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~ ANP PROJECT PROGRESS REPORT fixed midway between the two half cells was formerly used as the cell temperature. In order to refine the temperature measurements, a calibrated thermocouple, enclosed in a nickel tube, was sub stituted for an electrode in a dummy cell. In the temperature range of interest (550 to 750OC) the melt temperatures found were 10 f 2OC higher than the melt temperatures at the center between the two crucibles. Thus all the temperatures reported in connection with previous potential measurements should be revised upward by 10°C. Only the solubility data are sufficiently temperature sensitive to be appreciably affected. Application of the temperature correction to the solubility data previously reported' gave the following new expressions for the solubility of MF,.ZrF, in NaF-ZrF, (53-47 mole %): 36.0~ 103 IogN = - + 6.87 , for FeF,*ZrF, 4.576 T 40.1 103 log N = - + 8.36 , for CrF,*ZrF,, 4.576 T 28.8 103 109 N = - + 4.72 , for NiF,.tF,,16 4.576 T where N is the mole fraction of MF2*ZrF4 and T is temperature in OK. The corrected heats of solution and "ideal" melting points are now 36.0, 40.1, and 28.8kcal/mole MF,.ZrF, and 875, 775, and 1060OC for the Fe, G, and Ni compounds, respectively. Solubility data obtained by analyses of filtrates from saturated solutions, as described in the pre- ceding sections of this chapter ("Equilibrium Reduction of NiF, by H, in NaF-ZrF," and 'lSolu- bility and Stability of Structural Metal Fluorides in Molten NaF-ZrF,"), did not agree with the elec- trometr ica I I y determined so I ubi I i t ies, particular I y in the case of NiF,. Since the filtration measurements were carried out by adding NiF, rather-than NiF,.tF, as solute (and similarly with FeF, and Cr F,), the electrometric determinations were re- peated with NiF, as solute so that the data could 16From this investigation and x-ray and petrographic examinations of quenches of NaF-ZrF4 melts, NiF, is now believed to exist in a ternary compound, rather than as NiF2*ZrF4, in saturated solutions. The equation for the solubility was revised to include additional measurements, as well as the temperature correction. 104 be compared. X-ray and petrographic examinations of the solidified melt from the half cells should have sufficed to identify either or both of the joins W as quasi-binary; in practice, however, both NiF,*ZrF, and a new phase were found in the slowly cooled half cells. The new phase is thought to be a ternary compound, since it has never been found in the binary systems. Gradient quenches (510 to 540°C) along the two joins revealed only the new phase, with no NiF,*EF,. Such ambiguous results were disappointing, since on a quasi-binary join the solubility does not vary with the amount of solute added, as it does along a random join. Cells containing MF, in NaF-ZrF, (53-47 mole %), with no addition of ZrF,, gave the solubilities of the structural metal salts shown in Table 2.2.10 and Fig. 2.2.4 for NiF, and Table 2.2.11 for FeF,. The solubilities of the nickel salts along the joins NiF2eZrF4-7NaF*6ZrF4 and Ni F2-7NaF*6ZrF4, as well as the values for NiF, obtained by filtration methods, are plotted in Fig, 2.2.4. The discrepancy between the results of the various experiments has not been explained. The electrometrically determined solubilities appear to be virtually the some whether the solute is added as NiF, or as NiF,*tF,, and the same seems to be true for TABLE 2.2.10. SOLUBILITY OF NiF, IN NaF-ZrF, (53-47 MOLE %) &fsoln = 28.8 kcal Ideal melting paint = 106OoC Temperature NiF, Solubility (OC) wt % mole % 553 0.12 0.12 564 0.14 0.15 1 574 0.19 0.20 576 0.20 0.21 650 0.79 0.83 650 0.93 0.97 655 0.88 0.92 669 0.98 1.01 706 1.97 2.0 5 725 2.19 2.29 i
