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Thermodynamic Analysis of Methanol Synthesis viaCO2 Hydrogenation ReactionSuresh Kanuri
BITS Hyderabad: Birla Institute of Technology and Science - Hyderabad CampusSatyapaul A. Singh
BITS Hyderabad: Birla Institute of Technology and Science - Hyderabad CampusSantanu P. Datta
BITS Hyderabad: Birla Institute of Technology and Science - Hyderabad CampusChanchal Chakraborty
BITS Hyderabad: Birla Institute of Technology and Science - Hyderabad CampusSounak Roy
BITS Hyderabad: Birla Institute of Technology and Science - Hyderabad CampusSrikanta Dinda ( [email protected] )
BITS Hyderabad: Birla Institute of Technology and Science - Hyderabad Campushttps://orcid.org/0000-0001-5566-1891
Research Article
Keywords: CO2 hydrogenation, Methanol synthesis, Aspen simulation, Equilibrium analysis
Posted Date: August 6th, 2021
DOI: https://doi.org/10.21203/rs.3.rs-721475/v1
License: This work is licensed under a Creative Commons Attribution 4.0 International License. Read Full License
1
Thermodynamic Analysis of Methanol Synthesis via CO2 Hydrogenation Reaction 1
Suresh Kanuri1, Satyapaul A. Singh1, Santanu P. Datta2, Chanchal Chakraborty3, Sounak Roy3, and 2
Srikanta Dinda1* 3
1Department of Chemical Engineering, 2Department of Mechanical Engineering, 3Department of Chemistry, 4
Birla Institute of Technology and Science Pilani, Hyderabad Campus, Hyderabad, Telangana-500078, India. 5
6
*Corresponding Author: 7
Srikanta Dinda, Email: [email protected]; Telephone: +91–4066303586; Fax: +91–4066303998 8
9
Abstract 10
The most inspiring opportunity to reduce greenhouse gas emissions is direct hydrogenation of CO2 into a 11
commodity of products, which is also an appealing choice for generating renewable energy. CO2 hydrogenation 12
can yield methanol which has a broad range of applications. In the present study, a thermodynamic feasibility 13
analysis of the CO2 hydrogenation reaction is carried out using the Aspen Plus tool. CO2 hydrogenation to 14
methanol, reverse-water-gas-shift (RWGS), and methanol decomposition reactions were considered in this 15
analysis. The effect of different parameters such as temperature (ranging from 50 to 500 °C), pressures (ranging 16
from 1 bar to 50 bar), and CO2:H2 molar ratio (ranging from 1:3 to 1:20) on methanol yield has been investigated. 17
The Aspen predicted data is compared with the fixed-bed reactor experimental data. High pressure and low-18
temperature conditions are found to be the favourable option for a higher value of methanol yield. The CO2 19
conversion and CH3OH selectivity are favourable when the H2/CO2 molar ratio is greater than 3. A substantial gap 20
between the Aspen predicted equilibrium conversion of CO2 and the experimental value of CO2 conversion is 21
observed in the study. 22
23
Keywords: CO2 hydrogenation, Methanol synthesis, Aspen simulation, Equilibrium analysis. 24
25
2
1. Introduction 26
The growing trend of global warming, the declining trend of fossil fuel reserves, and the need for an 27
alternative to fossil fuels are the most critical challenges of the twenty-first century. CO2 levels in the atmosphere 28
have already exceeded the pre-industrial era by about 280 ppm and now reached 410 ppm (Li et al. 2018; Chen et 29
al. 2021). In this context, scientists and researchers concentrated on two key technologies: carbon capture and 30
storage (CCS) (Atsonios et al. 2016) and carbon capture and utilization (CCU) (Han et al. 2021). For reducing 31
CO2 concentrations in the atmosphere, the CCU has begun to emerge as a more appealing alternative than CCS 32
(Sha et al. 2020). When considering CCU, CO2 hydrogenation pathways have become essential for producing 33
useful chemicals such as syngas (CO2, CO, and H2), methane (CH4), methanol (CH3OH), ethanol (C2H5OH), 34
dimethyl ether (CH3OCH3), and formic acid (CH2O2) (Leonzio et al. 2019; Sharma et al. 2021). Methanol 35
