4,6-二甲基-N-苯基-2-嘧啶胺的低温热容和热力学性质

通过小样品精密自动绝热量热计测定了合成并提纯的 4,6 二甲基 N 苯基 2 嘧啶胺 (嘧霉胺 )在 78～ 3 91K温区的摩尔热容 .量热实验发现 ,该化合物在 3 63～ 3 72K温区 ,有一固 -液熔化相变过程 ,经三次重复测量 ,得其熔化温度、摩尔熔化焓及摩尔熔化熵分别为 :( 3 70 78± 0 0 8)K ,( 2 1 2 3 3± 0 0 13 )kJ·mol-1 和 ( 5 7 2 7± 0 15 )J·mol-1 ·K-1 .通过分步熔化法得到该物质绝对纯样品的熔点为 3 71 0 3 1K .用差示扫描量热 (DSC)技术对该物质的固 -液熔化过程作了进一步研究 ,结果与绝热量热法一致     

卟啉化合物的热化学研究Ⅰ. 精密燃烧量热装置及标定

本文报道了一套用热敏电阻作测温元件的精密静弹燃烧量热装置。数据处理用电子计算机按自编程序完成。用中国计量科学院提供的量热基准苯甲酸标定了量热计的能当量, 其精密度(2s.d.m计)为0.01％。利用此仪器测得三羟甲基氨基甲烷的燃烧能为△_cu°(298.15 K)=-20030.3±6.0 Jg~(-1), 与文献值吻合, 证实了本装置的可靠性。     

精密溶解量热装置的建立与标定

本文报道了自行建立的用热敏电阻作为测温元件的精密溶解量热装置,并用量热标准物质光谱纯氯化钾和美国国家标准局提供的三羟甲基氨基甲烷(TRIS)对仪器进行了标定,在25℃所得实验结果:KCI溶解焓为17518±15 J·mol~(-1);TRIS与0.1 mol/L HCI的反应焓为-29729±31J·mol~(-1),与文献值吻合,检验了该装置的可靠性.     

苯氧威 (C17H19NO4) 的热容和热力学性质

通过小样品精密自动绝热量热计测定了自己合成并提纯的苯氧威 (C₁₇H₁₉NO₄) 在79 ～ 360 K温区的低温摩尔热容。量热实验发现, 该化合物在320 ~ 330 K温区, 有一固 - 液熔化相变过程, 其熔化温度为（326.31±0.14）K, 摩尔熔化焓、摩尔熔化熵及化合物的纯度分别为：(26.98±0.04) kJ• mol^-1和（82.69 0.09）J•mol^-1•K^-1和 (99.53±0.01 )%。并计算出了80-360 K的热力学参数。用分步熔化法得到绝对纯化和物的熔点为326.60±0.06 K。用差示扫描量热 (DSC) 技术对该物质的固-液熔化过程作了进一步研究，结果与绝热量热法一致。     

4-硝基苯甲醇的低温热容和标准摩尔生成焓

用精密自动绝热量热计测定了4-硝基苯甲醇（4-NBA）在78 ~ 396 K温区的摩尔热容。其熔化温度、摩尔熔化焓及摩尔熔化熵分别为:(336.426 ± 0.088) K, (20.97 ± 0.13) kJ×mol-1 和 (57.24 ± 0.36) J×K-1×mol-1.根据热力学函数关系式,从热容值计算出了该物质在80 ~ 400 K温区的热力学函数值 [HT - H298.15 K] 和[ST - S298.15 K]. 用精密氧弹燃烧量热计测定了该物质在T＝298.15 K的恒容燃烧能和标准摩尔燃烧焓分别为 (C7H7NO3, s)＝- ( 3549.11 ± 1.47 ) kJ×mol-1 和 (C7H7NO3, s)＝- ( 3548.49 ± 1.47 ) kJ×mol-1. 利用标准摩尔燃烧焓和其他辅助热力学数据通过盖斯热化学循环, 计算出了该物质标准摩尔生成焓 (C7H7NO3, s)＝- (206.49 ± 2.52) kJ×mol-1 .     

