# Total Oxidation of Isopropanol in Its Liquid Phase, at a Low Temperature in the Presence of Prepared and Characterized Zinc Oxide

Authors: Younes Dehmani; Abdellatif Amhoud; Sadik Abouarnadasse
Journal: International Journal of Analytical Chemistry
 (2021)

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## Abstract

The complete oxidation of isopropanol in its liquid phase at a low temperature was studied in the presence of zinc oxide (ZnO). This solid was prepared with the precipitation method. Structural analysis (infrared in Fourier transform and diffraction of X-rays) and textured (adsorption/desorption of N2) were conducted for the wurtzite structure results, an IV type isotherm with a type H3 hysteresis. This solid presents a good catalytic activity against the complete oxidation of isopropanol, a constant of selectivity equal to 1; however, the studied temperatures were 40, 60, and 80°C. In addition, a kinetic study of the oxidation was performed and showed that the reaction follows a successive mechanism isopropanol-acetone-carbon dioxide. The low value of the apparent energy of the activation of this solid confirms the high value of the initial rate of the catalytic oxidation reaction of isopropanol in the temperature range studied.


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## Body

## 1. Introduction

Volatile organic compounds (VOCs) are a major source of pollution. These compounds bring together various families: alkanes, alkenes, aromatics, ketones, alcohols, acetates, aldehydes, and chlorine [1]. The volatility of these compounds gives them the ability to propagate more or less far from their place of emission, thus leading to direct (toxicity and odor) and indirect impacts [2–5] (“Smog” and warming) on the air. Concern over this observation has prompted many countries to control their emissions of gases into the atmosphere [6].Several processes have been proposed for their destruction, and among them is the catalytic oxidation of these pollutants into carbon dioxide and water. Catalytic oxidation has many advantages over thermal oxidation, such as low cost [7]. It is, above all, profitable for treating effluents which are less concentrated in pollutants, thermal destruction then being discredited due to excessive energy consumption, in particular when the solvent content is low. However, the choice of catalyst is a very important parameter for obtaining the expected success in this type of process. This will allow the reaction rate to increase and operate at much lower temperatures [8–10].Oxides of transition metals such as Cr, Fe, Ni, Mn, Cu, Co, and Zn are both typical and cost-effective catalysts for the complete oxidation of VOC. The properties to be attributed to this class of catalyst such as selectivity, durability, nontoxicity, and low cost (commercially accessible (approachable)) make it a considerable area of research under development [7].The objective of our work is to test the catalytic potential of ZnO, in the reaction of the decomposition of isopropanol in the liquid phase and at low temperature. The choice of isopropanol in this study is based on its classification among VOC. The studied transition metal oxide was prepared by the precipitation method [11]. Characterization of catalyst is carried out by physicochemical methods such as structural, XRD and FTIR, and textural, adsorption/desorption of N2 gas [12, 13]


## 2. Experimental Part

### 2.1. Catalyst Preparation

A mass of zinc nitrate dihydrate (Zn(NO3)2.6H2O) was dissolved in a volume of distilled water. To this mixture, we added (7 ml/min) 20 ml molar solution of ammonia (NH4OH) dropwise. The resulting mixture was heated with constant stirring at 40°C for 1 hour and then filtered in vacuum. The resulting solid was washed several times with distilled water and dried overnight in oven at 100°C. The dried powder was calcined at 500°C for 3 hours [14].


### 2.2. Catalyst Characterization

(i)
XRD: the patterns were recorded using an X'PERT MPD-PRO wide-angle X-ray powder diffractometer equipped with a diffracted beam monochromator and CuKɑ radiation filtered with Ni (λ = 1, 5406 Å) [12, 13].(ii)
FTIR: characterization and structural changes were collected using the JASCO 4100 FTIR spectrometer with a resolution of 4 cm-1 and an accumulation of at least 64 scans [12, 13].(iii)
BET: BET adsorption measurements: N2 at T = −196°C was carried out using a Micromeritics ASAP 2010. The specific surface area and the mean pore diameter were determined, respectively, according to the standard BET and BJH (Barrett, Joyner, and Halenda) [12, 13].