synthesis from CO2 hydrogenation receives increasing emphasis than other commodities due to its environmental 36
friendliness, lack of toxic emissions when burned, and other uses (Din et al. 2019; Salehi et al. 2021). Methanol is 37
used as a solvent and a raw material to produce a wide range of chemicals (Dalena et al. 2018; Cai et al. 2020; 38
Zhong et al. 2020). The mission is to minimize the CO2 concentration, reduce Carbon emissions, and fulfil the 39
requirement for the chemicals listed above. 40
The synthesis of methanol from CO2 using Cu, Ag, Au, and Pd-based heterogeneous catalysts has also 41
been studied by a group of scientists and experts. Witoon et al. (2013) studied the CO2 hydrogenation to methanol 42
using Cu/ZnO catalyst at 180 °C and 20 bar. Their results revealed that the CH3OH selectivity is 98%, whereas 43
CO2 conversion is only 5%. Rui et al. (2020) investigated the in-situ characterizations using time-resolved X-ray 44
diffraction, ambient-pressure X-ray photoelectron spectroscopy, and X-ray absorption spectroscopy using 45
Au/In2O3 catalyst. Due to the gold-indium oxide strong metal-support interactions and the dispersion of gold, their 46
investigation demonstrated that methanol selectivity reaches 100% at 225 °C temperature and 50 bar pressure, but 47
CO2 conversion is only 1.3%. In another study, it is observed that Ce+3 ions increased the oxygen-vacant sites of 48
the PdZn/CeO2 catalyst, resulting in 100% methanol selectivity and 7.7% CO2 conversion at 220 °C and 30 bar 49
(Malik et al. 2018). Many scientists have performed experimental investigations on the hydrogenation of CO2 for 50
methanol synthesis using different catalysts for a wide range of pressure. Surprisingly, in many articles, nearly 51
100% methanol selectivity has been reported, but all of them experienced poor (<15%) CO2 conversion. 52
Therefore, the design of highly efficient, high-stability, and low-cost catalysts are immediately required to enable 53
the CO2 conversion for large-scale production. The thermodynamic analysis of any reactive system can anticipate 54
the feasibility of the maximum amount of desired products and the optimum conditions required to obtain the 55
desired yield. Therefore, understanding the thermodynamic aspects of the methanol synthesis reactions is essential 56
for the strategic development of the catalytic CO2 hydrogenation process. 57
In the present study, the thermodynamic feasibility of CO2 hydrogenation into CH3OH, RWGS, and 58
CH3OH decomposition reactions was investigated. The effects of various parameters such as temperature, 59
pressure, and feed composition on CO2 conversion and methanol selectivity have been examined. Furthermore, 60
the simulated data has been elaborated with figures and charts to understand the optimum operating conditions for 61
a specific conversion and selectivity. Also, the Aspen predicted data is compared with the experimental data 62
obtained from various literature. 63
3
2. Methodology 64
The Gibbs free energy minimization approach can precisely define the equilibrium composition of a 65
reaction system. The overall Gibbs free energy (G) of the system is minimum at equilibrium. The equilibrium 66
reactor model (REquil) in Aspen Plus software was used in the present work. The Peng-Robinson equation of 67
state (PENG-ROB EOS) model was considered to introduce non-ideal behaviour in the Gibbs energy values 68
(Miguel et al. 2015). In order to obtain a better understanding of the concept of hydrogenation of CO2 into 69
methanol, we focused on three possible reactions, namely methanol synthesis from CO2 hydrogenation (Eq. 1), 70
RWGS (Eq. 2), and CH3OH decomposition (Eq. 3). 71
CO2 + 3H2 ⇌ CH3OH + H2O ∆H298K = -49.5 kJ mol-1 (Eq. 1) 72
CO2 + H2 ⇌ CO + H2O ∆H298K = +41.1 kJ mol-1 (Eq. 2) 73
CH3OH ⇌ CO + H2 ∆H298K = +90.6 kJ mol-1 (Eq. 3) 74