一种精密恒温环境微量燃烧-溶解-反应多用量热计的设计及应用

将SRC-100型溶解-反应量热计改进成了一种精密恒温环境微量燃烧-溶解-反应多用量热计。采用电能法标定了量热计的能当量,其值为Ccalor=(987.63±0.61)J×K~(-1)。用该量热计分别测定了苯甲酸和丁二酸的标准质量燃烧热,分别为ΔcU~θ_(m,B)(cr,T=298.15 K)=-(26425.99±10.70)J?g~(-1)和Δ_cU~θ_(m,S)(cr,T=298.15 K)=-(12621.97±5.30)J?g~(-1)。测量的不确定度小于0.04%,精度高于0.05%。     

用于α-胰凝乳蛋白酶固定化的氨基超顺磁纳米凝胶的光化学合成与表征

通过霍夫曼降解光化学原位聚合制备的聚丙烯酰胺包覆的Fe3O4纳米粒子得到了氨基化磁性纳米凝胶, 用缩合剂1-乙基-3-(3-二甲胺)碳二亚胺成功地将α-胰凝乳蛋白酶固定到氨基化磁性纳米凝胶上, 并采用光子相关光谱、傅里叶变换红外光谱、透射电子显微镜、X射线粉末衍射和热重-示差扫描量热联用等多种手段对其进行了表征. 固定化了的α-胰凝乳蛋白酶平均粒径约为31 nm; 热重法测得每克凝胶上的载酶量为69 mg, BCA 法测得每克凝胶上的载酶量为61 mg; 酶的固定化和氙灯辐照并未改变Fe3O4的晶形结构; 固定化酶比活力为0.93 U/(mg·min), 为自由酶活力的59.3%; 磁含量高达88%, 具有优异的磁响应性能, 可应用于诸多生物医药领域的快速检测、分离及酶的再生利用.     

5-氯-2-甲氧基苯甲酸与1,10-邻菲啰啉稀土配合物的合成、表征及热分解机理

合成了三种稀土配合物[Ln(5-Cl-2-MOBA)3phen]2(Ln=Nd(1),Eu(2),Ho(3);5-Cl-2-MOBA:5-氯-2-甲氧基苯甲酸根;phen:1,10-邻菲啰啉),通过元素分析、热重-微分热重-差示扫描量热(TG-DTG-DSC)、红外光谱(IR)、紫外光谱(UV)及摩尔电导等技术对标题配合物进行了表征.荧光光谱表明配合物(2)发出铕离子的特征荧光.用热分析/傅里叶变换红外(TG-DSC/FTIR)联用技术,阐明标题配合物的热分解反应机理,并分析了逸出气体的三维(3D)红外光谱.     

用于α-胰凝乳蛋白酶固定化的氨基超顺磁纳米凝胶光化学合成与表征

通过霍夫曼降解光化学原位聚合制备的聚丙烯酰胺包覆的Fe3O4纳米粒子得到了氨基化磁性纳米凝胶,用缩合剂1-乙基-3-(3-二甲胺)碳二亚胺成功地将α-胰凝乳蛋白酶固定到氨基化磁性纳米凝胶上,并采用光子相关光谱、傅里叶变换红外光谱、透射电子显微镜、X射线粉末衍射和热重-示差扫描量热联用等多种手段对其进行了表征.固定化了的α-胰凝乳蛋白酶平均粒径约为31 nm;热重法测得每克凝胶上的载酶量为69 mg,BCA 法测得每克凝胶上的载酶量为61 mg;酶的固定化和氙灯辐照并未改变Fe3O4的晶形结构;固定化酶比活力为0.93 U/(mg·5min),为自由酶活力的59.3%;磁含量高达88%,具有优异的磁响应性能,可应用于诸多生物医药领域的快速检测、分离及酶的再生利用.     

腈菌唑的热容和热力学性质

通过小样品精密自动绝热热量计测定了自己合成并提纯的腈菌唑 (C₁₅H₁₇ClN₄) 在78 ～ 368K温区的低温摩尔热容。量热实验发现, 该化合物在363 ~ 372 K温区, 有一固-液熔化相变过程, 其熔化温度为 (348.800±0.06)K, 摩尔熔化焓、摩尔熔化熵及化合物的纯度分别为：(30931±11) J•mol^-1、(88.47±0.02) J•mol^-1•K^-1和0.9941(摩尔分数)。用差示扫描量热(DSC) 技术对该物质的固-液熔化过程作了进一步研究，结果与绝热量热法一致。     

