Calculation of standard
enthalpy of formation and determination of constant–volume combustion energy for rare earth sulfocompounds
Zhu Li a, Jia Jinliang a,
Yang Xuwub, Gao Shenglib
( aSouth China of
Agricultural University, Science of College, Guangzhou, Guangdong, 510642, China; bShaanxi Key Laboratory of Physico-Inorganic
Chemistry, Department of Chemistry, Northwest University, Xi'an Shanxi, 710069, China)
Received March 12, 2008; South China of
Agricultural University for financial Support (4900K07283)
Abstract Thirteen solid
complexes were synthesized with sodium diethyldithiocarbamate (NaEt2dtc·3H2O),
1,10-phenanthroline (o-phen·H2O) and hydrated lanthanide chlorides in
absolute ethanol, which are identified as a general formula of RE(Et2dtc)3(phen)
(RE=La, Pr, Nd, Sm~Lu). IR results revealed that two sulfur atoms in NaEt2dtc
and two nitrogen atoms in o-phen coordinate to RE3+ in bidentate fashion,
respectively. UV spectrum of the complexes suggested energy transfer between o-phen and RE3+
is the primary process, and the main absorbtion peaks showed a slight red shift than that
of o-phen. The constant-volume combustion energies of complexes were determined by a
precise rotating-bomb calorimeter at 298.15K. The standard enthalpies of combustion and
standard enthalpies of formation were calculated for these complexes, respectively. The
experiment results showed "triplet effect" of rare earth.
Keywords rare earth sulfocompound; constant-volume combustion
energy; standard enthalpy of combustion; standard enthalpy of formation; triplet effect
The series of complexes containing lanthanide
sulfide have well biological activity, the usage of them as antiseptic and insecticide
have been attended widely[1]. they also could be used as the precursors of
ceramics and thin film materials[2], grease additive and accelerant of
vulcanizing rubber[3]. Preparation, spectroscopic properties and the crystal
structure of some complexes had been reported [4-5].
Thermodynamic data could offer better interpretation to the essence of
lanthanide-sulfide bonds and stability of this series of complexes, and part investigation
has been carried out concerning the thermochemical properties for these complexes[6-7].In
this paper, constant–volume combustion energy of
thirteen complexes have been determined, the standard enthalpies of combustion and
standard enthalpies of formation have been calculated on the basis of the constant-volume
combustion energies of the complexes, respectively. The gained thermodynamic quantities
presented the "triplet effect" of rare
earth, suggesting that a certain amount of covalence is present in the chemical bonds of
the complexes.
1 EXPERIMENTAL
1.1 Reagents
Lanthanide chloride hydrate, NaEt2dtc ·3H2O,
o-phen·H2O, absolute ethanol and CHCl3 are
the same as the Ref.[6-7]. thianthrene (mass fraction: 99 %, Tokyo Kasei Kogyo
Co. Ltd.) and benzoic acid (purity: 99.999 % , Chengdu chemical reagent company) have been
recrystallized and sublimed three times before using, respectively. The final products
were kept in vacuum over P4O10 to dryness.
1.2 Preparation and composition of the complexes
The methods of preparation for the complexes are the same as those in Ref.[6-7].
RE3+ was determined with EDTA by complexometric titration; C, H, N and S
analyses were carried out by Vario EL III CHNOS of German. The final results are showed in
Table 1. they are identified as a general formula of RE(Et2dtc)3(phen).
1.3 Apparatus and experimental conditions
The constant-volume combustion energies of the complexes were determined by a precise
rotating-bomb calorimeter (RBC-type II), The main experimental procedures and structure
were described previously[8]. The correct value of the heat exchange was
calculated according to Linio-Pyfengdelel-Wsava formula[9].The initial
temperature was regulated to (25.0000 ± 0.0005) ℃,
and the initial oxygen pressure was 2.5MPa. The digital indicator for temperature
measurement was used to promote the precision and accuracy of the experiment.