The following expressions (Eq. 4-7) are used to define the CO2 conversion, methanol selectivity and yield, and 75
CO selectivity. 76
Conversion of CO2 (%)= [1-FCO2, out
FCO2, in]×100 (Eq. 4) 77
Selectivity of CH3OH (%)= [ FCH3OH, out
FCH3OH, out + FCO, out]×100 (Eq. 5) 78
Yield of CH3OH (%) = [FCH3OH, out
FCO2, in]×100 (Eq. 6) 79
Selectivity of CO (%)= [ FCO, outFCH3OH, out + FCO, out
]×100 (Eq. 7) 80
where Fi,in and Fi,out (i = CO2, CO, CH3OH) is the reactor inlet and outlet molar flowrates of species ‘i’, 81
respectively. All thermodynamic simulations are carried out under isothermal conditions. The results are shown in 82
terms of CO2 conversion, CH3OH yield, and selectivity of both CH3OH and CO for specific reaction conditions. 83
84
3. Results and Discussion 85
3.1. Effect of temperature on enthalpy, entropy, and Gibbs free energy change: 86
The shift in Gibbs free energy governs the spontaneity of a chemical reaction. Fig. 1(a-c) shows the 87
effect of temperature in enthalpy (ΔH), entropy (ΔS), and Gibbs free energy (ΔG) change of the CO2 88
hydrogenation, RWGS, and CH3OH decomposition reactions under 1 bar pressure. As observed in Fig. 1(a) and 89
Fig. 1(b), the ΔH and ΔS values for CO2 hydrogenation reaction are less than zero as the temperature rises from 90
25 °C to 500 °C. This signifies that the CO2 hydrogenation to methanol reaction is exothermic and decreases the 91
randomness. In contrast, the ΔH and ΔS values for both the RWGS and CH3OH decomposition reactions are 92
greater than zero with temperature. This implies that the RWGS and CH3OH decomposition reactions are 93
endothermic with increasing molecular disorder. As shown in Fig. 1(c), the ΔG for methanol synthesis reaction 94
has greater than zero and increases with temperature, which means this reaction is favourable at lower 95
4
temperatures. The ΔG for the RWGS reaction has positive values and decreases with temperature, implying this 96
reaction is favourable at higher temperatures. 97
On the other hand, the ΔG for methanol decomposition reaction has positive values with decreasing trend 98
up to 130 °C. This suggests that the methanol decomposition starts or favourable from 130 °C. Therefore, the CO2 99
hydrogenation to CH3OH reaction is exothermic and spontaneous at lower temperatures. In contrast, the RWGS 100
and methanol decomposition reactions are endothermic and spontaneous at higher temperatures. 101
50 100 150 200 250 300 350 400 450 500-100
-80
-60
-40
-20
0
20
40
60
80
100
50 100 150 200 250 300 350 400 450 500-80
-60
-40
-20
0
20
40
60
80
100
120
50 100 150 200 250 300 350 400 450 500
-0.2
-0.1
0.0
0.1
0.2
0.3∆G
(kJ/m
ol)
Temperature (°C)
(c)
CO2 + 3H2 CH3OH + H2O
CO2 + H2 CO + H2O
CH3OH CO + 2H2
∆H (k
J/mol
)
Temperature (°C)
(a)
CO2 + 3H2 CH3OH + H2O
CO2 + H2 CO + H2O
CH3OH CO + 2H2
∆S (k
J/mol
-K)
Temperature (°C)
CO2 + 3H2 CH3OH + H2O
CO2 + H2 CO + H2O
CH3OH CO + 2H2
(b)
102
Fig. 1: Effect of temperature on (a) ΔH, (b) ΔS, and (c) ΔG for CO2 hydrogenation, RWGS, and CH3OH 103
decomposition reactions under 1 bar pressure. 104
105
3.2. Influence of temperature and pressure on CO2 conversion and CH3OH selectivity: 106
According to Le Chatelier’s principle and thermodynamic feasibility, higher pressure and lower 107
temperature seem to be favourable conditions for higher methanol selectivity (Eq. 1). RWGS and methanol 108
decomposition reactions are also limited under these conditions due to their endothermic nature. Hence, high 109
pressures and low temperatures can be the optimum operating conditions to improve methanol selectivity and, at 110
the same time to reduce CO selectivity. The impact of temperature and pressure on CO2 conversion, CH3OH 111
selectivity, and CO selectivity was examined, and the outcomes are shown in Fig. 2(a-c). 112
The plots show that the equilibrium conversion of CO2 is regulated by both temperature and pressure. As 113
the temperature rises, the methanol formation reaction becomes less favoured, and the RWGS and methanol 114
