NBSIR 73-338
CALCULATED LIQUID PHASE THERMODYNAMIC PROPERTIES AND
LIQUID-VAPOR EQUILIDRIA FOR
Cryogenics Division
Institute for Basic Standards
National Bureau of Standards
Boulder, Colorado 80302
September 1973
Final Report
Prepared
for:
The National Aeronautics and Space Administration
Lewis Research Center
-Ciei^land, Ohio
/oo
(JLSU
/fl3
44135
1
NBSIR 73-338
CALCULATED LIQUID PHASE THERMODYNAMIC PROPERTIES AND
LIQUID-VAPOR EQUILIBRIA FOR
FLUORINE-OXYGEN (FLOX] MIXTURES
W.
M.
R.
J.
Parrish
Hiza
Cryogenics Division
Institute for Basic Standards
National Bureau of Standards
Boulder, Colorado 80302
September 1973
Final
Report
Prepared
for:
The National Aeronautics and Space Administration
Lewis Research Center
Cleveland, Ohio 44135
U.S.
DEPARTMENT OF COMMERCE.
NATIONAL BUREAU OF STANDARDS
Frederick B. Dent, Secretary
Richard
W
Roberts Director
CONTENTS
1.
INTRODUCTION
i
2.
CALCULATION METHODS
3
3.
RESULTS
8
4.
ACKNOWLEDGMENTS
10
5.
REFERENCES
11
TABLES
13
^-
A-1
13
A-2
14
*B-1
21
*B-2
22
The thermodynamic properties given
thermochemical BTU = 1054. 35J.
iii
in
these tables are based on the
CALCULATED LIQUID PHASE THERMODYNAMIC PROPERTIES
AND LIQUID-VAPOR EQUILIBRIA
FOR FLUORINE-OXYGEN (FLOX) MIXTURES>;=
W. R, Parrish and M.
J,
Hiza
Cryogenics Division
National Bureau of Standards
Boulder, Colorado 80302
ABSTRACT
Liquid phase thermodynamic properties and liquid
vapor equilibria of fluorine-oxygen mixtures, for which no
experimental data exist, have been calculated. The results
are based on excess properties predicted from the SniderHerrington equations, with an adjusted combining rule, and
the corresponding data for the pure fluids. Mixtures con-
sidered are
of fluorine
0. 6,
0. 7,
from
55 to
0. 8,
0.
90K up
88, and 0. 9 weight fraction
to 70 x 10
Pa. In the com-
pressed liquid, molar volumes, enthalpy, entropy, and
constant pressure specific heat were determined. Along
the saturation boundary, coexistent vapor compositions
and solution vapor pressures were determined as well.
Corresponding properties of pure fluorine from experimental data have also been included. Results are tabulated
in both British and S.I. units.
Key Words: Calculated properties;
enthalpy; entropy;
mixtures; hard- sphere
model; liquid-vapor equilibria; specific heat; volume.
liquid; fluorine; fluorine-oxygen;
1.
INTRODUCTION
Liquid mixtures of fluorine and oxygen are potential candidates
for oxidizers in chemical rocket propulsion systems.
is
As such, there
a need for thermophysical properties of selected mixtures over a
range of temperatures and pressures, for which experimental data do
not exist.
It is
the
purpose of
this study to
provide the "best" calculated
mixture properties within the current state-of-the-art.
*This study was carried out at the National Bureau of Standards under
the sponsorship of the National Aeronautics and Space Administration.
To predict
liquid
the
thermodynamic properties and phase equilibria
mixtures reliably,
it is
some
essential at
of
point to introduce
appropriate numerical data on the components of the mixture and on the
nature of the unlike molecule interactions.
The latter information
is
generally obtained by evaluating some experimental data on the fluid
mixture, not necessarily on the property of interest,
inadequacies of the combining rules.
the
property of interest, preferably
to
account for
Calculations can then be
in
made on
regions where some data are
available to assess the degree to which the real mixture values are
reproduced.
Recent work on hard-sphere perturbation models has resulted
at least
in
one set of relatively simple equations for liquid mixtures, i.e.
,
which represent the correct tem-
the Snider-Herrington equations [1],
perature dependence of thermophysical excess properties.
