Thermodynamic properties of some isomeric 5-(nitrophenyl)-furyl-2 derivatives

Background The aim of the current work was to determine thermodynamical properties of 5-(nitrophenyl)-2-furaldehyde oximes and 3-[5-(nitrolphenyl)-2-furyl]acrylic acids. Results The temperature dependences of saturated vapor pressures of 5-(nitrophenyl)-2-furaldehyde oximes and 3-[5-(nitrolphenyl)-2-furyl]acrylic acids were determined by the Knudsen effusion method. The results are presented by the Clapeyron–Clausius equation in linear form, and via this form, the standard enthalpies of sublimation of compounds were calculated at 298.15 K. The standard molar formation enthalpies of compounds in crystalline state at 298.15 K were determined indirectly from the corresponding standard molar combustion enthalpy, obtained using combustion bomb calorimetry. The non-nearest neighbour interactions (strain) in molecule were defined. The ideal-gas enthalpies of investigated compounds formation and the data available from the literature were used for calculation of group-additivity parameters and the correction terms useful in the application of the Benson correlation. Conclusion Determining the thermodynamic properties for these compounds will contribute to solving practical problems pertaining to optimization processes of their synthesis, purification and application. It will also provide a more thorough insight regarding the theoretical knowledge of their nature and are necessary for the application of the Benson group-contribution correlation for calculation of \documentclass[12pt]{minimal} \usepackage{amsmath} \usepackage{wasysym} \usepackage{amsfonts} \usepackage{amssymb} \usepackage{amsbsy} \usepackage{mathrsfs} \usepackage{upgreek} \setlength{\oddsidemargin}{-69pt} \begin{document}$$ \Delta {}_{f}H_{{m(298.15{\text{K}})}}^{o} $$\end{document}ΔfHm(298.15K)o(g)calc. Electronic supplementary material The online version of this article (10.1186/s13065-019-0619-2) contains supplementary material, which is available to authorized users.


Introduction
The rapid growth of pharmaceutical and chemical industries using nitrogen-containing heterocyclic compounds requires a continuous diversification of these products. New synthesized compounds with complex structure have no description of their thermodynamic properties. Recently, numerous reactions of synthesis of nitrogencontaining compounds with a phenyl furan fragment, which exhibit various types of biological activity, have been investigated. This allows them to be widely used in various fields of medical chemistry [1][2][3][4][5][6][7][8][9][10].
3-(2-Furyl)acrylic acids are widely used in the synthesis of polymeric materials for the production of polymeric glass, light stabilizers and luminophores [10], as well as for the synthesis of compounds with antimicrobial properties [16].

BMC Chemistry
*Correspondence: vdibriv@polynet.lviv.ua 1 National University "LvivPolytechnic", S. Bandery Str.,12, Lviv 79013, Ukraine Full list of author information is available at the end of the article The analysis of the properties of positional isomers of disubstituted benzene derivatives shows that a change in the functional group position in an aromatic ring can substantially change the applied properties of compounds, whereas the change in their thermodynamic properties is often unknown. Therefore, the aim of this work is to investigate enthalpy properties of 5-(nitrophenyl)-2-furaldehyde oximes and 3-[5-(nitrolphenyl)-2-furyl] acrylic acids differ in the position of the nitro group. Thermodynamic properties allow finding the most energetically favourable ways of synthesis and application of compounds with the maximum economic benefit.
Joint analysis of thermodynamic properties of 5-(nitrophenyl)-2-furaldehyde oximes and 3-[5-(nitrolphenyl)-2-furyl] acrylic acids will reveal many theoretically important patterns of mutual influence of atoms in a molecule and enable to calculate the formation enthalpies of free radicals, energy relations, tension, cyclization, determine the group contributions to the additive schemes.

Effusion measurements
Primary effusion measurement results, including the saturated vapor pressure P of the researched compounds, are shown in Table 2. The measurement results were   processed by the least squares method and presented as  a linear equation: lnP (Pa) = A + B/T with correlation coefficient ρ, by means of which the standard molar enthalpies � g cr H o m ( T ) = B·R were calculated at average temperatures of measurement interval T (  Table 3.

