American Journal of Physics and Applications
Volume 3, Issue 3, May 2015, Pages: 97-105

Utilization of Pure Silica Extracted from Rice Husk and FTIR Structural Analysis of the Prepared Glasses

H. A. Saudi1, *, S. M. Salem2, S. S. Mohammad2, A. G. Mostafa2, M. Y. Hassaan2

1Department of Physics, Faculty of Science, Al-Azhar University, Nasr City, Cairo, Egypt

2Department of Physics, Faculty of Science (Girls' Branch), Al-Azhar University, Nasr City, Cairo, Egypt

Email address:

(H. A. Saudi)

To cite this article:

H. A. Saudi, S. M. Salem, S. S. Mohammad, A. G. Mostafa, M. Y. Hassaan. Utilization of Pure Silica Extracted from Rice Husk and FTIR Structural Analysis of the Prepared Glasses. American Journal of Physics and Applications. Vol. 3, No. 3, 2015, pp. 97-105. doi: 10.11648/j.ajpa.20150303.16


Abstract: Egyptian rice husk was subjected to different chemical and thermal treatment methods, aiming to extract high pure silica. Three samples (S1, S2 and S3) were prepared applying three different chemical treatment methods. Two sets of the obtained samples were prepared, where the first set was calcinated at 600oC and the other set was calcinated at 750 oC by slow heating (starting at RT and ending at the desired calcinations temperature for 2 h).XRF was applied to identify the chemical composition and purity of the extracted silica, while XRD was applied to confirm the amorphous nature and the presence of some induced carbon black in the obtained silica. It was found that S3 slowly heated at 750 oC presents the highest silica content (98.6 %). Such sample was fed directly to the calcinations furnace at 750 oC (sudden heating for comparison) where it presents only 90.6% silica, and 3.74 % residual carbon black. However, the extracted silica from sample S3 was used to prepare glasses obeying the composition (75-x) mol% RH-silica, x mol% Bi2O3, 25 mol% Na2O, (where 0 ≤ x ≤ 20).FTIR spectroscopic analysis was applied to investigate the internal structure of the prepared glasses, where the glass networks were found to contain mainly SiO4, BiO3 and BiO6 structural groups, as well as some bridging and non-bridging oxygen anions. Also, some O-H and H-O-H groups were also detected which may be due to the used KBr disk technique.

Keywords: Silica from Rice Husk, Silicate Glasses, Bi-Na-Silicate Glass, XRD, XRF, Infrared Spectroscopy


1. Introduction

Rice is a primary source of food for billions of people and it covers about 1% of the earth’s surface. It ranks as the second to wheat in terms of area and production. Globally, approximately 600 million tones rice are produced each year, and for every 1000 kg of paddy milled, about 220 kg of rice husk (RH) is produced (about 22%). RH is therefore an agricultural residue, and it is either burnt or dumped as waste [1,2]. Little of the RH is converted into useful end products such as feedstock [3], adsorbent [4], etc., while the most has burnt openly, causing environmental and health problems especially in poor and developing countries. Therefore, it is very important to find other pathways to utilize rice husk.

It was discovered as early as 1938 that silica can be extracted from RH as sodium silicate by using different extraction methods [5,6]. Its potential recovery had been realized since 1984 [7], where RH can be considered a good source of silica. It was found that silica in RH undergoes structural transformations depending on the conditions of combustion (time and temperature). Accordingly the extracted silica has different properties and it is important to treat RH by the correct specification for particular end use (See Fig. (1))[8]. Even though the use of silica extracted from RH is still limited.

It was found that, RH contains silica in the range of 20 – 25 wt %, in an amorphous form like silica gel [9-10]. Thermal degradation and pyrolysis of RH followed by combustion of the char result in highly porous and amorphous silica with a varying percentage of unburned carbon [11].

According to Kapur [11], when RH is burnt under controlled conditions, the resulting ash is considered, the cheapest bulk source of highly reactive silica. Furthermore, since the ash is obtained as a fine powder, it does not require further grinding [12] and thus, making it the most economical source of Nano-scale silica [13].

As reviewed also by Real et al [9], a number of published literatures [14,15] had concluded that RH are an excellent source of high-grade amorphous silica. The silica obtained from RH ash is a good material for synthesis of very pure silicon [16-18], silicon nitride [19], silicon carbide [20,21] and magnesium silicide [22]. In addition, the obtained silica has been claimed [17,18 and 23] to be an excellent source of very pure silicon, useful for manufacturing solar cells and for photo-voltaic power generation as well as various types of semiconductors [24,25].