### 2.3. Catalytic Test

To a ball to pass lapped 250 ml, used as reactor, are added 0.15 mL of isopropanol (reactive), 120 mg of catalyst, and 200 mL of distilled water successively. The temperature (the temperature of the water bath heating (reaction temperature)) is adjusted to the desired value (40°C, 60°C, and 80°C) before you plunge the ball serving reactor. Air (oxidizing reagent) is then admitted in the reactor using a lateral tubing under a flow of the order 40 mL/min (more than enough to make the solution constantly saturated in oxygen). The reaction mixture is stirred continuously for the duration of the test in order to facilitate the accessibility of the grains of the reagent catalyst and to ensure work in chemical plan. It should be recalled that each catalytic test was performed with one taken Virgin catalyst test. The chromatographic analysis was conducted using the SHIMADZU CR15A fitted with a column under the following conditions: the column temperature is 80°C and PN2 = 24.525 KPa, PH2 = 39.24 KPa, and Pair = 49.05 KPa [15].


## 2.1. Catalyst Preparation

A mass of zinc nitrate dihydrate (Zn(NO3)2.6H2O) was dissolved in a volume of distilled water. To this mixture, we added (7 ml/min) 20 ml molar solution of ammonia (NH4OH) dropwise. The resulting mixture was heated with constant stirring at 40°C for 1 hour and then filtered in vacuum. The resulting solid was washed several times with distilled water and dried overnight in oven at 100°C. The dried powder was calcined at 500°C for 3 hours [14].


## 2.2. Catalyst Characterization

(i)
XRD: the patterns were recorded using an X'PERT MPD-PRO wide-angle X-ray powder diffractometer equipped with a diffracted beam monochromator and CuKɑ radiation filtered with Ni (λ = 1, 5406 Å) [12, 13].(ii)
FTIR: characterization and structural changes were collected using the JASCO 4100 FTIR spectrometer with a resolution of 4 cm-1 and an accumulation of at least 64 scans [12, 13].(iii)
BET: BET adsorption measurements: N2 at T = −196°C was carried out using a Micromeritics ASAP 2010. The specific surface area and the mean pore diameter were determined, respectively, according to the standard BET and BJH (Barrett, Joyner, and Halenda) [12, 13].


## 2.3. Catalytic Test

To a ball to pass lapped 250 ml, used as reactor, are added 0.15 mL of isopropanol (reactive), 120 mg of catalyst, and 200 mL of distilled water successively. The temperature (the temperature of the water bath heating (reaction temperature)) is adjusted to the desired value (40°C, 60°C, and 80°C) before you plunge the ball serving reactor. Air (oxidizing reagent) is then admitted in the reactor using a lateral tubing under a flow of the order 40 mL/min (more than enough to make the solution constantly saturated in oxygen). The reaction mixture is stirred continuously for the duration of the test in order to facilitate the accessibility of the grains of the reagent catalyst and to ensure work in chemical plan. It should be recalled that each catalytic test was performed with one taken Virgin catalyst test. The chromatographic analysis was conducted using the SHIMADZU CR15A fitted with a column under the following conditions: the column temperature is 80°C and PN2 = 24.525 KPa, PH2 = 39.24 KPa, and Pair = 49.05 KPa [15].


## 3. Results and Discussion

### 3.1. Catalyst Characteristics

#### 3.1.1. Diffraction of X-Rays (XRD)

The sample of the solid ZnOcalcined at 500°C for 3 hours was analyzed by diffraction of X-rays. The diffractogram of X-rays obtained is presented in Figure1.Figure 1
XRD of ZnO.The diffractogram of zinc oxide shows some peaks of diffraction at 20 = 31.77°, 34.25°, 36.25°, 47.54°, 57.77°, 62.85°, 66.46°, 67,93°, and 69° that can be effected into the crystalline plan of ZnO (100), (002), (101), (102), (110), (103), (200), (112), and (201). All the reflexions can be indicated during ZnO phase hexagonal wurtzite with network constants = 0.3249 nm andc = 0.5205 nm, which is accurate with the standard data (card JCPDS N° 79-2205) [16]. The clearness and the intensity of the pick indicate the good crystalline nature of the prepared sample. No appearance of a line in the ZnO diffractogram indexed to the Zn(OH)2 structure, which means that Zn(OH)2 has been completely decomposed into ZnO at 500°C for 3 hours [17, 18].


#### 3.1.2. Fourier Transform Infrared (FTIR) Spectroscopy

The FTIR spectra obtained for ZnO (Figure2) show bands located at 406, 506, and 806 cm−1 characterizing ZnO. In addition, bands located at 3420; 1637, and 1385 cm−1 corresponding to the vibration of the hydroxyl group of water and carbon dioxide are also identified. [18, 19].Figure 2
Spectrum of ZnO.