Staveley
[2]
showed that results calculated from these equations compare much better
with newer data than with
some
of the data originally
This led Miller, Kidnay, and Hiza
equations
to the infinite dilution
system with marked success.
ment
to
dict
Henry's constants for the neon-krypton
the adjust-
account for the inadequacy of the combining rule for the energy
it
unnecessary
tion on the unlike
for a
apply the Snider-Herrington
In these latter calculations,
parameters was consistent with
making
[3] to
used by the authors.
number
the correlation of
to sacrifice
experimental data
molecule interactions.
of other
Hiza and Duncan
Miller
[5]
to obtain
[4],
informa-
also demonstrated that
systems, the deviation parameters needed
to
pre-
mixture properties with the Snider-Herrington equations are consis-
tent with those obtained
from independent gas phase
most part are properly represented
in
correlation.
2
data,
which for the
magnitude by the Hiza-Duncan
Fluorine -oxygen mixtures are particularly intriguing in the above
context, since appropriate data are not available to determine the inade-
quacies of the combining rules nor
to
determine the reliability
However, accurate data for
calculations.
and oxygen[7], are available.
If
the
of
any
pure fluids, fluorine
[6j
one can postulate something about the
nature of the unlike molecule interactions,
fluorine -oxygen mixture properties
from
it is
the
possible
pure
obtain liquid
to
properties data
fluid
and the excess properties determined with the Snider -Her ring ton equations.
Though
is
not available, previous experience with comparable oxygen systems
can be applied
sible
molecule
To model
it
the desired information for fluorine -oxygen interactions
to this
in
problem, since oxygen appears
to
be the respon-
exceptions encountered in the correlation effort
the fluorine -oxygen
must be assumed
system
[4].
after other simple oxygen systems,
that fluorine is well-behaved, and that the
mixtures
formed are purely physical solutions.
In this study, the
argon-oxygen system was used as
estimate an adjustment to the geometric
mean combining
the
model
to
rule for the
characteristic energy parameter of the fluorine -oxygen system.
Fluorine-
oxygen liquid mixtures containing 0,6, 0,7, 0.8, 0.88, and 0.9 weight
fraction of fluorine and pure fluorine
calculations
90K.
from
the saturation
were considered
boundary up
to 70
in the
x 10
5
present
Pa from
55 to
The properties determined were molar volume, enthalpy, entropy,
Along the saturation boundary, the
and constant pressure specific heat.
coexistent vapor phase compositions and solution vapor pressures were
determined as well,
2,
CALCULATION METHODS
The equations used
in these calculations are well
documented; thus,
only the specific logic and unique features of the present calculations are
included here.
3
The form
of the equation of state of
upon which the mixture equations
Pv/RT
where
^ = p /v
and
term represents
=
[(1
P is the
+
^
of Snider
+
f )/(l
-
Longuet-Higgins and
and Herrington are based
?f
]
(a/RTv)
-
1
hard- sphere volume, (—
6
NA
3
TT
r
).
[8],
is:
(1)
The second
a uniform attractive potential field.
Assuming constant "a" and "3" parameters implies
figurational
Widom
= 0.
that the con-
Recently, Blinowska, Herrington, and Staveley
[9]
have taken into account the fact that these parameters are not constant
over a range of temperatures.
To avoid evaluation
of
temperature and
density dependencies in the present calculations, the parameters "a" and
"P" were evaluated
interest.
from
the pure fluid properties at each
temperature
of
The "a" parameter was evaluated from the configurational
internal energy (the configurational internal energy of an ideal gas
zero); thus, "P", the hard-sphere
volume
is the
is
only unknown in equation
(1).
In applying their equations. Snider and
molar G
Herrington used the equi-
(excess Gibbs energy) at one temperature
of the cross
determine the value
Sacrificing mixture data in any
parameter, "a
the present calculations
to
was not possible.
form
in
Thus, a different scheme had
to be devised.
In correlating deviations
for the characteristic energy
from
the
parameters
equation was developed:
4
geometric mean combining rule
[4j,
the following empirical
where
component with
is the
=
(1
defined as:
(3)
characteristic potential energy parameter.
is
1
(2)
is
-kj^) (Uo, U^^)'/'
cipated that the deviation parameter k
comparing predictions
In
the subscript one denotes the
The parameter k^^
the larger value.
