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Submitted on 1 Jan 1982
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Evidence of production of H2CN+-N2. Application to
the atmosphere of Titan
C.V. Speller, M. Fitaire, A.-M. Pointu
To cite this version:
C.V. Speller, M. Fitaire, A.-M. Pointu. Evidence of production of H2CN+-N2. Application to the atmosphere of Titan. Journal de Physique Lettres, Edp sciences, 1982, 43 (14), pp.499-503. �10.1051/jphyslet:019820043014049900�. �jpa-00232082�
Evidence
of
production
of
H2CN+
-N2.
Application
to
the
atmosphere
of
Titan
(*)
C. V.
Speller (**),
M. Fitaire and A.-M. PointuLaboratoire de Physique des Gaz et des Plasmas (***), Université Paris-Sud, 91405 Orsay Cedex,
France
(Re~u le 23 avril 1982, accepte le 1-juin 1982)
Résumé. 2014 La molécule
H2CN+-N2
est mise en évidence dans un mélange N2-CH4 soumis aurayonnement alpha d’une source radioactive. La constante d’équilibre est mesurée et la valeur de
l’enthalpie de la réaction a été déterminée
(|
0394H0|
= 7,65 ± 0,09 kcal.mole-1).
Abstract. 2014 The molecule
H2CN+-N2
has been observed in a mixture of N2-CH4 irradiated byalpha particles from a radioactive source. The equilibrium constant has been measured and the
enthalpy of the reaction has been calculated
(|
0394H0|
= 7.65 ± 0.09 kcal . mole-1).
Classification
Physics Abstracts 82.30 - 96.30M
1. Introduction. -
Titan,
thelargest
satellite ofSaturn,
is one of the smallestobjects
in the solar system to have anatmosphere.
Evidence ofcomplex
chemicalphenomena
arising
in thisatmosphere
is of greatinterest,
both incosmochemistry
and inexobiology.
This concernsparti-cularly
chemical processes involved in the formation ofprebiotic
molecules,
probably
similarto those which could have acted in the
primitive
earth’satmosphere.
Infrared measurements
performed by
VOYAGER Ishow
that Titan’satmosphere
ismainly
composed
of molecularnitrogen
(~
90%) [1]
and methane( ~
5%).
Small amounts ofH 2,
C2H2,
C2H4,
C2H6,
C3Hg
andC4H2 produced by photolysis
ofmethane,
have beendetected,
and also nitriles :
HCN,
C2N2
andHC3N [2],
which are ableto
play a
fundamental role in theformation of other
prebiotic
molecules.Moreover,
it is reasonable to presume that morecomplex
organic compounds
are also present in Titan’satmosphere,
suchas
CH3CN,
C2H3CN,
C2HSCN
and,
maybe,
nitriles ofhigher
order[3, 4].
~ ,
Probably three-body
association reactions aremainly
involved in thesynthesis
of such nitriles[3, 5]
in Titan’s loweratmosphere :
infact,
high
pressures and low temperatures arepropitious
conditions,
while ionization results from cosmic raysimpinging
on theatmosphere. Among
allthe ions able to
play a
role,
H 2CN +
isprobably
of greatimportance :
it isassumed
to beres-ponsible
for HCN formation[6],
while further more it can be combinedwith
moleculesN ~,
(*) La version française de cet article a été proposee pour publication aux Comptes Rendus de 1’Academie des Sciences.
(**) Supported by C.N.Pq. and CAPES (Brazil). (***) Associated with the C.N.R.S.
L-500 JOURNAL DE PHYSIQUE - LETTRES
CH4
andC2H2
toproduce compounds
such asCH3CN, C2H3CN,... through three-body
reactions.
Until now,
only
little information is known about chemical reactionsinvolving
such ions.Figure
1 illustrates somepossible
schemesleading
toH2CN+
formation in Titan’satmosphere
[3, 6].
In thefollowing,
we shall present results oflaboratory
measurementsconcerning
the for-mation ofH2CN+-N2
fromH2CN+.