#### 3.1.3. Adsorption and Desorption of N2

In heterogeneous catalysis, the catalyst activity depends on the active available surface; many settings can influence the accessibility of this surface to the catalytic oxidation reaction, such as the number of active sites, the form, and the pores’ dimensions. The technique that we used to determine the specific surface is based on the physic adsorption of inert gas, generally, at the temperature of the liquid nitrogen (−196°). Figure3 shows that the isotherm can be classified in type IV with a loop of hysteresis H3 depending on the classification of the UPAC. The hysteresis cycle is observed in a high relative pressure between 0.8 and 1. This result is due to the presence of dilated pores on the prepared samples.Figure 3
Isotherm of adsorption/desorption of N2 on ZnO.The presence of hysteresis sample in this isotherm is associated with the secondary process of capillary concentration, which is translated by filling completely the measured P/P0 < 1. The diameter of the pores was calculated based on the model of Barret, Joyner, and Halenda (BJH). The results confirm the presence of mesopores of size 14.067 nm; the Zinc oxide textural parameters are grouped in Table 1 [20].Table 1
Textural characteristics of solids.
SolidSpecific surface (m2/g)Volume (cm3/g)Pore diameter (Å)ZnO80.750.573220


### 3.2. Catalytic Test: Catalytic Oxidation of Isopropanol

#### 3.2.1. Blind Test

The tests were performed without a catalyst in the same pressure and temperature conditions, which show the absence of every catalytic activity in the homogenous phase, and same results were obtained by Sahroui et al. [21].


#### 3.2.2. Catalyst Mass Effect

We are interested in the evaluation of the impact of the mass of a catalyst on the activity of the oxidation reaction of isopropanol in its liquid phase at a low temperature of 80°C. We tested the zinc oxide with three masses: 120, 100, and 140 mg.The specific activity is defined as the number of moles of isopropanol disappeared per unit of time and unit of mass of the catalyst [15].(1)asmol⋅g−1⋅s−1=−1mdndt.The influence of the amount of catalyst on the specific activity is illustrated in Figure4. The initial specific activity relating to the disappearance of isopropanol keeps a constant value whatever the amount of catalyst is. This means that, under these conditions, the catalyst operates in the chemical regime and is not the diffusion regime.Figure 4
Mass effect on the isopropanol conversion.


#### 3.2.3. Evolution of the Conversion with Time

The tests of the catalytic oxidation of isopropanol’s performances in the liquid phase were conducted at reaction temperatures of 40°C, 60°C, and 80°C by ZnO. The results are presented in Figure5. The decomposition of isopropanol is catalyzed by zinc oxide conducted to the acetone, as a product of a reaction that dehydrogenates this alcohol. Figure 5 represents the evolution of the global transformation rate of isopropanol in terms of time, which indicates that this solid has good catalytic characteristics.Figure 5
Rate of isopropanol transformation in terms of the presence of ZnO.Zinc oxide allows a total conversion of isopropanol into carbon dioxide, and the water lasts no longer than 100 min, 120 min, and 140 min at a temperature of 80°C, 60°C, and 40°C. It can be concluded from this that the total destruction of isopropanol in the liquid phase is carried out rapidly at slightly moderate temperatures in the presence of this synthetic solid. These results of zinc oxide activity have been noted by many authors [22–26].The catalyst activity concerning the disappearance of a reactive is defined by the number of the reported moles by the unit of time that disappeared at the moment of the reaction. In addition to the temperature of the reaction and the composition of the reactor’s mixture, the catalytic activity depends on the nature of the catalyst and the structural textural properties. This dependence is expressed by the specific activity defined in the following. This dependence is expressed by the specific activity and defined as the ratio of the catalytic activity and the mass of catalyst as (mole/g·s) follows:(2)TTG=n0−nn0son=n01−TTGetV=−dndtestv0=n0∗dTTGdt,t=0,as=−dndt!t=0=nomc∗dTTGdt!t=0mole∗g−1∗s−1.The basic characteristics of the zinc oxide aqueous solution may explain the elevated rate of acetone in the catalytic oxidation of isopropanol and a high specific activity that increases with temperature and a high specific activity that increases with temperature (Table2). The obtained results show high efficiency in comparison with other works that used other catalysts that were used such as Al2O3, Cu4O3, and zeolite NaX [2, 27–32].Table 2
Kinetic settings of the reaction of the decomposition of isopropanol.
OxideT°Cas (mole·g−1·s−1)v0 (mole·s−1)Ln (as)Ln (vo)ZnO404.25E-065.09E-07−12.369600−14.4898641604.28E-065.13E-07−12.362667−14.4829315804.96E-065.95E-07−12.214868−14.3351319