Determination of the enthalpy of solute-solvent interaction from the enthalpy of solution: aqueous solutions of erythritol and L-threitol

In this work the enthalpy of the solute-solvent interaction of erythritol and L-threitol in aqueous solution was determined from the values obtained for the enthalpy of solvation. The values for this property were calculated from those determined for the enthalpies of solution and sublimation. To determine the values of the enthalpy of solute-solvent interaction, the solvation process is considered as taking place in three steps: opening a cavity in the solvent to hold the solute molecule, changing the solute conformation when it passes from the gas phase into solution, and interaction between the solute and the solvent molecules. The cavity enthalpy was calculated by the scaled particle theory and the conformational enthalpy change was estimated from the value of this function in the gas phase and in solution. Both terms were determined by DFT calculations. The solvent effect on the solute conformation in solution was estimated using the CPCM solvation model. The importance of the cavity and conformational terms in the interpretation of the enthalpy of solvation is noted. While the cavity term has been used by some authors, the conformational term is considered for the first time. The structural features in aqueous solution of erythritol and L-threitol are discussed.     

Solvation of amides of formic and acetic acids in water-glycerol mixture. Additivity of thermochemical characteristics of solutions

Values of the solution enthalpy of are measured and values of solvation enthalpy are calculated for formamide and N,N-two-substituted methyl-and ethylamides of formic and acetic acids in the mixed solvent: water-glycerol. Enthalpy coefficients of pair interactions between amides and glycerol in aqueous solutions are calculated. The influence of mixture composition and also of a structure and properties of the dissolved compounds on enthalpy characteristics is considered. Within the frames of the offered additive scheme the contributions from the structural fragments of molecules of amides to enthalpy characteristics of solutions are established. It has allowed us to analyze quantitatively the role of nonspecific and specific solvation of amides in solution, to predict the enthalpy of evaporation, solution, solvation, the enthalpy coefficients of pair interactions of experimentally unstudied N-methylformamide, N-ethylformamide, N-methyl-N-ethylformamide, N-methylacetamide, N-ethylacetamide, and N-methyl-N-ethylacetamide in the mixtures of water-glycerol, and also to evaluate the donor numbers of these specified amides.     

Theoretical calculation of the retention enthalpy effect on the viscous heat dissipation band broadening in high performance liquid chromatography columns with a fixed wall temperature

The problem of the additional band broadening arising from the trans-column temperature profile under conditions of significant viscous heat dissipation has been extended by including the retention enthalpy effect. This effect can significantly aggravate the trans-column migration velocity profile of retained species as compared to the already known zero-retention enthalpy case. An approximate analytical solution for the accompanying additional band broadening could be established. The solution is valid in nearly all practically relevant cases and shows how the additional band broadening varies as a function of the generated heat, the retention coefficient and the retention enthalpy. Surveying all possible HPLC operating conditions, it was found that the inclusion of the retention enthalpy effect leads to significantly larger viscous heating plate height contributions than those predicted by the zero-retention enthalpy solution (up to a factor of 10 or more).     

Thermal behaviour of some sugar alcohols

The glass transition of isomalt and its components, the enthalpy of solution (crystalline state, glassy state) and the enthalpy of melting are reported. From the measured data (solution enthalpy, enthalpy of fusion and heat capacities) a cycle like the BORN-HABER cycle can be constructed. It is possible to calculate the amounts of amorphous isomalt from measured solution enthalpies; however, the values obtained do not agree with those provided by X-ray powder diffraction studies.This study was supported by Südzucker AG, Mannheim/Ochsenfurt. We thank Dr. M. Kunz and G. Witte of Südzucker AG for discussions.     

Thermochemical properties of dinitramidic acid salts

Enthalpies of formation and solution of hydrazinium, guanidinium, aminoguanidinium, and triaminoguanidinium salts of nitric and dinitramidic (HN(NO₂)₂, DN) acids were determined by combustion and solution calorimetry methods. Enthalpies of formation of respective cations in infinitely dilute aqueous solution were calculated using the enthalpy of formation of the nitrate ion. The enthalpy of formation of the DN acid anion was determined based on the enthalpy of formation and solution of the acid salts. The weight-average enthalpy of formation of the DN acid anion equal to 8.40±0.13 kcal mol⁻¹ was obtained. The enthalpy of solution of ammonium dinitramide (ADN) was measured (8.71±0.01 kcal mol⁻¹). From these data, the enthalpy of formation of ADN was calculated (−32.14±0.14 kcal mol⁻¹). The energy of combustion of ADN was measured by the calorimetry method, and the enthalpy of formation of ADN was calculated for a sample with purity above 99.9% (−32.20±0.19 kcal mol⁻¹). The weight-average enthalpy of formation of ADN equal to −32.16±0.11 kcal mol⁻¹ is recommended for use. Enthalpies of formation of sodium, potassium, and cesium salts of DN acid were determined.     