Uoi2
where Uq
eV and
ionization potential in
is the
I
^
It is
anti-
always positive.
of the deviation
parameter from equation
with observed values for oxygen systems specifically, equation
consistently over-predicts the magnitude of k
effective ionization potential for oxygen,
served value of 12.08 eV [10],
is
This suggests that an
.
J.
w
somewhat larger than
necessary
to
(2)
make
the ob-
the predictions for
oxygen systems consistent with experiment.
The ionization potential for fluorine
almost the same as that for argon,
that,
in the fluorine -oxygen
15. 79
is
15.70
15. 94
-
eV
-
15. 83
[12].
eV[ll],
If
one assumes
system, fluorine will be well-behaved and
oxygen can be blamed for the unusual behavior noted above, the argonoxygen system can be used as a model system for the fluorine -oxygen
system.
This
is
precisely the assumption
made
in the
present
calculations
In the
where "r"
combining rule used by Miller, Kidnay, and Hiza
is the
hard-sphere diameter, a k
of
0.015 was selected for
^
the fluorine
-oxygen system by examination of the equimolar G
argon-oxygen liquid-vapor equilibria data
[3]
E
from
[4],
Since the liquid-vapor equilibria data for argon-oxygen are well
represented by the two-suffix Margules equation [13], this framework
5
was used here
phase
to establish the liquid
total
vapor pressure and the
vapor composition of the fluorine-oxygen system.
excess Gibbs energy and the activity coefficient
and y ^, are related
to the liquid
of
sense, the
In this
each component,
phase mole fractions, x^ and x^,
with a single constant. A, by
=
A
x^ x^
RT
In
RT
In Y
(5)
2
A
=
(6)
A
^21
2
x^
=
(7)
The standard expression for the activity coefficient
RT
In
RT
In Y2 =
=
RT
In (y^ P/x^po^) + (B^^
RT
In
(y2P/x2 P02) +
can then be related to equations
unknowns,
i.e. the solution
mole fraction, y
where
22
(6)
v^^) (P
~ ^""2^
and
(7)
each component
Py^
p^^) +
-
"
^02^ +
to obtain
h
(8)
^^1^2
^"^^
two equations in two
vapor pressure, P, and the vapor phase
+y^
(y
-
of
= 1).
B
,
v
and Po
.
>
and the
corresponding terms with a subscript two, are the pure component
second virial coefficient, saturated liquid molar volume, and vapor pressure respectively.
is
6
J.
an excess interaction second virial coefficient
Ld
term defined by
'
=
6
12
2B
-
B
12
-
II
B
22
The second virial coefficients were calculated using
6
(10).
B (T/T
)
=
^
y]
V
-
C
C
c
1
i
=
(l-i)/4
(T/T
B.
(11)
)
l
are the reduced form of the fitted polynomial coefficients B
where B
i
of
i
pure fluorine second virial coefficients given by Prydz and Straty
The relationship between the two sets of coefficients
[6],
is
v(l-i)/4
B.
r
=
c
(12).
V
1
c
Since the reduced polynomial coefficients for pure oxygen are essentially
parameter corresponding
identical to those for fluorine, i,e„ two
states is satisfied, the values of
for fluorine
B.''~
were used.
To obtain
1
from equation
B
J.
^
mixing rules were used
the following
(11),
cl2
c
2
c2
cl
^
^'^^
'
and
T
T
c
equal
with a value of k
1
The value
^
=
cl2
to
(1
-
k
)
12
(T
T
clc2
of the constant
Snider-Herrington equations.
the
(14)
0.015.
A
in equations (5),
evaluated at each temperature from the equimolar
from
)1/^
G
(6),
E
and
(7)
was
calculated
from
the
All pure component parameters were taken
experimental data [6,7].
7
RESULTS
3.
The properties
were deterrained
of interest
temperature in both British and
liquid phase compositions at each
The properties along the saturation boundary and those
units.
compressed
liquid are given in
S.
units in tables
I.
The corresponding properties
ively.
B-1 and B-2.
of the
for the selected
All calculations
S.
I.
in the
A-1 and A-2, respect-
in British units are given in tables
were done on
a
molar basis, though some
properties are given on a weight basis for the convenience of the
Fluorine and oxygen molecular weights of
intended user.
respectively,
32, 00,
were used
38. 00
and
in these conversions.
The mixture molar volumes, enthalpies, and entropies are the
algebraic
sum
from
contribution.
