Lipika Das1, Koushik Guha Biswas2* and Jayanta Kumar Basu3
1Department of Chemical Engineering, Haldia Institute of Technology, India
2Department of Chemical Engineering, Rajiv Gandhi Institute of Petroleum Technology, India
3Department of Chemical Engineering, Indian Institute of Technology, India
*Corresponding author: Koushik Guha Biswas, Department of Chemical Engineering, Rajiv Gandhi Institute of Petroleum Technology, Amethi, Uttar Pradesh, Pin-229304 India, Email: firstname.lastname@example.org.
Submission: January 01, 2018; Published: February 15, 2018
ISSN 2637-8035Volume1 Issue1
Phenol is nitrated selectively by dilute nitric acid over alumina and a remarkable ortho-selectivity is observed in liquid phase nitration.
i. The solid acid catalyst (Gamma-alumina) was prepared by control precipitation method.
ii. Phenol was selectively nitrated in liquid phase using dilute nitric acid (30%) in presence γ-alumina.
iii. The nitration reaction was carried out at room temperature and produce ortho-nitrophenol.
iv. The activation energy of the reaction was 11.272 KJ/mol.
v. The kinetic study was also observed.
Phenol was selectively nitrated in liquid phase to produce ortho-nitrophenol using dilute nitric acid (30%) at room temperature in presence of hydrochloric acid treated γ-alumina. Initially Al (NO3) and NH4HCO3 were reacted to prepare Al (OH)3 which on successive calcinations at 550 0C for 5h produce γ-alumina. The γ-alumina was characterized by BET, XRD, SEM and NH3-TPD analysis. The XRD profile confirmed the crystalline structure of the solid acid catalyst γ-alumina. The NH3-TPD analysis showed the development of lewis acidity on the surface of hydrochloric acid treated γ-alumina. The effects of various parameters such as concentration of reactants, types of catalyst, weight of the catalyst, solvent, temperature and time of reaction have been studied. The kinetics of the reaction was also investigated.
Keywords: Gamma alumina catalyst; Nitration reaction; Ortho-nitrophenol; Rate constant
Nitration ofaromatic substances has great industrial importance because nitro-aromatics are extensively used as raw material for manufacturing dyes, pharmaceuticals, perfumes and plastics [1,2]. It is found from the previous study that the nitration of phenol using a mixture of nitric and sulfuric acid gives 2-nitrophenol and 4-nitrophenol in a ratio of 1.42 . The limitation of this process lies in the use of corrosive liquid mixture of nitric and sulfuric acid which produce large amounts of wastes. The other problems are the chance of over nitration, poor selectivity and high cost of the process etc. . To overcome these difficulties a new and simpler technique such as solid acid nitration should be employed. In the solid acid nitration process the solid acid is used as a catalyst instead of sulfuric acid to produce nitronium ion. It is found from various literature that the nitration of phenol was carried out using different catalysts such as hydrous zirconia , tetra butyl ammonium bromide [5,6], sulfated titania , N2O5-ClNO2 , p-Toluenesulfonic acid , ZSM-5 Zeolite , sulfated titania  and SnO2 . The selectivity of the product is increased by using proper solvent with solid acid catalyst. In the last few years various nitration procedures have been performed using different aromatic solvents such as N-nitropyrazole/ BF3, Zn(NO3)2•6H2O/2,4,6- trichloro-1,3,5-triazine in acetonitrile  and ionic liquid . On the other hand alumina has extensive applications in organic reactions, either as an active participant or as an inert support. Alumina-based solid acid catalysts are potentially attractive due to the easy removability of substrate-product and easy recycling. The ortho-nitrophenol which is a major product of nitration reaction used for synthesis of valuable compounds. Some of these methods have contributed significantly for enhancing the scope of nitration reaction but very little work has been done on the region selectivity of phenol over alumina as a catalyst .
In the present work a suitable solid acid catalyst was investigated for nitration of phenol to ortho-nitrophenol. The region selectivity of phenol was studied using dilute nitric acid as nitrating agent over alumina as solid acid catalyst. The selectivity of the reaction is increased by using carbon tetra chloride as a solvent with the catalyst. The effects of different process parameters such as type of catalyst, weight of catalyst, time, temperature, reactant concentration, type of solvents and HCl treatment were observed. The kinetic study was also performed.
Aluminium nitrate (Al(NO3)3, 9H2O, 95%) of GR grade, ammonium bi carbonate (NH4HCO3, 98%) of GR grade, acetone (CH3COCH3), carbon tetrachloride (CCl4), methanol, sodium hydroxide (NaOH) and phenol(C6H5OH) were procured from Merck (India) Ltd., Mumbai, India. Ethanol (C2H5OH) was supplied by Jiangsu Huaxi International Trade Co. Ltd., China and nitric acid (HNO3) was procured from S. d. fine Chem Ltd. Hydrochloric Acid (HCl) was procured from Sarabhai M Chemicals.