FeF,. The FeF, saturation points were not so well defined or reproducible, however, as those for FeF,eZrF,, especially at temperatures above 650OC The potentials of many of the cells flux- tuated greatly and were much lower than the values predicted from the Nernst eqiation (where complete .- E 0.40 , I 0.05 I 0.02 c - r 0.04 - 0 E > 5 0.005 2 0.002 0.001 I I I UNCLASSIFIED ORNL-LRDWG 94636 I I EMF DATA: I I 0 NiF 0 NiF2. ZrF4 1 I I FILTRATION DATA FOR NiF 0.0005 l l i 800 750 700 650 600 550 500 TEMPERATURE PC) Fig. .2.2.4. Solubility of NiF, and NiF,-ZrF in NaF-ZrF, (53-47 mole X). TABLE 2.2.1 1. TENTATIVE VALUES FOR M E SOLUBILITY OF FeF2 IN NaF-ZrF, (53-47 MOLE %) Temperature FeF2 Solubllily (OC) wt % mole 96 535 0.13 0.14 561 0.25 0.27 565 0.31 a. 34 608 0.72 0.78 630 1.08 1.16 1.10 1.18 1.45 1.56 2.44 2.63 3.23 3.47 7 10 7.22 7.75 742 9.9 1 10.59 PERIOD ENDING JUNE 10, 1956 solution in both half cells was expected). X-ray and petrographic examinations revealed a better- defined ternary complex in low-temperature (535OC) quenches of FeF, melts than in hi&-temperature (672OC) quenches; the FeF, ternary complex gives the same x-ray pattern as that given by the NiF, ternary complex. FREE ENERGIES OF FORMATION OF COMPLEX METAL FLUORIDES MF2*ZrF4 L. E. Topol For a saturated solution of MF2*ZrF4 in a molten electrolyte, the following equili brim holds: + ZrF4(so1n) I AF = 0. In NaFeZrF, (53-47 mole %) as the solvent, the activities of MF,(soln) and ZrF4(svln~ are known, at least approximately, in a few.cascs, and, since the activity of solid MF2*ZrF4 is unity, the free energy of formation of MF,*ZrF, is the only unknown in the following relations as applied to the saturation equilibrium: a ~ a ~ ~ 2 ~ ~ 4 AF 5 0 = AFO + RT In - a M F ,a Z, F , where N is mole fraction and a and y are, respectively, the activity and the activity coefficient based on the pure solid as the standard state. The free energy of complexing of MF2*ZrF4 from solid MF, and solid ZrF, is Hence a knowledge of the activity of the dissolved MF, and ZrF, suffices to yield the free energy of complexing, AFcomp; this quantity has been calculated for the proposed family of complexes CrF,.tF4, FeF,*ZrF,, and NiF,*ZrF,, as shown in Table 2.2.12. Since for NiF,*ZrF,, AFeomp is positive, there is additional evidvce that this 1 05
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Part 1 AIRCRAFT REACTOR ENGINEERING
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STATUS OF ART DESIGN Design work on
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of pressure loads. The idealized mo
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UPPER DECK 7 @ PRESSURE SHEL PERIOD
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SOD,UM r--- INCONEL TANK ROOF 0 0.5
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TABLE 1.1.1. NaK PUMP SPEEDS AND HO
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62 CALCULATED HEATING (w/crn3) N w
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where I = radius of source (taken a
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heat exchanger was used. The heatin
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head which are bounded by various t
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h bd * W - EcBRc+ ORNL-LR-DWG I4918
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PERIOD ENDlNC JUNE 10. 1956 TABLE 1
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ENRICHER ACTUATOR J. M. Eastman Spe
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hd - Thus, even with an input signa
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- . 140 120 p 100 g d 80 8 L s In y
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and lose their hardness in the pres
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p. W 2.5 0.5 0 400 OPERATING TIME (
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i 20 too 80 40 20 PERIOD ENDING JUN
Page 39 and 40: c' I - + r 500 450 400 3 50 300 2 2
Page 41 and 42: 01) 0V3H 5: N 0 2 s 0 0 0 5: 0 2 s
Page 43 and 44: the first 200OF and B0F/sec for the
Page 45 and 46: PERIOD ENDING JUNE 10, 1956 TABLE 1
Page 47 and 48: L 0 _, I, -* t; - PERIOD ENDING JUN
Page 49 and 50: LJ 0.005 in. on the diameter and a
Page 51 and 52: I 3 -I W CALROD HEATER 1500 I 1400
Page 53 and 54: -17 Inconel I .._I_ I" .. _ _ ~ ._
Page 55 and 56: i E ART FACILITY F. R. McQuilkin Co
Page 57 and 58: L7i PERIOD ENDING JUNE 10, 1956 Fig
Page 59 and 60: PERIOD ENDING JUNE 10, 1956 Fig. 1.
