# Study of Lactic Acid Thermal Behavior Using Thermoanalytical Techniques

Authors: Andrea Komesu; Patricia Fazzio Martins Martinez; Betânia Hoss Lunelli; Johnatt Oliveira; Maria Regina Wolf Maciel; Rubens Maciel Filho
Journal: Journal of Chemistry
 (2017)

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## Abstract

Actually, there is a growing interest in the biotechnological production of lactic acid by fermentation aiming to substitute fossil fuel routes. The development of an efficient method for its separation and purification from fermentation broth is very important to assure the economic viability of production. Due to its high reactivity and tendency to decompose at high temperatures, the study of lactic acid thermal behavior is essential for its separation processes and potential application. In the present study, differential scanning calorimetry (DSC) analyses showed endothermic peaks related to the process of evaporation. Data of thermogravimetry (TG/DTG) were correlated to Arrhenius and Kissinger equations to provide the evaporation kinetic parameters and used to determine the vaporization enthalpy. Activation energies were 51.08 and 48.37 kJ·mol−1 and frequency values were 859.97 and 968.81 s−1 obtained by Arrhenius and Kissinger equations, respectively. Thermogravimetry, coupled with mass spectroscopy (TG-MS), provided useful information about decomposition products when lactic acid was heated at 573 K for approximately 30 min.


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## Body

## 1. Introduction

Lactic acid or 2-hydroxypropionic acid, an organic acid manufactured by fermentation from renewable sources, such as corn, potato, and other agriculture products, is an alternative to conventional petroleum raw materials routes. It has a wide variety of applications, in cosmetics (moisturizers, skin-lightening agents, skin-rejuvenating agents, pH regulators, antiacne agents, humectants, and antitartar agents), in pharmaceutical products (dialysis solution, mineral preparations, pills, prostheses, surgical sutures, and controlled drug delivery systems), in chemistry (descaling agents, pH regulators, neutralizers, chiral intermediates, green solvents, cleaning agents, slow acid release agents, and metal complexing agents), and in food (acidulants, preservatives, flavours, pH regulators, microbial quality improving agents, and mineral fortification) [1, 2]. Furthermore, it is used as precursor of several other products, such as propylene oxide, acetaldehyde, acrylic acid, propionic acid, 2,3-pentanedione, ethyl lactate, and polylactic acid [3]; the latter is used for production of biodegradable polymers with medical applications. Over the last decade, more and more attention has been paid to its potential productivity due to its increasing demand in practice. However, it is still difficult to recover high quality lactic acid from a fermentation broth because of its characteristics such as high viscosity and thermal sensitivity [4].The thermal sensitivity and high reactivity of lactic acid can be explained due the presence of two adjacent functional groups, acid and alcohol, in a small molecule with only three carbon atoms, as well as their tendency to decompose at high temperatures [5]. However, from literature review, no accurate study detailing the monomer lactic acid thermal behavior could be found. On the other hand, the polylactic acid (PLA), polymer produced by polymerization of lactic acid, has been extensively studied [6–10].The development of an efficient method for separation and purification of carboxylic acids from fermentation broth is very important to allow its biotechnological production in commercial scale, since these steps are responsible for 30–40% of the total production costs [11]. However, for recovery and concentration of thermally unstable molecules, such as lactic acid, it is essential to understand how these molecules behave at high temperatures, which can be achieved through thermal analyses as differential scanning calorimetry (DSC), thermogravimetry (TG), and thermogravimetry coupled with mass spectroscopy (TG-MS).DSC is performed by difference in energy supplied to the sample and the reference pan in function of temperature. By varying the energy of the sample as a function of temperature, physical and chemical phenomena can be observed. In general, phase transitions, dehydration, reduction, and decomposition reactions produce endothermic effects, whereas crystallization, oxidations, and some decomposition reactions produce exothermic effects [12]. DSC is often used because of its speed, simplicity, and availability [13]. Several reviews covering the fundamentals concepts, instrumentation, and general applications are available in the literature [13–16].TG is a technique that records variation of mass while the sample is heated. The mass loss can be related to many phenomena such as dehydration, sublimation, evaporation, and decomposition. TG has been used to estimate the kinetic parameters, such as activation energies, reaction orders, and the Arrhenius preexponential factor, of degradation [17] and evaporation processes [18] and to determine physical properties as vapor pressure and vaporization enthalpy [19].TG-MS is a powerful hyphenated technique combining the direct measurement of weight loss as a function of temperature with the use of sensitive spectroscopic detectors. Such detectors permit qualitative and quantitative determination of the evolved volatile products to provide kinetic information about the specific reaction mechanisms [20]. Other advantages are speed, reduced sample handling, unique sample, and absence of retention time [21]. Research articles have been published about instrumentation and applications of TG [22–24] and TG-MS [21, 25, 26].So, in this work, the objective was to study the lactic acid thermal behavior using DSC, TG/DTG, and TG-MS. The obtained results provided a better understanding of the lactic acid thermal behavior, allowing the development of adequate separation processes.


