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 44135

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1
NBSIR 73-338

CALCULATED LIQUID PHASE THERMODYNAMIC PROPERTIES AND

LIQUID-VAPOR EQUILIBRIA FOR

FLUORINE-OXYGEN (FLOX] MIXTURES

W. R. Parrish

M. J. 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. Frederick B. Dent, Secretary

NATIONAL BUREAU OF STANDARDS 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 in these tables are based on the

thermochemical BTU = 1054. 35J.

iii

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 considered are 0. 6, 0. 7, 0. 8, 0. 88, and 0. 9 weight fraction

of fluorine from 55 to 90K up to 70 x 10 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 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;

liquid; fluorine; fluorine-oxygen; mixtures; hard- sphere

model; liquid-vapor equilibria; specific heat; volume.

1. INTRODUCTION

Liquid mixtures of fluorine and oxygen are potential candidates

for oxidizers in chemical rocket propulsion systems. As such, there

is 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 the thermodynamic properties and phase equilibria of

liquid mixtures reliably, it is essential at some 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, to account for

inadequacies of the combining rules. Calculations can then be made on

the property of interest, preferably in 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 in

at least one set of relatively simple equations for liquid mixtures, i.e. , the Snider-Herrington equations [1], which represent the correct temperature 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 used by the authors.

This led Miller, Kidnay, and Hiza [3] to apply the Snider-Herrington

equations to the infinite dilution Henry's constants for the neon-krypton

system with marked success. In these latter calculations, the adjustment to account for the inadequacy of the combining rule for the energy

parameters was consistent with the correlation of Hiza and Duncan [4],

making it unnecessary to sacrifice experimental data to obtain information on the unlike molecule interactions. Miller [5] also demonstrated that

for a number of other systems, the deviation parameters needed to predict mixture properties with the Snider-Herrington equations are consistent with those obtained from independent gas phase data, which for the

most part are properly represented in magnitude by the Hiza-Duncan

correlation.

2
Fluorine -oxygen mixtures are particularly intriguing in the above

context, since appropriate data are not available to determine the inadequacies of the combining rules nor to determine the reliability of any

calculations. However, accurate data for the pure fluids, fluorine [6j

and oxygen[7], are available. If one can postulate something about the

nature of the unlike molecule interactions, it is possible to obtain liquid

fluorine -oxygen mixture properties from the pure fluid properties data

and the excess properties determined with the Snider -Her ring ton equations.

Though the desired information for fluorine -oxygen interactions

is not available, previous experience with comparable oxygen systems

can be applied to this problem, since oxygen appears to be the responsible molecule in exceptions encountered in the correlation effort [4].

To model the fluorine -oxygen system after other simple oxygen systems,

it must be assumed that fluorine is well-behaved, and that the mixtures

formed are purely physical solutions.

In this study, the argon-oxygen system was used as the model to

estimate an adjustment to the geometric mean combining rule for the

characteristic energy parameter of the fluorine -oxygen system. Fluorineoxygen liquid mixtures containing 0,6, 0,7, 0.8, 0.88, and 0.9 weight

fraction of fluorine and pure fluorine were considered in the present

5 calculations from the saturation boundary up to 70 x 10 Pa from 55 to

90K. The properties determined were molar volume, enthalpy, entropy,

and constant pressure specific heat. Along the saturation boundary, the

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 Longuet-Higgins and Widom [8],

upon which the mixture equations of Snider and Herrington are based is:

Pv/RT = [(1 + ^ + f )/(l - ?f ] - (a/RTv) (1)

1 3 where ^ = p / v and P is the hard- sphere volume, (— N TT r ). The second

6 A

term represents a uniform attractive potential field.

Assuming constant "a" and "3" parameters implies that the configurational = 0. 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 from the pure fluid properties at each temperature of

interest. The "a" parameter was evaluated from the configurational

internal energy (the configurational internal energy of an ideal gas is

zero); thus, "P", the hard-sphere volume is the only unknown in equation

(1).

In applying their equations. Snider and Herrington used the equimolar G (excess Gibbs energy) at one temperature to determine the value

of the cross parameter, "a Sacrificing mixture data in any form in

the present calculations was not possible. Thus, a different scheme had

to be devised.

