# Study of Zn-Cu Ferrite Nanoparticles for LPG Sensing

Authors: Anuj Jain; Ravi Kant Baranwal; Ajaya Bharti; Z. Vakil; C. S. Prajapati
Journal: The Scientific World Journal
 (2013)

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## Abstract

Nanostructured zinc-copper mixed ferrite was synthesized using sol-gel method. XRD patterns of different compositions of zinc-copper ferrite,Zn(1-x)CuxFe2O4 (x=0.0, 0.25, 0.50, 0.75), revealed single phase inverse spinel ferrite in all the samples synthesized. With increasing copper concentration, the crystallite size was found to be increased from 28 nm to 47 nm. The surface morphology of all the samples studied by the Scanning Electron Microscopy there exhibits porous structure of particles throughout the samples. The pellets of the samples are prepared for LPG sensing characteristics. The sensing is carried out at different operating temperatures (200, 225, and 250°C) with the variation of LPG concentrations (0.2, 0.4, and 0.6 vol%). The maximum sensitivity of 55.33% is observed at 250°C operating for the 0.6 vol% LPG.


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## Body

## 1. Introduction

Gas sensors are important for environmental monitoring, home safety, and chemical controlling. There is an increasing interest in the development of new materials in order to develop high performance solid-state gas sensors. Many different semiconducting oxides in bulk ceramic, thick film, and thin film forms have been studied as a sensor element for gas sensing [1, 2]. Nowadays, ferrite materials are being increasingly studied as gas sensor as their selectivity and sensitivity for some gases are comparatively better than n-type semiconducting oxides. Spinel-type oxide semiconductors with formula MFe2O4 have been reported to be sensitive materials to both oxidizing and reducing gases. Conduction in spinel ferrites occurs via transfer of charge carrier (electron or hole) between equal cations located in octahedral sites [3]. The main advantage of spinel-type ferrites compared to traditional metal oxide semiconductor based sensors is the ability of regulating the type of conductivity and the value of resistance by changing cation composition [4] stoichiometry [5] or annealing conditions [6]. However, information about the ferrite gas sensor in comparison with metal oxide gas sensor is still limited as reported by Sutka et al. [7]. Rezlescu et al. [8] investigated MFe2O4 (M = Cu, Cd, and Zn) as the sensing element to detect the acetone, ethanol, and LPG. Kamble and Mathe [9] reported the sensing response of nanocrystalline NiFe2O4 to various gases, namely, O2, LPG, ammonia, and Cl2. Multifunctional cubic spinel ferrite materials such as magnesium ferrite are nowadays being studied extensively for the magnetic, catalytic, biomedical, and gas sensing applications. Chen et al. [10] revealed that MgFe2O4 and CdFe2O4 were the most sensitive and selective to LPG and C2H2. Xiangfeng and Chenmou reported the gas-sensing properties of ferrites MFe2O4 (M = Zn, Cd, Mg, and Cu) thick films sensors for the sulfide sensing [11].Gadkari et al. [12] observed that the gas sensitivity considerably depends on the ferrite composition. The mixed ferrites with varying compositions have not been studied extensively for gas sensing. Sutka et al. [7] studied the gas sensing properties of Zn-doped p-type nickel ferrite for acetone. Tang et al. [13] investigated the selectivity of NH3 by the Co1-xNixFe2O4/multiwalled carbon nanotube nanocomposites. Recently nanosized ferrite materials have offered new opportunities for enhancing the properties and performances of gas sensors [14–17]. Jeseentharani et al. [18] reported the different spinel ferrite materials (MeFe2O4, M = Co, Cu, Mg, Ni, and Zn) nanoparticles for the humidity sensor. Kadu et al. [19] reported zinc-manganese Zn1-xMnxFe2O4 (x=0.0, 0.2, and 0.4) nonmaterial for the sensing of LPG, CH4, CO, ethanol, and their selectivity. Darshane and Mulla [20] examined the LPG sensing phenomenon of magnesium ferrite (MgFe2O4) powder and the effect of palladium doping on operating temperature. Singh et al. [21] investigated the LPG sensing at room temperature for the nanorods and mixed shaped copper ferrite (CuFe2O4). The nickel ferrite (NiFe2O4) shows the high response for LPG sensing with respect to ethanol vapor, hydrogen sulfide, ammonia, and hydrogen at 200–450°C temperatures investigated by Darshane et al. [22]. Khandekar et al. [23] discussed the cerium (Ce) doped copper ferrite (CuFe2O4) for the gas sensing of reducing gases LPG, acetone, ethanol, and ammonia. Darshane et al. [24] reported the zinc ferrite (ZnFe2O4) nanoparticles for the LPG sensing at 250°C temperature. Banerjee et al. [25] reported the spinel ferrite Zn1-xCuxFe2O4 (x=0.0, 0.25, 0.50, 0.75, 1.0) for the catalytic activity.In the present study, copper and zinc mixed nanoferrite was synthesized by the sol-gel self-combustion method described in [26] and tested to sense LPG. The effect of copper concentration is studied on the sensing response of LPG as compared to pure zinc ferrite.