### 3.3. The Kinetics of the Reaction

#### 3.3.1. Reaction Mechanism: Variation of TTG, TTact, and TTCO2

The curves of Figure6 present the rate evolution of global transformation TTG, acetone transformation TTact, and carbon dioxide TTCO2 in terms of TTG through different temperatures (40, 60, and 80°C).Figure 6
The rate evolution of the transformations TTG and TT acetone and TTCO2 in terms of TTG at different temperatures.The analysis of the results shows that the oxidation of isopropanol in carbon dioxide and water is complete at the temperature of 80°C for a reacting duration of 100 min; also, the transformation in carbon dioxide reaches two very important values which are 97% at 60°C and 93% at 40°C. The secondary product formed is acetone, with a trend higher than 72.04% at 80°C. The significant quantity of acetone produced by the decomposition reaction of isopropanol confirms the properties of the zinc oxide surface as a base [33, 34]. The results enable us to conclude that this catalyst presents basic sites and leads a predisposition to form acetone, a result that is confirmed in the bibliography [12]. The power of ZnO catalytic can be explained by the elevated capacity of transporting oxygen, as well as shifting easily between its reduced and oxidized form (the mechanism of Mars–van Krevelen) [2, 34, 35]. These curves behave the same way regardless of the temperature. The curve represents the rate of transformation of acetone in terms of the rate of global conversion pass by a maximum; therefore, the one corresponding to CO2 grams between 0 and 100 [31]. Therefore, this allows suggesting a mechanistic diagram of the form(3)Isopropanol⟹Acetone⟹Carbon's dioxide+waterThis was confirmed by the work of Ismagilov et al. [36] who showed that the isopropanol oxidizes in the presence of the plaques of alloy Al2O3 and Deepak Kullkarni who used several catalysts with a base of transitioning metals such as the catalyst used in the oxidation of isopropanol for example [34].


#### 3.3.2. Appeared Energy of Activation

The evolution curve of conversion of isopropanol that we obtained previously can be exploited to determine the kinetic parameters, such as the speed constantk and the appeared energy of activation and the oxidation reaction at constant temperatures [21].Specific activity can be expressed asas = A exp (−Ea/RT)f, where A is a preexponential Arrhenius factor and f a function of active constituents concentrations and catalyst mass.Then, at constant concentrations and variable temperature, a leaner expression of temperature inverse can be written as follows:(4)Logas=LogA+Logf−EaRT.The relation of Arrhenius by tracing the linelnas=lnA−Ea/R∗T.Figure7 presents the variation ln (as) = f (1/T); from this, we find the value of the appeared activation energy in the order of 3,48 kJ/mol for zinc oxide. It has to be noted that the weakest value of the activation energy is relative to the dispersion of isopropanol and is due to the strongest value of the initial speed in the domain of the studied temperature [21]. The obtained results in this study show weak activation energy in comparison to what Deepak Kulkarni’s work has shown [34]. This approves the big catalytic potential of zinc oxide.Figure 7
Logarithm variation of the initial speed in terms of 1/T (K−1).


## 3.1. Catalyst Characteristics

### 3.1.1. Diffraction of X-Rays (XRD)

The sample of the solid ZnOcalcined at 500°C for 3 hours was analyzed by diffraction of X-rays. The diffractogram of X-rays obtained is presented in Figure1.Figure 1
XRD of ZnO.The diffractogram of zinc oxide shows some peaks of diffraction at 20 = 31.77°, 34.25°, 36.25°, 47.54°, 57.77°, 62.85°, 66.46°, 67,93°, and 69° that can be effected into the crystalline plan of ZnO (100), (002), (101), (102), (110), (103), (200), (112), and (201). All the reflexions can be indicated during ZnO phase hexagonal wurtzite with network constants = 0.3249 nm andc = 0.5205 nm, which is accurate with the standard data (card JCPDS N° 79-2205) [16]. The clearness and the intensity of the pick indicate the good crystalline nature of the prepared sample. No appearance of a line in the ZnO diffractogram indexed to the Zn(OH)2 structure, which means that Zn(OH)2 has been completely decomposed into ZnO at 500°C for 3 hours [17, 18].