The calorimeter was
calibrated with benzoic acid of 99.999 % purity, which has an isothermal heat of
combustion of -26434 J·g-1
at 25℃, and the
experimental result were (17775.09 ± 7.43) J·K–1 (Table 2), the precision was 4.18×10-4.
To determine the standard combustion energies of sulfur-containing compounds, the
constant-volume combustion energy of thianthrene has been determined as being (-33507.76
± 14.13) J·g–1 (Table 2) ,which is in good agreement with (-33468 ± 4 ) J·g–1 [10]. The
precision and the accuracy were 4.22×10-4 and 1.19×10-3,
respectively, the calorimetric system is accurate and reliable.
The analytical
methods of final products (gas, liquid and solid) were the same as these in Ref.[8],
the analytical results of the final products indicated that the combustion reactions were
complete.
Table 1 Analytical results related to
the compositions of the complexes (%)
Sample |
RE |
S |
C |
N |
H |
La(Et2dtc)3(phen) |
18.21(18.18) |
42.53(42.45) |
9.09(9.17) |
25.07(25.18) |
4.87(5.01) |
Pr(Et2dtc)3(phen) |
18.30(18.40) |
42.23(42.36) |
9.10(9.14) |
25.07(25.12) |
4.79(5.00) |
Nd(Et2dtc)3(phen) |
18.59(18.75) |
42.08(42.16) |
9.01(9.10) |
24.87(25.01) |
4.69(4.98) |
Sm(Et2dtc)3(phen) |
19.42(19.39) |
41.81(41.82) |
9.00(9.03) |
24.79(24.81) |
4.97(4.94) |
Eu(Et2dtc)3(phen) |
19.57(19.56) |
41.72(41.74) |
9.04(9.01) |
24.77(24.76) |
4.89(4.93) |
Gd(Et2dtc)3(phen) |
20.12(20.10) |
41.44(41.46) |
8.97(8.95) |
24.56(24.59) |
4.91(4.90) |
Tb(Et2dtc)3(phen) |
20.28(20.27) |
41.29(41.37) |
8.99(8.93) |
24.52(24.54) |
4.92(4.89) |
Dy(Et2dtc)3(phen) |
20.85(20.63) |
40.77(41.18) |
8.80(8.89) |
24.89(24.43) |
4.68(4.86) |
Ho(Et2dtc)3(phen) |
20.99(20.88) |
24.82(24.36) |
40.82(41.05) |
8.81(8.86) |
4.57(4.67) |
Er(Et2dtc)3(phen) |
20.30(20.27) |
24.50(24.54) |
41.26(41.37) |
8.99(8.93) |
4.95(4.89) |
Tm(Et2dtc)3(phen) |
21.10(21.28) |
24.32(24.23) |
40.67(40.85) |
8.89(8.82) |
4.76(4.82) |
Yb(Et2dtc)3(phen) |
21.47(21.68) |
24.18(24.11) |
40.81(40.64) |
8.85(8.78) |
4.68(4.80) |
Lu(Et2dtc)3(phen) |
22.01(21.87) |
24.10(24.05) |
40.65(40.54) |
8.64(8.75) |
4.64(4.79) |
a The data in brackets are calculated
values.