## 2. Experimental

### 2.1.  Material Synthesis

Four samples with chemical compositions as ZnFe2O4, Zn0.75Cu0.25Fe2O4, Zn0.50Cu0.50Fe2O4, and Zn0.25Cu0.75Fe2O4 were prepared by sol-gel autocombustion method. The prepared samples have been referred to as F1, F2, F3, and F4, respectively, hereinafter in the text.  The samples are prepared using following analytically pure (AR) grade Zn(NO3)2·6H2O (mol. wt. 287.49 gm/mol), Cu(NO3)2·3H2O (mol. wt. 241.60 gm/mol), and Fe(NO3)3·9H2O (mol. wt. 404.00 gm/mol) as starting materials. Citric acid (AR Grade, molecular weight: 210.14 g/mol) was used as chelating agent. In order to make ferrite, these reagents in desired stoichiometric ratio were mixed with citric acid in distilled water. Cold stirring was done on magnetic stirrer for 1 hour to obtain homogeneous solution. The mixture was neutralized (pH=7) by using ammonia solution. The resulting solution was dried in an oven at 70°C for 18 hours to make the solution concentrated. Gel was obtained by constant stirring and heating the solution at 80°C temperature. The gel was subjected to calcinations at 650°C for 4.5 hours in a furnace to obtain the combusted flake form material. By grinding the flakes in mortar and pestle, powdered form of material was obtained.


### 2.2. Structural and Sensing Measurement

Structural analysis of powdered samples was carried out using X-ray diffractometer (Philips 3710, PANalytical) using Cu-Kα radiation with wavelength (λ=1.5406Å), and the surface morphology of the samples was investigated with a Scanning Electron Microscope (JEOL-JXA-8100 SEM).The 10 mm diameter size of pellet was made using polyvinyl alcohol (PVA) as binder of each sample for ferrite powder. Two-gram powder sample was uniformly mixed with 5 wt% by weight of PVA. The mixture was pressed in a die and punch arrangement using a hand press machine. The prepared pellets were sintered at 400°C for 2 hours to remove organic PVA. Highly conducting silver paste was applied with the help of n-butyl acetate to make the surface conductive on both sides of each pellet.A homemade gas sensing setup was used for LPG sensing as shown elsewhere [27].  The gas-sensing characteristics were recorded with reference to time at different operating temperatures and as a function of gas concentration. The sensing response was calculated using the given formula [27]:
(1)S(%)=[(Ra-Rg)Ra]×100,
where Ra and Rg are the resistance in the air and in the presence of tested gas, respectively.


## 2.1.  Material Synthesis

Four samples with chemical compositions as ZnFe2O4, Zn0.75Cu0.25Fe2O4, Zn0.50Cu0.50Fe2O4, and Zn0.25Cu0.75Fe2O4 were prepared by sol-gel autocombustion method. The prepared samples have been referred to as F1, F2, F3, and F4, respectively, hereinafter in the text.  The samples are prepared using following analytically pure (AR) grade Zn(NO3)2·6H2O (mol. wt. 287.49 gm/mol), Cu(NO3)2·3H2O (mol. wt. 241.60 gm/mol), and Fe(NO3)3·9H2O (mol. wt. 404.00 gm/mol) as starting materials. Citric acid (AR Grade, molecular weight: 210.14 g/mol) was used as chelating agent. In order to make ferrite, these reagents in desired stoichiometric ratio were mixed with citric acid in distilled water. Cold stirring was done on magnetic stirrer for 1 hour to obtain homogeneous solution. The mixture was neutralized (pH=7) by using ammonia solution. The resulting solution was dried in an oven at 70°C for 18 hours to make the solution concentrated. Gel was obtained by constant stirring and heating the solution at 80°C temperature. The gel was subjected to calcinations at 650°C for 4.5 hours in a furnace to obtain the combusted flake form material. By grinding the flakes in mortar and pestle, powdered form of material was obtained.