In correlating deviations from the geometric mean combining rule

for the characteristic energy parameters [4j, the following empirical

equation was developed:

4
where I is the ionization potential in eV and the subscript one denotes the

component with the larger value. The parameter k^^ is defined as:

Uoi2 = (1 -kj^) (Uo, U^^)'/' (3)

where Uq is the characteristic potential energy parameter. It is anticipated that the deviation parameter k is always positive.

1 ^ In comparing predictions of the deviation parameter from equation

(2) with observed values for oxygen systems specifically, equation (2)

consistently over-predicts the magnitude of k . This suggests that an

J. w effective ionization potential for oxygen, somewhat larger than the observed value of 12.08 eV [10], is necessary to make the predictions for

oxygen systems consistent with experiment.

The ionization potential for fluorine is 15.70 - 15. 83 eV[ll],

almost the same as that for argon, 15. 79 - 15. 94 eV [12]. If one assumes

that, in the fluorine -oxygen 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 combining rule used by Miller, Kidnay, and Hiza [3]

where "r" is the hard-sphere diameter, a k of 0.015 was selected for

^ E

the fluorine -oxygen system by examination of the equimolar G from

argon-oxygen liquid-vapor equilibria data [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 to establish the liquid phase total vapor pressure and the

vapor composition of the fluorine-oxygen system. In this sense, the

excess Gibbs energy and the activity coefficient of each component,

and

y

^, are related to the liquid phase mole fractions, x^ and x^,

with a single constant. A, by

= A x^ x^ (5)

2 RT In = A (6)

2 RT In Y^21= A x^ (7)

The standard expression for the activity coefficient of each component

RT In = RT In (y^ P/x^po^) + (B^^ - v^^) (P - p^^) + Py^ h (8)

RT In Y2 = RT In (y2P/x2 P02) + 22 ~ ^""2^ " ^02^ + ^^1^2 ^"^^

can then be related to equations (6) and (7) to obtain two equations in two

unknowns, i.e. the solution vapor pressure, P, and the vapor phase

mole fraction, y where (y +y^ = 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. 6 is an excess interaction second virial coefficient

J. Ld term defined by

' 6 = 2B - B - B (10). 12 12 II 22

The second virial coefficients were calculated using

6
^ - (l-i)/4

B (T/T ) = V y] B. (T/T ) (11)

C C 1 c

i = l

where B are the reduced form of the fitted polynomial coefficients B

i i of pure fluorine second virial coefficients given by Prydz and Straty [6],

The relationship between the two sets of coefficients is

v(l-i)/4

r c

B. = (12).

1 V

c Since the reduced polynomial coefficients for pure oxygen are essentially

identical to those for fluorine, i,e„ two parameter corresponding

states is satisfied, the values of B.''~ for fluorine were used. To obtain

1 B from equation (11), the following mixing rules were used

J. ^

c cl2 2

^ cl c2 ' ^'^^

and

T T = (1 - k ) (T T )1/^ (14)

c cl2 12 clc2

with a value of k equal to 0.015.

1 ^ The value of the constant A in equations (5), (6), and (7) was

E

evaluated at each temperature from the equimolar G calculated from the

Snider-Herrington equations. All pure component parameters were taken

from the experimental data [6,7].

7
3. RESULTS

The properties of interest were deterrained for the selected

liquid phase compositions at each temperature in both British and S. I.

units. The properties along the saturation boundary and those in the

compressed liquid are given in S. I. units in tables A-1 and A-2, respectively. The corresponding properties in British units are given in tables

B-1 and B-2. All calculations were done on a molar basis, though some

of the properties are given on a weight basis for the convenience of the

intended user. Fluorine and oxygen molecular weights of 38. 00 and

32, 00, respectively, were used in these conversions.

