-\ug. 3, 1933 [CONTRIBUTION SO. 73
TIIERRIODYN:.IRIIC PROPERTIES FROM THE
3830
O F PENT;IFLUOROCIILOROETII.\NE
CRYOGENIC LABORATORY OF THE COLLEGE OF CHEMISTRY A N D PHYSICS OF THE P E S N S Y L V A N I A S T A T E c:SlVERSITI.]
The Heat Capacities from 10.9"K., Heats of Transition, Fusion and Vaporization, Vapor Pressures and Entropy of Pentafluorochloroethane, the Barrier Hindering Internal Rotation1 nY
J. c.,4STON, P.E.
'r. 1'.
IvILLS AND
%OI.KI
RECEIVED MARCH5 , 195.5 The heat capacities of peritafluorochloroethane from 10.9"K. to the normal boiling point are tabulated. Temperatures of a rotational transition and the triple point are tabulated as well as vapor pressure.;, heats of transitioi1, fusion and vaporization. The calorimetric entropy of the vapor a t the normal boiling point when coinpared with value calculated frorn spectroscopic data yields a barrier of 5300 cal. mole-' hitidering internal rotation.
Introduction The barrier hindering internal rotation2 in ethyl chloride is 4700 cal. mole-' while that in ethane is 2750 cal. m01e-l.~ The barrier is 4350 cal. mole-' so that one would place the in perfl~oroethane~ barrier in pentafluorochloroethane as somewhat above 5000 cal. mole-'. The present investigation describes the thermal data necessary for the determination of the third law entropy at the normal boiling point t o be used in a comparison with the entropy calculated from spectroscopic data leading to a barrier near 5000 cal. mole-'. The calculation of the entropy from these data together with a calculation of the spectrosccpic entropy has already been given in a note for purposes of expediency.j Experimental The Material.-The sample used had less than 0.01 mole per cent. impurity. It was supplied by the Jackson Laboratory of E. I. du Pont de Semours and Company through the courtesy of A . F. Benning and needed no further purification. It was neighed in a small high pressure cylinder. The Apparatus.-Calorimeter C6 was used. Standard thermocouple S-7 was used as primary temperature standard w-ith occasional checks against s-4 which showed no changes in calibration greater than 0.05' since the last comparison of both with hydrogen and oxygen vapor pressures in 1944. The Heat Capacities.-The molal heat capacities are tabulated a t rounded temperatures in Table I and graphed in Fig. 1 which is constructed in such a way t h a t the experimental points may be obtained within experimental error by interpolation from the table and addition of the deviation of the point from the curve representing the d a t a of Table I. XVith the exception of the points below 40°K., near 80°K. and near 150°K. the accuracy is about 0.27,. Below G 0 K . the error may fall to over 1% due to the insensitivity of the thermocouples and the changing resistance thermometer derivatives. S e a r 80°K. and near 150'K. changes in resistance thermometer derivative limit the accuracy t o about
TABLE I MOLALHEATCAPACITY OF ClFjCl
(1) This research was carried out in part on Contract N6-ONR-269, T. 0. I11 of the Office of Naval Research. (2) J . Gordon and W . F. Giauque, THISJOURNAL, 7 0 , 1506 (1948). (3) G. B. Kistiakowsky, J. R . Lacher and Fred Stitt, J. Chcrn. P h y s . , 7 , 289 (1939). ( 4 ) E. L. Pace and J. G. Aston, THISJOURNAL, T O , 566 (1918). ( 5 ) J. G. Aston and R. P. Zolki, ibid., 77, 804 (19.55). (6) (a) J. G. Aston and G. H. Messerly, ibid.. 58, 2354 (1936); (b) C.. T i . RIe-serly and J . G. Aston, ibid , 62, 886 (1940).
INTEGRAL TEMPERA-
Mole wt. 154.477; 0°C. = 273.16OK.; 1 cal. = 4.1833 int. ioules.
15 16 17 18 19 20 21 22 23 24 25 30 35 40 45 50 55 60 65
4.22 4.70 5.22 5.76 6.26 6.673 7.02 7.34 7.65 7 945 8.23 9.58 10.68 11.57 12.31 12.96 13.56 14.15 14.75
70
15.40 160 163 16.16 80.24 17. 13 Solid I 170 80 24 23.00 173.72 85 23.18 Fusion 90 23.37 173.72 95 23.58 175 100 180 23.81 105 24.07 185 110 190 24.36 115 24.67 195 120 25.00 200 125 205 25.35 130 210 25.72 135 215 26.11 140 26.53 220 145 26.99 225 130 27.48 230 155 28.00 234.04 c-
/J
28.55 29.15 29.80 30.33 a t 173.72 31.13 log 31.18 31.36 31.57 31.80 32.07 32.38 32.71 33.04 33.38 33.73 34.08 34.44 34.72
The Transition and Melting Points.-The equilibrium temperatures for certain fractions transformed during transition and melting are given in Table I1 along with the deduced transition and melting temperature and mole per cent. impurity deduced in the customary manner.
TABLE I1 TRANSITION A N D MELTISGPOINTS OF PESTAFLUOROCHLOROETHASE
o.4yo.
The values of the solid immediately below the melting point have been corrected for premelting based on 0.008 mole per cent. impurity. The values in the liquid near the normal boiling point have been corrected for vaporization into the filling line assuming the vapor t o be a perfect gas and using heats of vaporization calculated from t h e vapor pressure equation on the same assumption. This assumption produces negligible error.
AT
TURES
Temp., O K .
%
Transformed
80.243 27 80.233 46 80.237 65 80.24 K. (transition point)
0°C. = 273.1F"K. Gio Temp.,
Melted
OK.
(XI
1/s
173.681 31 3.2 173,692 62 1.61 173.726 86 1.16 173.72 1.OO (extrap.) 173.71 0 . 0 0 (extrap.) Melting point (triple point) 173.71O R . Impurity: 0.008 mole y6
The Heats of Transition and Fusion.-Tables I11 and IV summarize the data and average values. The penultimate column in Tahle I V gives the cof-rection t o the heat of fusion for material already melted at the start of the deterniinat ion.
J. C;. A l ~ P.E. ~I ~~I L~ L A NS DT T. P. , ZOLKI
3940
100 125 I50 173 200 225 Temperature, 'K. of d a t a : (a) 0, points of a continuous run; ( b ) 0 , check points; ( c ) 0 , ( a ) on top of (b)
25 Fig. 1.-Plot
50
c-
IU
TABLE 111 HEATOF TRANSITIOS OF ClFjCl AT 80.24"K;. Mol. wt. 154.477; 0OC. = 273.16'K.; 1 cat. = 4.1833 int. joules. Temp. interval, OK.
79.287-80,967 78.973-83.902 79.041-83.144 79,087-83.148
Heat input, cal. mole-'
679.561 797.4814 768.852 767.507
JCDdl. cal. mole-1
A H transition, cal. mole-'
- 54.806 -166.872 -141.277 -140.082 Mean AH =
624.7