decomposition reactions become more favoured, resulting in U-shaped curves in the CO2 conversion patterns. 115
Increased pressure enhances CO2 conversion in the low-temperature zone (e.g., 50 °C to 300 °C). However, at 116
high temperatures (between 300 °C and 500 °C), increasing pressure has almost no influence on CO2 conversion, 117
5
and this is why the CO2 conversion curves eventually converged at these temperatures. The methanol synthesis 118
reaction is improved by rising pressure, whereas the RWGS and methanol decomposition reactions are mostly 119
unchanged. This fact illustrates that, as pressure rises, both the CH3OH and CO selectivity curves shift to 120
extremely high temperatures. Several scientists have confirmed this phenomenon by employing various reaction 121
schemes and the Soave-Redlich-Kwong equation of state (Stangeland et al. 2018; Ahmad and Upadhyayula 2019). 122
50 100 150 200 250 300 350 400 450 5000
10
20
30
40
50
60
70
80
90
100
50 100 150 200 250 300 350 400 450 500
0
10
20
30
40
50
60
70
80
90
100
50 100 150 200 250 300 350 400 450 500
0
10
20
30
40
50
60
70
80
90
100
CO
2 C
onver
sion (
%)
Temperature (°C)
1 bar 20 bar
3 bar 30 bar
5 bar 40 bar
10 bar 50 bar
(a)
Temperature (°C)
1 bar 20 bar
3 bar 30 bar
5 bar 40 bar
10 bar 50 bar
CH
3O
H S
elec
tivit
y (
%) (b)
CO
Sel
ecti
vit
y %
Temperature (°C)
1 bar 20 bar
3 bar 30 bar
5 bar 40 bar
10 bar 50 bar
(c)
123
Fig. 2: Effect of pressure and temperature on (a) CO2 conversion, (b) CH3OH selectivity, and (c) CO selectivity, 124
for H2/CO2 mole value of 3. 125
126
The effect of pressure on the optimum value of operating temperature and CO2 conversion to achieve 127
99% CH3OH and 1% CO selectivity is concluded in Fig. 3. When the pressure rises from 1 bar to 50 bars, the CO2 128
conversion is noticeable, i.e., from 13% to 48%. Hence, the optimum value of operating parameters to obtain 99% 129
methanol selectivity and 48% CO2 conversion is about 172 °C and 50 bar for the H2/CO2 molar value of 3. 130
6
72
95
107
125
145
157
167172
13
2024
29
3640
4448
1 3 5 10 20 30 40 50 --
25
50
75
100
125
150
175
200
Temperature
CO2 Conversion
Pressure (bar)
Tem
per
ature
(°C
)
0
20
40
60
80
100
CO
2 C
onver
sion (
%)
131
Fig. 3: Effect of pressure on CO2 conversion and reactor temperature to achieve 99% CH3OH selectivity for 132
H2/CO2 molar value of 3. 133
134
3.3. Influence of feed gas composition on CO2 conversion and CH3OH selectivity: 135
To investigate the influence of feed composition on CH3OH selectivity, the CO2:H2 molar ratio was 136
varied between 1:3 to 1:20 for a fixed value of 50 bar pressure. The simulation was performed for a temperature 137
range between 150 °C to 400 °C, and the results are shown in Fig. 4(a-c). The plot shows that the increase of H2 138
partial pressure promotes both CO2 conversion and CH3OH selectivity. The methanol formation from CO2 139
decreased as the temperature increased, and consequently, the CO2 consumption diminishes. As a result, the 140
observed increase in CO2 conversion at higher temperatures suggests that extra H2 promotes the RWGS reaction. 141
As the CO2:H2 ratio was increased from 1:3 to 1:12, the most significant change in CO2 conversion occurs. 142
Further increase of CO2:H2 ratio from 1:13 to 1:17, there seems to be a lower improvement of CO2 conversions. 143
From 1:18 to 1:20, almost similar conversions were obtained. 144
Fig. 5 depicts the influence of feed gas composition on CO2 conversion and optimum temperature to 145
obtain 99% CH3OH and 1% CO selectivity under 50 bar reactor pressure. The simulation shows the CO2 146
conversion improved from 48% to 87% when the CO2:H2 molar ratio increased from 1:3 to 1:20. About 87% CO2 147
conversion and 99% methanol selectivity can be achievable at 187 °C under 50 bar pressure and a CO2:H2 ratio of 148