Fig. 1. - Schematic
diagram of N + ion-molecule reactions with CH4 and N2 leading to production of
H2CN+.
2.
Experimental
device. - Anexperimental
set up has beendesigned
to allow the observation of ionsproduced
invariable,
relatively high
pressure and low temperature gas( 1
to 700 torr, 10 to 300K)
from lowactivity alpha
sources(2 41
Am,
40IlCi/cm2).
Ionsresulting
fromprimary
ionization are
subjected
to collisions with neutralspecies
which lead to formation of severalsecondary
ionicspecies.
These are extracted from the gas chamberthrough
a small hole(diameter
0 =
50~m),
then driven to aquadrupole
mass spectrometer(MS)
acting
as an ionanalyser.
A cryostat allows one to vary the gas temperature which is measured
using
an AsGaprobe
situated in the gas chamber. The neutral gas
composition
is determinedby
means of a secondMS downstream from the
extracting
hole.3.
Experimental
results and discussion. 2013Figure
2 shows anexample
of
a recorded spectrum in the caseof a N2-CH4
( ~
100 :1 )
mixture at a pressure p = 40 torr and a temperature T = 262 K.Amplitudes
ofm/e
= 28 and 56 observedpeaks
aremainly
duerespectively
toH2CN +
andH2CN+ -N2.
This has been shownby
substituting CD4
forCH4
in the sameproportion
mixture : the twoprevious
peaks
are then observed atm/e
= 30 and58,
andnothing
remains atm/e
= 28and 56 but low
amplitude peaks
attributed toN;
andN4 .
Theidentity
of these last ions has been confirmedsimilarly by
substituting
for mass 14nitrogen
anisotopic
mixture ofequal quantity
ofmass 14 and mass 15
nitrogen :
thepeak
corresponding
tomle
= 28 is thensplitted
into twopeaks
of
comparable amplitude
atm/e
= 28 and29 ;
thepeak
atmle
= 56,
whichimplies
threenitrogen
atoms, then appears at
m/e
=56, 57,
58 and 59.Such recorded
spectra
allow one to determine theequilibrium
constant[3] K 1 corresponding
to the reactionIn the
following,
we shall assume that reaction(1)
is reversible. This will be verified later.K,
isFig. 2. - Mass
spectrum in a mixture of
N2-CH....
BeyondH2CN+
andH2CN+-N2
ions, the probable chemical formula attributed for other detected ionic species are indicated (traces of hydrogen and of hydro-carbons (C2H6,C3Hø,
...) contribute for the production of some of the ionic species). With MS sensitivity chosen for spectrum clarity, the amplitude of theH2CN+-N2
peak is out of scale; this peak is thus shown with a MS sensitivity divided by ten for comparison with the other peaks.where brackets indicate densities of
corresponding compounds.
In ourexperiment,
the ratio ofionic densities is
equal
to the ratio ofpeak amplitudes
for masses 56 and28,
andnitrogen density
is
given by
the pressure measured in the gas chamber.Figure
3 shows variations ofLog K 1
as a function of T(Van’t
Hoffplot).
These variations arededuced from measurements at several
nitrogen
pressures and several molar fraction of methaneas well in the case
of CD4
or 15N.
One can observe a linear
variation,
independent
ofnitrogen
pressure in theregion
studied(20
to 80
torr)
andindependent
of the methaneproportion
(I
to 5%).
This indicates that athermo-dynamic equilibrium
is reached and that thereversibility assumption
is validPoints
corresponding
to measurements withCD4
deviatenotably
from the drawn line. This is due to oxygen, present in smallproportion
in the gas, which leads to formation of NO + ions withL-502 JOURNAL DE
PHYSIQUE -
LETTRESFig. 3. - Van’t Hoff
plot of the
H2CN+
+ 2 N2 #H2CN+ -N2
+ N2 reaction for a N2-CH4 mixture(~ 100: 1) : x ; 20 torr; 0, 40 torr; +, 80 torr ; 0, measured in N2 (m --fit 14 and 15)~CH~; CL measured
in,N2-CD4..
’ ~
..