## 2.2. Structural and Sensing Measurement

Structural analysis of powdered samples was carried out using X-ray diffractometer (Philips 3710, PANalytical) using Cu-Kα radiation with wavelength (λ=1.5406Å), and the surface morphology of the samples was investigated with a Scanning Electron Microscope (JEOL-JXA-8100 SEM).The 10 mm diameter size of pellet was made using polyvinyl alcohol (PVA) as binder of each sample for ferrite powder. Two-gram powder sample was uniformly mixed with 5 wt% by weight of PVA. The mixture was pressed in a die and punch arrangement using a hand press machine. The prepared pellets were sintered at 400°C for 2 hours to remove organic PVA. Highly conducting silver paste was applied with the help of n-butyl acetate to make the surface conductive on both sides of each pellet.A homemade gas sensing setup was used for LPG sensing as shown elsewhere [27].  The gas-sensing characteristics were recorded with reference to time at different operating temperatures and as a function of gas concentration. The sensing response was calculated using the given formula [27]:
(1)S(%)=[(Ra-Rg)Ra]×100,
where Ra and Rg are the resistance in the air and in the presence of tested gas, respectively.


## 3. Results and Discussion

### 3.1. X-Ray Diffraction Analysis

The observed XRD patterns of each sample have been shown in Figure1 and found to be in good agreement with the JCPDS card 82-1042. The XRD pattern shows single peak corresponding to each diffraction angle; hence, it shows the single phase of inverse spinel zinc-copper ferrite.Figure 1
XRD spectra of the zinc-copper ferrite nanoparticles.The lattice constant (a=b=c) has been calculated from the most prominent peak using the formula [28]
(2)1d2=(h2+k2+l2)a2.
The crystallite size (D) and the lattice strain (ε) of the prepared ferrite samples have been determined using the Debye-Scherrer formula (3) [29] and the tangent formula (4) [29] as follows:
(3)D=0.9λβcosθ,(4)ε=β4tanθ,
where λ is the X-ray wavelength equal to 1.5406 Å, θ is the Bragg diffraction angle, and β (radians) is the full width at half maximum.The lattice constant, the crystallite size, and the lattice strain of the samples thus obtained are listed in Table1.  It is observed that the crystallite size of the composite ferrites increases on increasing the Cu concentration. This is due to the decrement in the densities of nucleation centers in the doped samples which results in the formation of larger crystallite size.Table 1
Structural properties of the Zn-Cu ferrites.
Zn-Cu ferrites
Positions2θ(°)
d-spacing observed (Å)
d-spacing (JCPDS) (Å)
h
k
l
TC
Crystallite size(Å)
Lattice strain(%)
a
=
b
=
c
(Å)
a-(JCPDS) (Å)
29.915
2.9860
2.9851
2
2
0
0.4792
26.495
0.0051
35.158
2.5517
2.5457
3
1
1
0.5485
28.214
0.0041
8.463
8.443
36.877
2.4366
2.4347
2
2
2
0.4687
23.086
0.0048
ZnFe2O4