1:20. Though the boosting of H2 partial pressure in the feed promotes the conversion of CO2, it has a detrimental 149
impact on the process economics. 150
7
175 200 225 250 275 300 325 350 375 4000
20
40
60
80
100
175 200 225 250 275 300 325 350 375 4000
20
40
60
80
100
175 200 225 250 275 300 325 350 375 40020
30
40
50
60
70
80
90
100
CH
3O
H S
elec
tiv
ity
(%
)
Temperature (°C)
1:3 1:9 1:15
1:4 1:10 1:16
1:5 1:11 1:17
1:6 1:12 1:18
1:7 1:13 1:19
1:8 1:14 1:20
(b)
CO
Sel
ecti
vit
y (
%)
Temperature (°C)
1:3 1:9 1:15
1:4 1:10 1:16
1:5 1:11 1:17
1:6 1:12 1:18
1:7 1:13 1:19
1:8 1:14 1:20
(c)
CO
2 C
on
ver
sio
n (
%)
Temperature (°C)
1:3 1:9 1:15
1:4 1:10 1:16
1:5 1:11 1:17
1:6 1:12 1:18
1:7 1:13 1:19
1:8 1:14 1:20
(a)
151
Fig. 4: Effect of CO2:H2 molar ratio on (a) CO2 conversion, (b) CH3OH selectivity, and (c) CO selectivity at 152
50 bar reactor pressure. 153
154
172176
179181182183183184185185185186186186186186187187
48
55
6165
6972
75 77 78 80 81 82 83 84 85 86 86 87
1:4 1:6 1:8 1:10 1:12 1:14 1:16 1:18 1:20
100
110
120
130
140
150
160
170
180
190
200
210 Temperature (°C)
CO2 Conversion (%)
CO2:H2 molar ratio
Tem
per
ature
(°C
)
0
20
40
60
80
100
120C
O2 C
onver
sion (
%)
155
Fig. 5: Effect of CO2:H2 molar ratio on CO2 conversion and desired temperature to achieve 99% CH3OH 156
selectivity under 50 bar reactor pressure. 157
8
158
4. Comparison of CO2 conversion and CH3OH selectivity between simulation predicted and experimental 159
results 160
For a similar range of reactor temperature, pressure, and feed gas composition conditions, the simulation 161
predicted and experimental results for CO2 conversion are shown in Fig. 6. The experimental findings are reported 162
in the presence of Au/In2O3 (Rui et al. 2020) and Cu/ZnO/Al2O3 (Gaikwad et al. 2016) catalysts. The simulation 163
results obtained from the present investigation are comparable and match well with the simulation data reported 164
by Stangeland et al. (2018). However, a substantial gap between the theoretical and experimental values of CO2 165
conversion is noted. The equilibrium CO2 conversion and experimental CO2 conversions (over Au/In2O3 and 166
Cu/ZnO/Al2O3 catalysts) show more deviation at lower temperatures. However, the gap reduces gradually with the 167
increase of reactor temperature. The lower value of CO2 conversion in the presence of catalysts can be related to 168
the weak activity of the catalysts. 169
We further compared the equilibrium CH3OH selectivity data with experimental CH3OH selectivity 170
results, as shown in Fig.7. The Cu/ZnO/Al2O3 catalyst shows a significant deviation from the equilibrium CH3OH 171
selectivity, whereas the gap is much less for the Au/In2O3 catalyst. The methanol selectivity of the Au/In2O3 172
catalyst is greater than the equilibrium CH3OH selectivity and which may be due to the presence of Auδ+-In2O3-x 173
interfacial sites in the Au/In2O3 catalyst. A summary of literature data on CO2 conversion, CH3OH selectivity is 174
shown in Table 1, along with the present simulation results. 175
176
175 200 225 250 275 300 325
0
10
20
30
40
50
CO
2 C
on
ver
sio
n (
%)
Temperature (°C)
Present work (Theoretical study @ 50 bar)
Stangeland et al. (Theoretical study @ 50 bar)
Rui et al. (Au/In2O
3 study @ 50 bar)
Gaikwad et al. (Cu/ZnO/Al2O
3 study @ 46 bar)
177
Fig. 6: Comparison of theoretical and experimental CO2 conversion for CO2: H2 molar ratio of 1:3. 178
9
175 200 225 250 275 300 325
0
30
60
90
120
150
CH
3O
H S
elec
tivit
y (
%)
Temperature (°C)
Present work (Theoretical study@ 50 bar)
Stangeland et al. (Theoretical study @ 50 bar)
Rui et al. (Au/In2O3 study @ 50 bar)
Gaikwad et al. (Cu/ZnO/Al2O3 study @ 46 bar)
179
Fig. 7: Comparison of theoretical and experimental CH3OH selectivity for CO2: H2 molar ratio of 1:3. 180
181
182
Table 1: A comparison between the simulation and experimental findings on CO2 conversion and CH3OH
selectivity for the methanol synthesis via CO2 hydrogenation.
