdorf and I.Prigogine,
Thermodynamic Theory
of Structure,StabilityandFluctuations,
Wiley,
London 1971.98 S. Vepbbk
Fig.1. Experimental arrangement for the transport of carbon in nitrogen plasma. Description see text. The length scale to be
applied
only for thedis-charge
tubeSpectral
puregraphite
tube 9(Ringsdorff Company,
diameters15/8
mm)
isplaced
in nickelinlay
10. Thetemperature
ofthegraphite
surface inside tube 9 is measuredby
anoptical
pyrometer
through
orifice 11. Because of the
non-equilibrium
radiation ofplasma
under theseconditions,
direct measurement of surfacetemperature
is notpossible
in the activedischarge.
Comparable
measurements of thetemperature
ofthegraphite
surface inside tube 9 and in borehole 11 afterswitching
off thedischarge
show that the difference between both values are smaller than 40° at atemperature
of about 900°C.Experiment
No. I50—100mg carbon are
transported
per hour from the inside ofgraphite
tube 9 into the silicainlay
12 at a total pressure of 1Torr,
a gas flow of about 100Torr
cm3/sec
and a h.f. current between2 and 4A. The
temperature
of thegraphite
surface reaches a valuebetween 950 and 1000°C in the tube 9 and about 800°C in zone a and b of silica
inlay
12.Discharge
tube 1 is isolated with asbestos(heat-isolation)
15 on the left of electrode 2'.Fig.
2 shows the carbondeposited
inzone ofinlay
12(cf.
Fig.
1).
Thereis
large
amount ofsootdeposited
inzone a and a small amountin zone c on the left of the electrode 2'. No paracyanogen
(CN)X
hasbeen found in the carbon
deposited
under these conditions(IR-
andmass
spectrometry).
The amount of
transported
carbon increases withincreasing
h.f.Fig.2. Carbon
deposited
in thezone6 ofFig.
1.A) surface in contactwith thesubstrate (silica), B) growth surface, C) a cut through the
layer. Scanning
electron
microscope
(stereoscan) picture; 1500Xtemperature
of theplasma
increasesimultaneously3'20.
The variations of thetemperature
of the carbon surface in tube 9 are smaller thanthe accuracy of its measurements.
Experiment
No. IIThe
graphite
tube 9 and the nickelinlay
10are shiftedto electrode 2' and heat isolation 15 is removed(cf.
Fig.
1).
The distance between electrode 2' and nickelinlay
10 is about 5 mm. The total pressure,gas flow and h.f. current are
kept
at the same value as before. Thereis a
mingling
ofcarbon(soot)
and paracyanogendeposited
onthe leftof electrode 2'. The material
deposited
in zone c contains morepa-racyanogen than material of zone d
(IR-
and massspectrometry,
habitus).
Experiment
No. IllThe
arrangement
of thedischarge
tube isshowninFig.
3.Graphite
rod 17
(diameter
13 mm,length
35mm)
is fixed with silica stick 1620S.Veprbk, Dissertation,
University
ofZurich, 1972.100 S. Vepèek
Fig.
3. Experimentalarrangement forexperiment
No. III.Description
see textin the middle of
discharge
tube 1. The h.f.discharge
takesplace
between electrodes 2 and 2'. The inner diameter of thedischarge
tube around thegraphite
rod may be variedby
inserting
silica tubes 18. Thepressure, gas flow and h.f. currentare thesame asinexperiments
No. Iand II. Neither
transport
ofcarbon,
nordeposition
ofparacyano-gen takes
place
withoutinlay
18. If theinlays
18 are mounted intotube
1,
deposition
of carbon in zone d and of paracyanogen in zone c is observed. The smallest inner diameter of theinlay
used aroundgraphite
rod 17 was 25 mm.Experiment
No. IVThe
graphite
rod from theprevious experiment
isnowfixed in themiddle of a
discharge
tube with the diameter of 100 mm. Thetem-perature
ofgraphite
is measured with a gas thermometer. AWrede-Harteck gauge
(cf.
e.g.7,
p.76)
is used formeasurement of thedegree
ofnitrogen
dissociation in thedischarge.