,~
-
-... .
calculation
of K 1
erroneous.Complementary measurements
showthat
the
proportion
ofNO +
increases with
decreasing
temperatures and isnegligible
at room temperature. Thepoint
obtainedfor 300 K is thus the
only
one to be valid."
Another
point
can also beplotted
on theK
1 curve, deduced from a recorded spectrumusing
14 Nand’15N
mixture.Nevertheless,
itsprecision
isatso smaller
because it was necessary to add theamplitudes
ofthe four
peaks
ofions
H~CN~-N~
andthe two peaks
of ionsH2CN+
todeduce
theionic
densities ofinterest.,
.,..’,~, " ..
The standard
enthatpy,
A7~,
of reaction(1)
can beestimated,
using
the curveof K,
as drawnon
figure
3,
and
the relation - .’
’
, ,
R is the
perfect
gases constant and it is assumed that the variation in entropy,AS~,
is small in the range of studied temperatures(200-300 K).
Weobtain
0~° ~
I -
7.65 ±0.09 kcal.mole-1
(the
relative error is determined
using
statistic deviation from Van’t Hoffplot):
Such a value ofOH°
K 1
value at 150 K can be deducedby extrapolating
results offigure
3. We obtainK
1 = 2.95 x103 torr-1. If the value
k+
=10 - "
cm 6 . S - 1 is attributed[3]
to the constant of the forwardreaction,
leading
to the formation ofH2CN+-N2,
it is thenpossible
tocalculate,
using
ourK,
ivalue,
the reaction constant,k_,
for the reverse process. We obtaink I x 10
cm3 . s" ~ at150 K.
Besides the results
presented
above,
analysis
of spectra obtained at low temperature(T ~
150K)
for pressures around 40 torr, suggest that the ionH2CN+
can bepossibly
associated with severalnitrogen
molecules. Association of other ionicspecies
withN2
orCH4
is also evidenced in thesespectra. Ions of
global
formulaC2Hj, C3Hj, ...
have been detected and identifiedusing,
aspre-viously, isotopic
methane ornitrogen.
4. Conclusion. - Our results indicate that the reaction
H2CN+
+ 2N2 f:+
H 2CN + -N 2
+N2
is
possible
and can lead to formation of the ionH 2CN + -N 2
in Titan’satmosphere.
Equilibrium
constants of this reaction have been measured for temperatureranging
from 200 to300 K
allowing
one to deduce theenthalpy
(I
AH 0
1
= 7.65 ± 0.09kcal. mole - 1).
Furthermore,
existence of other
possible
association reaction ofH2CN+
ion withN2
or withCH4
has been shown. Such results are in agreement with someexpectations
pointed
out in a recentstudy
[3,
6].
References
[1] HANEL, R. A., et al., Science 212 (1981) 192.
[2] SAMUELSON, R. E., HANEL, R. A., KUNDE, V. G. and MAGUIRE, W. C., Nature 292 (1981) 686.
[3] CAPONE L. A., PRASAD, S. S., HUNTRESS, W. T., WHITTEN, R. C., DUBACH, J. and SANTHANAM, K.,
Nature 293 (1981) 45.
[4] MOUREY, D. and RAULIN, F., Nouveaux développements dans la connaissance du Système Solaire,
Joumée d’Etudes de l’ATP de Planétologie, I.N.A.G. (CNRS) Paris (1981) p. 98.
[5] ALLEN, M. and YUNG, Y. L., 13 DPS Meeting, Bull. Am. Astron. Soc., vol. 13/3 (1981) 702.
[6] CAPONE, L. A., DUBACH, J., WHITTEN, R. C., PRASAD, S. S. and SANTHANAM, K., Icarus 44 (1980) 72.
[7] KEBARLE, P., SEARLES, S. K., ZOLLA, A., SCARBOROUGH, J. and ARSHADI, M., J. Am. Chem. Soc. 89
(1967) 6393.
[8] CASTLEMAN Jr., A. W., HOLLAND, P. M., LINDSAY, D. M., and PETERSON, K. I., J. Am. Chem. Soc. 100