Gamma alumina was prepared using control precipitation technique. Initially 15.42gm of ammonium bicarbonate and 40gm of aluminum nitrate was dissolved separately in 600ml of deionized water. The solutions were added drop wise to 400ml deionized water in a reaction vessel (Eq. 1). The reaction vessel was placed in a water bath and the temperature was maintained at 70 0C. The mixture was stirred for 30 minutes. The pH of the solution was adjusted by using HNO3 or NaOH to precipitate Al cations in the form of hydroxide (Eq. 2). Then the precipitate was aged at 70 oc for 3hours and washed thoroughly with warm de-ionized water, ethanol followed by acetone to avoid contamination of Na ions. The washed material was air-dried at 120 oc for 12hours. After air drying the precipitate was calcined in a programmable furnace at 550 oc for 5hours. The various reactions involved in the preparation of alumina are given bellow.
Alumina powder was activated using hydrochloric acid (HCl). It was soaked for 30hours in de-ionized water and different percentages of HCl at room temperature. Then the material washed thoroughly with distilled water and dried overnight at 120 oc. The sample was then calcined at 350 oc for 2hours in presence of oxygen.
The characterization of the catalyst was done by using the BET surface area analyzer (AUTOSORB-ic- USA), scanning electron microscope (Hitachi model SU-70), chemical composition of the catalyst, NH3-TPD (Quantachrome Instruments) and x-ray diffractometer (Philips PW183).
Nitration of phenol to orthonitro phenol was performed in a. three necked round bottom flask type glass reactor (6.5cm I.D) with a capacity of 250cm3. The reactor was equipped with a four- leg vertical baffle (2.0cm diameter) which is located at a height of 1.5cm from the bottom of the reactor. Two gram of phenol was taken in a flask containing 3ml carbon tetrachloride. Then lg of alumina and 4ml of dilute nitric acid (30%) were added into it. The reaction mixture was stirred at room temperature for varying period of time to study the progress of the reaction. The products were analyzed by HPLC((Column -Zorabax C-18 Reverse phase, Column Length-250mm, Column Dia-4.6mm, Pump-(Perkin Elmer, series 200, Isocratic pump), Detector-(Perkin Elmer, series 200, UV/VIS Detector), Mobile Phase- 50% Methanol / 50% Water, Flow Rate- 1.0ml/min, Wavelength-254n).
The kinetic study was performed in the same glass reactor as above. The reaction mixture was agitated for 180minutes and samples were collected at different time intervals. The experimental data were analyzed by pseudo first and second order kinetics mechanism. Although the reaction is carried out heterogeneously, but a homogeneous reaction mechanism with a second-order kinetics is assumed to interpret the experimental data. The isothermal reaction under constant-volume conditions results in the rate equation of the following form
Where A is limiting reactant phenol and B is excess reactant nitric acid.
After integrating equation (5) the final form is represented as equation (6).
Where CA0 and CB0 represent the initial concentrations of reactants A and B respectively and k is the reaction rate constant. CB0
Arrhenius equation describes the effect of temperature on activation energy E and the frequency factor A. The value of E can be calculated from the rate constants at three different temperatures (T). The temperature dependency of reaction rate, k, is given by the Arrhenius equation,
k = Ae-E/RT (7)
The rate constant k can be obtained from equation (6). It is an average of values calculated at various experimental kinetic data points (i.e., reactant concentrations at various reaction times).
Table 1: Characteristics of different catalysts.
Figure 1: SEM analysis of γ-Al2O3.
The surface area, pore volume and the average pore size of alumina and acid treated alumina were analyzed in BET surface area analyzer. The values are shown in Table 1. The scanning electron microscope (SEM) image (Figure 1) of the alumina catalyst indicates strong agglomeration of alumina particles. The scanning electron microscope (SEM) image also confirms the formation of a gamma phase (y -Al2O3) on alumina catalyst. Quantitative as well as qualitative composition analysis of prepared alumina was determined by EDS spectrum obtained from SEM. The elemental analysis of prepared alumina shows that it contains 59.42% O and 40.58% Al. The NH3-TPD spectra of the γ-alumina powder and acid treated γ- alumina powder is shown in Figure 2. It is seen that the TPD spectra (Figure 2) of the γ-alumina powder contain intense peaks in the temperature range of 100-800 0C. These peaks can be assigned to the NH3 desorbed from the acidic sites with medium to high strengths. Therefore, it can be concluded that the acid treated γ-alumina powder possesses strong surface acidic sites as compared to the γ-alumina powder. So the acid treatment improves the surface area and surface acidity of γ-Al2O3 Thus, the resulted γ-Al2O3 gave more lewis acidity and acid density. The x-ray diffraction (XRD) profile of the γ-Al2O3 confirms spinal lattice structure of the catalyst (Figure 3). The peaks indicate the amorphous nature of γ-A12O3. The crystallite sizes calculated by using the Scherrer equation were found to be in the range of 4.5-5.5nm.
Figure 2: NH3-TPD profiles of γ-alumina and acid treated γ-alumina.
Figure 3: X-ray diffraction pattern of γ-alumina.
Figure 4: Effect of the solvents (Volume of phenol- 5ml, volume of CCl4 - 7.5ml, HNO3 (30%)-3ml, weight of γ-alumina-3gm, reaction time-3h, stirrer speed-400rpm).