At the total pressure of1.35 Torr and h.f. current of 6.3
A,
agraphite
temperature
of 590°Canda
degree
ofdissociationof about50%
arefound20. Thetemperature
ofthetube wall lies between 200 and 300°C.
Under these
conditions,
about 1.5 mg carbon perhour reacts withnitrogen,
and paracyanogen isdeposited
on the wall of thedischarge
tube between the electrodes. No
deposition
ofcarbon canbe observedin this
experiment.
The reaction rate increases withincreasing
h.f.current. At the same time also the
temperature
ofgraphite
in-creases(e.g.
up to 630°C at the h.f. current of 10A).
The reaction is not observable when thetemperature
ofgraphite
is too low(e.g. 300°C)
although
adegree
of dissociationhigher
than20%
isfound20.
In all
experiments
careful efforts have been made to excludetraces of
humidity
from thereacting
system.
No HCN has been detected in carbon and paracyanogendeposited
in theseexperiments
3. Discussion
A
comparison
ofexperiments
No.I,
III and IV shows that bothhigh
energy content andhigh
translationaltemperature (resp.
thetemperature
of carbon in thestarting
zone)
are necessary for theformation of cyanogen.
Experiment
No. II indicates that the "carboncarrying species"
during
thetransport
is the cyanogen monomer CN(cf.
also 21).
Thelargest
part
of the inner energy oftheplasma
cor-responds
to the dissociation energy when thedegree
ofdissociation ishigher
than about50°/o.
Thus,
thedegree
ofdissociation may be usedas a
rough
measure of theplasma
energy under these conditions.The dissociation of
nitrogen
increases with anincreasing
ratio h.f.current vs. tube
diameter,
I/R3'20.
Because of thecontinuity
of theelectric
current,
theI/R
ratio islarger
ingraphite
tube 9(see
Fig.
1)
than in silicainlay
12. Carbon is thentransported
in the direction of lowerplasma
energy 2-* .We shall now discuss the
elementary
processesoccuring
in theplasma.
The reaction of carbon with molecularnitrogen
Gs
+
Ì
2 ß
^CHg
(1)
is
strongly
endothermic( °2
= 109kcal/mole
22)
and asignificant
concentration of cyanogen arises under
thermodynamical equilibrium
condition in the gas
phase only
at veryhigh
temperature.
It has beensuggested
that theratedetermining
step
inthecarbon-nitrogen
reac-tion is the
adsorption
ofV2
ontwoadjacent
carbon atoms(23,
p.194).
Because of the
high
dissociation energy of thenitrogen
molecule,
the reactionproceeds
with asignificant
rateonly
above 2000°C. There is also some evidence that the CH moleculeleaving
the carbon surfaceis
electronically
excited( 2
state)24.
The
transport
of carbonproceeds
in thedischarge according
tothe reaction
(2).
0.
+
1/ ·, * ß.
(2)
Here,
N*>g
stands fornitrogen
in aplasma
state with ahigh
energycontent. The necessary
energies
of theN*>g
species
participating
in21C. Haggartand C.Winkler, Cañad. J. Chem. 38 (1960) 329. 22JANAF Thermochemical Tables, US Nat. Bur. Stand., second
edition,
NSRDS-NBS 37 (1971).
23Gmelins Handbuch der
anorg. Chemie, Bd. 14, Dl,VerlagChemie,
Wein-heim/Bergstr.
1971.102 S. VepSek
reaction
(2)
have to beequal
to orhigher
than AH° of reaction(1).
Moreover,
for the chemicalequilibrium
of reaction(2)
tobeestablished,
thereaction has to be fast.We will now discuss the nature of the
particles participating
in reaction(2).
Considerstarting
from theplasma
state with a lowcon-centration of cyanogen which does not disturb the
composition
ofdischarge
in purenitrogen
significantly.
This low concentration canoriginate
either from a low value oftheplasma
energy or from a lowtranslational
temperature (see later).
