Title
Author(s)
Citation
Issue Date
URL
On the thermodynamic properties of acetylene under high
pressures
Teranishi, Hiroshi
The Review of Physical Chemistry of Japan (1955), 25(1): 2533
1955-08-01
http://hdl.handle.net/2433/46722
Right
Type
Textversion
Departmental Bulletin Paper
publisher
Kyoto University
The
ON
THE
THERMODYNAMIC
UNDER
Review
PROPERTIES
HIGH
of Physical
OF
Chemistry
of Japan
Vol. 25 No.
ACETYLENE
PRESSURES
BY 11fRO5HI
TFiRAVISHI
Inkreduction
With
the development
of acetylene
some knowledge
on the thennodynamic
high pressures.
Nevertheless,
reported
in detail.
acetylene
chemistries,
properties
these properties
Sameshimatl
of acetylene
necessary
to have
for handling
it under
under high pressures
and Rimarski'1
and, however, their measurements
it has become
investigated
have not yet been
the P-V-T
were Limited in the narrow
relations
ranges
of
of tem-
perature (0-25'G) and pressure (0.5--2flatm).
The van der Waals equation of state fur
acetylene' which was computed from these data shows more than 50°o deviation in the
value of volume under even 50 atm, and can scarcely serve as the basis for the evaluations
of other thermodynamic
properties
1n our laboratory,
the P-V-T
Ikegami
of acetylene
relations
under high pressures.
of ac°tylene
and Inoue over the wide ranges of temperature
145atm), and the method and results
in 1951st. In the present
acetylene
(-8--250`C)
of the measurements
paper, the author
which are estimated,
were measured
by Kiyama,
and pressure
were reported
(11 -~
schematically
will mention in detail the Y-V-T relations
on the basis of ahove•mentioned
measurements,
of
by the
inter- and extrapolation
of the temperature
and pressure and by making the sufficient
corrections for the votame and especially for the critical conditions, and will report the
thermodynamic
properties
from the P-V-T
values.
of acetylene
under high pressures
P-V-T
Several
methods
and on the estimation
~
1)
2)
3)
4)
37fi (1931);
Relation
have been reported°~ on the correction
of some
which have been evaluated
other thermodynamic
of P-V-T
Properties
relation
of a gas
of the gas from
the
(P}4.39/V=)(V-0.0514)=RY'
(atm liters/molt),
I. R[. Klotz, Cleennedd Tkennodyrmn:ies, P. ti9, Prentice•Hall, Inc., New York, 1.950
J. Sameshima, Bnd1. Ghmu. Sat. Japmb 1, 41 (1926)
W, Rimarski and M. Konschak, Anlagen¢ d4c:a!lGeaf6eiGnrg, 2ti, 129 (1933)
R. Kiyama, T. Ikegami and K. Inoue, TGis jcarrwl, 21, 58 (1951)
A. iwiidiels e! al., P!¢ysicn, 3, 569, 597 (1930) ; Proc. Ray. Soc., A153, 201,'214 (1936) ~A1fi0,
-9pp. Sci. R¢s., 1, 94, 103 (1948)
W. C. L•'dmister, Ind. Eng. Cle¢nr„ 28, 1112 (193fiJ; 30, 325 (1938)
S. H. h-Iaron and D. Turnbull, Ind. Eng. CG¢ru., 3#, 544 (]942); J. Aur. Cpen:. Soc., 63, <H (1942)
J. R. Roebuck and H. Osterberg, Pkys. Reu., 45, 33'2 (1934) ; 4R, 450. (1935)
1 (1955)
The Review of Physical
Chemistry
Vol. 25 No. 1 (1955)
of Japan
H. Teranishi
26
P-V-T
relation.
laborious
Although
the residual
volume method of Deming and Shupe~> is most
among them, yet it is thought to be most accurate
The residual volumes
in its results
of estimation.
d and a are defined as follows:
d-V1KT-ll
In the residual
(1)
volume method, J or a is computed
ments and plotted against
of d or a -~ P isotherms
and temperature,
measure-
smoothed lines
The volume at desired
is evaluated readily from the value of d or a at the conditions
the reasonable coincidence has been found in its two values
from both d valve and a value.