Table 2 Experimental results for the
combustion energies of benzoic acid and thianthrene
Samples |
Mass of complexes
m /g |
Calibrated heat of combustion wire qc/J |
Calibrated heat of acid
qN/J |
Calibrated
/K |
Combustion energies of complexes
-/(J·g-1) |
|
0.99702,0.78940 |
10.35, 8.10 |
24.78, 20.89 |
1.4834, 1.1746 |
17790.45, 17789.88 |
benzoic acid |
0.83060, 0.96869 |
12.60,12.60 |
20.43, 17.43 |
1.2382, 1.4418 |
17758.93, 17780.82 |
|
0.99485, 0.90036 |
12.60, 9.28 |
20.80, 21.67 |
1.4800, 1.3429 |
17798.18, 17745.97 |
|
|
|
|
mean±SD |
17775.09±7.43 |
|
0.48860, 0.48886 |
12.60, 11.70 |
1383.69, 1384.41 |
0.9998, 1.0015 |
33514.62, 33558.98 |
thianthrene |
0.49011, 0.48798 |
12.60, 12.60 |
1387.90, 1381.96 |
1.0028, 0.9977 |
33511.58, 33484.26 |
|
0.48835, 0.48823 |
12.60, 12.60 |
1382.99, 1382.65 |
0.9977, 0.9992 |
33456.78, 33520.31 |
|
|
|
|
mean±SD |
33507.76±14.13 |
SD=
2 RESULTS AND DISCUSS
2.1 IR spectra of the complexes
IR spectra of the complexes are similar because of their similar structure[11,12]:
the peaks of about 3340 cm-1 are assigned to the characteristic absorption of
hydroxyl group in hydrated lanthanide chlorides and ligands, which is not present in the
complexes , showing that the complexes does not contain water. The skeleton vibration and
the nC–H bend vibration of benzene ring of o-phen in
the complexes are shift to higher wave number compared to that of the free ligand,
suggesting that two nitrogen atoms of o-phen coordinate to RE3+. In
contrast to that of 1477 cm-1 in the ligand diethyldithiocarbamate, nCN
of the complex shiftes to higher wave number(1480~1517 cm-1), and presentes a
double-bond character in the complex, which can be attributed to two main forms of
vibration in the NCS group [13]:
(i) and (ii) the vibration intensity of the later will be enhanced when the two sulfur
atoms of the ligand diethyldithiocarbamate coordinate to RE3+ to form the new
cycle (ⅲ), thus nCN
moves to a higher wave number. Comparing with 986cm-1 of
diethyldithiocarbamate, the increment of 9~18 cm-1 in wave number of ncss
stretching vibration in the complexes can be attributed to the new formed cycle, because
its formation increases the vibration intensity of nCN[12]. The changes in nCN and
nCSS
indicate that the sulfur atoms of diethyldithiocarbamate coordinate to RE 3+
in bidentate manner. The coordinate number is eight. The main IR absorbtion data of the
ligands and the complexes were listed in Table 3.
(i)
(ii)
(iii)
2.2 UV spectra of the complexes
The UV spectra of the complexes and ligands were determined by a instrument of Perkielmer
Lambda 40 of America, the lmax were listed in Table 3. Intraligand
transition (p→p*, n→p*) were displayed at about
329.56nm and 380.12nm for the free ligand NaEt2dtc·3H2O
[14], and characteristic transition (p→p*) of o-phen was present at 265.05 nm[15]. As for
the complexes, the absorption peaks were well similar, whether shape, absorbency or place
of peaks (Fig.1), which demonstrate that energy transfer between o-phen and RE3+
is the primary process[15], and strong absorption of o-phen fully or partly
shield that of NaEt2dtc·3H2O in the complexes[17]. In
addition, the main absorption peaks of the complexes show a slight red shift than that of
o-phen, which was due to pelectrons of nitrogen atoms of o-phen have excursion to the 5d
blank orbits of RE3+, and resulting to the increment of p electron conjugate action for
the whole system, when s-coordinate band of the complexes were formed between
nitrogen atoms of o-phen and RE 3+.