Page 61 and 62: ART OPERATING MANUAL W. B. Cottrell
Page 63 and 64: Part 2 CHEMISTRY W. R. Grimes
Page 65 and 66: W 2.1. PHASE EQUILIBRIUM STUDIES' C
Page 67 and 68: - 0 Q 3 G 4000 900 800 700 a w a 5
Page 69 and 70: - a t a w 1000 900 000 - P 700 3 2
Page 71 and 72: - 0 e 4 000 900 800 5 700 I- a a W
Page 73 and 74: ZrF4 9t2 PERIOD ENDING JUNE 10, 795
Page 75 and 76: U c * NaF*BeF2-2NaF*BeF2 triangle c
Page 77 and 78: THE SYSTEM MgF2-CaF2 L. M. Bratcher
Page 79 and 80: 2.2. CHEMICAL REACTIONS IN MOLTEN S
Page 81 and 82: I id PERIOD ENDING JUNE 10, 1956 an
Page 83 and 84: PERIOD ENDlNG JUNE 10, 1956 V which
Page 85 and 86: u the salt-metal interface, and the
Page 87 and 88: of this reaction will be made at th
Page 89: +- + z 6 e 6 5 3 3 > k i m 3 2 2 1
Page 93 and 94: UNIF, = yN should be unity (a pure
Page 95 and 96: Although it appears that the solubi
Page 97 and 98: , . 2.3. PHYSICAL PROPERTIES OF MOL
Page 99 and 100: -0 a rn u) u) DO2 oot c ;o rn OS g
Page 101 and 102: IL, - PERIOD ENDING JUNE 70, 7956 O
Page 103 and 104: 8 00 700 600 - 0 0, w 500 a 3 I- U
Page 105 and 106: supporting plaque is loaded into th
Page 107 and 108: u 2.4. PRODUCTION OF FUELS c G. J.
Page 109 and 110: half of fiscal year 1957. This esti
Page 111 and 112: 2.5. COMPATIBILITY OF MATERIALS AT
Page 113 and 114: volume of 1 M tartaric acid solutio
Page 115 and 116: After the trap has been opened, bot
Page 117 and 118: \ Part 3 METALLURGY W. D. Manly
Page 119 and 120: FLUORIDE FUEL MIXTURES IN INCONEL F
Page 121 and 122: PERIOD ENDING JUNE 10, 1956 TABLE 3
Page 123 and 124: Fig.3.1.3. Region of Maximum Attack
Page 125 and 126: (d . terminated after 1217 and 1339
Page 127 and 128: - . LJ BRAZING ALLOYS IN LIQUID MET
Page 129 and 130: PERIOD ENDING JUNE 10, 1956 NaK wer
Page 131 and 132: I PERIOD ENDING JUNE 10, 1956 I Fig
Page 133 and 134: 0. PERIOD ENDING JUNE 10, 1956 Fig.
Page 135 and 136: Fig. 3.2.10. Apparatus for Studying
Page 137 and 138: STATIC TESTS OF INCONEL CASTINGS R.