M is
of the
pure component prop-
the excess property of the mixture cal-
the Snider -Herrington equations,
and the ideal mixing
This relationship is simply expressed as
Mm
where
mole fraction average
from experiment,
erties taken
culated
of the
=
M
X
1
+ x^M^ +
1
2
+ M^^®^^
(15)
'
2
^
the property of interest, the subscript
and the superscript E denotes excess.
The
m
denotes mixture,
last term,
the ideal mixing
contribution, is zero except for entropy and thus Gibbs energy, the ideal
entropy of mixing being -RI^x. In
the mixture,
it
was assumed
In calculating the heat capacity of
x..
that the excess heat capacity is zero.
The
pure fluorine properties for the compressed liquid listed here have been
corrected for a computational error in the original internal energy and
enthalpy values given in reference
correct as given„
were
Revised thermophysical properties tables for fluorine
have been prepared by G.
soon.
the saturated liquid properties
6;
The reference
Straty and L. A.
state for the pure
erties is the ideal gas at zero K.
8
Weber and
will be published
component thermodynamic prop-
is
It
worth noting that the saturated liquid mixture densities
(more correctly, specific weights), reported graphically by Schmidt
from "proportional interpolation"
from
significantly
the values
[14]
pure fluid properties, differ
of the
determined
in this study.
It is
clear that
Schmidt's values were determined by weight fraction averaging of the
weights per unit volume of the pure saturated liquids.
Thus, his mixture
values are not consistent with the traditional definition of an ideal liquid
mixture,
%
70 weight
mole fraction average
approximately
is
4% due
1.
to nonideality
same pure
method
15)
1.
of
4%
For
to the
0.
2.
a
2% lower than the corresponding value
4% due
to the difference in
two different methods
of
pure fluid properties
averaging, and
0.
considerations accounted for in the present study.
fluid properties
were
4% due
If
the
used, for this mixture, Schmidt's
averaging results in a negative excess molar volume (equation
of the ideal
excess volume
0.
4%
The validity
assessed in the
while the present calculations result in a positive
of the ideal.
of the calculated results given
final analysis by
two kinds of data
at a single
requirement.
T
-
here can only be
comparison with appropriate experi-
mental data, which are not available
this
molar volumes.
This difference can be accounted for in three
this study (Table B-1).
parts (approximately):
used,
of the
fluorine mixture at 140R, the saturation specific volume taken
from Schmidt
from
the
i. e.
at the
present time.
At a minimum,
x point for the liquid mixture can satisfy
These are precise values
of the solution
vapor pressure
and the saturated liquid excess molar volume for the equimolar liquid
mixture
at a single
temperatures
of the
temperature, preferably far removed from the critical
pure components.
An
additional piece of experimental
data which is desirable, but not absolutely necessary, is the vapor phase
composition in equilibrium with the equimolar liquid solution.
9
Without
this information,
it
is
hoped that these results are
a significant
raent over values of the subject properties obtained by simple
improve-
mole
fraction averaging of the pure fluid (molar) properties.
4.
ACKNOWLEDGMENTS
Support
of this study
by the National Aeronautics and Space
Administration
is gratefully
acknowledged.
G. C. Straty and L. A.
pure fluid properties
Weber
for providing
of interest.
10
The authors wish
to
thank
computer programs for the
REFERENCES
5.
1.
N. S. Snider and T.
J.
2.
Chem, Phys.
R. C. Miller, A.
J.
4.
M.
_53,
J.
3136 (1970).
Kidnay, and M.
4,
J.
Hiza
807 (1972).
Hiza and A. G. Duncan
J.
J. j_6,
733 (1970).
R. C. Miller
J.
6.
2248 (1967),
Chem. Thermodyn.
AIChE
5.
47,
L. A. K. Staveley
J,
3.
Chem. Phys,
M, Herrington
Chem. Phys.
55,
l6l3 (1971).
R. Prydz and G. C. Straty
Nat. Bur. Stand. Tech. Note 392 (October 1970).
7.
R. D.
McCarty and
L. A.
Weber
Nat. Bur. Stand. Tech. Note 384 (July 1971).
8.
H. C. Longuet-Higgins and B.
Mol. Phys.
9.
8,
Widom
549 (1964).
A. Blinowska, T, M. Herrington, and L. A. K. Staveley
Cryogenics 21, 85 (1973).
