# Synthesis, Characterization, and Use of Novel Bimetal Oxide Catalyst for Photoassisted Degradation of Malachite Green Dye

Authors: K. L. Ameta; Neema Papnai; Rakshit Ameta
Journal: Journal of Materials
 (2014)

---

## Abstract

This work reports a simple, novel, and cost effective synthesis of nanobimetal oxide catalyst using cerium and cadmium nitrates as metal precursors. The cerium-cadmium oxide nanophotocatalyst was synthesized by coprecipitation method and characterized by X-ray powder diffraction method to analyze the particle size. XRD study reveals a high degree of crystallinity and 28.43 nm particle size. The photocatalytic efficiency of the synthesized nanobimetal catalyst was examined by using it for the photocatalytic degradation of malachite green dye. Experiments were conducted to study the effect of various parameters, such as the pH of the dye solution, concentration of dye, amount of catalyst, and light intensity on the rate of dye degradation. The progress of the dye degradation was monitored spectrophotometrically by taking the optical density of the dye solution at regular intervals. Experimental results indicate that the dye degrades best at pH 8.0 with light intensity 600 Wm−2 and catalyst loading 0.03 g/50 mL of dye solution. The rate constant for the reaction was 7.67 × 10−4 s−1.


---

## Body

## 1. Introduction

Clean water is a vital commodity, as it is a prerequisite for life. An adequate water supply in both quantity and quality is essential to human existence [1]. But one of the most serious threats related to water is the accumulation of nonbiodegradable and toxic compounds in the ecosystem leading to the degradation of the quality of water [2, 3]. Due to the nature of various chemical processing of textiles, large volume of wastewater with numerous pollutants is discharged [4, 5]. Photocatalysis has been considered and proved as a cost effective alternate for the purification of dye-containing wastewater [6–10]. Studies have demonstrated that photocatalysis can be used to destroy dye compounds using semiconductor photocatalysts under light irradiation. The photocatalysts are able to photosensitize the complete mineralization of a wide range of compounds, like dyes, phenols, and pharmaceutical drugs, without producing harmful by-products at near room temperature and pressure [11–13].Lately, there have been extensive studies done by researchers around the globe on many photocatalytic systems (UV/semiconductors) since they have been found to be very effective in degrading various organic dyes. Many catalysts like TiO2, ZnO, ZrO2, WO3, Fe2O3, CeO2, CdS, and ZnS have been attempted for the photocatalytic degradation of a wide variety of environmental contaminants [14–21]. Studies have also demonstrated that bimetal catalyst has advantage of low metal leaching during the catalytic reaction, avoiding secondary metal contamination to the treated wastewater [22].With this view, the present study was planned to investigate the degradation of malachite green dye with photocatalytic system using bimetal oxide. For this, a novel bimetal nanophotocatalyst, that is, cerium-cadmium oxide, was synthesized and the effect of different parameters such as pH of the dye solution, concentration of dye, the amount of catalyst, and intensity of visible light on the rate of dye degradation with cerium-cadmium oxide were assessed. Since sunlight is an abundantly available natural energy source, its energy can be conveniently exploited for the irradiation of semiconductor material. The kinetics of the absorption process was evaluated to study the absorption mechanism of dye molecule.


## 2. Experimental

### 2.1. Synthesis of Bimetal Cerium-Cadmium Oxide

The synthesis of novel cerium-cadmium oxide was achieved by coprecipitation method. The mixed oxide was prepared by adding an aqueous solution of 1 M NaOH dropwise to the aqueous solution of 0.1 M of both Ce(NO3)3·6H2O and Cd(NO3)2·4H2O with concurrent stirring. The pH of the mixed solution was adjusted at different pH in the alkaline range, but at pH 8, complete precipitation was observed so the pH 8 was maintained. After 4 hours of continuous stirring, the precipitate was filtered and repeatedly washed with deionized water. The residue was dried in an oven at 110°C overnight and then grounded in acetone with mortar and pestle. The powder received was then calcined at 500°C for 4 hours under static air in a muffle furnace.


### 2.2. Characterization of the Synthesized Bimetal Cerium-Cadmium Oxide

X-ray powder diffraction study was performed to establish the phase purity and crystalline nature of the synthesized bimetal oxide by X-ray diffractometer. The particle size of the synthesized photocatalyst was determined using the Scherrer equation.