The basic P-V-T
relations
in which the postulation
the ideal gas law at 1 atm and each temperature
of 99.3
from the data of P-V-T
and then reasonable
and d or a ^ T isobars are determined.
pressure and temperature
and determined so that
which are evaluated
pressure
purity at several points of pressure
that the acetylene
is assumed
between
are measured
gas follows
on acetylene
11.40 and 145.30atm on every iso-
therms of -8.0, 0.1, 20.5, 3D.3, 40.0, 52.4, 60.5, 72.5, 79.5,100.0, 150.5. 200.0, and 250.0`C.
1.0
~.
~'C
?a'C
vlffC
In
o.a
~~r
~~'~.
~~~
os
,Q,Y.
~~
~x
~z
~n
~~
o.a
~~
o.z
20
0
5)
N.
E. Deming
60
80
100
Pressure, atm
Fig. 1 PV/RTP isotherms of acetylene
O : calculated from the vapor pcessure
1'l0
40
and
data
L. E. Shupe, PHys. Rer,•.,37, 633 (1930): 36, 2245 (1931.) 40, S48 (1932)
The
On the Thermodynamic
't'able
Properties
1
P-V-T
Review
of Acetylene
relation
of Physical
Chemistry
of Japan
under High Pressures
Vol. 25 No.
27
of acetylene
(V :liters/mole)
P, etm
10
C~
V
PV/RT
V
PV/RT
V
PV/RT
V
PV/HT
zso
225
200
175
150
100
90
80
70
ti0
50
40
30
?0
10
0
The values
30
40
50
60
70
80
90
100
110
]20
130
4.279 2.120 1392 1.025 0.805 0.659 0.558 0.484 0.427 0.382 0.345 0.314 0:287
0.997 0.986 0.973 0.955 0.937 0.921 0.910 0.902 0.896 0.891 0.884 0.876 0.8(19
4.073 2.014 1.319 0.969 0.759 0.620 0.525 0.455 0.401 0.357 0.321 0.291 0.266
0.996 0.986 0.965 0.998 0928 0.910 0.898 0.890 0.882 0373 0.864 0.854 0.844
3.866 1.908 1.246 0.912 0.712 0.581 0.490 0.424 0.372 0.331 0.'197 0.268 0.214
0.996 0.983 0.963 0.940 0917 0.898 0.884 0.873 0.862 0.852 0.841 0.828 O.S17
3.G58 1.801 1172 0.854 O.6Cu 0.541 0:455 0.391 0.342 0.303 0.271 0.244 0.221
0.995 0.979 0.956 0929 0.904 0.882 0.866 0.852 0.837 0.82A 0.810 0.796 0.782
3.450 1.693 1.096 0.795 0.614 0.497 0.417 0.357 0.310 0.273
0.994 0.975 0.947 0916 0384 0.860 0.890 0.8~ 0.809 0.787
PV/RT
V
PV/RT
V
P4%RT
V
PV/RT
V
PV/RT
i/
PV/RT
V
PL'/RT
V
PV/KT
V
PV/RT
V
PV/RT
I'
PV/RT
V
PV/RT
V
PV/RT
Yv
2D
0.243 0.218 0.198
0.769 0.752 0.73.5
3.211 1.584 1.019 0.733 0.562 0.451 0.373 0.315 0.271 0.236 0.208 0.189 0.164
o.99z osss os35 D.BSS o.BSO osz7 o.7ss o.772 0.747 0.723 os9s os7s ossa
3.031 1.971 0.938 0.067 0.505 0.398 0.323 0.268 0226 0.193 0.166 0.143 0.125
0.990 0.961 0.919 0.872 0.825 0.780 0.738 0.700 O.fi64 0.629 0.595 0.562 0.530
2946 1.424 0905
0.988 0.956 0911
0.690 0.981 0.376 0.301 0247 0.206 0.173 0.147 0.125 0.106
0.860 0.303 0.75G 0.708 D.664 0.621 0.580 0.541 0.505 0.473
2.858 1.375 0.869 0.6I1 0.457 0.353 0.279 0.224 0.182 0.150 0.125 0.106 0.093
0.98(1 0.949 0.900 0.644 D.788 0.730 0.673 0.618 0.566 0.517 0.474 0.439 0.4]8
2.705 1.321 0331 0.580 0.430 0327 0.251 0.192 0.146 0.118 0.099 0.088 0.081
0.982 0.939 0.885 0.825 0.764 0.697 0.624 0.546 0.4(18 0.418 0.887 0.374 0.374
2.66,5 l.'L69 0.790 0.547 0.399 0,297 0.216 0.151 0.109 0.086 0.079 0.075 0.072
0.975 0.925 0.866 U.S00 0.730 0.(i52 0.552 0.493 0.358 0.323 0.316 0.328 0.343
2.563 1.205 0.746 0.511 0.364 O.L57 0.163 0.103
0.967 0.909 0.844 0.770 0.687 0.532 0.431 0.311
0.078 0.088 0.066 U.1%5 0.lHi5
0.26.5 0.257 0.273 0.296 0.320
2.460 1.145 0.701 0.471 0.324 0.198 0.100 0.047
0.957 0,891 0.818 0.739 0.631 0.463 0.273 0.146
2.356
0.947
'1
.2x0
0935
1.US3 0.653 0.428 0.269
D.870 0.788 0.688 0.591