### 3.1.2. Fourier Transform Infrared (FTIR) Spectroscopy

The FTIR spectra obtained for ZnO (Figure2) show bands located at 406, 506, and 806 cm−1 characterizing ZnO. In addition, bands located at 3420; 1637, and 1385 cm−1 corresponding to the vibration of the hydroxyl group of water and carbon dioxide are also identified. [18, 19].Figure 2
Spectrum of ZnO.


### 3.1.3. Adsorption and Desorption of N2

In heterogeneous catalysis, the catalyst activity depends on the active available surface; many settings can influence the accessibility of this surface to the catalytic oxidation reaction, such as the number of active sites, the form, and the pores’ dimensions. The technique that we used to determine the specific surface is based on the physic adsorption of inert gas, generally, at the temperature of the liquid nitrogen (−196°). Figure3 shows that the isotherm can be classified in type IV with a loop of hysteresis H3 depending on the classification of the UPAC. The hysteresis cycle is observed in a high relative pressure between 0.8 and 1. This result is due to the presence of dilated pores on the prepared samples.Figure 3
Isotherm of adsorption/desorption of N2 on ZnO.The presence of hysteresis sample in this isotherm is associated with the secondary process of capillary concentration, which is translated by filling completely the measured P/P0 < 1. The diameter of the pores was calculated based on the model of Barret, Joyner, and Halenda (BJH). The results confirm the presence of mesopores of size 14.067 nm; the Zinc oxide textural parameters are grouped in Table 1 [20].Table 1
Textural characteristics of solids.
SolidSpecific surface (m2/g)Volume (cm3/g)Pore diameter (Å)ZnO80.750.573220


## 3.1.1. Diffraction of X-Rays (XRD)

The sample of the solid ZnOcalcined at 500°C for 3 hours was analyzed by diffraction of X-rays. The diffractogram of X-rays obtained is presented in Figure1.Figure 1
XRD of ZnO.The diffractogram of zinc oxide shows some peaks of diffraction at 20 = 31.77°, 34.25°, 36.25°, 47.54°, 57.77°, 62.85°, 66.46°, 67,93°, and 69° that can be effected into the crystalline plan of ZnO (100), (002), (101), (102), (110), (103), (200), (112), and (201). All the reflexions can be indicated during ZnO phase hexagonal wurtzite with network constants = 0.3249 nm andc = 0.5205 nm, which is accurate with the standard data (card JCPDS N° 79-2205) [16]. The clearness and the intensity of the pick indicate the good crystalline nature of the prepared sample. No appearance of a line in the ZnO diffractogram indexed to the Zn(OH)2 structure, which means that Zn(OH)2 has been completely decomposed into ZnO at 500°C for 3 hours [17, 18].


## 3.1.2. Fourier Transform Infrared (FTIR) Spectroscopy

The FTIR spectra obtained for ZnO (Figure2) show bands located at 406, 506, and 806 cm−1 characterizing ZnO. In addition, bands located at 3420; 1637, and 1385 cm−1 corresponding to the vibration of the hydroxyl group of water and carbon dioxide are also identified. [18, 19].Figure 2
Spectrum of ZnO.


## 3.1.3. Adsorption and Desorption of N2

In heterogeneous catalysis, the catalyst activity depends on the active available surface; many settings can influence the accessibility of this surface to the catalytic oxidation reaction, such as the number of active sites, the form, and the pores’ dimensions. The technique that we used to determine the specific surface is based on the physic adsorption of inert gas, generally, at the temperature of the liquid nitrogen (−196°). Figure3 shows that the isotherm can be classified in type IV with a loop of hysteresis H3 depending on the classification of the UPAC. The hysteresis cycle is observed in a high relative pressure between 0.8 and 1. This result is due to the presence of dilated pores on the prepared samples.Figure 3
Isotherm of adsorption/desorption of N2 on ZnO.The presence of hysteresis sample in this isotherm is associated with the secondary process of capillary concentration, which is translated by filling completely the measured P/P0 < 1. The diameter of the pores was calculated based on the model of Barret, Joyner, and Halenda (BJH). The results confirm the presence of mesopores of size 14.067 nm; the Zinc oxide textural parameters are grouped in Table 1 [20].Table 1
Textural characteristics of solids.
SolidSpecific surface (m2/g)Volume (cm3/g)Pore diameter (Å)ZnO80.750.573220


## 3.2. Catalytic Test: Catalytic Oxidation of Isopropanol

### 3.2.1. Blind Test

The tests were performed without a catalyst in the same pressure and temperature conditions, which show the absence of every catalytic activity in the homogenous phase, and same results were obtained by Sahroui et al. [21].