Enthalpy of solution of phenoxyalcohols solubilized in aqueous sodium dodecylsulfate and hexadecyltrimethylammonium bromide solutions

The enthalpy of solution of phenoxy 2-ethanol, 1 phenoxy,-3 propanol and benzylalcohol was determined at 25 °C in aqueous sodium dodecylsulfate and hexadecyltrimethylammonium bromide solution, up to 0.2 mol/kg surfactant concentration. Using the pseudo-phase model, the standard enthalpy of transfer and the partition coefficient of the alcohols between micelle and water are calculated. The latter quantity is found to be systematically larger when derived from enthalpy than from free energy measurements. Using the so-called compensation plot, the solution thermodynamics of aromatic and aliphatic alcohols in aqueous sodium dodecylsulfate and in the octane+water systems are compared. Aromatic alcohols display an anomalous behavior in the octane+ water system but not in the micellar one.The standard enthalpy of solution of various alcohols presents, when plotted against hexadecyltrimethylammonium bromide concentration, a shoulder in the region around 0.05 mol/kg; a discussion is presented on the evidence for alleged micellar structural changes in aqueous micellar systems.     

Enthalpies of solution in water of urotropine as function of concentration and temperature

Enthalpies of solution of Hexamethylenetetramine in water at several molal concentrations and at four temperatures (278.15, 288.15, 298.15, and 308.15) K were determined. The values of enthalpy of solution at infinite dilution were combined with the enthalpy of sublimation to get the corresponding enthalpies of hydration. The change in heat capacity at infinite dilution was calculated.     

Thermochemistry of complex salts of transition metal perchlorates with tetrazole ligands

The combined use of combustion and solution calorimetry was proposed as a method for determining the standard enthalpy of formation of the complex salts of transition metals, viz., cobalt(II), nickel(II), and zinc, with the organic ligand (5-aminotetrazol-1-yl)acethydrazide. The enthalpies of solution in water and in a 0.1 M solution of hydrochloric acid were measured for the complex salts and ligand. The enthalpy of combustion of the ligand was determined by the combustion calorimetry method, and its standard enthalpy of formation was calculated. The thermochemical cycle was developed for determining the standard enthalpy of formation of the complex salts. The reliable values of the enthalpies of formation of the salts in the standard states were obtained, and the enthalpies of formation of the earlier unknown complex ions were determined.     

量热法测定氯化钐与甘氨酸配合物的标准生成焓

稀土在生命科学领域的研究日益受到人们关注,稀土化合物所具有的抑菌、抑癌、消炎等作用及其作用机理的探讨已有报道［１～３］。最近几年稀土在生物领域中的研究又有了新的突破和进展,从稀土与氨基酸、蛋白质、膜脂及膜蛋白的作用到其对ＤＮＡ。ＲＮＡ的影响［１,４］,从稀土的分子水平、细胞及亚细胞水平到动物整体实验的系统研究［５,６］等,分别从不同的层次、不同的水平研究了稀土的生物效应。但至目前为止,稀土的生物效应机理及其对人体的影响尚未得到令人满意的解释。由于氨基酸是构成人体蛋白质的基本单位,故研究稀土与氨基…     

Effect of NaCl on the excess enthalpies of binary liquid systems

The excess molar enthalpies h^E₁₊₂₃ of ethanol+(water+NaCl), benzylalcohol+(water+NaCl), and cyclohexane+(methanol+NaCl) were measured at 298.15 K, those of methanol+(water+NaCl) at 298.15 and 323.15 K. An LKB flow microcalorimeter was used and a special flow-mix cell was developed with regard to the corrosive electrolyte solutions. Knowing the integral enthalpy of solution and the solution enthalpy at infinite dilution for a salt (3) in a solvent (2), the molar excess enthalpy h^E₁₂₃ can be calculated.