Short communicationExcess molar enthalpies of dibromomethane with acetonitrile, furan and acetophenone at 303.15 K
Introduction
As a part of our continuous efforts to obtain thermodynamic quantities on liquid mixtures of organic compounds [1], [2], [3], [4], [5], we report here excess molar enthalpies of dibromomethane (CH2Br2) (DBM) with acetonitrile, furan and acetophenone at 303.15 K. Binary systems of CH2Br2 with acetonitrile, furan and acetophenone are of considerable interest due to specific interactions between these components in the liquid state. This is caused by the presence of two Br and two H atoms in CH2Br2, which can thus act as σ-acceptors towards, and be involved in the hydrogen bond formation with acetonitrile, furan and acetophenone. The latter will act as n-donors. A literature survey revealed that extensive studies on such systems have not been carried out to date. The data obtained for excess molar enthalpies have been interpreted in this paper.
Section snippets
Experimental
Dibromomethane (Fluka) has been purified by fractional distillation, only the middle fraction was used for experiments. Acetonitrile (B.D.H.), furan (A.R.) and acetophenone (A.R.) were dried over freshly activated molecular sieves before use. The chemicals have a minimum purity of 99.0 mol% as determined by GLC. The purities of chemicals used, as determined by GLC for the samples of dibromomethane, acetonitrile, furan and acetophenone are found to be 99.8, 99.8, 99.3 and 99.0 mol%, respectively.
Results and discussions
Excess molar enthalpies, HE, for various systems are summarized in Table 1. The observed values are fitted with the Redlich–Kister equation by means of the least squares method:where x1 refers to the mole fraction of CH2Br2. The least square parameters, along with the standard deviations, σ are reported in Table 2. The standard deviations, σ, are calculated using equation:where HE is experimental excess enthalpy and is calculated
Acknowledgement
Author is extremely grateful to Mr. Ajay Sagar, Managing Director, Osaw Industrial Products Pvt. Ltd., Ambala Cantt, India, for his valuable co-operation and encouragement during this investigation.
References (10)
- et al.
Thermochim. Acta
(1995) - et al.
J. Chem. Thermodyn.
(1969) - et al.
J. Chem. Thermodyn.
(1997) - et al.
J. Chem. Eng. Data
(1983) - et al.
Thermochim. Acta
(1992)
Cited by (3)
Contribution enthalpic in the interaction of activated carbon with polar and apolar solvents
2013, Arabian Journal of ChemistryCitation Excerpt :When a solid and a liquid are contacted a certain amount of heat is generated by the surface and chemical reactions, and this can be determined by means of suitable calorimetric techniques, which leads to the determination of the immersion enthalpy as a characteristic thermodynamic parameter for a specific system (Silvestre-Albero et al., 2001; Stoeckli and Centeno, 2005). If one thinks that the system is formed by the solid and the liquid one can suppose that the immersion enthalpy is due to the contribution of each one of these, as it happens with the thermodynamic partial molar properties in the case of multicomponent solutions (Tripathi, 2010). In this work, from the experimental enthalpies obtained when carbon is activated with solvent mixes, it is possible to calculate the enthalpic contributions that present the activated carbon and water or hexane at the immersion enthalpy of the solid in the liquid; the calculation is made possible by the similarity with the partial molar enthalpies in the solutions.
Thermodynamic study of mixtures containing dibromomethane. II: volumes and enthalpies at 298.15 K
2020, Journal of Thermal Analysis and CalorimetryDetermination of partial immersion enthalpy in the interaction of water and activated carbon
2011, Journal of Thermal Analysis and Calorimetry