Closer to home, rice production in Egypt is concentrated in the agricultural space around Nile-delta where nearly 8 million tons of rice are produced annually, leading to the generation of large volumes of rice husk as agricultural wastes. Uncontrolled burning is often considered the most cost-effective disposal method for such by-product. This seasonal and highly localized massive burning generates excessive air pollution that lowers air quality in the neighboring of Cairo, which has become a serious health concern for citizens and authorities.

However, in this article, a trial will be carried out aiming to enrich the silica produced from Egyptian RH via chemical and thermal methods. Then they obtained silica will be used to prepare some silicate glasses and the obtained samples will be characterized applying infrared analysis.

Fig. (1). Various utilizations of the RH silica. [8]

2. Experimental Procedure

Enrichment of silica:

The RH was provided from Banha, Al-Qalyobia, Egypt. Such RH was firstly combusted in open air to obtain non-acid leached and thermally untreated sample of RHA, only for comparison.

On the other hand, RH was subjected to acid leaching in three different ways to obtain three different samples applying different chemical treatment methods. The aim of this step is to improve the purity and the white color of the extracted silica [26-31].

The first sample (S1):

A 100 g sample of RH was fed into 3N HCl solution in de-ionized water, and boiled for 1.5 h. After thorough washing with de-ionized water, the residue was filtered and finally dried in an oven at 100 oC for 1 h.

The second sample (S2):

Another 100 g sample of RH was treated firstly by feeding into a solution consists of (265 ml ethyl alcohol and 735 ml de-ionized water) and boiled for 1.5h. After thorough washing with de-ionized water, the residue was filtered and dried in an oven at 100oC for 1 h. This sample was then fed into 3N HCl solution in de-ionized water, and boiled for 1.5 h. After thorough washing with de-ionized water, the residue was filtered and finally dried in an oven at 1000C for 1 h.

The third sample (S3):

Similarly, another 100 g sample of RH was treated firstly by feeding into a solution consists of (265 ml ethyl alcohol and 735 ml tap water) and boiled for 1.5h. After thorough washing with tap water, the residue was filtered and dried in an oven at 1000C for 1 h, and then this sample was fed into 3N HCl solution in a tap water, and boiled for 1.5h. After thorough washing with tap water, the residue was filtered and finally dried in an oven at 1000C for 1 h.

Two sets of the above obtained samples (S1, S2 and S3) were prepared in a way that, twenty gram of each sample were placed in porcelain crucibles and they were then introduced into an electrically heated muffle furnace where calcinations were conducted at 600 and 750 ºC for each set respectively. In case of slow heating, the samples were loaded into the furnace at room temperature, and they were held at the calcinations temperature (600 or 750 oC) for 2 h.

In case of sudden heating and in order to compare sudden and slow heating, only twenty g of the sample number three (S3) was fed in a porcelain crucible and was loaded into the furnace directly at 750 ºC for 2 h.

The extracted silica of all chemical and thermal procedures were then analyzed using XRF apparatus model (PANalytical Axios advanced, Netherlands).

In addition, XRD was also used to examine the amorphous nature of the extracted silica as well as the presences of some unburned carbon. XRD patterns were obtained by using Rigaku RINT 2100 apparatus, in the range of 2θ from 10° to 80° with an intervals and scanning rate of 0.02° and 5° min-1, respectively. The apparatus was outfitted with Cu Kα radiation (λ = 0.1541 nm) with tube voltage and current equal 50 kV and 300 mA respectively. The detected crystalline phases were identified with the reference data compiled by the International Center for Diffraction Data (ICDD).

For preparing the glass samples an appropriate amount of Na2O, Bi2O3 and SiO2 (obtained from S3) were weighted using an electronic balance having accuracy of 0.0001 g. The batches were mixed in compositions [x % Bi2O3. (75 - x)% RH-SiO2. 25% Na2O (x = 0, 5, 10, 15 and 20 wt.%). The obtained mixed powders were melted in porcelain crucibles at 1300 oC for 2 h using an electric furnace, and they were stirred several times during melting in order to obtain homogeneous glass samples. Then the melts were quenched in air between two copper plates. Just, after sitting the solid glasses were directly transferred to the annealing furnace at 350 oC and the furnace was turned off and was left to cool to room temperature over-night.