The mixture molar volumes, enthalpies, and entropies are the

algebraic sum of the mole fraction average of the pure component properties taken from experiment, the excess property of the mixture calculated from the Snider -Herrington equations, and the ideal mixing

contribution. This relationship is simply expressed as M = X M + x^M^ + + M^^®^^ (15) m 1 1 2 2

^

'

where M is the property of interest, the subscript m denotes mixture,

and the superscript E denotes excess. The last term, the ideal mixing

contribution, is zero except for entropy and thus Gibbs energy, the ideal

entropy of mixing being -RI^x. In x.. In calculating the heat capacity of

the mixture, it was assumed 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 6; the saturated liquid properties were

correct as given„ Revised thermophysical properties tables for fluorine

have been prepared by G. Straty and L. A. Weber and will be published

soon. The reference state for the pure component thermodynamic properties is the ideal gas at zero K.

8
It is worth noting that the saturated liquid mixture densities

(more correctly, specific weights), reported graphically by Schmidt [14]

from "proportional interpolation" of the pure fluid properties, differ

significantly from the values 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, i. e. the mole fraction average of the molar volumes. For a 70 weight % fluorine mixture at 140R, the saturation specific volume taken

from Schmidt is approximately 2. 2% lower than the corresponding value

from this study (Table B-1). This difference can be accounted for in three

parts (approximately): 0. 4% due to the difference in pure fluid properties

used, 1. 4% due to the two different methods of averaging, and 0. 4% due

to nonideality considerations accounted for in the present study. If the

same pure fluid properties were used, for this mixture, Schmidt's

method of averaging results in a negative excess molar volume (equation

15) 1. 4% of the ideal while the present calculations result in a positive

excess volume 0. 4% of the ideal.

The validity of the calculated results given here can only be

assessed in the final analysis by comparison with appropriate experimental data, which are not available at the present time. At a minimum,

two kinds of data at a single T - x point for the liquid mixture can satisfy

this requirement. These are precise values of the solution vapor pressure

and the saturated liquid excess molar volume for the equimolar liquid

mixture at a single temperature, preferably far removed from the critical

temperatures of the 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. Without

9
this information, it is hoped that these results are a significant improveraent over values of the subject properties obtained by simple 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. The authors wish to thank

G. C. Straty and L. A. Weber for providing computer programs for the

pure fluid properties of interest.

10
5. REFERENCES

1. N. S. Snider and T. M, Herrington

J. Chem. Phys, 47, 2248 (1967),

2. L. A. K. Staveley

J, Chem, Phys. _53, 3136 (1970).

3. R. C. Miller, A. J. Kidnay, and M. J. Hiza

J. Chem. Thermodyn. 4, 807 (1972).

4. M. J. Hiza and A. G. Duncan

AIChE J. j_6, 733 (1970).

5. R. C. Miller

J. Chem. Phys. 55, l6l3 (1971).

6. 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. Widom

Mol. Phys. 8, 549 (1964).

9. A. Blinowska, T, M. Herrington, and L. A. K. Staveley

Cryogenics 21, 85 (1973).

10. K. Watanabe

J. Chem. Phys. 26, 542 (1957).

11. 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 of Fluid-Phase Equilibria [Prentice

Hall, Englewood Cliffs, New Jersey, 1969], see pg. 194.

14. H. W. Schmidt

NASA SP-3037 (1967).

11

TAB-E A-1. THERiOOYNA'^IC PROPERTIES OF LIQUID FL UCR IN' E-0 X YG EN MIXTURES

ON THE SaTJRATION POUNOARY

TEMPERATURE WT. FRACTION F2

LIQUID

PRESSURE V0LU1E

lO^PA

3 CM /10L

ENTHALPY

J/MOL

ENTROPY

J/MOL

p

MCL-K

55.0

0. 6000

0.70 00 0. 8000

0.8800

0. 9000

1.0000

,756?

>) l't6

, i 721*

0 .9329

1.1000

0.00338

0. 00355

0. DC 372

0 . 0 0 38<*

0 . 0 0 38 7

0 . OOi^O 1

? 3.1.

23.19

22.9'. 22.7 U 22.be

22.^1

•596 3.^7

•59'.7. 1.2 693 7. 7 7 ^935. 1.0 5935.6 3 Tgi.?. 16

70.86

69. 85 66. 31. 66. 66

66. 15 62. 39

5 1. . 0 2 5 1. . 1

5 1. . 5?