42.841
2.1102
2.1108
4
0
0
0.4900
19.289
0.0049
53.142
1.7229
1.7234
4
2
2
4.0714
23.237
0.0033
56.664
1.6239
1.6248
5
1
1
0.4830
22.743
0.0032
62.21
1.4918
1.4925
4
4
0
0.4561
21.695
0.0030
29.9547
2.9821
2.9851
2
2
0
0.3350
69.665
0.1104
35.3146
2.5408
2.5457
3
1
1
0.4229
47.097
0.1392
8.427
8.443
36.9433
2.4324
2.4347
2
2
2
0.3608
60.809
0.1032
Zn0.75Cu0.25Fe2O4
42.8465
2.1100
2.1108
4
0
0
0.4949
72.291
0.0753
53.21
1.7209
1.7234
4
2
2
4.3134
90.330
0.0491
56.6971
1.6230
1.6248
5
1
1
0.5616
53.751
0.0779
62.2277
1.4914
1.4925
4
4
0
0.5064
64.460
0.0597
30.3572
2.9435
2.9851
2
2
0
0.4177
139.581
0.0544
35.6702
2.5163
2.5457
3
1
1
0.5220
70.696
0.0918
8.346
8.443
37.393
2.4042
2.4347
2
2
2
0.5294
85.270
0.0727
Zn0.50Cu0.50Fe2O4
43.3111
2.0884
2.1108
4
0
0
0.7036
108.657
0.0496
53.7481
1.7049
1.7234
4
2
2
3.5573
90.5445
0.0486
57.102
1.6125
1.6248
5
1
1
0.4084
28.731
0.1448
62.6886
1.4815
1.4925
4
4
0
0.6800
78.789
0.0485
30.1933
2.9591
2.9851
2
2
0
0.3682
69.705
0.1095
35.5827
2.5223
2.5457
3
1
1
0.4296
47.132
0.1380
8.365
8.443
37.2095
2.4156
2.4347
2
2
2
0.3699
85.225
0.0731
Zn0.25Cu0.75Fe2O4
43.1625
2.0952
2.1108
4
0
0
0.6696
118.707
0.0455
53.5478
1.7108
1.7234
4
2
2
4.1639
64.599
0.0683
57.0276
1.6144
1.6248
5
1
1
0.4622
75.369
0.0553
62.6281
1.4828
1.4925
4
4
0
0.5312
55.369
0.0691The texture coefficient has been calculated to describe the preferential orientation (hkl) using the following relation [30]:
(5)TC(hkl)=I(khl)/IO(khl)(1/N)∑NI(hkl)/IO(hkl),
where N is the number of diffraction peaks and I(hkl) and IO(hkl) are, respectively, the measured and corresponding recorded intensities according to JCPDS (082-1042) card. Texture coefficient as shown in Table 1 revealed that the crystalline nature corresponding to all the observed diffraction peaks is lower compared to the matched JCPDS card except at (422) peak. The crystallinity along this peak first increased as copper doped from F1 to F2 and then decreased to other compositions of F3 and F4 with increasing copper concentration into the zinc ferrite lattice as shown in Table 1. It is reasoned that initially copper incorporation with zinc ferrite provides the lattice energy along (422) peak growth and increases the crystallinity. As the ratio of zinc with copper is further decreased, the crystalline nature along (422) plane decreases due to increment of the substitution of zinc ion (Zn2+=0.83Å) by copper ion (Cu2+=0.70Å) in the zinc ferrite crystal structure. This phenomenon may be confirmed by observing the increase in the shift of the diffraction peak towards the higher angle due to the increased substitution of copper ion  in place of zinc ion  into the crystal lattice. This can also be explained on the basis of Vegard’s law [31]. Therefore, lattice parameter also decreases with increasing copper concentration into the host lattice.