The IR absorption spectra of the prepared glasses were recorded in the wave number range from 4000 to 400 cm-1 by using a Fourier transform computerized IR spectrometer type (JASCOo FT/IR-430, Japan). The glasses were investigated in the form of fine powders which were mixed with pulverized KBr in the ratio (3:200 mg glass to KBr, respectively). The weighted mixture was then pressed to produce clear homogeneous discs. The IR absorption spectra were measured immediately after preparing the desired discs.

3. Results of Enrichment of Silica

Egyptian RH was treated chemically and thermally in various ways in order to elevate both the concentration and purity of the extracted silica. The XRF results of the chemically treated samples (S1, S2 and S3) slowly heated at 600 or 750 oC for calcinations, are all exhibited in Table 1, in addition to the XRF analysis of the RH burned openly for comparison.

Table (1). XRF analysis in wt. % for the chemically and thermally treated samples (S1, S2 & S3) slowly heated at 600 & 750 oC and RH burned openly.

Constituents (Weight %) SiO2 (total purity) K2O CaO Fe2O3 MnO2 TiO2 CuO NiO Cr2O3 Cl SO3 Carbon residue
  RH 61.4 8.78 6.03 3.51 1.10 0.31 0.18 0.11 0.08 8.9 2.0 7.6
Slow heating 600 oC S1 89.9 2.85 2.03 2.5 1.08 0.23 0.12 0.09 0.06 --- --- 2.14
S2 92.9 1.05 1.97 1.42 0.62 0.10 0.08 0.04 0.021 --- --- 1.80
S3 94.6 0.88 1.89 0.97 0.12 0.23 0.10 0.09 0.08 --- --- 1.04
750 oC S1 91.3 1.03 2.71 3.04 0.16 0.10 0.09 0.011 0.035 --- --- 1.52
S2 96.5 0.886 1.54 0.713 0.102 0.087 0.057 0.015 0.019 --- --- 0.08
S3 98.6 0.23 0.688 0.28 0.042 0.08 0.05 0.01 0.011 --- --- ------

Inspecting the obtained values, it can be observed that sample S3 slowly heated up to 750 oC, calcinated for 2 h, possess the highest amount of silica (98.6%) and the lowest amount of K2O content, in comparison with all other samples as well as that of the RH burned openly which possess only 61.4% of silica, 7.6% carbon black and 8.78 K2O.

On the other hand and in order to show the effect of sudden heating, the S3 sample after chemically treated was subjected to sudden heating at 750 oC, and the obtained results are exhibited in Table (2) together with the obtained values of the same sample when slowly heated, for comparison. From the exhibited data, it can be seen that, S3 slowly heated is the best sample, since it contains the highest silica content and the lowest impurities, especially K2O, with on unburned carbon black.

Table (2). XRF analysis in wt. % of S3 sample slowly and suddenly heated at 750 oC..

Constituents (Weight %) SiO2 (total purity) K2O CaO Fe2O3 MnO2 TiO2 CuO NiO Cr2O3 Cl SO3 Carbon residue
slow heating S3 98.6 0.23 0.688 0.28 0.042 0.08 0.05 0.01 0.011 --- --- ------
sudden heating S3 90.6 2.56 2.48 0.28 0.051 0.07 0.08 0.05 0.09 --- --- 3.74

The XRF data of all samples were then translated and exhibited in a histogram, where the comparison of the extracted silica from all samples becomes so easy. Such histogram can be seen in Fig. 2.

On the other hand, the untreated RH burned openly, that contains only 61.4% silica, appeared black in color indicating the presence of some unburned carbon, while all the chemically treated samples slowly heated at 750 oC appeared milky white.

It can be observed that, the chemical treatment leads to higher SiO2 contents and decreases also the amount of alkali contaminants such as K2O, where the presence of potassium reduces the melting temperature of silica, but it serves as an accelerator for its crystallization during combustion. In addition, it may increase the alkali-aggregation reaction potential of the mixtures incorporating some black unburned carbon [26-30].

The substantial decrease in the K2O content (observed in Table 1 for acid leached RH is expected to decrease the crystallization probability of SiO2 during vigorous and prolonged combustions. But this lower K2O content will leads consequently to higher melting temperature of SiO2. That is, surface melting of the silicate skeleton is substantially reduced for the acid leached samples.