## 2. Experimental

### 2.1. Material

DL-lactic acid (molecular weight 90.08 kg·mol−1, CAS number 50-21-5) ~90% standard supplied by Sigma-Aldrich (St Louis, Missouri, EUA) was used in the thermal analysis by DSC, TG/DTG, and TG-MS without prior purification. Water and residual substances are impurities reported by the supplier.


### 2.2. Differential Scanning Calorimetry

DSC experiment was carried out using Shimadzu equipment (Japan), model DSC-50. A dynamic scan was performed at heating rate of 10 K·min−1 over a temperature range from 294 K to 773 K. The sample was analyzed under a nitrogen dynamic atmosphere at flow rate of 50 mL min−1. The experiments were carried out with a sample size of ~7 mg. The samples were weighed into open aluminum pans and hermetically sealed.


### 2.3. Thermogravimetry

TG experiments were carried out using Shimadzu thermal analyser (Japan), model TGA-50. Constant heating rates of 5, 10, 15, 20, 25, and 30 K·min−1 were applied. Data were collected in the temperature range from 296 K to 773 K under a nitrogen dynamic atmosphere (50 mL·min−1). The masses of samples were nearly 15 mg. The equipment recorded TG and DTG (derivative thermogravimetric analysis) data simultaneously. Data obtained by TG were used to determine evaporation kinetic parameters and evaporation enthalpy. Data obtained by DTG were useful to show the evaporation stages and the effect of heating rate.


### 2.4. Thermogravimetry Coupled with Mass Spectrometer

TG-MS analysis was carried out using Setaram SetSys Evolution 16/18 coupled with a mass spectrometer (MS) Thermostar Pfeiffer Vacuum GSD 301T. MS was responsible for monitoring the masses of compounds that have evolved from the sample during heating. Initially, the sample was heated from 298 K to 773 K at heating rate of 10 K·min−1 under nitrogen atmosphere (16 mL·min−1) in order to observe the temperature range in which the evolution of mass occurred. Afterwards, the analysis was performed with a mass spectrometer coupled, heating the sample from 293 K to 573 K at heating rate of 10 K·min−1 under nitrogen atmosphere (16 mL·min−1). In addition, an isothermal at 573 K was built during 2 h. In this case, a scan of all fragments evolved from the sample during the heating time was used to obtain the thermal and mass spectrum. Finally, TG-MS was performed monitoring fragments of higher intensity. Data were collected and used to obtain the lactic acid thermal behavior and degradation products as a function of temperature and time.


### 2.5. Kinetic Models

Thermogravimetry is the most common technique used for kinetic analysis. Sample mass variation by temperature data obtained by TG/DTG was used to determine evaporation kinetic parameters. The frequency factor (A) and activation energy (Ea) were obtained using Arrhenius and Kissinger methods.Calculations are based on the following kinetic equation [18]: (1)dαdt=k×1-αn,where α corresponds to the amount of vaporized material, t is the time, n is the apparent reaction order, and k is the rate constant.The amount of vaporized material (α) is defined as (2)α=m0-mtm0-mf,where m0 is the sample initial mass, mt is the sample mass at time t, and mf is sample final mass.k depends on temperature following Arrhenius equation: (3)k=Aexp⁡-EaRT,where A is the frequency factor, Ea corresponds to the activation energy, and R is the gas constant.Considering (1) and (3), the following expression is derived: (4)dαdt=Aexp⁡-EaRT×1-αn.