### 3.2.2. Catalyst Mass Effect

We are interested in the evaluation of the impact of the mass of a catalyst on the activity of the oxidation reaction of isopropanol in its liquid phase at a low temperature of 80°C. We tested the zinc oxide with three masses: 120, 100, and 140 mg.The specific activity is defined as the number of moles of isopropanol disappeared per unit of time and unit of mass of the catalyst [15].(1)asmol⋅g−1⋅s−1=−1mdndt.The influence of the amount of catalyst on the specific activity is illustrated in Figure4. The initial specific activity relating to the disappearance of isopropanol keeps a constant value whatever the amount of catalyst is. This means that, under these conditions, the catalyst operates in the chemical regime and is not the diffusion regime.Figure 4
Mass effect on the isopropanol conversion.


### 3.2.3. Evolution of the Conversion with Time

The tests of the catalytic oxidation of isopropanol’s performances in the liquid phase were conducted at reaction temperatures of 40°C, 60°C, and 80°C by ZnO. The results are presented in Figure5. The decomposition of isopropanol is catalyzed by zinc oxide conducted to the acetone, as a product of a reaction that dehydrogenates this alcohol. Figure 5 represents the evolution of the global transformation rate of isopropanol in terms of time, which indicates that this solid has good catalytic characteristics.Figure 5
Rate of isopropanol transformation in terms of the presence of ZnO.Zinc oxide allows a total conversion of isopropanol into carbon dioxide, and the water lasts no longer than 100 min, 120 min, and 140 min at a temperature of 80°C, 60°C, and 40°C. It can be concluded from this that the total destruction of isopropanol in the liquid phase is carried out rapidly at slightly moderate temperatures in the presence of this synthetic solid. These results of zinc oxide activity have been noted by many authors [22–26].The catalyst activity concerning the disappearance of a reactive is defined by the number of the reported moles by the unit of time that disappeared at the moment of the reaction. In addition to the temperature of the reaction and the composition of the reactor’s mixture, the catalytic activity depends on the nature of the catalyst and the structural textural properties. This dependence is expressed by the specific activity defined in the following. This dependence is expressed by the specific activity and defined as the ratio of the catalytic activity and the mass of catalyst as (mole/g·s) follows:(2)TTG=n0−nn0son=n01−TTGetV=−dndtestv0=n0∗dTTGdt,t=0,as=−dndt!t=0=nomc∗dTTGdt!t=0mole∗g−1∗s−1.The basic characteristics of the zinc oxide aqueous solution may explain the elevated rate of acetone in the catalytic oxidation of isopropanol and a high specific activity that increases with temperature and a high specific activity that increases with temperature (Table2). The obtained results show high efficiency in comparison with other works that used other catalysts that were used such as Al2O3, Cu4O3, and zeolite NaX [2, 27–32].Table 2
Kinetic settings of the reaction of the decomposition of isopropanol.
OxideT°Cas (mole·g−1·s−1)v0 (mole·s−1)Ln (as)Ln (vo)ZnO404.25E-065.09E-07−12.369600−14.4898641604.28E-065.13E-07−12.362667−14.4829315804.96E-065.95E-07−12.214868−14.3351319


## 3.2.1. Blind Test

The tests were performed without a catalyst in the same pressure and temperature conditions, which show the absence of every catalytic activity in the homogenous phase, and same results were obtained by Sahroui et al. [21].


## 3.2.2. Catalyst Mass Effect

We are interested in the evaluation of the impact of the mass of a catalyst on the activity of the oxidation reaction of isopropanol in its liquid phase at a low temperature of 80°C. We tested the zinc oxide with three masses: 120, 100, and 140 mg.The specific activity is defined as the number of moles of isopropanol disappeared per unit of time and unit of mass of the catalyst [15].(1)asmol⋅g−1⋅s−1=−1mdndt.The influence of the amount of catalyst on the specific activity is illustrated in Figure4. The initial specific activity relating to the disappearance of isopropanol keeps a constant value whatever the amount of catalyst is. This means that, under these conditions, the catalyst operates in the chemical regime and is not the diffusion regime.Figure 4
Mass effect on the isopropanol conversion.