Catalyst CO2:H2
ratio
TR
(°C)
PR
(bar)
XCO2
(%)
SMeOH
(%)
Reference
PdZn/CeO2 1:3 220 30 7.7 100 (Malik et al. 2018)
Au/In2O3 1:3 225 50 1.3 100 (Rui et al. 2020)
Pd-Zn/CNTs 1:3 250 30 6.3 99 (Liang et al. 2009)
Cu/ZnO 1:3 180 20 5 98 (Witoon et al. 2013)
Cu/ZnO/Al2O3 1:3 240 46 20 40 (Gaikwad et al. 2016)
Cu/ZnO/Al2O3 1:3 170 50 25 73 (Liu et al. 2007)
- 1:3 200 50 39 98 Stangeland et al. (2018)
- 1:3 250 50 28 68 Stangeland et al. (2018)
- 1:3 172 50 48 99 Present work
- 1:3 250 50 28 72 Present work
- 1:10 184 50 77 99 Present work
- 1:10 250 50 51 80 Present work
- 1:20 187 50 87 99 Present work
where, TR = Reaction temperature; PR = Reaction pressure; XCO2 = CO2 conversion, SMeOH = Methanol
selectivity.
183
5. Conclusions 184
A comprehensive and detailed thermodynamic investigation of CO2 conversion to methanol is presented 185
in this study. Based on the thermodynamic feasibility findings, the methanol decomposition reaction has a higher 186
endothermicity than the RWGS reaction, while methanol production from CO2 is an exothermic reaction. The 187
methanol decomposition reaction has a greater entropy change with temperature than the methanol and RWGS 188
10
reactions. Due to more negative changes in Gibbs free energy, the methanol decomposition reaction is more 189
spontaneous at higher temperatures. In the methanol synthesis, the effect of various critical parameters such as 190
pressure, temperature, feed gas composition on CO2 conversion, and methanol selectivity is investigated. Low 191
temperature, high pressure, and a high CO2:H2 feed ratio are found to be favourable conditions to facilitate 192
methanol production from CO2 and H2. The CO2 conversion is prominent at a 1:3 CO2:H2 feed gas molar ratio if 193
the pressure builds up from 1 bar to 50 bar, i.e., from 13% to 48%. At 50 bar pressure, the CO2 conversion 194
improved from 48% to 87% with the increase of CO2:H2 mole ratio from 1:3 to 1:20. However, methanol 195
synthesis at higher (> H2:CO2 mole ratio of 5) H2 partial pressure may not be economically viable. The gap in CO2 196
conversion between the simulation predicted and experimental data may be due to the insufficient activity of the 197
catalyst. Therefore, to enhance the CO2 conversion and CH3OH selectivity, developing a highly efficient, 198
thermally and chemically stable, and low-cost catalyst is essential. 199
. 200
201
Declarations: 202
Ethics approval and consent to participate: ‘Not applicable’ 203
Consent for publication: ‘Not applicable’ 204
Availability of data and materials: very few data have been extracted from published articles for comparison 205
purpose, and same has been mentioned in the manuscript with proper reference. 206
Conflict of interest statement: The authors declare that they have no known competing financial interests or 207
personal relationships that could have appeared to influence the work reported in this paper. 208
Funding: This research did not receive any specific grant from funding agencies. 209
Authors' contributions: SK: Conceptualization, Investigation, Data generation, Writing-original draft; SAS: 210
Conceptualization, Methodology, Result validation; SPD: Resources, Data validation; CC: Project administration; 211
SR: Project administration, data validation; SD: Conceptualization, Supervision, result validation, Writing- review 212
and editing; ‘All authors read and approved the final manuscript." 213
214
215
Acknowledgment: The authors express their gratitude to BITS-Pilani Hyderabad Campus for providing the 216
necessary support for the present study. 217
218
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