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Thermochemistry of the ternary complex Nd(Et n dtc) 3 (phen)
Author(s) -
Fan XueZhong,
Chen SanPing,
Gao ShengLi,
Jiao BaoJuan,
Hu RongZu,
Shi QiZhen
Publication year - 2004
Publication title -
chinese journal of chemistry
Language(s) - English
Resource type - Journals
SCImago Journal Rank - 1.28
H-Index - 41
eISSN - 1614-7065
pISSN - 1001-604X
DOI - 10.1002/cjoc.20040220805
Subject(s) - chemistry , thermochemistry , standard enthalpy of formation , enthalpy , ternary operation , thermochemical cycle , standard enthalpy of reaction , neodymium , gibbs free energy , calorimetry , enthalpy of atomization , calorimeter (particle physics) , analytical chemistry (journal) , standard enthalpy change of formation , thermodynamics , catalysis , organic chemistry , laser , physics , hydrogen production , electrical engineering , engineering , detector , computer science , optics , programming language
The ternary solid complex has been synthesized with sodium diethyldithiocarbamate (NaEt 2 dtc·3H 2 O), 1,10‐phenanthroline ( o ‐phen·H 2 O) and hydrated neodymium chloride in absolute ethanol. The title complex was identified as the general formula of Nd(Et 2 dtc) 3 (phen) by chemical and elemental analyses. IR spectrum of the complex showed that the Nd 3+ coordinated with six sulfur atoms of three NaEt 2 dtc and two nitrogen atoms of o ‐phen. It was assumed that the coordination number of Nd 3+ is eight. The enthalpy change of liquid‐phase reaction of formation, Δ r H Θ m(1), was determined as (‐12.274±0.050) kJ·mol −1 at 298.15 K by a microcalorimeter, the enthalpy change of the solid‐phase reaction of formation, Δ r H Θ m(s), was calculated as (149.069±0.314) kJ·mol −1 on the basis of a thermochemical cycle. The thermodynamics of reaction of formation was studied by changing the temperature of liquid‐phase reaction. The constant‐volume combustion energy of the complex, Δ c U , was determined as (‐18674.22±8.33) kI·mol −1 by a precise rotating‐bomb calorimeter at 298.15 K. Its standard enthalpy of combustion, Δ c H Θ m , and standard enthalpy of formation, Δ f H Θ m , were calculated as (‐18693.43 ± 8.33) kJ·mol −1 and (‐47.03 ± 9.17) kJ·mol −1 , respectively.