Fig. (2). The amounts of the extracted silica from all the studied samples subjected to different chemical and thermal treatment methods.

Fig. (3). XRD patterns of the extracted silica due to S1, S2 and S3 obtained by slow heating at 750 0C.

Fig. (4). XRD patterns of the extracted silica obtained from S3 when slowly or suddenly heated at 750 ºC.

The brightness increased with increasing the temperature of calcinations, and rapid or sudden heating resulted in the formation of some fixed black carbon. At lower temperature (600 ºC), S1, S2 and S3 yielded charred RH. Increasing the calcinations temperature the whiteness increased. At 750 ºC, the acid treated RH (S1, S2 and S3) yielded bright white silica in comparison to other samples.

From another point of view, XRD technique has been applied to study the extracted silica whether it has crystalline or amorphous form as well as the presence of carbon black in some samples. However Fig. 3 shows the XRD patterns of S1, S2 and S3, where, all patterns show broad hump around 2θ is about 22. These broad humps indicated that all the extracted silica showed an amorphous nature. There is no difference in XRD patterns of the S2 and S3 slowly heated at 750 oC. But the XRD pattern of S1 show a slight peak around 2θ = 26, indicating the presence of some unburned carbon, while both the other two patterns - due to S2 and S3 - appeared free of this peak indicating that the chemical and thermal treatments act to yield pure amorphous silica except S1 which exhibits amorphous silica but not of high purity of all carbon black. These results were found in complete agreement with those obtained from XRF analysis.

It was observed generally that the level of impurities decreased considerably after acid treatment. The highest quantity of carbon residue was observed in the sample that suddenly heated at 750 oC only. This was clearly observed in Fig. 4 that presents the XRD patterns of S3 when slowly and suddenly heated at 750 oC.

4. Discussion of Silica Enrichment

When RH is subjected to acid treatment, cellulose which forms the main body of RH is reduced and carbohydrates are blackened due to the removal of oxygen. The proteins in the RH are decomposed into amino acids and the cellulose of larger molecular weight is leached out as smaller molecular weight compounds, [31]. From the chemical analysis obtained from XRF and presented in Table 1, it can be notice that the impurities in RH are substantially removed by acid treatment. The major impurity in RH is potassium oxide and it act to accelerate the carbon fixation through RH silica. On the other hand, potassium oxide which dissociates upon heating at 620 ºC forms elemental potassium whose melting point is 337 ºC. However, it causes surface melting and accelerates the crystallization of amorphous silica to form cristobalite [32]. Hanafi et al [33] and Ibrahim et al [34] have studied the surface properties and crystal structure of RH silica. Crystallization was observed in the samples fired at and above 800ºC. Krishnarao et al [35] reported that a change in the morphology of RH silica takes place after crystallization at 1200 ºC.

When RH is heated from room temperature, the organic materials like cellulose, lignin… etc., decomposed into carbon. The rise in temperature causes oxidation of carbon. Before the removal of all carbon, if the temperature is raised to the decomposition temperature of K2O where surface melting of the ash occur, the carbon will get entrapped in the melt. If RH is slowly heated, the carbon could oxidize before it reaches the dissociation temperature of K2O. During sudden heating of the RH silica where the samples were suddenly introduced into the furnace maintained at higher temperature. This causes simultaneous oxidation of carbon formed from decomposition of organic substances and dissociation of K2O followed by surface melting. Once carbon is entrapped in the potassium rich melt, it cannot be oxidized as it is not in direct contact with air. As the temperature of calcination increases, the tendency of carbon fixation increases during sudden heating. Therefore, a large amount of black particles were observed in the suddenly heated RH silica at 750 ºC.

During slow heating the carbon formation and its oxidation occurs before the dissociation of K2O and surface melting. So the tendency of silica for retention of carbon is eliminated. But the silica formed from untreated RH is not so bright (white) as silica formed from treated RH. This is due to the removal of impurities including potassium by acid treatment.