Table 3 The main UV and IR
absorbtion data of the ligands and the complexes
Ligands and complexes |
nOH |
nC═C |
nC─H |
nCN |
nCSS |
(CSS ) |
lmax |
LnCl3·nH2O (n<4) |
3349-3393 |
|
|
|
|
|
o-phen ·H2O |
3388 |
1617,1587, 1561, 1504 |
854, 739 |
|
|
|
265.05 |
NaEt2dtc ·3 H2O |
3366 |
|
|
1477 |
986 |
|
329.55
|
La(Et2dtc)3(phen) |
|
1624, 1588, 1572, 1516 |
848, 729 |
1480, 1516 |
995 |
9 |
266.59 |
Pr(Et2dtc)3(phen) |
|
1622, 1589, 1570, 1515 |
851, 730 |
1480,1515 |
997 |
11 |
266.93 |
Nd(Et2dtc)3(phen) |
|
1624, 1589, 1572, 1516 |
851, 730 |
1482, 1516 |
997 |
11 |
267.26 |
Sm(Et2dtc)3(phen) |
|
1623, 1589, 1571, 1516 |
852, 730 |
1481, 1516 |
995 |
9 |
267.77 |
Eu(Et2dtc)3(phen) |
|
1624, 1589, 1572, 1516 |
852, 730 |
1482, 1516 |
1002 |
16 |
267.49 |
Gd(Et2dtc)3(phen) |
|
1624, 1589, 1572, 1516 |
852, 730 |
1481, 1516 |
1003 |
17 |
267.94 |
Tb(Et2dtc)3(phen) |
|
1624, 1589, 1572, 1516 |
852, 730 |
1482, 1516 |
1003 |
17 |
267.91 |
Dy(Et2dtc)3(phen) |
|
1624, 1589, 1572, 1517 |
853, 730 |
1482, 1517 |
1001 |
15 |
267.85 |
Ho(Et2dtc)3(phen) |
|
1625, 1589, 1572, 1517 |
853, 730 |
1482, 1517 |
1006 |
20 |
268.10 |
Er(Et2dtc)3(phen) |
|
1625, 1590, 1572, 1517 |
853, 730 |
1482, 1517 |
1007 |
21 |
267.30 |
Tm(Et2dtc)3(phen) |
|
1625, 1590, 1572, 1517 |
853, 730 |
1482, 1517 |
1007 |
21 |
268.39 |
Yb(Et2dtc)3(phen) |
|
1625, 1590, 1572, 1517 |
854, 730 |
1481, 1517 |
1006 |
20 |
267.95 |
Lu(Et2dtc)3(phen) |
|
1625, 1590, 1572, 1517 |
854, 730 |
1482, 1517 |
1004 |
18 |
267.89 |
Figure 1 UV absorption curves of ligand o-phen(1)
and Complexes La(Et2dtc)3(phen)(2),Sm(Et2dtc)3(phen)(3)
and Lu(Et2dtc)3(phen)(4)
2.3 Combustion energies,
standard combustion enthalpies and standard enthalpies of formation for the complexes
The methods of determination and calculation of the constant-volume combustion
energies () for the complexes are the same
as benzoic acid and thianthrene[6].
The standard combustion enthalpies of the complexes () refer to the combustion enthalpy change of the
following ideal combustion reaction at 298.15 K and 100 kPa.
RE(Et2dtc)3(phen) (s) + O2 (g) = RE2O3
(s) + 27CO2 (g) + 19 H2O+ 6 SO2 (g) + N2 (g) (1)
(RE=La, Pr, Nd, Sm~Lu)
The standard combustion enthalpies of the complexes are calculated by
the following equations:
(complex, s, 298.15K) =(complex, s, 298.15K) +RT (2)
= ng (products) - ng(reactants)
(3)
where ng is the total amount in mole of gases which present in products
or in reactants, R = 8.314 J·K-1·mol-1,
T = 298.15K.