].017 0.600 0.373
0.846 0.798 0.620
2.143 0.999 OS36
.922 0.817 0.692
'1.035 0.873
0.908 0.779
of critical
constants
,0
which were reported
previouslysl
seem to have some
errors due to the impurity of 0.7 contained in the gas and the difficulty in determining
the critical values and, therefore, in the present estimation,
the most reasonable
values
reported
in literaturesl
the next table together
are used for the critical
with the fundamental
constants
numerical
constants
and they are shown in
which
in the calculation.
C_Ii: = 26.036
P. = 61.6 atm
0"C = 273,16`K
R=0.082(1544
t~ = 36.0°C
liters atm/deg
1 literatm=24.2179ca1/mole
V,=113
cc/mole
p,=0.231g/cc
6) K. A. Kobe and R. E. Lynn, )r., Cpenr. Rev., 52, 117 (1953)
are employed
1 (1955)
a
The
lA
Review
Ii.
of Physical
Chemistry
of Japan
1 (1955)
Vol. 25 No.
Teranishi
0
fo .
,~
~0
~C~
-U .05
G c-U
a •~ ~:
yr i
\7
~c~
~` :
~,~`
~~
C.N. ~360'C
616atm
.10
~L`
`fit`
~~
54.1 atm
`bl`
431 atm
-U .15
m
IPC
T Sl9atm
pf.
_= 926-M1atm
-U .'LU
149atm(11.4
0?
2
4
ti
p, mOleS~hter
isotherms and isobars of acetylene
FiK. 2 J-o
J
calculated from the vapor pressure data
U.6
0.8 LU
The results of the estimation
130atm are tabulated
10'C7
of V and PV/RT
in Table
1, and PV/RT
^-P
isobars are shown in Fig. 1 and Fig.2 respectively.
in Figs. 1 and 2 are calculated
in International
respective
Critical
isotherms
from the data
Tablesn
isotherms
LU
211
of 0 -250 C and ill -
and d - p isotherms
The values corresponding
on the vapor pressures
and show good coincidence
of the present
In the basic data of P-V-T
in the ranges
x
to sign O
of acetylene
to the extrapolated
and
listed
lines of
results.
relations, the errors
of the measurements
of temperature.
pressure and volume are ~U.05°C, X0.017-VU.05atm and -2x1U"litersJmole
respectively and the relative errors of the volume (U.16 -1.SSS) are most effective in the errors
of the PV/RT
except that at the miltimum
where
error
relative
correcting
procedure,
of the volume
the smoothed
7) Inter. Gil. !'pbfes, 3, P. 230
pressure
is comparable
in the measurements
to that of pressure.
lines of every isotherms
(11.4Uatm)
In the present
and isobars of 9 and n have
The
On the Thermodynamic
been corrected
reasonably
dition which are evaluated
liters/mole,
Properties
Review
of Acetylene
under
of Physical
High
Chemistry
of Japan
29
Pressures
so that the two values of the volume under any desired
from both d and a values respeMively
i. e. the half of the errors
of volume
Owing
errors
of PVI RT are calculated,
to the postulation
also the postulation
temperature.
and there-
that the acetylene
and the
by the least square method"l, to be 0.09 ~ 0.9;6.
in the basic data, the results
If the real values
cai-
coincide within 0.001
in the basic measurements,
fore, each value of volume listed in Table 1 has the error of -!-0.001 liters/mole
relative
Vol. 25 No.
gas under
latm
of volume of acetylene
of the present
estimation
have
obeys the ideal gas law at each
under the standard
condition
(0`C, latm) and its thermal expansion coefficients at latm reported until the present"
are used instead of the ideal behaviors, the values of volume in Table 1 have 0.86, (1.72,
0.30, and 0.0716 deviations
Thermal
at 0°, 10°, 100', and 250`C respectively.