### 2.3. Photocatalytic Degradation of Dye

A stock solution of malachite green (structure is shown in Figure1) of 1.0 × 10−3M was prepared by dissolving 0.365 g of malachite green in 1000 mL of double distilled water. The absorption maximum of the dye was determined with the help of a spectrophotometer (Systronics Model 106).Figure 1
Chemical structure of Malachite green.Photocatalytic degradation of malachite green dye was studied by exposing the dye solution to light in the presence of synthesized nanobimetal oxide. For irradiation purpose, 200 W tungsten lamp (Philips) was used. The intensity of light was measured by solar power meter (TENMARS model TM 207). A water filter was used to cut off thermal radiation. The pH of the solution was measured by a digital pH meter (Systronics Model 324) and the desired pH was adjusted by the addition of 0.1 N sodium hydroxide and 0.1 N sulphuric acid solutions. The progress of photocatalytic degradation of the dye was monitored by withdrawing definite quantity of the reaction mixture at regular time intervals and measuring the absorbance by the UV-VIS spectrophotometer at a maximum wavelength(
λ
max
⁡
=
620
nm
). Additional experiments were conducted to verify that the observed reaction was indeed photocatalysis. For this, the dye solution was irradiated with solar/UV light without adding photocatalyst and with photocatalyst in the absence of solar/UV light.


## 2.1. Synthesis of Bimetal Cerium-Cadmium Oxide

The synthesis of novel cerium-cadmium oxide was achieved by coprecipitation method. The mixed oxide was prepared by adding an aqueous solution of 1 M NaOH dropwise to the aqueous solution of 0.1 M of both Ce(NO3)3·6H2O and Cd(NO3)2·4H2O with concurrent stirring. The pH of the mixed solution was adjusted at different pH in the alkaline range, but at pH 8, complete precipitation was observed so the pH 8 was maintained. After 4 hours of continuous stirring, the precipitate was filtered and repeatedly washed with deionized water. The residue was dried in an oven at 110°C overnight and then grounded in acetone with mortar and pestle. The powder received was then calcined at 500°C for 4 hours under static air in a muffle furnace.


## 2.2. Characterization of the Synthesized Bimetal Cerium-Cadmium Oxide

X-ray powder diffraction study was performed to establish the phase purity and crystalline nature of the synthesized bimetal oxide by X-ray diffractometer. The particle size of the synthesized photocatalyst was determined using the Scherrer equation.


## 2.3. Photocatalytic Degradation of Dye

A stock solution of malachite green (structure is shown in Figure1) of 1.0 × 10−3M was prepared by dissolving 0.365 g of malachite green in 1000 mL of double distilled water. The absorption maximum of the dye was determined with the help of a spectrophotometer (Systronics Model 106).Figure 1
Chemical structure of Malachite green.Photocatalytic degradation of malachite green dye was studied by exposing the dye solution to light in the presence of synthesized nanobimetal oxide. For irradiation purpose, 200 W tungsten lamp (Philips) was used. The intensity of light was measured by solar power meter (TENMARS model TM 207). A water filter was used to cut off thermal radiation. The pH of the solution was measured by a digital pH meter (Systronics Model 324) and the desired pH was adjusted by the addition of 0.1 N sodium hydroxide and 0.1 N sulphuric acid solutions. The progress of photocatalytic degradation of the dye was monitored by withdrawing definite quantity of the reaction mixture at regular time intervals and measuring the absorbance by the UV-VIS spectrophotometer at a maximum wavelength(
λ
max
⁡
=
620
nm
). Additional experiments were conducted to verify that the observed reaction was indeed photocatalysis. For this, the dye solution was irradiated with solar/UV light without adding photocatalyst and with photocatalyst in the absence of solar/UV light.


## 3. Results and Discussion

### 3.1. Characterization of the Synthesized Bimetal Cerium-Cadmium Oxide

The XRD pattern of cerium-cadmium oxide is shown in Figure2. The graph has been plotted between intensity (cycles per second) and 2
θ values (in degrees). For general consideration, 2
θ values range from 20 to 80°, as the characteristic peaks for ternary oxides of cerium and lanthanum with transition metals appear in the same range. The synthesized catalyst is in nanoform (28.43 nm) as determined by the Scherrer equation.Figure 2
X-ray powder diffraction pattern of cerium-cadmium oxide.