Of the molecular
species arising
in thenitrogen low-pressure
dis-charge
with asignificant
concentration there arepredominantly
mole-cules in the
ground
( 1
+)
and the metastable( 3
+)
states. Theground
statecan bevibrationally
excitedtoseveraleV,
butthehigher
levels have short relaxation times. Therelatively high
concentration of vibrational excited molecules in thenitrogen afterglow
of the microwavedischarge
(about
30%25 Corresponds predominantly
tothe first vibrational level
( 1
ß+,
= 126)
having
a mean life timeof about 50 msec at 1 Torr under the
experimental
conditions. Theenergy released
by
the deactivation of thevibrationally
excitedspecies
was found to beonly
about 2kcal/mole
25.Highfrequency
discharges produce
quite
small amounts of vibrational excited mole-cules and also the vibrational deexcitation may beexpected
to be fasterin activedischarge
than in theafterglow
(e.g.
the deactivation ofvibrationally
excited02
in collisions with atoms can be two ordersof
magnitude
faster than in collisions with molecules 27). Then,
theground
electronic state ofmolecules canbe assumednot toparticipate
inthe reaction
(2).
The metastable
N2
( 3
,+)
canarise inrelatively high
concentra-tionsinthe
plasma,
but itsenergy(6.17
eV for =0)
isnot sufficientforthe formation of GN molecules. This process may
perhaps
be fea-siblethrough
some surface reaction underparticipation
of more ofsuch
species,
but because of a short life time of the( 3
+)
state(radiative
life time between 10~4 and 10~2 sec8,
pp.96—97)
it seemstobe
improbable.
Theothermolecularspecies
have veryshortradiative life times(10~6—10~8 sec)
and will notplay
anysignificant
role.25 F.Kaufman and J.Kelso, J. chem.
Physics
28 (1958) 510. 26 K.Dressler, J. chem. Physics30 (1959) 1621.27 R.
Gordon, W.Klemperer and J. Y.Steinfeld, in Annual Review
of
Phys.
Chem., Vol. 19, ed. H.Eyring, G. BantaComp.
Inc., Palo AltoNitrogen
Generally,
it seemslikely
that any molecular excitedspecies
will bedeactivated at the surface of a solid rather than
undergo
a chemicalreaction withit.
The situationbecomes
quite
different ifatomicspecies participate
in reaction
(2).
Thereare theground
stateA(4£)
and the metastablesN(2D)
andN(2P)
which havelong
radiative life times of 26hours and 12 secondsrespectively
(8,
p.82—83).
The deactivation of the metastablespecies proceeds predominantly through
collisions with the wall or otherspecies.
Reaction(2)
isweakly
exothermic[AH°W&
=—4
kcal/mole
22),
with atomicnitrogen
in theground
state and it becomes much more exothermic when the metastablesparticipate.
In the active
discharge
innitrogen
a veryhigh degree
of dissociation canbe obtained at the pressure of 1 Torr(cf.
3·20).
At a lowerdegree
of dissociation of
nitrogen,
theground
state(*8)
willpredominate
but the concentrationof metastables[mainly
N(2D)]
becomessignifi-cant ata
degree
of dissociation closeto one[e.g.
only 1/500
ofnitrogen
atoms are metastable in the
afterglow,
but about5—20°/o JV(4$)
atoms occur in the
discharge
in a mixture ofnitrogen
with inertgas
8,
p.82]
At 1
Torr,
the atomsdisappear
eitherby
recombination on thewall and to a lower extent in the gas
phase
orby
reaction(2).
Thevalue of the recombination coefficient of
nitrogen
onquartz
is of theorder of 10~3—10~4
(8,
p.170)
and leads to a mean life time of theatoms of the order of lO^1—10^2 sec. The recombination coefficient
changes relatively
little withtemperature (activation
energy between0 and 2
kcal/mole).
We do not know any value for the recombination coefficient ofnitrogen
ongraphite.
Measurements of surfacetempera-tures of different solids in
nitrogen plasma
indicate that therecom-bination of
nitrogen
atoms on the carbon surface is slower than onquartz.
Especially
athigher
temperatures (900
°K)
thecatalytic
heating
of the carbon becomes lower and itapproaches
the value ofa
quartz
surface"poisoned"
withHPO3
20.The reactionrateofatomic
nitrogen
withgraphite
canbe calculatedfrom the values of the activation energy and
entropy
of about18.5
kcal/mole
and —2.7cal/mole deg
respectively
as measuredby
Goldstein12. These data
give
theprobability
of reactionCs
-\-Ng-+CNg
for anitrogen
atomstriking
the carbon surface of about 2.7 · 10~5 at890° and 1.8 · 10~4 at 1275
°K,
whichseems to be very low for
setting
upthe chemicalequilibrium
of the reaction(2). However,
two factors have to be accounted for when the reactionproceeds
in an104 S. Veprek
active
discharge*
:First,
the excited atoms may beresponsible
for thehigher
reaction rate incomparison
with the reaction outside theplasma.