Expansion
CoefFicienk
ak Conskank
Pressure
Generally it is almost impossible to obtain the accurate (dVldT), values from the
slopes of V--~T isobars, because the latter are nearly straight lines except at the conditions
near the critipl point and liquefying points. On the other hand, it is comparatively easy
to determine the values of (dJ/dT), or (da/dT), from the slopes of .! ~T or a-T
iso•
bars, and hence (dVldT), is obtained readily by substituting these values into the
following equations:
~V~~dT~,
Rl -`V/`r(T~a,
l+.,V
(3)
1V~\dT~,
PV V\dT!n'
(4)
The two values of (dV/dT), at the same conditions which are obtained from Eqs. (3) and
(4) respectively are plotted in (T/VXdV/dT)r ~ P, (dV/dT),.--T'r
and PV(dV/dT), -T
graphs and are corrected, by smoothing the curve of each isotherm or isobar, so that the
values of (dVldT), at each condition thus obtained from these curves show reasonable
coincidence among one another. Demiag and Shupe have discussed that the PV(dVJdT)o
-T isobars have turned out to be straight lines . In the present estimation, the isobars
show the same behavior, except those near the critical condition and liquefying conditions
and are very efficient for reasonable correction of (dV/dT),. The values of (dV/dT),
thus obtained are listed in Table 2 and (dV/dT),-T
isobars are shown in Fig. 3.
On the accuracy of (dV/dT),,, Deming and Shupe have discussed "a 1 percent error
in estimating khe slope of d vs. T or an a vs. T isobar may mean only a few hundredths
** Volume at 0°C,1 atm: 2'L'L'Cl'L
liters/mole
Thermal expansion coefficientsat la[m: 0.003771(at 0°C),0.003798(0°--100°C)
L:[cr. Crrl. Tables,3, P. 9, 10
9) lt. Livingston,PGysico-Clunrieol
Experiu:enls,Y. 21, Macmillan Co., (1939)
1 (1955)
The
H.
Table
2
The thermal
Review
of Physical
Chemistry
of Japan
1 (1955)
Vol. 25 No.
Teranishi
expansion
ccefi'icient
of acetylene
'
1dV\'
\~/
x10', (liters deg-~mole-~)
n
at constant
pressure
P,abn
10
20
30
40
50
/~
70
80
90
lao
uo
120
130
LLO
1.6U
1.93
1.88
1.71
0.800
1.09
1.54
1.65
1.60
0.593
0.771
1.04
1.40
1.46
T, •C
a
io
2a
30
d0
10.9
10.5.
]0.1
9.76
9.48
7.96
7.15
6.53
8.U7
5.67
6.70
5.73
5.01
4.5fi
6.29
5.00
425
5.90
4.53
5.92
3.70
50
fi0
70
80
90
9.23
9.01
S.S4
8.71
3.61
5.37
5.14
4.94
4.79
4.68
4.22
3.94
3.72
3.55
3.42
3.73
3.ao
3.16
297
2.82
3.72
3.19
2.86
265
2.49
4.18
3.35
278
247
229
3.51
3.08
2.63
'L34
214
3.15
281
249
222
'2.02
2.61
271
'lam
2.12
1.91
1.75
2.'LS
2 .'L2
2.01
1.81
100
125
150
175
200
8.53
8.40
8.34
5.32
8.30
4.59
4.41
9.34
929
4.26
3.31
3.14
3.04
'L.99
'1.94
2.37
'L
.16
2.04
1.95
1.89
2.15
1.9'1
1.78
1.68
1.81
200
1.74
1.59
1.48
1.41
L87
1.60
1,45
1.34
1.'27
1.78
1.47
1.33
1.22
1.17
1.67
1.37
1.23
1.13
1.07
L56
1.'L9
1.14
1.08
LOl
1.47
1.21
1.07
0.989
0.947
1.39
1.14
LO1.