### 3.2. SEM Analysis

Figures2(a)–2(c) show the SEM micrographs for all the prepared samples of ferrites. The SEM images show formation of the microagglomerated particles and also some voids. Porosity is located at the junctions of the agglomerates. It is clearly seen in the micrographs that the grains of the Zn-Cu ferrite are very rough, which allow adsorption of oxygen species on the sensing surface. Adsorption of oxygen species is responsible for gas sensing as described in Section 3.3.SEM micrographs of (a) Zn1.0Cu0.0Fe2O4, (b) Zn0.75Cu0.25Fe2O4, and (c) Zn0.25Cu0.75Fe2O4.
(a)
(b)
(c)


### 3.3. LPG Sensing

The pellets fabricated as detailed in Section2.2 were subjected in the static setup as reported in [27] for studying their sensitivity for LPG at different concentrationds of 0.2, 0.4, and 0.6 vol% at the different operating temperatures (200°C, 225°C, and 250°C). The resistance of the pellet before and after inserting the test gas was recorded. The sensitivity is then computed using (1). The results are shown in the Figure 3. As the copper concentration increased, the sensitivity increased due to more adsorption of oxygen species on the sensing sites. LPG sensing may be due to multiple microstructures such as nanoparticles, nanostructured hollow spheres, porous nature of spheres, and fine hillocks of ferrite materials dispersed uniformly on the surface. Oxygen adsorption plays an important role in the sensing properties of the pellets formed by nanosized ferrite material with multiple microstructures. Reactive oxygen species such as O2-, O2-, and O-  are adsorbed more on the surface of ferrite material at elevated temperature, and the amount of such chemisorbed oxygen ions depends strongly on operating temperature. The reaction kinetics is as follows [32, 33]:
(6)O2(air)⟷O2(ads),(7)O2(ads)+e-⟷O2-(ads),(8)O2-(ads)+e-⟷2O-(ads).
The oxygen species capture conduction electrons from the materials, which leads to a decrease in the electron concentration. The conversion of LPG molecule is possible at oxide surface (in presence of adsorbed oxygen ions) by dehydration as follows:
(9)CnH2n+2+2O-→H2O+CnH2n:O+e-(dehydration).
Besides, further oxidation of the formed products is also possible; it should result in sensor response growth. Thus, the process most often proceeds through the oxidizing dehydrogenation mechanism as follows:
(10)CnH2n:O+O-→CO2+H2O+e-(oxidizingdehydrogenation).
Here, CnH2n+2 represents CH4, C3H8, C4H10, and so forth, while CnH2n : O represents partially oxidized intermediates on the hollow sphere surface. Thus, during oxidation LPG liberates electrons into the conduction band, thereby decreasing the resistance of the pellet upon exposure to LPG [27].LPG response characteristics of (a) Zn1.0Cu0.0Fe2O4, (b) Zn0.75Cu0.25Fe2O4, (c) Zn0.50Cu0.50Fe2O4, and (d) Zn0.25Cu0.75Fe2O4.
(a)
(b)
(c)
(d)Figure4 shows the dynamical response of sample F4 for all the used LPG concentrations at fixed operating temperature 250°C, and it is observed that with increasing the LPG concentration, the response time and recovery time increased. This may be due to taking larger time to thermally break and react with oxygen species for higher concentration and come back to the original state for further testing. The response time recovery time of the Zn0.25Cu0.75Fe2O4 (F4) for the LPG at different concentrations 0.2, 0.4, and 0.6 vol% at operating temperatures (200°C, 225°C, and 250°C) are mention in Table 2. The maximum response found in the present study is 55.3% for 0.6 vol% LPG concentration at 250°C for F4 ferrite.Table 2
Response time and recovery time for Zn0.25Cu0.75Fe2O4sensor.
Conc. of LPG
Temp.
200°C
225°C
250°C
Response time (min.)
Recovery time (min.)
Response time (min.)
Recovery time (min.)
Response time (min.)
Recovery time (min.)
0.2% vol
3.75
2
3.75
2.5
3.5
2.5
0.4% vol
3.75
4.25
5.5
3.5
6
3
0.6% vol
4.5
5
5.5
4
6.25
3.5Figure 4
Transient response characteristics of Zn0.25Cu0.75Fe2O4 at operating   temperature of                     250°C.