Page 139 and 140: t (JnOOSll 3n918-3NOt IOH (JoOOSI)
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after the l00hr test. The extent of
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tests of the Lindsay Mix specimens,
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LJ DEVELOPMENT OF NICKEL-MOLYBDENUM
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LJ PERIOD ENDING JUNE 10, 1956 Fig.
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2. Canning of the billets with '/,-
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165 . c, e . c3 a PERIOD ENDING JUN
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u allow the billet to start through
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NEUTRON SHIELD MATERIAL FOR HIGH-TE
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PERIOD ENDfNG JUNE 10, 7956 Fig. 3.
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wrought plate used as base material
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J point. A mixture of 50-50 vol % L
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WELDING PROCEDURE: VERTICAL FIXED,
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4 2 t 4 2 in. t 2 WCLASSFKO ORNL-LR
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FABRICATION OF JOINTS BETWEEN PUMP
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* h WELDING PROCEDURE PERlOD ENDING
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1 1 6 in. PUMP BARREL t SECTION AA
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'4 x 6 x 20-in. INCONEL PLATES (/*-
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UNCLASSIFIED PHOTO 17248 Fig. 3.4.1
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through the radiator by passing col
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L, . 1 Q t V ERIOD ENDING JUNE 10,
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to permit the examination of indivi
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LJ . t L t * I LJ Fig. 3.4.33. Tube
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Fig. 3.4.37. Inner Surface of Tube
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EFFECTOF ENVIRONMENTONCREEP- RUPTUR
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PERIOD ENDING JUNE 10, 1956 UNCLASS
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Fig. 35.7. Surface Effect on the St
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44,000 42,000 40,000 - ._ (D 8000 v
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\:r 1 U UNCL 1158 W ioo,ooo 80,000
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fuel mixture (No. 30) NaF-ZrF -UF,
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i u * ‘*$ , .\. The Lindsay Chemi
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6, * c L . c e 4 gi depths greater
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i 4 Part 4 HEAT TRANSFER AND PHYSIC
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4.1. HEAT TRANSFER AND PHYSICAL PRO
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This relationship gives the ratio o
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The parameters of the’experiment
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t Fig. 4.1.7. Fuel Annulus of the V
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uncooled wall temperature that woul
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SHIELD MOCKUP REACTOR STUDY L. C. P
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Liquid (688 to 8986C) I . HT - H3Q
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THERMAL CONDUCTIVITY W. D. Powers T
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cd Fig.4.2.4. Slingers from MTR In-
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a plug when they came in contact wi
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couples were used on this loop to e
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0 20 40 60 80 lo0 I20 440 (60 180 2
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"fast" neutron in a graphite reacto
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eached thermal equilibrium in an in
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0.5 0.4 - a3 l- W z 0.2 0.1 UNCLASS
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TABLE 4.2.3. RESULTS OF EXAMINATION
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U could be evacuated was used for t
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! j * . x - iu I PERlOD ENDlNG JUNE
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CRITICAL EXPERIMENTS FOR THE COMPAC
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. I) a W PERIOD ENDING JUNE 10, 195
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U I I R i c . --. in. long, 18’4,
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I, . R t 3 4 . C 7 6 5 W 5 a c3 E4
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1 a
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ANP PROJECT PROGRESS REPORT ot(E) =
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ANP PROJECT PROGRESS REPORT TABLE 5
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ANP PROJECT PROGRESS REPORT TABLE 5
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6 ANP PROJECT PROGRESS REPORT 2 lo7
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ANP PROJECT PROGRESS REPORT GAMMA-R
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ANP PROJECT PROGRESS REPORT 5.3.3,
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ANP PROJECT PROGRESS REPORT A I P I
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ANP PROJECT PROGRESS REPORT SECTION
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ANP PROJECT PROGRESS REPORT .. .._
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