0.938
0.888
827
8.26
4.24
422
2.92
2.91
272
252
240
233
228
'L.2G
L85
1.83
1.56
1.54
1.37
1.34
1.23
1.21
1.13
110
1.04
t.0'2
0.968
0.946
0.909
0.385
0.857
0.832
I
zzs
•rsa
2.22
]2
]0
,
_
IOatm
9
m
J
6
.5
X
_e
fly
?Datm
4
70a1m
W atm
Siam
90a~m
40aun
2
SOaun
®atm
IOOam
110atm
12Ualm
13Dam
u
Fia.
sa
3
The
thermal
ira
Temperature,
eXpanSipn
ccef6cient
>50
`C
of acetylene
zoo
at constant
2so
pressure
The
Review
of Physical
Chemistry
of Japan
On the Thermodynamic Properties of Acetylene under High Pressures
Vol. 25 No.
31
percent error in (dVldT)„
since by Eqs. (3j and (4) the slopes (dJldT),. and (daldT)„
enter as correction terms to the slope that the v vs. T isobar would have if the gas were
perfect"
However, all of their estimation are urider such the conditions that Tr is more
than 1-66 for N:, CO and H:, and on the other hand, in such the conditions that T. is 0.88
-1 .69, as in the case of the present estimation, the deviations from the ideal gas law,
that is the values of d and a, become larger
absolute
considered
and, especially
near the critical
values become as large as that of the volume, and consequently,
that the error of (dJ/dT),
or (da/dT),
point, their
it would be
would be more effective to the error
of (dV/dT), than that reported by Deming and Shupe. Considering from the differences
between the two values of (dV/dT),
under the same conditions which are estimated
from (dd1dT)„ and (da1dT),,,
the values listed in Table 2 are taken to have the following
errors.
Maximum
100 - 250`C
0-°-100`C
a
Heat
The next
stant
pressure
thermodynamic
below P.
above P.
Capacity
equation
(,a)
Average (;e)
0.8
0.6
2.8
5-6
0.9
2.0
ak Conskank
Pressure
is used for estimating
the heat
capacity
at con-
Ca,
i
By integration
with
P, the following
equation
is obtained,
C,=C,.`+JC,=C„°J-J
~ie-Tld'l"-"-~
dP,
P
(6)
where Co is the value of C,, under the standard state at each temperature, and in the
present estimation, l atm is taken as the standard state, and the value of Cy for acetylene
at each temperature is obtained by the following equation which is calculated by Spencers>from the spectroscopic measurements on acetylene, that is,
C,'=12.184+3.879 x 10-'T-2.SS1 x lOaT-= cal deg 'mole '.
(7)
The equation is reported to be applicable for the temperature between 298,16and 1500°K
within the error maximum 1.24 and average 0.59 "*'. (d=VldT=), is evaluated from the
slope of the (dV/dT),~T
isobar and dC, is obtained by graphical integration of
T(d'V/dT')~ ^-P isotherm from latm to the desired pressure. The results of the estimation of ~C" and C, for acetylene are listed in Table 3 and C, ~ P isotherms are shown in
Fig. 4It is difficult to mention the accuracy of (d°VIdT'), as a whole, and however, its
ass For the evaluation of Co values of 0°, 10°,and 20°C,the Eq. (7) has been used, because
more adequate method of evaluation has not been obtained otherwise.
9) li. M. Spencer,Ind. Eng. Chem.,40, 2152 (1998)
1 (1955)
D
The
32
Review
of Physical
Chemistry
of Japan
Vol. 25 No.
1 (1955)
H. Teranishi
Tahle
3
The
heat
capacity
of acetylene
at constantpressure
dCn
=~~ T(dT)dP;(cal
deg-'mole-i)
P, atm
1
T,
l0
20
3a
40
°C
0
10
20
40
50
00
70
80
100
1'LS
150
175
200
225
'lS0
dCp
Cp
dCp
Cp
drp
Cp
dCp
Cp
dCp
Cp
dCp
Cp
dCp
Cp
dCp
Cp
dCp
Cp
dCp
C:.