### 2.6. Arrhenius Method

This approach assumes Arrhenius behavior and zero-order reaction kinetics. Taking the natural logarithm in (4), the following expression is derived: (5)ln⁡dαdt=ln⁡A1-αn-EaRT.For zero-order reactions (n=0), the equation becomes(6)ln⁡dαdt=ln⁡A-EaRT;dα/dt can be calculated by (7). The value of dm/dt is provided by DTG plot. (7)dαdt=-dm/dtm0-mf.Thus, plottingln⁡dα/dt versus 1/T and correlating the values by the least-square methods to obtain a straight line, the slope will provide the activation energy after being multiplied by R. The intercept of this equation will be equivalent to ln⁡A.


### 2.7. Kissinger Method

Kissinger developed a model-free nonisothermal method where there is no need to calculateEa for each conversion value in order to evaluate kinetic parameters [27]. This method is based on the study of the rate equation at the maximum reaction rate, which means that d2α/dt2 is equal to zero. Equation (4) can be written as (8)ln⁡βTm2=ln⁡AREa-ERTm,where β is the heating rate β=dT/dt and Tm is the temperature peak of the DTG curve.The activation energy is determined from the TG data at different heating rates by liner regression of theln⁡β/Tm2 versus Tm-1 plot, and the activation energy (Ea) is calculated from the slope of the resulting straight line.


### 2.8. Vaporization Enthalpy

Thermogravimetry is a rapid and convenient technique used for determination of vaporization enthalpy. The theoretical basic of the TG procedure is the Langmuir equation [19]: (9)1admdt=pαM2πRT,where dm/dta is the rate of mass loss per unit area (kg s−1 m−2), p is the vapor pressure (Pa), M is the molecular weight of the vapor of the evaporating compound (kg mol−1), R is the gas constant (J K−1 mol−1), T is the absolute temperature, and α is the vaporization coefficient.Rearranging the Langmuir equation gives(10)p=kν,where k=2πR/α and ν=1/adm/dtT/M.A plot ofln⁡ν against 1/T should give a straight line plot of slope ΔH/R.


## 2.1. Material

DL-lactic acid (molecular weight 90.08 kg·mol−1, CAS number 50-21-5) ~90% standard supplied by Sigma-Aldrich (St Louis, Missouri, EUA) was used in the thermal analysis by DSC, TG/DTG, and TG-MS without prior purification. Water and residual substances are impurities reported by the supplier.


## 2.2. Differential Scanning Calorimetry

DSC experiment was carried out using Shimadzu equipment (Japan), model DSC-50. A dynamic scan was performed at heating rate of 10 K·min−1 over a temperature range from 294 K to 773 K. The sample was analyzed under a nitrogen dynamic atmosphere at flow rate of 50 mL min−1. The experiments were carried out with a sample size of ~7 mg. The samples were weighed into open aluminum pans and hermetically sealed.


## 2.3. Thermogravimetry

TG experiments were carried out using Shimadzu thermal analyser (Japan), model TGA-50. Constant heating rates of 5, 10, 15, 20, 25, and 30 K·min−1 were applied. Data were collected in the temperature range from 296 K to 773 K under a nitrogen dynamic atmosphere (50 mL·min−1). The masses of samples were nearly 15 mg. The equipment recorded TG and DTG (derivative thermogravimetric analysis) data simultaneously. Data obtained by TG were used to determine evaporation kinetic parameters and evaporation enthalpy. Data obtained by DTG were useful to show the evaporation stages and the effect of heating rate.