10.
K.
J.
11.
Watanabe
Chem. Phys.
26,
542 (1957).
A. W. Potts and W. C. Price
Trans. Faraday Soc. 67, 1242(1971).
12.
D.
W. Turner, C. Baker, A. D. Baker, and C. R. Brundle
Molecular Photoelectron Spectroscopy [John Wiley, London, 1970].
13.
J.
M. Prausnitz
Molecular Thermodynamics
Hall,
14.
Englewood
Cliffs,
of
New
Jersey, 1969], see pg. 194.
H. W. Schmidt
NASA SP-3037
Fluid-Phase Equilibria [Prentice
(1967).
11
TAB-E A-1.
TEMPERATURE
THERiOOYNA'^IC PROPERTIES OF LIQUID FL UCR IN' E-0
ON THE SaTJRATION POUNOARY
WT. FRACTION F2
PRESSURE
V0LU1E
ENTHALPY
X
YG EN
MIXTURES
ENTROPY
p
J/MOL-
MCL-K
3
lO^PA
LIQUID
0. 6000
0.70 00
55.0
0.
1.0000
60.0
0.
0.
0.
6000
7000
8000
0.8800
0.90 00
1.
65.0
7
0.0
75.0
0000
5.0
1. .
85
5
1.
.
31.
.
5?
22.7 U
22.be
22.^1
5
5
1.
1.
.
1.1.
5 I. .
51..
1.7
,
i
.9329
1.1000
0
0
0
. 0
.
0 38<*
0 0 38 7
0
.
OOi^O
1
726
C. 01299
0. 01367
0. 011.32
0.9212
0. 011.81
0
.
7521.
3.^132
0
.
8
0. 9333
1. 1000
.
C
1
55
3.81.
3.61
39
75. 58
63
^666.69
70.92
67.
51.
21..
21..
2 8
51.1 9.60
79. 95
0
•51.01
.21
le
78.98
3.15
23. IC
03996
569 2. 3
5575.2:
15
22.82
2
0
Tgi.?. 16
66
51.. 01
51.. If5 1. . 3 1
51.. 1*3
51.. 1.6
23.36
0.011.93
C
2
2
^935.
5935.6
0 2
1
5661.. 51.
-5661 . 32
-5661 .3?
71..
59
7 3. IC
7 1. 1.3
1 8
.
62
8 711.
0
38 00
90 00
J
.
^21
0. 01.552
0. 01. "^89
0. 01.769
2
3.39
23.5 3
2 3.25
^•3 81.. 7 9
-5381.. 50
5388.31
51
75. 36
75. 36
71.61.
0 . 10 326
0. 10853
0. 11 356
C . 11 71.1.
0. 11839
0 . 12 302
21.. 75
21.. 5 1
511.5.
81+.
01
83.
81.
79.
79.
75.
07
62
99
51.
51.
51.
51.
1.9
51.. 39
80
55.10
87. 81
86. 89
85. 1.7
8 3. 35
8 3. 36
79. 69
51.. 70
51*
5 1.
.
71.63
0.8130
1.0003
0.6000
0
0. 70 00
0.3 059
0.8000
3
.
.
71.32
3691.
0. 3800
0. 9000
1.00 00
0.920 3
0. 9332
0. 6000
0. 7000
0
0.8000
0.8800
1.3 030
.7333
Q.
0. 01.20 3
.
3.3670
0. 25511*
0. 26373
P. 26583
.
25.78
0.51308
0,53008
0 .
.
25.5 5
5.30
25.0 8
25.0 2
0.1.9116
2
.531.26
0. 551*73
0
0
.
86232
.
0
90 31.2
9003
72J8
7932
3625
0.9170
0. 9337
0.
3
1.0033
1.3 030
1.
0.
0.7151*
0.
0.
0.7896
1.0000
76
0. 1.6837
6000
0.7003
SOOO
8800
9000
21*.
7267
7971
1.3 030
6000
0.7000
25.2 5
2 5.01
21.1.01*
.361.6
1.0000
6000
7003
8003
0. 8800
0. 9000
1.0000
3.71
0.27612
9192
0.9130
3.9315
0. 8000
0. 8803
2
21*. 55
21*. 1.9
2 1..2 0
.