## 3.1. X-Ray Diffraction Analysis

The observed XRD patterns of each sample have been shown in Figure1 and found to be in good agreement with the JCPDS card 82-1042. The XRD pattern shows single peak corresponding to each diffraction angle; hence, it shows the single phase of inverse spinel zinc-copper ferrite.Figure 1
XRD spectra of the zinc-copper ferrite nanoparticles.The lattice constant (a=b=c) has been calculated from the most prominent peak using the formula [28]
(2)1d2=(h2+k2+l2)a2.
The crystallite size (D) and the lattice strain (ε) of the prepared ferrite samples have been determined using the Debye-Scherrer formula (3) [29] and the tangent formula (4) [29] as follows:
(3)D=0.9λβcosθ,(4)ε=β4tanθ,
where λ is the X-ray wavelength equal to 1.5406 Å, θ is the Bragg diffraction angle, and β (radians) is the full width at half maximum.The lattice constant, the crystallite size, and the lattice strain of the samples thus obtained are listed in Table1.  It is observed that the crystallite size of the composite ferrites increases on increasing the Cu concentration. This is due to the decrement in the densities of nucleation centers in the doped samples which results in the formation of larger crystallite size.Table 1
Structural properties of the Zn-Cu ferrites.
Zn-Cu ferrites
Positions2θ(°)
d-spacing observed (Å)
d-spacing (JCPDS) (Å)
h
k
l
TC
Crystallite size(Å)
Lattice strain(%)
a
=
b
=
c
(Å)
a-(JCPDS) (Å)
29.915
2.9860
2.9851
2
2
0
0.4792
26.495
0.0051
35.158
2.5517
2.5457
3
1
1
0.5485
28.214
0.0041
8.463
8.443
36.877
2.4366
2.4347
2
2
2
0.4687
23.086
0.0048
ZnFe2O4
42.841
2.1102
2.1108
4
0
0
0.4900
19.289
0.0049
53.142
1.7229
1.7234
4
2
2
4.0714
23.237
0.0033
56.664
1.6239
1.6248
5
1
1
0.4830
22.743
0.0032
62.21
1.4918
1.4925
4
4
0
0.4561
21.695
0.0030
29.9547
2.9821
2.9851
2
2
0
0.3350
69.665
0.1104
35.3146
2.5408
2.5457
3
1
1
0.4229
47.097
0.1392
8.427
8.443
36.9433
2.4324
2.4347
2
2
2
0.3608
60.809
0.1032
Zn0.75Cu0.25Fe2O4
42.8465
2.1100
2.1108
4
0
0
0.4949
72.291
0.0753
53.21
1.7209
1.7234
4
2
2
4.3134
90.330
0.0491
56.6971
1.6230
1.6248
5
1
1
0.5616
53.751
0.0779
62.2277
1.4914
1.4925
4
4
0
0.5064
64.460
0.0597
30.3572
2.9435
2.9851
2
2
0
0.4177
139.581
0.0544
35.6702
2.5163
2.5457
3
1
1
0.5220
70.696
0.0918
8.346
8.443
37.393
2.4042
2.4347
2
2
2
0.5294
85.270
0.0727
Zn0.50Cu0.50Fe2O4
43.3111
2.0884
2.1108
4
0
0
0.7036
108.657
0.0496
53.7481
1.7049
1.7234
4
2
2
3.5573
90.5445
0.0486
57.102
1.6125
1.6248
5
1
1
0.4084
28.731
0.1448
62.6886
1.4815
1.4925
4
4
0
0.6800
78.789
0.0485
30.1933
2.9591
2.9851
2
2
0
0.3682
69.705
0.1095
35.5827
2.5223
2.5457
3
1
1
0.4296
47.132
0.1380
8.365
8.443
37.2095
2.4156
2.4347
2
2
2
0.3699
85.225
0.0731
Zn0.25Cu0.75Fe2O4
43.1625
2.0952
2.1108
4
0
0
0.6696
118.707
0.0455
53.5478
1.7108
1.7234
4
2
2
4.1639
64.599
0.0683
57.0276
1.6144
1.6248
5
1
1
0.4622
75.369
0.0553
62.6281
1.4828
1.4925
4
4
0
0.5312
55.369
0.0691The texture coefficient has been calculated to describe the preferential orientation (hkl) using the following relation [30]:
(5)TC(hkl)=I(khl)/IO(khl)(1/N)∑NI(hkl)/IO(hkl),
where N is the number of diffraction peaks and I(hkl) and IO(hkl) are, respectively, the measured and corresponding recorded intensities according to JCPDS (082-1042) card. Texture coefficient as shown in Table 1 revealed that the crystalline nature corresponding to all the observed diffraction peaks is lower compared to the matched JCPDS card except at (422) peak. The crystallinity along this peak first increased as copper doped from F1 to F2 and then decreased to other compositions of F3 and F4 with increasing copper concentration into the zinc ferrite lattice as shown in Table 1. It is reasoned that initially copper incorporation with zinc ferrite provides the lattice energy along (422) peak growth and increases the crystallinity. As the ratio of zinc with copper is further decreased, the crystalline nature along (422) plane decreases due to increment of the substitution of zinc ion (Zn2+=0.83Å) by copper ion (Cu2+=0.70Å) in the zinc ferrite crystal structure. This phenomenon may be confirmed by observing the increase in the shift of the diffraction peak towards the higher angle due to the increased substitution of copper ion  in place of zinc ion  into the crystal lattice. This can also be explained on the basis of Vegard’s law [31]. Therefore, lattice parameter also decreases with increasing copper concentration into the host lattice.