5 1. . 1.1. 5 I. . 1.7 51.. 63

60.0

0. 6000

0. 7000

0. 8000

0.8800

0.90 00

1. 0000

0 . 7521. 3.^132

0 . 8 726

0.9212

0. 9333

1. 1000

C. 01299

0. 01367

0. 011.32

0. 011.81 0.011.93

C . C 1 5 5 0

2 3.81.

2 3.61

23.36

2 3.15

23. IC 22.82

569 2. 3

5575.2:

5661.. 51. -5661 . 32 -5661 .3?

^666.69

75. 58

71.. 59

7 3. IC

7 1. 1.3 70.92

67. 1 8

51.. 01

51.. If- 5 1. . 3 1 51.. 1*3 51.. 1.6 51. . 62

65.0

6000

7003

8000

38 00 90 00 1.0003

0 . 71.63 0.8130

3 . 8 711.

J . ^21

0.9357

1.3030

Q. 03996

0. 01.20 3

0 . 01.1.0 1 0. 01.552

0. 01. "^89 0. 01.769

21.. 2 8 21.. 0 23. 3C

2 3.39

23.5 3 2 3.25

51.1 9.60

•51.01 .21 53 8 9. le

^•3 81.. 7 9 -5381.. 50 5388.31

79. 95 78.98

7 7. 51

75. 36

75. 36 71.61.

51.. 50

5 1. . 7?

51. . =6

5 5 . 16

5 5.21

55.1.6

7 0.0

0.6000

0. 70 00 0.8000

0. 3800

0. 9000

1.00 00

0 . 71.32 0.3 059

3 . 3691. 0.920 3 0. 9332

1.3 030

0 . 10 326

0. 10853

0. 11 356

C . 11 71.1. 0. 11839

0 . 12 302

21.. 75

21.. 5 1 2i..2fc

21.. 05

21.. 0 0 2 3.71

511.5. 5 0 -^125.6?

^•112.01

5106. 29 5105.65

-5107.68

81+. 01 83. 07

81. 62

79. 99

79. 1.9 75. 80

51. . 32

51. . 51

51. . 7(> 51. . 35

51.. 39 55.10

75.0

0. 6000

0. 7000

0.8000

0.8800

0. 90 00 1.0000

0 .7333

0.3011* 3.3670

3 . 9192

3.9323

1.3030

0. 2321.6

0 . 21.1.01* 0. 25511*

0. 26373

P. 26583

0.27612

25.2 5

2 5.01

21*. 76

21*. 55

21*. 1.9 2 1..2 0

•1.869. 73

1.81*8. 26

-1.832. 93

•1.825. 87

1.821.. 88 1.825. 0 7

87. 81

86. 89 85. 1.7 8 3. 35

8 3. 36

79. 69

51.. 5 1.

55,

5 5 , 5 5 , 55 ,

70

51* 1ft 38

1.3 69

8 0.0

0. 6003

0. 7000

0. 8000

0. 8803

0. 9000

1.0000

0 . 7267

0 . 7971

0 .361.6 0.9130

3.9315

1.3 030

0. 1.6837 0.1.9116 0.51308

0,53008

0 .531.26

0. 551*73

25.78

25.5 5 2 5.30

25.0 8 25.0 2 21*. 73

1.592, 60 1.569. 39 1.552, 15

1.51. 3 , 51. 1.51.2 . 1 6

•1.51*0, 38

91, 39

90, 1*9 6 9. 0 9 87, 1*9 8 7, 01

8 3, 36

51., 96

5 5.20

5 5. 55,

55.

5 6.