## 3.2.3. Evolution of the Conversion with Time

The tests of the catalytic oxidation of isopropanol’s performances in the liquid phase were conducted at reaction temperatures of 40°C, 60°C, and 80°C by ZnO. The results are presented in Figure5. The decomposition of isopropanol is catalyzed by zinc oxide conducted to the acetone, as a product of a reaction that dehydrogenates this alcohol. Figure 5 represents the evolution of the global transformation rate of isopropanol in terms of time, which indicates that this solid has good catalytic characteristics.Figure 5
Rate of isopropanol transformation in terms of the presence of ZnO.Zinc oxide allows a total conversion of isopropanol into carbon dioxide, and the water lasts no longer than 100 min, 120 min, and 140 min at a temperature of 80°C, 60°C, and 40°C. It can be concluded from this that the total destruction of isopropanol in the liquid phase is carried out rapidly at slightly moderate temperatures in the presence of this synthetic solid. These results of zinc oxide activity have been noted by many authors [22–26].The catalyst activity concerning the disappearance of a reactive is defined by the number of the reported moles by the unit of time that disappeared at the moment of the reaction. In addition to the temperature of the reaction and the composition of the reactor’s mixture, the catalytic activity depends on the nature of the catalyst and the structural textural properties. This dependence is expressed by the specific activity defined in the following. This dependence is expressed by the specific activity and defined as the ratio of the catalytic activity and the mass of catalyst as (mole/g·s) follows:(2)TTG=n0−nn0son=n01−TTGetV=−dndtestv0=n0∗dTTGdt,t=0,as=−dndt!t=0=nomc∗dTTGdt!t=0mole∗g−1∗s−1.The basic characteristics of the zinc oxide aqueous solution may explain the elevated rate of acetone in the catalytic oxidation of isopropanol and a high specific activity that increases with temperature and a high specific activity that increases with temperature (Table2). The obtained results show high efficiency in comparison with other works that used other catalysts that were used such as Al2O3, Cu4O3, and zeolite NaX [2, 27–32].Table 2
Kinetic settings of the reaction of the decomposition of isopropanol.
OxideT°Cas (mole·g−1·s−1)v0 (mole·s−1)Ln (as)Ln (vo)ZnO404.25E-065.09E-07−12.369600−14.4898641604.28E-065.13E-07−12.362667−14.4829315804.96E-065.95E-07−12.214868−14.3351319


## 3.3. The Kinetics of the Reaction

### 3.3.1. Reaction Mechanism: Variation of TTG, TTact, and TTCO2

The curves of Figure6 present the rate evolution of global transformation TTG, acetone transformation TTact, and carbon dioxide TTCO2 in terms of TTG through different temperatures (40, 60, and 80°C).Figure 6
The rate evolution of the transformations TTG and TT acetone and TTCO2 in terms of TTG at different temperatures.The analysis of the results shows that the oxidation of isopropanol in carbon dioxide and water is complete at the temperature of 80°C for a reacting duration of 100 min; also, the transformation in carbon dioxide reaches two very important values which are 97% at 60°C and 93% at 40°C. The secondary product formed is acetone, with a trend higher than 72.04% at 80°C. The significant quantity of acetone produced by the decomposition reaction of isopropanol confirms the properties of the zinc oxide surface as a base [33, 34]. The results enable us to conclude that this catalyst presents basic sites and leads a predisposition to form acetone, a result that is confirmed in the bibliography [12]. The power of ZnO catalytic can be explained by the elevated capacity of transporting oxygen, as well as shifting easily between its reduced and oxidized form (the mechanism of Mars–van Krevelen) [2, 34, 35]. These curves behave the same way regardless of the temperature. The curve represents the rate of transformation of acetone in terms of the rate of global conversion pass by a maximum; therefore, the one corresponding to CO2 grams between 0 and 100 [31]. Therefore, this allows suggesting a mechanistic diagram of the form(3)Isopropanol⟹Acetone⟹Carbon's dioxide+waterThis was confirmed by the work of Ismagilov et al. [36] who showed that the isopropanol oxidizes in the presence of the plaques of alloy Al2O3 and Deepak Kullkarni who used several catalysts with a base of transitioning metals such as the catalyst used in the oxidation of isopropanol for example [34].