The standard enthalpies of formation of the complexes () are calculated by Hess's law according to the
thermochemical equation above (1)
(RE(Et2dtc)3(phen), s) = [
(RE2O3, s) + 27 (CO2,
g) + 19 (H2O,l)
+ 6 (SO2, g) + (N2
, g)] - (RE(Et2dtc)3(phen),
s) (4)
where (RE2O3, s) = (-1793.14 ± 0.79) (La), (-1823.39 ±
6.69) (Pr), (-1808.12 ± 1.00) (Nd), (-1808.12 ±1.00) (Sm), (-1663.00 ± 1.62) (Eu),
(-1815.60 ± 3.60) (Gd), (-1827.6 ± 2.0) (Tb), (-1865.39 ± 3.89) (Dy), (-1880.92 ±
4.81) (Ho), (-1897.29 ± 4.88) (Er), (-1888.66 ± 5.86) (Tm), (-1814.50 ± 2.22) (Yb),
(-1881.96 ± 7.53) (Lu) kJ ·mol-1; (CO2, g) = (-393.51 ± 0.13) kJ·mol-1,
(H2O, l) = (-285.830 ± 0.042)
kJ·mol-1, (SO2,
g) = ( -296.81 ± 0.20) kJ·mol-1 [17,18], The final results are also
listed in Table 4.
Table 4 Combustion energies, standard
combustion enthalpies and standard enthalpies of formation of the complexes at 298.15K
Complexes |
/ (kJ·mol-1) |
/ (kJ·mol-1) |
/ (kJ·mol-1) |
La(Et2dtc)3(phen) |
-17455.98 ± 7.98 |
-17475.19 ± 7.98 |
-1257.78 ± 8.84 |
Pr(Et2dtc)3(phen) |
-17840.67 ± 10.38 |
-17859.88 ± 10.38 |
-888.22 ± 11.55 |
Nd(Et2dtc)3(phen) |
-18674.22 ± 8.33 |
-18693.43 ± 8.33 |
-47.03 ± 9.17 |
Sm(Et2dtc)3(phen) |
-17406.90 ± 9.69 |
-17426.11 ± 9.69 |
-1317.99 ± 10.45 |
Eu(Et2dtc)3(phen) |
-17410.63 ± 8.95 |
-17429.84 ± 8.95 |
-1238.06 ± 9.75 |
Gd(Et2dtc)3(phen) |
-18673.71 ± 8.15 |
-18692.92 ± 8.15 |
-51.28 ± 9.17 |
Tb(Et2dtc)3(phen) |
-17646.95 ± 8.64 |
-17666.16 ± 8.64 |
-1084.04 ± 9.49 |
Dy(Et2dtc)3(phen) |
-16730.21 ± 9.25 |
-16749.42 ± 9.25 |
-2019.68 ± 10.19 |
Ho(Et2dtc)3(phen) |
-18213.19± 8.18 |
-18232.40 ± 8.18 |
-544.46 ± 9.33 |
Er(Et2dtc)3(phen) |
-18436.62± 9.11 |
-18455.83 ± 9.11 |
-329.48 ± 9.91 |
Tm(Et2dtc)3(phen) |
-18161.61± 8.46 |
-18180.82 ± 8.46 |
-599.91 ± 9.73 |
Yb(Et2dtc)3(phen) |
-17954.08± 8.11 |
-17973.29 ± 8.11 |
-770.36 ± 9.02 |
Lu(Et2dtc)3(phen) |
-17898.22± 8.59 |
-17917.43 ± 8.59 |
-859.95 ± 10.12 |
Figure 2 plot of Dn( CSS ) against the atomic number (Dn(CSS) is the
stretching vibration difference between diethyldithiocarbamate
and complexes )
Figure 3 Plots of and
against the atomic numbers (ZRE) of rare-earth for the complexes
●; ■
3 CONCLUSIONS
and of the complexes are plotted against the atomic numbers of the elements in
the lanthanide series, as showed in Fig.3. The curves show the "tripartite
effect" of rare earth, which is consistent with
the observed result in Fig.2, suggesting that a certain amount of covalence is present in
the chemical bonds between RE3+ and ligands that is caused by the incomplete
shield of 5s25p6 orbital to 4f electrons. The
experimental results is in good agreement with Nephelauxetic effect of 4f electrons of
rare earth.
On the basis of Fig.3, the
corresponding thermochemical data (standard combustion enthalpies, standard enthalpies of
formation ) of Ce(Et2dtc)3(phen) and Pm(Et2dtc)3(phen)
could be estimated.