To select a suitable solvent the nitration of phenol was carried out at room temperature in presence of carbon tetrachloride (CCl4), methanol and acetone using γ-alumina catalyst. The reaction was carried out using dilute nitric acid (30%). The highest conversion of o-nitrophenol was obtained by using carbon tetrachloride as a solvent (Figure 4). The time required for completion of the reaction is also less in case of CCT4 Therefore CCL4 is selected as a suitable solvent for the further nitration study.
Figure 5: Effects of different catalysts.
The nitration of phenol was carried out separately in presence of γ- alumina and H-mordenite. The reaction was carried out at room temperature for three hours. For this purpose 5ml phenol and 3ml HNO3 (30%) were taken and 3g of catalyst was added into it. The CCl4 (7.5ml) was used as a solvent and the highest yield of o-nitro phenol was obtained using alumina catalyst. The yield of o-nitro phenol was decreased when the catalyst was changed from alumina to H-mordenite. The conversion of o-nitro phenol was low in this case because of less number of acid sites as well as porosity of H-mordenite. The reaction was also carried out in absence of catalyst and the conversion was further decreased, resulting nearly equal amount of ortho- and para- isomers. The effects are shown in Figure 5.
Effect of HCl treatment on alumina catalyst
Figure 6: Effect of HCl treatment on alumina catalyst.
The catalytic activity of alumina was enhanced by treating it with different percentage of hydrochloric acid. The catalytic activity is increased with increase in surface acidity and was found to be in the following order 7%HCl treated alumina>5%HCl treated alumina>3%HCl treated alumina . The effects are shown in Figure 6. The other reaction conditions such as type of solvent , amount of reactants , reaction time and temperature were remain same as before.
Figure 7: Effect of reaction time.
The nitration of phenol was carried out by varying reaction time in the presence of alumina catalyst (3gm) at room temperature. The reaction time was varied from 5-270min. In this case phenol (5ml) and dilute nitric acid (3ml) were used as reactants and CCl4 (7.5ml) was used as a solvent. The results indicate that the yield of o-nitro phenol increases with increasing reaction time because more number of nitronium ions are formed as the time proceeds, resulting higher conversion of phenol (Figure 7). Therefore the maximum yield of o-nitrophenol was obtained at 4.5h.
Figure 8: Effect of catalyst weight.
The conversion of o-nitrophenol also depends on the weight of catalyst. The nitration of phenol was carried out using dilute nitric acid (3ml) using different weight of alumina catalyst at room temperature. The effects are shown in Figure 8. The percent conversion of phenol increases with increasing weight of catalyst due to availability of more surface area. The reaction speed is also enhanced with increasing catalyst dose. Therefore the highest conversion was obtained using 5gm of catalyst.
Figure 9: Effect of reactant concentration (Volume of CCl4-7.5ml, HNO3 (30%)-3ml, reaction time= 3h, reaction temperature-room temperature and stirrer speed-400rpm).
The effect of concentration of phenol and nitric acid is studied on the rate of reaction and the effects are shown in Figure 9. As the concentration of reactants (phenol and nitric acid) is increased, the rate of reaction also increases.
Figure 10: Second order model fit.
The pseudo second order rate expressions were taken into consideration to correlate the kinetic data. Here the second order rate model (Equation 6) was fitted with data of nitration reaction (Figure 10). The kinetic study was carried out by varying the amount of nitric acid from 10-15ml. The other reaction conditions are kept as before for both the cases. It was observed that the kinetics of nitration for both the cases obeys the pseudo second order rate equation. The values of kinetic parameters are shown in Table 2. It can be seen from the following figures that for two different volume of nitric acid (10 and 15ml) the values of rate constant is 5.839 and 6.353L mole-1 sec-1 respectively.
Figure 11: Effect of temperature of the reaction.
The kinetic study was also performed by varying the reaction temperature from 30-80 0C to investigate the Arrhenius Equation. The values of different parameters such as amount of phenol, amount of solvent, weight of catalyst and the reaction time were maintained as before throught out the reaction. Fifteen ml of nitric acid was taken in this case. The values of rate constant at different temperature are obtained from Figure 11. The activation energy is calculated from the slop of Figure 12 and it is found to be 11.272KJ/ mol.
Figure 12: Temperature dependency of a reaction according to Arrhenius law.
Phenol is selectively nitrated to ortho-nitrophenol in high yields with dilute nitric acid in carbon tetrachloride solvent over gamma-alumina catalyst. The gamma-alumina catalyst could be easily separated from the reaction mixture by filtration for recycle and the workup procedure is simple as compared to the other conventional process. The region selectively nitration of phenol using dilute nitric acid over solid acid catalyst without any use of acetic anhydride/acyl nitrate, metal nitrates or sulfuric acid is a comparatively clean and environmental friendly process.
© 2018 Lipika Das, et al. This is an open access article distributed under the terms of the Creative Commons Attribution License , which permits unrestricted use, distribution, and build upon your work non-commercially.