5. Results and Discussion of Infrared Analysis

According to the above studies and from the trails carried out to extract silica from RH, it was found that, S3 slowly heated at 750 oC is the best sample that yield an amount of silica equals 98.6%. Such silica will be designated in this article as RH-silica. Therefore the extracted silica from such sample was used to prepare glasses having the molecular composition [x % Bi2O3 (75 – x) % SiO2 25% Na2O (x = 0, 5, 10, 15 and 20 wt. %). The internal structure of the prepared samples was thoroughly investigated by using IR spectroscopy and Fig. 5 exhibits the obtained IR spectra in the range from 400 to 4000 cm-1.

Inspecting the as measured IR spectra, it can be observed easily that the range of interest is only in between 400 to 1600 cm-1. Therefore such range was undergoing to the de-convolution technique (program) in order to inspect the functional groups in the obtained glass networks as really as possible. However Fig. 6 shows the de-convoluted IR absorption spectrum of sample no. (4) which contains 15 mol% Bi2O3, as representative figure. The analyzed bands of all samples are summarized in Table 3.

Fig. (5). The as measured IR spectra of all samples.

Table (3). The obtained IR frequencies for all glasses.

Peaks 1 2 3 4 5 6 7 8 9
sample 1 463 498 769 887 940 1027 1120 1181 1463
sample 2 456 507 738 872 919 1021 1114 1198 1465
sample 3 463 517 750 869 974 1025 1106 1208 1471
sample 4 466 518 751 838 923 1033 1149 1285 1471
sample 5 450 489 737 847 949 1042 1129 1213 1475

Fig. (6). The de-convoluted IR absorption spectrum of sample no. (4), as a representative figure. The effect of substituting a conventional glass former (SiO2) by an unconventional glass former (Bi2O3) on the structural properties of bismuth RH-silicate glasses was investigated by recording their Fourier Transform infrared (FTIR) spectra.

The positions of the absorption bands in the mid near infrared spectra of the present glasses are slightly different from the spectra usually obtained for the traditional silicate glasses and crystal [41] due to the presence of bismuth as heavy metal cations.

It was found that there appeared many IR absorption bands and these bands can be attributed to the following structural groups:

1.         The band appeared in the range from 450 to 466 cm-1 can be assigned to the vibration of silicon–oxygen bonds in SiO4 tetrahedral [36-39].

2.         The band appeared in the range from 489 to 518 cm-1 is assigned to Si-O-Si bending vibration [40-41]. It has been predicted by various authors [42-43] that this band may be related to Bi–O bond vibrations in BiO3 and BiO6 octahedra. The observed shift to higher wave number (518 cm-1) is due to the increase of the degree of the distortion by increasing (Bi2O3/SiO2) ratio. Dimitriev et al have also attributed the shift of the band appeared around 482–520 cm-1 to the vibration in the local symmetry of highly distorted BiO6 polyhedra and the same was also observed in IR spectra of other bismuth based glasses [44].

3.         The band appeared in the range from 737 to 769 cm-1 can be assigned to Si-O-Si and O-Si-O bending modes [41].

4.         The band appeared in the range from 838 to 887 cm-1 can be assigned to Si-O-Si symmetrical stretching vibration of bridging oxygen atoms between SiO4 tetrahedra [42-43]. This band appeared in the un-doped glass and its intensity showed gradual decreases as Bi2O3 was gradually increased accompanied by a shift to lower wavelength at 838 cm-1which may be due to the vibration of Bi-O linkages in BiO6 octahedral [42- 43].

5.         The band appeared in the range from 919 to 949 cm-1 is assigned to Si-O- stretching vibration of non-bridging oxygen atoms [41].

6.         The band appeared in the range from 1021 to 1042 cm−1 is due to SiO4 group bonded to two ions and the band at 1100–1150 cm−1 is associated with SiO4 tetrahedra bonded to four bridging oxygen ions [48, 49].

7.         The band appeared in the range from 1181 to 1285 cm−1 is assigned to Si-O-Si anti-asymmetric stretching vibration of bridging oxygen atoms within SiO4 tetrahedra [41].

8.         The band appeared in the range from 1463 to 1475 cm-1 can be assigned to the bending vibrations of O-H [49].

9.         The band appeared in the range from 1560 to 1631 cm-1 can be assigned to molecular water or hydroxyl-related bonds [50].

10.      All the as measured spectra showed a water bands in the range from 3412 to 4000 cm-1, and around 2900 cm-1. These bands can be attributed to the stretching vibration of –OH groups. Another band appeared around 1600 cm-1 which may be due to the -OH bending vibration mode and some absorbed water. The presence of these bands may be due the used KBr technique [49- 51].