## 2.4. Thermogravimetry Coupled with Mass Spectrometer

TG-MS analysis was carried out using Setaram SetSys Evolution 16/18 coupled with a mass spectrometer (MS) Thermostar Pfeiffer Vacuum GSD 301T. MS was responsible for monitoring the masses of compounds that have evolved from the sample during heating. Initially, the sample was heated from 298 K to 773 K at heating rate of 10 K·min−1 under nitrogen atmosphere (16 mL·min−1) in order to observe the temperature range in which the evolution of mass occurred. Afterwards, the analysis was performed with a mass spectrometer coupled, heating the sample from 293 K to 573 K at heating rate of 10 K·min−1 under nitrogen atmosphere (16 mL·min−1). In addition, an isothermal at 573 K was built during 2 h. In this case, a scan of all fragments evolved from the sample during the heating time was used to obtain the thermal and mass spectrum. Finally, TG-MS was performed monitoring fragments of higher intensity. Data were collected and used to obtain the lactic acid thermal behavior and degradation products as a function of temperature and time.


## 2.5. Kinetic Models

Thermogravimetry is the most common technique used for kinetic analysis. Sample mass variation by temperature data obtained by TG/DTG was used to determine evaporation kinetic parameters. The frequency factor (A) and activation energy (Ea) were obtained using Arrhenius and Kissinger methods.Calculations are based on the following kinetic equation [18]: (1)dαdt=k×1-αn,where α corresponds to the amount of vaporized material, t is the time, n is the apparent reaction order, and k is the rate constant.The amount of vaporized material (α) is defined as (2)α=m0-mtm0-mf,where m0 is the sample initial mass, mt is the sample mass at time t, and mf is sample final mass.k depends on temperature following Arrhenius equation: (3)k=Aexp⁡-EaRT,where A is the frequency factor, Ea corresponds to the activation energy, and R is the gas constant.Considering (1) and (3), the following expression is derived: (4)dαdt=Aexp⁡-EaRT×1-αn.


## 2.6. Arrhenius Method

This approach assumes Arrhenius behavior and zero-order reaction kinetics. Taking the natural logarithm in (4), the following expression is derived: (5)ln⁡dαdt=ln⁡A1-αn-EaRT.For zero-order reactions (n=0), the equation becomes(6)ln⁡dαdt=ln⁡A-EaRT;dα/dt can be calculated by (7). The value of dm/dt is provided by DTG plot. (7)dαdt=-dm/dtm0-mf.Thus, plottingln⁡dα/dt versus 1/T and correlating the values by the least-square methods to obtain a straight line, the slope will provide the activation energy after being multiplied by R. The intercept of this equation will be equivalent to ln⁡A.


## 2.7. Kissinger Method

Kissinger developed a model-free nonisothermal method where there is no need to calculateEa for each conversion value in order to evaluate kinetic parameters [27]. This method is based on the study of the rate equation at the maximum reaction rate, which means that d2α/dt2 is equal to zero. Equation (4) can be written as (8)ln⁡βTm2=ln⁡AREa-ERTm,where β is the heating rate β=dT/dt and Tm is the temperature peak of the DTG curve.The activation energy is determined from the TG data at different heating rates by liner regression of theln⁡β/Tm2 versus Tm-1 plot, and the activation energy (Ea) is calculated from the slope of the resulting straight line.


## 2.8. Vaporization Enthalpy

Thermogravimetry is a rapid and convenient technique used for determination of vaporization enthalpy. The theoretical basic of the TG procedure is the Langmuir equation [19]: (9)1admdt=pαM2πRT,where dm/dta is the rate of mass loss per unit area (kg s−1 m−2), p is the vapor pressure (Pa), M is the molecular weight of the vapor of the evaporating compound (kg mol−1), R is the gas constant (J K−1 mol−1), T is the absolute temperature, and α is the vaporization coefficient.Rearranging the Langmuir equation gives(10)p=kν,where k=2πR/α and ν=1/adm/dtT/M.A plot ofln⁡ν against 1/T should give a straight line plot of slope ΔH/R.