Second,
for thesetting
up of the chemicalequilibrium
of reaction(2)
the ratio of the reactionprobability
to the recombination coefficient is more decisive than the absolute values are. The surfacerecombination takes
place
between an atomstriking
the surface andanotherone
being
adsorbed there(e.g.28·30).
Thus,
ifthedesorption
ofCW-radicals from the surface
increases,
the surface recombination ofatoms will decrease.
(A
similar effect has been observed alsoby
re-combination of
nitrogen
atoms on a nickel surface at atemperature
ofabout
1000°C31).
The measurements of the surface
temperature (see above)
and thecomparison
ofthe amount oftransported
carbon with the value calculated from Goldstein's data(see
4,
Tab.l)
show that the reaction ofatomswith carbon is faster than its surfacerecombinationat a
high
temperature.
What is therate
determining
step
in the reactionCs
-+-
Ng
-*CNgl
At a carbon
temperature
up to 800°C this reactionproceeds slowly
(cf.
41)
in purenitrogen,
but the formation of HCNproceeds
quickly
when asmall amountofhydrogen
is added32·33. The decreaseof the
catalytic efficiency
of the carbon surface for thenitrogen
recombination athigher
temperature
in theplasma
suggests
thatthe
nitrogen
atoms arestrongly
chemisorbed on the surfaceand the slowest
step
is thedesorption
of the CNspecies
from the surface.This molecule canleave the surface
by
being electronically
excitedinto the
( 2
)
or( 2
+)
states(cf.
24 and34),
but in view of theirshort radiative life times
(3.5
· 10~6sec and 8.5 10~8secrespective-ly23),
theground
state( 2
+)
of CN willpredominate
in the gas* Goldsteinsmeasurementhas been done under conditions hotsolid-cold
gas. Due to the thermal accomodation of the gason the hotsurface, the
re-action rate is lower undersuch conditions than inour case ofequal
tempera-tures.
28 Handbuch der
Katalyse,
Vol.IV, ed. G.Schwab,Wien 1943.29Chemical Reactions in Electrical
Discharges,
ed. .Blaustein, Adv. Chem. Ser. 80,Amer. Chem. Soc,Washington
D.C. 1969.3»F.Kaufman, in 29,
p. 29—47.
si N.Buben and A.Schechter, Acta
physicochim.
URSS 10 (1939) 371.32W.Zinman, J. Amer. chem. Soc. 82 (1960) 1262. 33M. Coulon and L.Bonnetain,
Compt.
Rend. C 269 (1969) 1469.Nitrogen
phase.
Also a very fast collisionalquenching
of these states hasto beaccounted for
(cf.
quenching
of Bfi+ 35).
The other
species occuring
in theplasma,
e.g. short livedhigh
excited atoms and molecules as well asions,
can influence the overallreaction
rate,
butthey
do not contribute to the energy balance of thesystem
significantly
and can beneglected
in this consideration.TheCN molecule in the gas
phase
caneitherdecompose
orundergo
collisions with other CN
species
andpolymerize.
These processes will be considerednow. Thedecomposition
canproceed
eitherby
electronimpact
orby
collisions with otherheavy
species
or on the wall.A
simple
assessment shows that in theplasma
underconsideration,
the mean life time of the CN molecule
being decomposed only by
electron excitation is 10~2—10~3 sec or
longer
4.(The
dissociationenergy of CN molecule is found to be between 7.86eV 23 p.
11,
and8.1 eV
36.)
Because of the low vibrational
temperature,
thedecomposition
of CN in the gasphase
canproceed only by
reaction suchas*CNg
+
Ng^ N2,g
+
Cg (AH
= -47kcal/mole).
(3)
Using
the value of 4 1013 cm3 mole^1 for the reaction rate at atem-perature
ofabout8000°K37 andanactivation energy of about25kcal/
mole
(lower
limit),
a mean life time of more than 10~2 sec can beexpected
for CN in the above reaction. Thedecomposition
may be fasteratthe wall of thedischarge
tubeathigh
temperature (23,
pp.65 to66)
aswellasby
ion-molecule reactions in the gasphase
(homogeneous
condensation).