3.9323
1.3030
0
0
2i..2fc
21.. 05
21.. 0 0
0. 2321.6
0
3
23. 3C
01.1.0 1
0.3011*
0. 6003
0. 7000
0. 8000
0. 8803
0. 9000
0.
0.
0.
22.9'.
1.2
7 7
1.0
3
.
0.
95.0
5
69.
66.
66.
66.
62.
0.9357
1.3030
0.
90.0
70.86
•59'.7.
693 7.
3
0.
8
•596 3.^7
23.19
0
1.0000
0.0
? 3.1.
0. 00355
0. DC 372
6000
7003
8000
0. 90 00
8
0.00338
l't6
721*
>)
8000
9000
J/MOL
,756?
0.8800
0.
/10L
CM
.
53 8 9.
5106. 29
5105.65
-5107.68
•1.869.
1.81*8.
-1.832.
•1.825.
1.821..
73
26
93
87
88
1.825.
0 7
1.592, 60
1.569. 39
1.552, 15
91, 39
90, 1*9
1.51. 3
,
51.
87,
1*9
1.51.2
.
1
6
01
36
73
•1.51*0,
38
26.35
26.12
-1.31 3.
57
91..
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27
FORM NBS-114A
(«-7l)
DEPT. OF COMM.
U.S.
1.
BIBLIOGRAPHIC DATA
PUBLICATION OR REPORT NO.
AnaCTr)
n
i
o
IN ijoiK IJ-JJO
-i
SYi££j
2.
Gov't Accession
^
i
Calculated
Liquid Phase Thermodynamic
Properties and Liquid-Vapor Equilibria for Fluorine -Oxygen
4.
TITLE
iiiLt AINU
AND SUBTITLE
suDiiiLt
i
i
.
9.
AUTHOR(S)
Recipient's Accession No.
5.
Publication Date
September 1973
t.Pctlotmiag Organization Code
(FLOX) Mixtures
7.
3.
-3
n Parrish
u and
j i.^
W. R.
M.
-,,r
•
-r
J.
8.
ttHiza
PERFORMING ORGANIZATION NAME AND ADDRESS
NATIONAL BUREAU OF STANDARDS
DEPARTMENT OF COMMERCE
Boulder, Colorado
12. Sponsoring Organization
,
SUPPLEMENTARY NOTES
16.
ABSTRACT
Project/Task/Work Unit No.
11.
Contract/Grant No.
2750547
Purchase Req.C-32369--C
80302
13.
Center
Type of Report & Period
Covered Final
Nov
21000 Brookpark Rd.
Cleveland, Ohio 44135
15.
10.
Boulder Laboratories
Name and Address
NASA Lewis Research
Performing Organization
14.
(A 200-word or less factual summary of most significant information.
bibliography or literature survey, mention it here.)
If
'72 -- Sept '73
%>onsoring Agency Code
document includes
a significant
Liquid phase thermodynamic properties and liquid-vapor equilibria of fluorine-
oxygen mixtures, for which no experimental data exist, have been calculated.
results are based on excess properties predicted
tions, with an adjusted
55 to 90
K
up
the Snider
-He rrington equa-
combining rule, and the corresponding data for the pure fluids.
Mixtures considered are
from
from
The
to 70
0
.
6
0.7, 0.8, 0.88, and 0. 9 weight fraction of fluorine
,
x 10
5
Pa.
In the
compressed
liquid,
molar volumes,
enthalpy, entropy, and constant pressure specific heat were determined.
Along the
saturation boundary, coexistent vapor compositions and solution vapor pressures
were determined as well.
Corresponding properties
data have also been included.
17.
KEY WORDS
Results are tabulated
(Alphabetical order, separated by semicolons)
of
pure fluorine from experimentkl
in both British and S.I. units.
Calculated thermophysical properties;
compressed
18.
liquid phase, fluorine -oxygen mixtures, hard-sphere model;
liquid-vapor equilibria.
21. NO. OF PAGES
19. SECURITY CLASS
AVAILABILITY STATEMENT
(THIS REPORT)
[3n UNLIMITED.
I
I
FOR OFFICIAL DISTRIBUTION. DO NOT RELEASE
TO NTIS.
UNCLASSIFIED
20.
SECURITY CLASS
22. Price
(THIS PAGE)
UNCLASSIFIED
USCOMM-DC 66244-P7I
USCOMH
tRl.