### 3.3.2. Appeared Energy of Activation

The evolution curve of conversion of isopropanol that we obtained previously can be exploited to determine the kinetic parameters, such as the speed constantk and the appeared energy of activation and the oxidation reaction at constant temperatures [21].Specific activity can be expressed asas = A exp (−Ea/RT)f, where A is a preexponential Arrhenius factor and f a function of active constituents concentrations and catalyst mass.Then, at constant concentrations and variable temperature, a leaner expression of temperature inverse can be written as follows:(4)Logas=LogA+Logf−EaRT.The relation of Arrhenius by tracing the linelnas=lnA−Ea/R∗T.Figure7 presents the variation ln (as) = f (1/T); from this, we find the value of the appeared activation energy in the order of 3,48 kJ/mol for zinc oxide. It has to be noted that the weakest value of the activation energy is relative to the dispersion of isopropanol and is due to the strongest value of the initial speed in the domain of the studied temperature [21]. The obtained results in this study show weak activation energy in comparison to what Deepak Kulkarni’s work has shown [34]. This approves the big catalytic potential of zinc oxide.Figure 7
Logarithm variation of the initial speed in terms of 1/T (K−1).


## 3.3.1. Reaction Mechanism: Variation of TTG, TTact, and TTCO2

The curves of Figure6 present the rate evolution of global transformation TTG, acetone transformation TTact, and carbon dioxide TTCO2 in terms of TTG through different temperatures (40, 60, and 80°C).Figure 6
The rate evolution of the transformations TTG and TT acetone and TTCO2 in terms of TTG at different temperatures.The analysis of the results shows that the oxidation of isopropanol in carbon dioxide and water is complete at the temperature of 80°C for a reacting duration of 100 min; also, the transformation in carbon dioxide reaches two very important values which are 97% at 60°C and 93% at 40°C. The secondary product formed is acetone, with a trend higher than 72.04% at 80°C. The significant quantity of acetone produced by the decomposition reaction of isopropanol confirms the properties of the zinc oxide surface as a base [33, 34]. The results enable us to conclude that this catalyst presents basic sites and leads a predisposition to form acetone, a result that is confirmed in the bibliography [12]. The power of ZnO catalytic can be explained by the elevated capacity of transporting oxygen, as well as shifting easily between its reduced and oxidized form (the mechanism of Mars–van Krevelen) [2, 34, 35]. These curves behave the same way regardless of the temperature. The curve represents the rate of transformation of acetone in terms of the rate of global conversion pass by a maximum; therefore, the one corresponding to CO2 grams between 0 and 100 [31]. Therefore, this allows suggesting a mechanistic diagram of the form(3)Isopropanol⟹Acetone⟹Carbon's dioxide+waterThis was confirmed by the work of Ismagilov et al. [36] who showed that the isopropanol oxidizes in the presence of the plaques of alloy Al2O3 and Deepak Kullkarni who used several catalysts with a base of transitioning metals such as the catalyst used in the oxidation of isopropanol for example [34].


## 3.3.2. Appeared Energy of Activation

The evolution curve of conversion of isopropanol that we obtained previously can be exploited to determine the kinetic parameters, such as the speed constantk and the appeared energy of activation and the oxidation reaction at constant temperatures [21].Specific activity can be expressed asas = A exp (−Ea/RT)f, where A is a preexponential Arrhenius factor and f a function of active constituents concentrations and catalyst mass.Then, at constant concentrations and variable temperature, a leaner expression of temperature inverse can be written as follows:(4)Logas=LogA+Logf−EaRT.The relation of Arrhenius by tracing the linelnas=lnA−Ea/R∗T.Figure7 presents the variation ln (as) = f (1/T); from this, we find the value of the appeared activation energy in the order of 3,48 kJ/mol for zinc oxide. It has to be noted that the weakest value of the activation energy is relative to the dispersion of isopropanol and is due to the strongest value of the initial speed in the domain of the studied temperature [21]. The obtained results in this study show weak activation energy in comparison to what Deepak Kulkarni’s work has shown [34]. This approves the big catalytic potential of zinc oxide.Figure 7
Logarithm variation of the initial speed in terms of 1/T (K−1).


## 4. Conclusions

In conclusion, we can conclude that the structural characteristics show a wurtzite structure, particles of this oxide with a hexagonal shape, that the textural characteristic rises, and that the isotherm is of type IV with a hysteresis loop H3.Zinc oxide prepared by the precipitation method presents a good catalytic activity against the reaction of decomposition of isopropanol in its liquid phase with a low temperature and acetone as a mediating product. An activity of the order4.25E − 06 mole·g−1·s−1 for the temperature of 40°C, 4.28E − 06 mole·g−1·s−1 for the temperature of 60°C, and 4.96E − 06 mole·g−1·s−1 for the temperature of 80°C are shown.Otherwise, the kinetic study of the reaction of the oxidation, in liquid phase of the realized isopropanol, showed that this reaction follows a successive mechanism of isopropanol.



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*Source: 6667551-2021-02-09.xml*