## 3. Results and Discussion

### 3.1. Differential Scanning Calorimetry Analysis

The DSC curve of lactic acid is presented in Figure1. From this figure, it can be observed that two endothermic peaks are related to the process of lactic acid and lactide evaporation, at 447.35 K and 625.24 K, respectively. The double small peak in the first peak (447.35 K) is noted; it probably occurred because of the presence of two isomers D(−) and L(+) lactic acid present in the sample.Figure 1
DSC lactic acid profile.


### 3.2. Thermogravimetry Analysis

The TG and DTG thermal profiles are shown in Figures2(a) and 2(b).Figure 2
TG (a) and DTG (b) curves of lactic acid as a function of temperature and heating rates (5, 10, 15, 20, 25, and 30 K⋅min−1).
(a)
(b)The weight loss profile in Figure2(a) shows the loss of mass with temperature at different heating rates. As can be seen in Figure 2(a), the curves do not show a plateau indicating thermal stability; conversely, evaporation process begins at temperatures around the room temperature and proceeds rapidly with increasing temperature until about 573 K.The effect of heating rate is shown in Figures2(a) and 2(b). Heating rates affect TG curve positions and shift maximum temperature peaks (Tm) towards higher temperatures. This phenomenon can be explained on the basis of heat transfer limitation. During the analysis, at low heating rate, a larger instantaneous thermal energy is provided in the system and a longer time may be required for the purge gas to reach equilibrium with the temperature of the furnace or the sample. While at the same time and in the same temperature region, higher heating rate has a short reaction time and the temperature needed for the sample to evaporate is also higher [27].DTG profiles showed three evaporation stages. The evaporation stages (heating rate of 10 K·min−1) occurred at ~347 K, ~459 K and ~612 K and mass loss percentage of 12.119%, 85.520%, and 1.483%, respectively. First was the evaporation of water and methanol impurities (~347 K) followed by lactic acid (~459 K) and probably lactide (~612 K).The Arrhenius plot for the calculation of activation energy is shown in Figure3(a). For a reaction to be considered an evaporation process, it is imperative that the mass loss according to the time or temperature should be a zero-order process [18]. Lactic acid presented in this work showed this behavior, as show in Figure 3(a), using heating rate of 10 K·min−1. The kinetic parameters determined from TG/DTG data are shown in Table 1. The advantage of Arrhenius model is the ability to directly determine the kinetic parameters from a single TG measurement.Table 1
Evaporation kinetic parameters of lactic acid by Arrhenius and Kissinger models.
Model
Heating rate/K⋅min−1
Ea/kJ⋅mol−1
A/s−1
R
2
Arrhenius
10
51.08
859.97
0.9962
Kissinger
48.37
968.81
0.9712Figure 3
Arrhenius plot (a) and Kissinger plot (b) for the calculation of the activation energy.
(a)
(b)Kissinger plot ofln⁡β/Tm2 versus Tm-1 is shown in Figure 3(b). The kinetic parameters were calculated according to (8) and are given in Table 1. The advantage of the model-free analysis is founded on its simplicity and on the avoidance of errors connected with the choice of a kinetic model [27].The values of activation energy and frequency factor obtained from the Kissinger method are consistent with the values obtained by Arrhenius method (deviation less than 10%). Kinetic parameters of the lactic acid evaporation process have not been reported in literature review, as described in this work.The plot ofln⁡ν against 1/T for the calculation of vaporization enthalpy (ΔHvap) is shown in Figure 4 using heating rate of 30 K min−1. The vaporization enthalpy calculated was 56.9 kJ mol−1. Experimental values for lactic acid vaporization enthalpy are very rare in the literature. Emel’yanenko et al. [28] reported a value of vaporization enthalpy of 69.1 kJ·mol−1 at 298.15 K using the transpiration method for the L-lactic acid. Comparing the results, deviations are lower than 18%, which is due to experimental errors and probably the presence of the DL-lactic acid isomer used in this work also influenced the results.Figure 4
The plot ofln⁡ν against 1/T for the calculation of vaporization enthalpy.