i»r, (^7 72

00

8 5.0

0. 6000

0.7003

0. 8000

0. 8803

0. 9003

1.0033

0 . 72J8

3 . 7932

J . 3625

0.9170

0. 9337

1.3 030

0. 86232

0 . 90 31.2 0. 91.315

0. 971.07

0 . 98168

1. 01909

26.35

26.12

25.8 7 2 5.65

25.6 0 2 5. 3 C

-1.31 3. 57

1.238 . 1.1. U269. 31. -1.259. 01. -1.257. 09 1.253. 2C

91.. 75 93. 86 92. 50

90. 93

9 C. 1.1. 86. 82

5 5.65

55.97

51^ . 31

5 6.59

5 6.67

5 7.03

90.0

0. 6000

0. 7003

0. 8003

0. 8800

0. 9000

1.0000

0.7151* 0.7896

0 . 360 5 0.9 161 0.9300

1.3 030

1. 1*71.87

1. 51.39 9 1.61112

1. 66359

1.67»^5i*

1 . 71. 0 31*

26.97

26.73

26.1.8 26.2 7 26.2 1 25.91

-1*031.96

-1.001.. 77 3933.51

•3971 .1.3 3969.16

3962. 81

9 7. 96

9 7. 11 95. 76

91.. 20

93. 72 90. 12

56.53

5 6.96

5 7 . 1.0 5 7. 76

5 7 . «6

5 8.33

95.0

0. 6000

0.7000

0. SOOO

0. 8800

0. 9000

1.0000

0,7101

0 , 7860

0 . 3 531. 3.9150

0.9291

1.3030

2.37502

2. 1.81.55 2. 5911.3 2.67529

2. 69601.

2. 79R1.9

2 7, 2 7, 27,

26,

2 6.

6 1.

'+ 1

1 6 95

39

26.3 9

•37i*6, 61 3717,20

3693, 57

•36 7 9, 7

•36 7 6, 9 6 3668. 1 fi

10 1,03

10 0.20

98. 37

97. 33

9 6. 36 93. 28

5 7 . 5 7.

5 a

58 . 53 , 5 5.

1763

10

1.9 5809

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27

FORM NBS-114A («-7l) U.S. DEPT. OF COMM. 1. PUBLICATION OR REPORT NO. 2. Gov't Accession BIBLIOGRAPHIC DATA AnaCTr) n -i i -3 o SYi££j IN ijoiK IJ-JJO

3. Recipient's Accession No.

4. TITLE iiit ANDINU SUBTITLE suDiiiLt ^ i i . i Calculated Liquid Phase Thermodynamic

Properties and Liquid-Vapor Equilibria for Fluorine -Oxygen

(FLOX) Mixtures

5. Publication Date September 1973

t.Pctlotmiag Organization Code

7. AUTHOR(S) -,,r W. n • u j i.^ -r tt- R. Parrish and M. J. Hiza 8. Performing Organization

9. PERFORMING ORGANIZATION NAME AND ADDRESS

NATIONAL BUREAU OF STANDARDS , Boulder Laboratories

DEPARTMENT OF COMMERCE

Boulder, Colorado 80302

10. Project/Task/Work Unit No. 2750547

11. Contract/Grant No. Purchase Req.C-32369-

12. Sponsoring Organization Name and Address NASA Lewis Research Center

21000 Brookpark Rd.

Cleveland, Ohio 44135

13. Type of Report & Period Covered Final

Nov '72 -- Sept '73

14. %>onsoring Agency Code

-C

15. SUPPLEMENTARY NOTES

16. ABSTRACT (A 200-word or less factual summary of most significant information. If document includes a significant

bibliography or literature survey, mention it here.) Liquid phase thermodynamic properties and liquid-vapor equilibria of fluorineoxygen mixtures, for which no experimental data exist, have been calculated. The

results are based on excess properties predicted from the Snider -He rrington equations, with an adjusted combining rule, and the corresponding data for the pure fluids.

Mixtures considered are 0 . 6 , 0.7, 0.8, 0.88, and 0. 9 weight fraction of fluorine

5 from 55 to 90 K up to 70 x 10 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 of pure fluorine from experimentkl

data have also been included. Results are tabulated in both British and S.I. units.

17. KEY WORDS (Alphabetical order, separated by semicolons) Calculated thermophysical properties;

compressed liquid phase, fluorine -oxygen mixtures, hard-sphere model;

liquid-vapor equilibria.

18. AVAILABILITY STATEMENT

[3n UNLIMITED.

I I FOR OFFICIAL DISTRIBUTION. DO NOT RELEASE

TO NTIS.

19. SECURITY CLASS

(THIS REPORT)

UNCLASSIFIED

20. SECURITY CLASS

(THIS PAGE)

21. NO. OF PAGES

22. Price

UNCLASSIFIED

USCOMM-DC 66244-P7I

USCOMH tRl.