高等学校化学学报

高等学校化学学报

• 研究论文 • 上一篇    下一篇

过渡金属离子液体[C2mim][FeCl4]的溶解热

张子富1, 王恒1, 房大维1,2, 杨家振1   

  1. 1. 辽宁大学化学学院, 沈阳 110036; 2. 中科院青海盐湖研究所, 西宁 810008
  • 收稿日期:2007-07-12 修回日期:1900-01-01 出版日期:2008-03-10 发布日期:2008-03-10
  • 通讯作者: 杨家振

Studies on the Enthalpy of Solution of Ionic Liquid [C2mim][FeCl4] Based on Transition Metal

ZHANG Zi-Fu1, WANG Heng1, FANG Da-Wei1,2, YANG Jia-Zhen1*   

  1. 1. College of Chemistry, Liaoning University, Shenyang 110036, China;2. The Institute of Salt Lakes, Chinese Academy of Sciences, Xining 810008, China
  • Received:2007-07-12 Revised:1900-01-01 Online:2008-03-10 Published:2008-03-10
  • Contact: YANG Jia-Zhen

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被引次数

5

摘要： 在干燥氩气氛下, 用等摩尔的高纯无水FeCl3和氯化1-甲基-3-乙基咪唑([C2mim][Cl])直接搅拌混合, 制备棕色透明的含过渡金属铁的离子液体[C2mim][FeCl4]. 在298.15 K下, 利用具有恒温环境的溶解反应热量计测定了这种离子液体的摩尔溶解焓(ΔsHm). 针对[C2mim][FeCl4]溶解于水后即分解的特点, 在Pitzer电解质溶液理论基础上, 提出了确定这种离子液体标准摩尔溶解焓的新方法, 得到了[C2mim][FeCl4]的标准摩尔溶解焓(ΔsH 0—m=-76.6 kJ/mol), 以及Pitzer焓参数组合: β(0)LFe,Cl+β(0)L[C2mim], Cl+ΦLFe,[C2mim]=0.072209和β(1)LFe,Cl+β(1)L[C2mim], Cl=0.15527. 借助热力学循环和Glasser离子液体晶格能理论, 用Fe3+, Cl-和[C2mim]+的离子水化焓数据以及[C2mim][FeCl4]标准摩尔溶解焓, 估算得到了配离子[FeCl4]-(g)解离成Fe3+(g)和4Cl-(g)的解离焓为5659 kJ/mol. 这个结果揭示了离子液体[C2mim][FeCl4]的标准摩尔溶解焓绝对值并不很大的原因, 即很大的离子水化焓被很大的[FeCl4]-(g)的解离焓相互抵消.

关键词: 离子液体, 溶解焓, Pitzer溶液理论, 恒温环境的溶解反应热量计

Abstract: A brown and transparent ionic liquid,[C2mim][FeCl4], was prepared by mixing anhydrous FeCl3 with 1-methyl-3-ethylimidazolium chloride([C2mim][Cl]), with molar ratio 1∶1 under stirring in a glove box filled with dry argon. The molar enthalpies of solution, ΔsHm, of [C2mim][FeCl4] in water with various molalities were determined by a solution-reaction isoperibol calorimeter at 298.15 K. In terms of Pitzer electrolyte solution theory, the standard molar solution enthalpy of [C2mim][FeCl4], ΔsH0m, and the sum of Pitzer parameters: (β(0)LFe,Cl+β(0)L[C2min],Cl+ΦLFe,[C2min]) and (β(1)LFe,Cl+β(1)L[C2min],Cl) were obtained, respectively. Using the values of the solution enthalpies and crystal energy of the ionic liquid, the dissociation enthalpy of [FeCl4]- anion, ΔHdis≈5659 kJ/mol, for the reaction: [FeCl4]-(g)→Fe3+(g)+4Cl-(g), was estimated. It is shown that the enthalpy of solution of the[C2mim][FeCl4] is small because the large hydration enthalpies of Fe3+, 4Cl- and [C2mim]- was compensated by the large dissociation enthalpy of [FeCl4]- anion, ΔdHm, in dissolution process of the IL.

Key words: Ionic liquid, Enthalpy of solution, Pitzer’s theory, Isoperibol calorimeter

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