### 3.3. Thermogravimetry Coupled with Mass Spectrometer Analysis

TG-MS analysis enabled the identification of vaporized molecules and thermal decomposition products from lactic acid at high temperatures. TG-MS profiles are shown in Figure5. From this figure, it was observed that water (m/z=18), hydroxyl (m/z=17), and methanol (m/z=32) were the main molecules eliminated during the heating. Water and methanol are impurities from DL-lactic acid commercially produced which has 90% of purity. Probably, water and methanol come from fermentation and separation processes, respectively. The hydroxyl group probably came from water. Lactide is also an impurity which was observed in DSC curve. The presence of lactide in the commercial lactic acid may be explained due to the tendency of lactic acid to polymerize in concentrated solutions. As described in the literature, above 30% of lactic acid concentration, the presence of lactide is observed [5]. Other mass fragments monitored during the thermal analysis appeared in low ionic current values.Figure 5
TG-MS profiles of lactic acid.Lactic acid can be conveniently converted into various value-added products, such as acrylic acid. For acrylic acid production, direct dehydration of lactic acid in high temperatures is an alternative. For better understanding the lactic acid thermal behavior at high temperatures, TG-MS isotherm of lactic acid at 573 K was performed as shown in Figure6. The isotherm profiles were divided into parts (a) and (b) for better visualization.Figure 6
TG-MS lactic acid isothermal at 573 K during the time. (a):m/z=17, 18, 32, 44, and 45. (b): m/z=72 and 74. The solid line in (b) is a type of noise from the equipment.
(a)
(b)Figure6 showed the fragments products of hydroxyl (m/z=17), water (m/z=18), methanol (m/z=32), acetaldehyde or/and carbon dioxide (m/z=44), formate (m/z=45), acrylic acid (m/z=72), and propionic acid (m/z=74). It can be concluded that various reactions occurred concurrently. At approximately 30 min of heating, the presence of dehydration reactions (11) as well as reduction (12) and decarboxylation reactions (13) was observed.(11)C3H6O3⟶C3H4O2+H2OLacticacid⟶acrylicacid+water(12)C3H6O3⟶C3H6O2+12O2Lacticacid⟶propionicacid+oxygen(13)C3H6O3⟶C2H4O+CO2+H2Lacticacid⟶acetaldehyde+carbondioxide+hydrogenAccording to the literature, the formation of self-reaction products such as lactide, which are subsequently more readily decomposed into fragments (e.g., carbon monoxide, acetaldehyde, and water), is the main reaction that competes with the dehydration process [29]. Data obtained from TG-MS are in agreement with the literature.Additionally, at the end of the analysis, the sample was found graphitized indicating that a quantity of the sample was reduced, also confirming the analysis of the mass profiles. It can be concluded that the decomposition process of lactic acid is related to temperature and the time of exposure to heat. In addition, only after 30 min of heating at 573 K lactic acid was decomposed into water, hydroxyl, methanol, acetaldehyde or/and carbon dioxide, formate, acrylic acid, and propionic acid as can be seen by increasing the current ionic at 30 min.Therefore, it is important work with separation processes, which minimize problems of thermal decomposition to avoid the formation of byproducts. Vacuum operations provide a substantial decrease in the boiling points of substances due to operating pressure reduction. This characteristic allows the separation of compounds that would be destroyed if the mixture is processed at normal pressures [30]. This characteristic is satisfied by the hybrid short path evaporation. It has been recognized as a promising technology mainly because of its low evaporation temperature and short residence time [31].


## 3.1. Differential Scanning Calorimetry Analysis

The DSC curve of lactic acid is presented in Figure1. From this figure, it can be observed that two endothermic peaks are related to the process of lactic acid and lactide evaporation, at 447.35 K and 625.24 K, respectively. The double small peak in the first peak (447.35 K) is noted; it probably occurred because of the presence of two isomers D(−) and L(+) lactic acid present in the sample.Figure 1
DSC lactic acid profile.