## 3.2. SEM Analysis

Figures2(a)–2(c) show the SEM micrographs for all the prepared samples of ferrites. The SEM images show formation of the microagglomerated particles and also some voids. Porosity is located at the junctions of the agglomerates. It is clearly seen in the micrographs that the grains of the Zn-Cu ferrite are very rough, which allow adsorption of oxygen species on the sensing surface. Adsorption of oxygen species is responsible for gas sensing as described in Section 3.3.SEM micrographs of (a) Zn1.0Cu0.0Fe2O4, (b) Zn0.75Cu0.25Fe2O4, and (c) Zn0.25Cu0.75Fe2O4.
(a)
(b)
(c)


## 3.3. LPG Sensing

The pellets fabricated as detailed in Section2.2 were subjected in the static setup as reported in [27] for studying their sensitivity for LPG at different concentrationds of 0.2, 0.4, and 0.6 vol% at the different operating temperatures (200°C, 225°C, and 250°C). The resistance of the pellet before and after inserting the test gas was recorded. The sensitivity is then computed using (1). The results are shown in the Figure 3. As the copper concentration increased, the sensitivity increased due to more adsorption of oxygen species on the sensing sites. LPG sensing may be due to multiple microstructures such as nanoparticles, nanostructured hollow spheres, porous nature of spheres, and fine hillocks of ferrite materials dispersed uniformly on the surface. Oxygen adsorption plays an important role in the sensing properties of the pellets formed by nanosized ferrite material with multiple microstructures. Reactive oxygen species such as O2-, O2-, and O-  are adsorbed more on the surface of ferrite material at elevated temperature, and the amount of such chemisorbed oxygen ions depends strongly on operating temperature. The reaction kinetics is as follows [32, 33]:
(6)O2(air)⟷O2(ads),(7)O2(ads)+e-⟷O2-(ads),(8)O2-(ads)+e-⟷2O-(ads).
The oxygen species capture conduction electrons from the materials, which leads to a decrease in the electron concentration. The conversion of LPG molecule is possible at oxide surface (in presence of adsorbed oxygen ions) by dehydration as follows:
(9)CnH2n+2+2O-→H2O+CnH2n:O+e-(dehydration).
Besides, further oxidation of the formed products is also possible; it should result in sensor response growth. Thus, the process most often proceeds through the oxidizing dehydrogenation mechanism as follows:
(10)CnH2n:O+O-→CO2+H2O+e-(oxidizingdehydrogenation).
Here, CnH2n+2 represents CH4, C3H8, C4H10, and so forth, while CnH2n : O represents partially oxidized intermediates on the hollow sphere surface. Thus, during oxidation LPG liberates electrons into the conduction band, thereby decreasing the resistance of the pellet upon exposure to LPG [27].LPG response characteristics of (a) Zn1.0Cu0.0Fe2O4, (b) Zn0.75Cu0.25Fe2O4, (c) Zn0.50Cu0.50Fe2O4, and (d) Zn0.25Cu0.75Fe2O4.
(a)
(b)
(c)
(d)Figure4 shows the dynamical response of sample F4 for all the used LPG concentrations at fixed operating temperature 250°C, and it is observed that with increasing the LPG concentration, the response time and recovery time increased. This may be due to taking larger time to thermally break and react with oxygen species for higher concentration and come back to the original state for further testing. The response time recovery time of the Zn0.25Cu0.75Fe2O4 (F4) for the LPG at different concentrations 0.2, 0.4, and 0.6 vol% at operating temperatures (200°C, 225°C, and 250°C) are mention in Table 2. The maximum response found in the present study is 55.3% for 0.6 vol% LPG concentration at 250°C for F4 ferrite.Table 2
Response time and recovery time for Zn0.25Cu0.75Fe2O4sensor.
Conc. of LPG
Temp.
200°C
225°C
250°C
Response time (min.)
Recovery time (min.)
Response time (min.)
Recovery time (min.)
Response time (min.)
Recovery time (min.)
0.2% vol
3.75
2
3.75
2.5
3.5
2.5
0.4% vol
3.75
4.25
5.5
3.5
6
3
0.6% vol
4.5
5
5.5
4
6.25
3.5Figure 4
Transient response characteristics of Zn0.25Cu0.75Fe2O4 at operating   temperature of                     250°C.


## 4. Conclusions

Mixed ferrite materialZn(1-x)CuxFe2O4 (x=0.0, 0.25, 0.50, 0.75) was successfully synthesized by sol-gel method, and structural studies proved the nanocrystalline nature of the samples. The effect of Cu concentration and temperature on the LPG sensing and maximum sensitivity is found to be 55.33% for 0.6 vol% concentration of LPG at operating temperature 250°C for F4 ferrite.



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*Source: 790359-2013-06-20.xml*