REFERENCES
[1] Marinho E.P., Sousa W.S.C., Melo D.M.A. Thermochim. Acta. 2000, 344: 67.
[2] Ivanoy, R. A., Korsakoy, I. E., Kuzmina, N. P. et al., Mendeleev Commun. 2000, 3: 98.
[3] Zhang W G., Yin X., Fan J. et al., J. Rare Earth(Xitu Xuebao). 2004, 22 (3): 299.
[4] Su C. Y., Tan, M. Y., Tang, N. et al., J. Coord. Chem. 1996, 38 (3): 207.
[5] Zhou R, Sun Y H. J. Xinjiang Univ.(Xinjiang Daxue Xuebao). 1997, 14 (4): 67.
[6] Zhu L., Yang X.W., Chen S.P., et al., J. Inorg. Chem. 2004, 20 (11): 1303.
[7] Zhu L., Jiao B.J., Shuai Q. et al., Chin. J. Org. Chem. 2004, 24 (11): 1417.
[8] Yang, X. W., Chen, S. P., Gao, S. L. et al., Instrum. Sci. & Technol. 2002,
30 (3): 311.
[9] Popov, M. M., Thermometry and Calorimetry, Moscow: Moscow University Publishing House,
1954: 382.
[10] Marthada, V. K., Journal of Research of the National Bureau of Standard, 1980, 85
(6): 467.
[11] Dong Q.N. IR Spectroscopy(Hongwai Guangpu), Chemical and Industrial Press,
Beijing,1979, p.194.
[12] Nakamoto K.( Huang D.H., Wang R.Q Translated) Infrared and Raman Spectra of Inorganic
and Coordination Compounds(Wuji Peihewu de Hongwai ji Laman Guangpu). 4th Edn. Beijing:
Chemical Industriy Press, 1991.
[13] Nakamoto K., Fujita J., Condrate R. A. et al., Chem. Phys. 1963, 39: 423.
[14] Crosby G.A., Whan R.E., Alire R.M. J. Chem. Phys.1961,34 (3): 743.
[15] Yan B., Zhang H.J., Wang S.B. J. Rare Earth(Xitu Xuebao).1998, 16 (4): 375.
[16] Sokolov V.V., Kamarzin A.A., Trushnikova L.N. et al., J. Alloy. Comp.1995, 225: 567.
[17] Rederick, D. R., Experimental Therrnochemistry. Interscience Publishers Ltd., 1956:
88.
[18] Robert, C. W., CRC Handbook of Chemistry and Physics, Chemical Rubber Publishing
Company, 1977-1978, 55: D45.
稀土含硫配合物的恒容燃烧能测定及标准摩尔生成焓计算
朱丽a 贾金亮a 杨旭武b 高胜利b
(a华南农业大学 理学院 广东 广州 510642; b西北大学化学系 陕西省物理无机化学重点实验室 陕西
西安 710069)
摘要 在无水乙醇中,通过二乙基二硫代氨基甲酸钠(NaEt2dtc),1,10-邻菲咯啉(o-phen)和水合氯化稀土盐反应制备得到了13种稀土含硫固态配合物,其通式为RE(Et2dtc)3(phen) (RE=La, Pr, Nd, Sm~Lu)。配合物的红外光谱表明配体NaEt2dtc中的硫原子和o-phen中的氮原子均与RE3+双齿配位。紫外光谱显示在配合物中邻菲咯啉与稀土离子之间的能量传递为主要过程,且其最大吸收峰的位置相对邻菲咯啉的都有微小红移。在298.15K下,通过RBC- II型精密转动弹热量计测定了配合物的恒容燃烧能,并分别计算了标准摩尔燃烧焓及标准摩尔生成焓。所得实验结果显示出了稀土元素的“三分组效应”。
关键词 稀土含硫配合物; 恒容燃烧能;
标准摩尔燃烧焓;标准摩尔生成焓;三分组效应
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