## 3.2. Thermogravimetry Analysis

The TG and DTG thermal profiles are shown in Figures2(a) and 2(b).Figure 2
TG (a) and DTG (b) curves of lactic acid as a function of temperature and heating rates (5, 10, 15, 20, 25, and 30 K⋅min−1).
(a)
(b)The weight loss profile in Figure2(a) shows the loss of mass with temperature at different heating rates. As can be seen in Figure 2(a), the curves do not show a plateau indicating thermal stability; conversely, evaporation process begins at temperatures around the room temperature and proceeds rapidly with increasing temperature until about 573 K.The effect of heating rate is shown in Figures2(a) and 2(b). Heating rates affect TG curve positions and shift maximum temperature peaks (Tm) towards higher temperatures. This phenomenon can be explained on the basis of heat transfer limitation. During the analysis, at low heating rate, a larger instantaneous thermal energy is provided in the system and a longer time may be required for the purge gas to reach equilibrium with the temperature of the furnace or the sample. While at the same time and in the same temperature region, higher heating rate has a short reaction time and the temperature needed for the sample to evaporate is also higher [27].DTG profiles showed three evaporation stages. The evaporation stages (heating rate of 10 K·min−1) occurred at ~347 K, ~459 K and ~612 K and mass loss percentage of 12.119%, 85.520%, and 1.483%, respectively. First was the evaporation of water and methanol impurities (~347 K) followed by lactic acid (~459 K) and probably lactide (~612 K).The Arrhenius plot for the calculation of activation energy is shown in Figure3(a). For a reaction to be considered an evaporation process, it is imperative that the mass loss according to the time or temperature should be a zero-order process [18]. Lactic acid presented in this work showed this behavior, as show in Figure 3(a), using heating rate of 10 K·min−1. The kinetic parameters determined from TG/DTG data are shown in Table 1. The advantage of Arrhenius model is the ability to directly determine the kinetic parameters from a single TG measurement.Table 1
Evaporation kinetic parameters of lactic acid by Arrhenius and Kissinger models.
Model
Heating rate/K⋅min−1
Ea/kJ⋅mol−1
A/s−1
R
2
Arrhenius
10
51.08
859.97
0.9962
Kissinger
48.37
968.81
0.9712Figure 3
Arrhenius plot (a) and Kissinger plot (b) for the calculation of the activation energy.
(a)
(b)Kissinger plot ofln⁡β/Tm2 versus Tm-1 is shown in Figure 3(b). The kinetic parameters were calculated according to (8) and are given in Table 1. The advantage of the model-free analysis is founded on its simplicity and on the avoidance of errors connected with the choice of a kinetic model [27].The values of activation energy and frequency factor obtained from the Kissinger method are consistent with the values obtained by Arrhenius method (deviation less than 10%). Kinetic parameters of the lactic acid evaporation process have not been reported in literature review, as described in this work.The plot ofln⁡ν against 1/T for the calculation of vaporization enthalpy (ΔHvap) is shown in Figure 4 using heating rate of 30 K min−1. The vaporization enthalpy calculated was 56.9 kJ mol−1. Experimental values for lactic acid vaporization enthalpy are very rare in the literature. Emel’yanenko et al. [28] reported a value of vaporization enthalpy of 69.1 kJ·mol−1 at 298.15 K using the transpiration method for the L-lactic acid. Comparing the results, deviations are lower than 18%, which is due to experimental errors and probably the presence of the DL-lactic acid isomer used in this work also influenced the results.Figure 4
The plot ofln⁡ν against 1/T for the calculation of vaporization enthalpy.