From the IR structural analysis, it can be observed that there are no any band appeared due to other cations except Si and Bi. This main that the impurity level is very low. It can be stated also that Si cations form the main glass former skeleton of the glass networks, while little Bi cations participate also as glass former forming BiO3 gropes. The rest of Bi cations act as modifier in the networks of the studied glasses forming BiO6. That is, as BiO3 was introduced into the glass networks at the expense of RH-silica, some Bi cations will forced to occupy the glass former positions.

6. Conclusions

According to the trials carried out to extract high pure concentrated silica and the IR structural analysis of the prepared glasses, the following conclusions can be drawn:

The maximum silica content of all the chemically treated samples (S1, S2 and S3) slowly heated at 600 oC was presented by S3, which was found to contain 94.06%. All these samples posses comparable amount of carbon black decreased on going from S1 to S3.

On the other hand, the maximum silica content of all samples slowly heated at 750 oC was also presented by S3, but it was found to be 98.6 %. The black carbon appeared only in S1.

All the extracted silica of all samples (with different chemical and thermal treatment) showed an amorphous nature.

On trying to show the effect of sudden heating on S3 at 750 oC, it can be concluded that sudden heating decreases the extracted silica content and act to induce a comparable amount of carbon black through the extracted silica.

The extracted RH-silica can be successfully used to prepare silicate glasses with different additives used for various applications.

The FTIR analysis showed the presence of different structural groups depends on Si4+ as former cations and the added heavy metal Bi3+ cations.

The low impurity level and the high concentration of the RH-silica showed that RH, which is an agricultural waste, can be converted into a valuable product which has so many industrial and domestic applications.

This study showed that rice husk can be used in many economic and technological applications, especially in the rice-producing countries like Egypt to extract highly pure silica which has various industrial and domestic applications and reduce the environmental impact of uncontrolled burning of the rice by-product.