Calorimetric measurements
Combustion energy ∆ c U(cpd) of the investigated substances was calculated by the equation: where m(cpd)-compound weight determined using gas analysis; ΔU Σ = W·∆T-total heat released in the experiment, W-energy equivalent of the calorimetric system, ∆T-real increase in temperature. Calculations were performed taking into account corrections for the combustion of cotton thread ΔU fuse , terylene container ΔU ter , soot to carbon dioxide ΔU carbon and also for formation in a bomb nitric acid solution U HNO 3 , using the following data for heats of combustion (J g −1 ): terylene 22,944.2 [21]; cotton thread 16704.2 [21]; soot to carbon dioxide − 32,763 [22]; formation of nitric acid 59 kJ mol −1 [22]. The results of determination of the compounds combustion energies ∆ c U(cpd) are listed in Table 4, which  The high rate of consistency of carbon dioxide content in substances (0.9952 to 1.0002) calculated by the formula (the results of its experimental determination are shown by the Rossini method) can also serve as an indirect confirmation of the sufficient purity of the compounds.

Table 1 Names and structural formulas of investigated compounds
The absence of significant systematic errors while measuring at the calorimetry installation was confirmed by the coincidence of our results of combustion enthalpies (kJ/mol) of secondary etalons (salicylic acid) and biphenyl − 3026.6 ± 3.1 and − 6246.9 ± 7.3 with recommended ones: − 3025.0 ± 5.0 and − 6250 ± 20 respectively [23].
The standard combustion enthalpies � c H o m (cr) (298.15K) of compounds were calculated taking into account the correction for the volume expansion work ∆nRT and the Washburn correction [24].
The calculation of formation enthalpies in condensed phase The gaseous state standard formation enthalpies of the investigated compounds were determined by the summation of the corresponding solid state formation enthalpies and their sublimation enthalpies according to the Eq. (5).
) enthalpies of the investigated compounds are listed in Table 5.
The standard gaseous state formation enthalpies of compounds � f H o m(298.15K) (g) calc are also calculated according to Benson additive scheme [26]. According to the scheme, the formation enthalpy of a compound in the gaseous state is the sum of the contributions of individual groups. Each group consists of a central atom and atoms of its first environment. Structural formulas of substances with indication of the serial number of increment, along with the values of group contributions � f H o m(298.15K) (g) calc which were used for calculations of the formation enthalpies are shown in the Tables 6 and (4)       the contribution of N i -(OH) group is approximately − 20.9 kJ/mol, but in the following works [28,29] this group is absent at all. Contributions of the groups C d -(C d )(N)(H) and N-(C d )(OH) in the Benson scheme are also absent. Therefore, the contribution of the fragment (C d )-CH=N-OH was calculated from the formation enthalpy of furfural oxime, which we have defined in [30]. It is the optimal choice because the oximes A, B, C can be considered as its derivatives. The values of the gaseous state standard formation enthalpies of the investigated compounds which were obtained experimentally exp Δ f H 298. 15 (g) and calculated theoretically calc Δ f H 298. 15 (g), as well as the difference between them δ are given in Table 5. The resulting difference cannot be explained by the errors of experiments or calculations.