These estimations lead to the conclusion that CN isa stable
species
in the gasphase
underplasma
conditions and itsdecomposition by
electrons is slower than its formation on the wall.This is in
agreement
with our observation thatonly
paracyanogen wasdeposited
onthe wall in thedischarge
zone attemperatures
lowerthan 800°C
(see
exp. No.IV).
Nodecomposition
to theelements,
butonly polymerization
was observed alsoby
other authors in thelow-* The dissociative deexcitation
CNg
-f Xg*->Cg
+ Ng + Xg has been discussed in38.35W. Jackson and J.Faris, J. chem.
Physics
56 (1972) 95.36B.Darwbnt, Bond Dissociation
Energies
inSimple
Molecules, US Nat.Bur.Stand., NSRDS NBS 31 (1970).
37M. Slack andE.
Fishburne, J. chem.
Physics
56 (1972) 95.38S.Veprek,H. R. Oswald andW.Peier,Z. angew.Math.
Physik
[Basel]106 S. Vefrek
pressure
discharge
in cyanogen(CN)2
(23,
p.67).
Thepolymerization
of CN to(CN)X
occurs in the gasphase
and can be acceleratedby
ions
(23,
pp. 22 and67).
The reverse reaction(CN)2,g-+ 2CNg
has ahigh
activation energy of 95—125kcal/mole
(23,
p.5)
and may beomittedhere.
From the
point
of view of the above discussion thetransport
of carbon innitrogen plasma proceeds by
thefollowing
steps
:g>
+
nb
'2> °
~* cn 2 > <800° >1200°(CN)*,,
Cs
+
\N2,g
T is the translational
temperature
and theplasma
energy. Thereac-tion
Cs
+
N(*S)
^CN(X*
+)
(5)
AHlm
= —4kcal/mole
is
weakly
exothermic and the chemicalequilibrium
is shifted to theright (log Kp
âî3 at 1300022),
but itssetting
uprequires
ahigh
temperature
of solid carbon in zone 2.This is illustrated
by
acomparison
of the amountofcarbontrans-ported
at different translationaltemperatures
with theoreticalpre-dictions
(see
4,
Table1).
If thetemperature
is too low(e.g. 890°K),
the formation of CN on thegraphite
surfaceaccording
to eq.(5)
proceeds slowly,
whereas at ahigher
temperature
(e.g.
1275°K)
it isfast. The theoretical considerations4 are based on the
assumption,
that the chemical reactions under
plasma
conditions are faster thanother processes of energy
dissipations.
Onecan seefrom thecomparison
mentioned
above,
that the theoreticalpredictions
andtheexperiments
agree better athigher
translationaltemperature.
This is animportant
limitationof
applicability
of thestatistical model4aswellasthe methodof
simple
energydiagrams2,
and it is asubject
ofour furtherpaper38.
4. Conclusions
Transport
ofcarbon takesplace
inanonisothermalnitrogen plasma
along
agradient
ofdecreasing plasma
energy when thedegree
ofdissociation and the translational
temperature
reachhigh
values in the"starting
zone". The discussion ofelementary
processes shows that the formation of gaseous CN radicals occursby
the reaction ofNitrogen
nitrogen
atoms with solid carbon. The translationaltemperature
of theplasma plays
animportant
kinetic role inthis reaction.We have shown in an earlier
paper2
how it ispossible
topredict
the direction of chemical
transport,
as well as the relative amount ofplasma
energy necessary for chemicaltransport
to takeplace
ina
plasma.
According
to the statisticalmodel4,
simple
energylevel-dia-grams can be used for this
prediction (cf.2).
The exactplasma
param-eters necessary for chemicaltransport
to takeplace
in asystem
ofinterest havetobe found
experimentally.
According
to ouropinion,
thisprocedure
can be arelatively
favourable
approach
inplanning
furtherexperiments
forcrystal
growth
andpreparation
of thin filmsby
the use of a nonisothermallow-pressure plasma.
Acknowledgment
The
experimental
part
of this work has been doneby
the authorat the Institute of