## 3.3. Thermogravimetry Coupled with Mass Spectrometer Analysis

TG-MS analysis enabled the identification of vaporized molecules and thermal decomposition products from lactic acid at high temperatures. TG-MS profiles are shown in Figure5. From this figure, it was observed that water (m/z=18), hydroxyl (m/z=17), and methanol (m/z=32) were the main molecules eliminated during the heating. Water and methanol are impurities from DL-lactic acid commercially produced which has 90% of purity. Probably, water and methanol come from fermentation and separation processes, respectively. The hydroxyl group probably came from water. Lactide is also an impurity which was observed in DSC curve. The presence of lactide in the commercial lactic acid may be explained due to the tendency of lactic acid to polymerize in concentrated solutions. As described in the literature, above 30% of lactic acid concentration, the presence of lactide is observed [5]. Other mass fragments monitored during the thermal analysis appeared in low ionic current values.Figure 5
TG-MS profiles of lactic acid.Lactic acid can be conveniently converted into various value-added products, such as acrylic acid. For acrylic acid production, direct dehydration of lactic acid in high temperatures is an alternative. For better understanding the lactic acid thermal behavior at high temperatures, TG-MS isotherm of lactic acid at 573 K was performed as shown in Figure6. The isotherm profiles were divided into parts (a) and (b) for better visualization.Figure 6
TG-MS lactic acid isothermal at 573 K during the time. (a):m/z=17, 18, 32, 44, and 45. (b): m/z=72 and 74. The solid line in (b) is a type of noise from the equipment.
(a)
(b)Figure6 showed the fragments products of hydroxyl (m/z=17), water (m/z=18), methanol (m/z=32), acetaldehyde or/and carbon dioxide (m/z=44), formate (m/z=45), acrylic acid (m/z=72), and propionic acid (m/z=74). It can be concluded that various reactions occurred concurrently. At approximately 30 min of heating, the presence of dehydration reactions (11) as well as reduction (12) and decarboxylation reactions (13) was observed.(11)C3H6O3⟶C3H4O2+H2OLacticacid⟶acrylicacid+water(12)C3H6O3⟶C3H6O2+12O2Lacticacid⟶propionicacid+oxygen(13)C3H6O3⟶C2H4O+CO2+H2Lacticacid⟶acetaldehyde+carbondioxide+hydrogenAccording to the literature, the formation of self-reaction products such as lactide, which are subsequently more readily decomposed into fragments (e.g., carbon monoxide, acetaldehyde, and water), is the main reaction that competes with the dehydration process [29]. Data obtained from TG-MS are in agreement with the literature.Additionally, at the end of the analysis, the sample was found graphitized indicating that a quantity of the sample was reduced, also confirming the analysis of the mass profiles. It can be concluded that the decomposition process of lactic acid is related to temperature and the time of exposure to heat. In addition, only after 30 min of heating at 573 K lactic acid was decomposed into water, hydroxyl, methanol, acetaldehyde or/and carbon dioxide, formate, acrylic acid, and propionic acid as can be seen by increasing the current ionic at 30 min.Therefore, it is important work with separation processes, which minimize problems of thermal decomposition to avoid the formation of byproducts. Vacuum operations provide a substantial decrease in the boiling points of substances due to operating pressure reduction. This characteristic allows the separation of compounds that would be destroyed if the mixture is processed at normal pressures [30]. This characteristic is satisfied by the hybrid short path evaporation. It has been recognized as a promising technology mainly because of its low evaporation temperature and short residence time [31].


## 4. Conclusions

In this work, thermal characterization of lactic acid using thermoanalytical techniques was presented. DSC analyses showed endothermic peaks related to the process of evaporation. Effect of heating rate on TG and DTG curves was also presented and the data were correlated to Arrhenius and Kissinger equations to provide the evaporation kinetic parameters. Activation energies were 51.08 and 48.37 kJ·mol−1 and frequency values were 859.97 and 968.81 s−1 obtained by Arrhenius and Kissinger equations, respectively. Enthalpy of vaporization calculated by TG was 56.9 kJ·mol−1. TG-MS curve profiles showed many decomposition products when lactic acid was heated at 573 K in approximately 30 min. It can be concluded that decomposition process of lactic acid is related to temperature and the time of exposure to heat. Therefore, separation and purification processes which work with vacuum and short residence time are favored.



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*Source: 4149592-2017-04-18.xml*