Table 6 Calculation of the formation enthalpies of the studied substances using the addictive Benson scheme for 5-nitrophenyl-2-furaldehyde oxime isomers
In Ref. [31] interactions between atoms which were by at least two other atoms were called non-nearest neighbour interactions. The result of such interactions caused in general a strain of a molecule. Authors define the strain of a molecule, as the difference between the experimental standard enthalpy of formation � f H o m(298.15K) (g) exp and the calculated sum of the strain-free increments � f H o m(298.15K) (g) calc . A strain of molecules between benzene and furan rings in tert-butylbenzene (9 kJ/mol) is determined [31]. It can exist in the compounds investigated by us. The strain of adjacent nitro and tert-butyl groups (− 25 kJ/mol) is defined in [31].
Moreover, there is an alternation of single and double conjugated bonds in the molecular structure of all studied compounds. It is known for such systems that the entire molecule is usually situated in the same plane due to the presence of common π-cloud [32]. To verify the assertion, we simulated the most energy-efficient spatial structures of the investigated molecules using the HyperChem software (PM3 geometry optimization method). Other computational calculations of different thermodynamical properties for various nitrogen-containing organical compounds can be found in [33][34][35][36]. The results confirmed that for the oximes A, B, C the flat configuration of the molecule is the most energy-efficient. However, for the acids D, E, F the minimum internal energy of the molecules is observed when the chain of atoms -CH=CH-C(O)-OH is in a plane almost perpendicular to the furan cycle plane. An example of a geometric model for 3-(furan-2-yl) acrylic acid is shown in Fig. 1. Thus, the strain caused by the furan cycle rotation relative to the chain in the acids D, E and F may exist.
According to the above-mentioned data, we predicted the presence of three different strains in the investigated compounds. The first one is provided by the rotation of the side chain plane relative to the furan cycle in the derivatives of furanacrylic acids (X), the second one corresponds to the interaction of the furan cycle and nitro group in the ortho-position (Y), and the third one is the interaction of the benzene and furan cycles (Z). To calculate interaction corrections in Benson additive scheme a redefined system of six linear equations with two unknowns (X) and (Y) was composed of the corresponding experimentally obtained formation enthalpies and strain-free increments. The correction (Z) of 9 kJ/mol was taken from [31]. The same correction was used to determine the contribution of the group C d -(C d )(O)(C B ) from the formation enthalpy of 3-substituted 2-cyanoacrylic acid ethyl ester [18]. As a result of the system solution, the correction terms (kJ/mol) were defined: 1-4 C b -(C b ) 2 (H) 13.8

Table 7 Calculation of the formation enthalpies of the studied substances using the addictive Benson schemefor 3-[5-nitrolphenyl-2-furyl]acrylic acid isomers
Furan cycle − 25.9 X = − 30.7, Y = − 29.5 It is clear that the corrections were determined for a small set of substances, and will be defined more exactly as additional experimental material is gained.

Materials
Furyl-2-oxime (A-C) derivatives were synthesized according to the following procedure. A mixture of appropriated furyl-2-carbaldehyde (0.023 mol), hydroxylamine hydrochloride (0.03 mol) and fused sodium acetate 2 g in 20 mL of ethanol was boiled for 4 h, 30 mL of water was added to the mixture under stirring after cooling. The resulting precipitate was filtered off and recrystallized from ethanol. Synthesis of 3-[5-(2-nitrolphenyl)-2-furyl] acrylic acids (D-F) was carried out according to the following procedure. 2-3 Drops of piperidine were added to a mixture consisting of appropriated furyl-2-carbaldehyde (0.01 mol) and malonic acid (0.01 mol) in 10 mL of pyridine. The reaction mixture was heated for 2-3 h in a boiling water bath, then cooled, diluted with water (20 mL) and acidified with diluted (1:1) hydrochloric acid. The solution was filtered off, washed with water and dried. The acids were recrystallized from ethanol or mixture of ethanol-DMF solvents. We used the samples obtained after 3-and 4-fold recrystallization.
The identification of substances was confirmed by NMR 1 H spectroscopy data. NMR 1 H spectra were recorded on Varian 600 (600 MHz) spectrometers in DMSO-d 6 or acetone-d 6 . Chemical shifts (δ, ppm) were determined in regards to the signal of DMSO (2.50 ppm). Spectral data for the investigated substances are shown below:

Effusion measurements
Taking into account low volatility of the analyzed substances, the temperature dependences of the saturated vapour pressures were determined by the integral Knudsen effusion method. The design of the apparatus has been adopted from [37]. Construction of the chamber, membranes and experimental procedure was conducted using the recommendations [38].
Three membranes with a diameter of holes № 1-2.050, № 2-2.100 and № 3-2.055 mm were used for effusional research presented in this paper. The membranes are made of nickel foil with a thickness of 0.09 mm. The vacuum of 0.1 Pa was achieved for 25 ± 15 s. The weight of the effunded substance m was determined using analytical scales VLR-20 (± 5·10 −6 g) as the difference of the effusion camera weight before and after the experiment. The measurement accuracy of the temperature (T) and effusion time (τ) was ± 0.5 K and ± 1 s, respectively. Effective time (estimated time of effusion in the steady state, in which the weight loss of the effunded substance is equal to that in the transient regime), determined in separate experiments with benzoic acid, equals to 25 ± 5 s and added to the total time of the experiment.
The vapor pressure in the effusion cell P k was calculated by equation [39]: where τ is the time of effusion through a hole in the membrane with area S; T-temperature, R-universal gas constant, M-molecular weight of the substance, αcondensation coefficient.
Investigated nitrophenyl-furyl derivatives are molecular crystals that sublime without a change in their geometry and molecule weight, which allowed us to admit α to be equal to 1 [40].
Clausing coefficient-K, which stands for the membrane's resistance to molecular flow of vapor for the hole in the membrane, with ratio of length (l) to radius (r) from 0 to 1.5, was determined by the empirical Kennard formula K = 1/[1 + 0.5(l/r)] [41].
The vapor pressure was calculated using correction factor according to the recommendations [42]. For three membranes used in the present work, the factors are equal to 5.12, 5.21 and 5.14 respectively.
Prior to this, the reliability of the effusion installation was checked by benchmark benzoic acid brand K − 1 (the shows the absence of significant systematic errors in the effusion installation.

Calorimetric measurements
The combustion enthalpies of the substances were determined by upgraded calorimeter V-08MA with the isothermal shell.
The temperature in the thermostat was maintained ± 0.03 K. The energy equivalent of the calorimetric systems W was estimated by combustion of the reference benzoic acid grade K − 1 (the major component content-99.995% mol, the heat of combustion, taking into account the Jessup factor-26,434.4 J g −1 ) in a series of 12 experiments. The value of W was 14,901 ± 11 J V −1 .
Before combustion beginning the crystalline A, B and C samples were grinded in chalcedony mortar, screened, placed in Terylene ampoules and ignited in the platinum cup. 1 mL of distilled water was added before combustion. The initial pressure of the oxygen, previously purified from the combustible impurities, carbon dioxide and water, was equal to 3.0 MPa. The The quantitative analysis of the combustion products for the presence of carbon oxide by the Rossini method [44] with the accuracy of ± 2·10 −4 g and nitric acid content by titration of the liquid phase in a bomb with a 0.1 M solution of NaOH was carried out after every experiment. The quantities of the carbon dioxide, formed from the combustion of 1 g of Terylene and the cotton thread, were equal to 2.2872 g and 1.6284 g respectively [45]. The anticipated carbon monoxide to be formed during the combustion of products by using detector tubes within ± 5·10 −6 g, was not encountered. The soot mass was determined by the weighting of the platinum cup before and after combustion with the accuracy of ± 5 × 10 −6 g. The reliability of gas analyses was controlled by benzoic acid combustion.
Combustion of the investigated compounds is represented by reaction: A more detailed description of the diffusion unit and combustion calorimeter, experimental procedure and calculations of primary results are presented in [17].

Conclusions
The determined thermodynamic properties of these compounds will contribute to solving practical problems pertaining to optimization processes of their synthesis, purification and application.
Temperature dependences of vapor pressure have their own practical value for calculation of the parameters for individual stages of the synthesis.
Determining of the thermodynamic properties for these compounds also provides a more thorough insight regarding the theoretical knowledge of their nature.
Using Hyper Chem software (PM3 geometry optimization method) the flat configuration of the phenyl-furan oxime derivatives molecules was established.
Phenyl-furan acid derivatives molecules have the minimum internal energy of the molecule, when the chain of atoms -CH=CH-C(O)-OH is in a plane almost perpendicular to the furan cycle plane.
The comparison of the formation enthalpies of the investigated substances in a gaseous state obtained experimentally with the ones calculated by the Benson scheme allowed to determine the energy of the interaction of a furan ring with a nitro group in the ortho position of the benzene ring (− 30 kJ/mol) as well as the energy of the chain -CH=CH-C(O)-OH rotation in the molecules of phenyl-furan acid derivatives (− 31 kJ/mol). The new group-additivity parameters and the correction terms for substituted nitrophenyl-furyl derivatives of oximes and acids allowed to applicate the Benson group-contribution correlation to estimate � f H o m(298.15K) (g) calc. of the compounds has not been investigated yet.

Additional file
Additional file 1: Appendix S1. Cartesian coordinates and computation results for the investigated compounds.