References

  1. J. James and M. S. Rao, J. Am. Ceram. Soc. Bull, 65 (1986) 1177.
  2. F. Adam, K. Kandasamy and S. Balakrishnan, J. Colloid. Interface Sci., 304 (2006) 137.
  3. S. Maiti, S. Dey, S. Purakayastha and B. Ghosh, J. Bio-resource Technology, 97 (2006) 2065.
  4. T. J. Hyun, K. P. Yoon, S. K. Young, Y. L. Ji and M. Bhagiyalakshmi, J. Greenh. Gas Control, 3 (2009) 545.
  5. R. V. Krishnarao, J. Subrahmanyam and T. Jagadish Kumar, European Ceramic Society, 21 (2001) 99.
  6. S. Chandrasekhar, S. Satyanarayana, K. G. Pramada, P. N. Raghavan and T. N. Gupta, J. Materials Science, 38 (2003) 3159.
  7. A. Kaupp, J. Materials Sci., 18 (1984) 303.
  8. J. Paya, J. Monzo, MV. Borrachero, A. Mellado and LM. Ordonez, J. Chem. Concr. Res, 31 (2001) 227.
  9. C. Real, M. Alcala and J. M. Criado, J. Am. Ceram. Soc., 79(8) (1996) 2012.
  10. M. Patel, A. Karera and P. Prasanna, J. Materials Sci., 22 (1987) 2457.
  11. P. C. Kapur, J. Power Technology, 44 (1985) 63.
  12. J. James and M. S. Rao, J. Thermochimica Acta, 97 (1986) 329.
  13. Liou T. Horng, J. Materials Science and Engineering, 364 (2004) 313.
  14. P. Mishra, A. Chakraverty and H.D. Banerjee, J. Mater. Sci, 20 (1985) 4387.
  15. A. Chakraverty, P. Mishra and H.D. Banerjee, J. Mater. Sci, 23 (1988) 21.
  16. J. A. Amick, J. V. Milewski and F. J. Wright, U. S. Patent No. 4,214(1980) 920.
  17. J. A. Amick, J. Electrochem. Soc., 129 (1982) 864.
  18. L. H. Hunt, J. P. Dismukes, J. A. Amick, A. Schee, and K. Larsen, J. Electrochem. Soc., 131(7) (1984) 1683.
  19. N. Yalçin, and V. Sevinç, J. Ceramics International, 27 (2001) 219.
  20. R. V. Krishnarao, and J. Subrahmanyam, J. Ceramics International, 22 (1995) 489.
  21. P. Gorthy, and M. G. Pudukottah, J. American Ceramic Society, 82(6) (1999) 1393.
  22. T. B. Ghosh, K. C. Nandi, H. N. Acharya and D. Mukherjee, J. Material Letters, 11 (1991) 6.
  23. A. Chakraverty, P. Mishra and H. D. Banerjee, J. Thermochimica Acta, 94 (1985) 267.
  24. S. B. Hanna, L. M. Farag and N. A. L. Mansour, J. Thermochimica Acta, 81(1984) 77.
  25. V. I. E. Ajiwe, C. E. Okeke and F. C. Akigwe, J. Bio-resource Technology, 73 (2000) 37.
  26. NP. Hasparyk, PJM. Monteiro and H. Carasek, J. ACI Mater., 97 (2000) 486.
  27. A. John, S. Alexanda and A. Larry, J. International Center for Diffraction Data, 44 (2001) 368.
  28. B. M. Jenkins, L. L. Baxter, Jr. Miles and T. R. Miles, J. Fuel Processing Technology, 54 (1998) 17.
  29. J. D. Jones, J. Can. Metals, 16 (1953) 22.
  30. L. Barbieri, I. Lancellotti, T. Manfredini, I. Queralt, J.M. Rincon and M. Romero, J. Fuel, 78(1999) 271.
  31. M. Tanaka, K. Niwano and Y. Kitano, UK Patent GB2 168, (18 June 1986) 333 A.
  32. Y. Nakata, M. Suzuki and T. Okutami. J. Thermochimica Acta, 97 (1989) 842.
  33. S. Hanafi, S. A. Abo-El-Enein, D. M. Ibrahim, and S. A. El-Hemaly, J. Thermochimica Acta, 37 (1980) 137.
  34. D. M. Ibrahim, S. A. El-Hemaly and F. M. Abdel Kerim, J. Thermochimica Acta, 37 (1980) 307.
  35. R. V. Krishnarao, J. Mater. Sci., Lett., 12 (1993) 1268.
  36. A. Witkowska, J. Rybicki and A. D. Cicco, J. Alloys Compd., 401 (2005) 135.
  37. A. DTTA, A. K. Giri and D. Chakravorty, J. Condens. Matter, 4(1992) 1783.
  38. A. Burns, H. P. Brack and W. M. J. Risen, J. Non-Cryst. Solids, 131 (1991) 994.
  39. R. S. Husung and R. H. Doremus, J. Mater. Res, 5 (1990) 2209.
  40. J. Wong and C. A. Angell,J. Mater. Sci.,9 (1967) 409.
  41. K. M. ElBadry, F. A. Moustaffa, M. A. Azooz and F. H. ElBatal, Indian J. Pure Appl. Phys., 38 (2000) 41.
  42. L. Baia, R. Stefan, W. Kiefer, J. Popp and S. Simon, J. Non-Cryst. Solids, 303 (2002) 379.
  43. F. H. ElBatal, J. Nucl. Inst. Meth. Phys. Res., 254 (2007) 243.
  44. S. Bale, M. Purnima, Ch. Srinivasu and S. Rahman, J. Alloys Compd., 457 (2008) 545.
  45. F. H. ElBatal, M. A. Azooz and F. M. Ezz ElDin, J. Phys. Chem. Glasses, 43 (5) (2002) 260.
  46. F.H. ElBatal, Egyptian J. Chem., 47 (1) (2004) 101.
  47. A. A. Akatov, B. S. Nikonov, B. I. Omelyanenko, S. V. Stefanovsky and J. C. Marra, J. Phys. Chem. Glasses, 35 (2009) 245.
  48. H. Moor and P. W. McMillan, J. Soc. Glass Technol., 40 (1956) 97.
  49. S. A. MacDonald, C. R. Schardt, D. J. Masiello and J. H. Simmons, J. Non-Cryst. Solids, 275 (2000) 72.
  50. M. S. Aziz, F. Abdel-Wahab, A. G. Mostafa and E. M. El Agwany, J. Mater. Chem. Phys., 91 (2005) 532.
  51. J. T. Quan and C. F. Adams, J. Phys. Chem., 70 (1966) 331.

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