dCp
C.,
dC,
C~
dCp
Cp
dCp
Cp
dCp
Cp
dCp
Cp
dCp
Cp
(dVldT)y-T
SO
90
100
110
120
130
3.8
3.8
13.6
3.6
11
21
70.06
3.3
3.3
13.9
3.4
R.1
18.1
19
24
10.32
2.8
13.1
G.4
t6.7
11
'LI
20
30
10.55
23
129
5.2
15.8
8.9
19,4
14
24
24
35
10.77
1.9
127
4.'L
15.0
7.0
17.7
11
21
17
27
30
41
10.97
1.6
125
3.3
14.2
5.5
1G.5
8.2
79.1
12
23
19
29
II_15
1.3
12.9
2.7
13.8
4.5
15.6
6.4
17.5
9.0
20.1
13
24
19
30
24
35
27
38
z7
38
zs
37
zs
34
zo
31
11.32
1.0
12.4
2.2
13.5
3.6
14.9
5.2
16.5
7.0
18.3
9.6
20.9
13
24
is
2s
zo
31
22
33
22
33
21
32
19
30
0.8fi
1.8
1234 13.3
29
14.4
4,3
11.49
1 5.S
5.7
17.'L
7.6
19.1
9.7
21.2
12
23
14
2fi
76
26
18
29
19
30
17
29
11.69
0.68
1231
]v
13.1
25
141
1 52
4.7
16.4
6.1
17.7
7.6
19.2
9.2
20.8
11
23
]2
24
14
?6
li
27
16
27
11.78
0 54
12.32
1,2
1.3.0
2.0
13.8
1 4.0
3.8
15.6
4.9
16.7
fi.l
17:8
7.3
ls.l
ss
zo.4
10.0 11
21.8 23
13
24
14
25
lz.la
0.33
1 z.93
0.74
izs4
12
13.3
7 3.9
2.4
14.5
3.0
15.1
3.7
15.8
4.5
16.6
5.2
17.3
8.U 6.9
7.6
18.1 19.U 19.7
R.4
'L0.5
0.22
1238
1 261
0.50
12.88
0.81
13.19
1 3.5
1.5
13.9
L9
14.3
2.3
14.7
2.8
15.2
3.3
15.7
3.8 4.3
4.8
16.2 1fi.7 17.2
5.3
17.6
1264
1 276
0.28
1292
0.96
0.67
1310 1 3.30
0.89
13.53
1.1
13.8
1.4
14.1
L7
14.4
2.0
14.7
2.3 27
15.0 15.3
3.0
15.7
3.3
16.0
12.87
1 295
0,20
13.06
0.32
0.47
13.19 1 3.33
0.62
13.48
0.79
13.65
0.96
13.83
1.1
14.0
1.4
14.2
1.6 1.8
14.4 14.6
20
19.8
'L.'L
15.0
13.08
0.07
13.14
D.15
13:L3
0.25
13.32
0.36
13.43
0.48
13.55
0.61
19.69
0.76
13.83
0.91
13.99
1.1
14.'L
1.'L 1.4
14.3 14.5
1.6
1.7
14,6 14.8
13.27
0.06
13.33
0.13
13.40
0.21
0.31
L?.84 13.58
0.41
13.69
0.52
13.79
0.65
13.92
0.78
14.05
0.91
14.18
1.1
14.3
1.3 1.5
14_ti 14.7
0.09
3.5
7.8
1.8
L1
which are calculated
isotherms
from the errors
U.82/
90°C, 40atm:0.S5sS
involved
1.2
14.5
of (dVl dT), and of the slopes of
are shown below.
175°C. 90atm:
The error
70
9.78
0.13
several examples
60
50
in the graphical
60°C, 110atm:
20°C,
integration
7,5^'
30atm:1.03b
is estimated
to be about
X0.2°:
and
considering these errors, the values of dC, in Table 3 are taken to have the probable
errors of 0.8 ^-8.09, and the ranges of the errors are shown by the dotted lines on both
sides of each isotherm
'fhe author
for his valuable
in Fig, 4.
has great .pleasure in expressing
guidance
and encouragement
his sincere khanks to Prof. Ryo Kiyama
throughout
the course of this work, and
The
On the Thermodynamic
Properties
Review
of Acetylene
of Physical
under
Chemistry
of Japan
HighPressures
Vol. 25 No
33
95
40
~~
J
35
~~`
=\
/~~
~
J
C
G
s
/'
~_
...; ..'"
J
U
.:.
U
`~~
;~
IS
m
0
the author
20
60
80
100
Yresaure, atm
Fig. 4 1'he heat capacity of acetylene. at constant pressure
is indebted
mental Scientific
40
to the Department
Research
of Education
for the Grant
120
in Aid for Funda-
shared out Pruf. Ityo Kiyama.
The Laboratory
of Pkysical
Kynlo Ut:iversil}'
Chenristr _v.
1 (1955)