### 3.2. Photocatalytic Degradation of Dye Using Nanosized Bimetal Oxide

A 2.0 mL of the solution was taken out from the reaction mixture, which contains dye and cerium-cadmium oxide at regular time interval and absorbance was measured spectrophotometrically atλ
max
⁡
=
620 nm. It was observed that the absorbance of the solution decreases with increasing time intervals showing thereby that the concentration of the dye decreases with increasing time of exposure. A plot of 2 + log O.D. versus time was linear and follows first-order kinetics. The rate constant was calculated by using the expression, k
=
2.303
×
Slope. The rate constant for the reaction was 7.67 × 10−4 s−1.The typical run for dye degradation is given in Table1 and graphically represented in Figure 3.Table 1
A typical run of malachite green dye degradation using cerium-cadmium oxidea.
Time (min.)
Optical Density (O.D.)
2
+
log
⁡
⁡
O.D.
0.00
1.240
2.0934
20.00
0.560
1.7482
40.00
0.213
1.3284
60.00
0.077
0.8865
80.00
0.036
0.5563
k
=
7.67
×
10
-
4
s
-
1
aReaction conditions: dye concentration = 2.50
×
10
-
5 M, light intensity = 600 W
m
-
2, cerium-cadmium oxide = 0.03 g in 50 mL dye solution, and pH = 8.Figure 3
Plot of 2 + log O.D. verses time for a typical run.


### 3.3. Effect of Different Variables on Photocatalytic Degradation of Dye

#### 3.3.1. Effect of pH

Attempts have been made to study the effect of pH on the rate of dye degradation under visible light irradiation as pH plays an important role both in the characteristics of textile wastewater and the generation of hydroxyl radicals. Hence, photodegradation process was examined at pH values from 6 to 10. The effect of pH on the rate of dye degradation is reported in Figure4.Figure 4
Effect of pH on degradation of malachite green. Reaction conditions: dye concentration = 2.50 × 10−5M, light intensity = 600 Wm−2, and cerium-cadmium oxide = 0.03 g in 50 mL dye solution.In both acidic and alkaline pH, it seems to increase the percentage degradation of the dye. As observed, the rate of reaction increased with increasing pH of the solution up to pH 8.0. However, a further increase in pH of solution resulted in a decreased reaction rate. An increase in the rate of photocatalytic degradation of malachite green with increase in pH may be due to the generation of moreOH
• radicals, which are produced from the reaction between −OH ions and hole (h+) of the semiconductor. Above pH 8.0, a decrease in the rate of photocatalytic degradation of the dye was observed, which may be due to the fact that the cationic form of malachite green converts in its natural form, which faces no attraction towards the negatively charged semiconductor surface due to adsorption of OH
- ions.


#### 3.3.2. Effect of Concentration of Dye

The effect of dye concentration on the rate of dye degradation was studied by varying the concentration of dye from1.50
×
10
-
5 to 4.50
×
10
-
5 M (Figure 5). It can be seen that rate of dye degradation increased with increasing the dye concentration up to 2.50
×
10
-
5 M; after that the rate of photodegradation decreased with further increase in the dye concentration. The possible explanation for this behavior is that as the concentration of dye was increased, more dye molecules were available for excitation and energy transfer and, hence, an increase in the rate was observed, but, on further increase in concentration, dye starts acting as a filter for the incident light and will not permit the light intensity to reach the semiconductor surface.Figure 5
Effect of dye concentration on degradation of malachite green. Reaction conditions: cerium-cadmium oxide = 0.03 g in 50 mL dye solution, pH = 8, and light intensity = 600 Wm−2.


#### 3.3.3. Effect of Semiconductor Amount

The effect of nanophotocatalyst loading on the rate of dye degradation has been examined by varying its amount from 0.02 to 0.08 g/50 mL of the dye solution. The results are presented in Figure6.Figure 6
Effect of amount of cerium-cadmium oxide on degradation of malachite green. Reaction conditions: dye concentration =2.50
×
10
-
5 M, light intensity = 600 Wm−2, pH = 8.It was observed that the rate of dye degradation increases rapidly with the increase in the amount of photocatalyst from 0.02 to 0.03 g/50 mL of the dye. With further increase in the amount of photocatalyst from 0.03 to 0.08 g, the rate of dye degradation decreases. This can be rationalized in terms of availability of active sites on catalyst surface and light penetration of photo activating substance into the suspension. The decreased degradation rate at higher catalyst loading may be due to deactivation of activated molecules by collision with ground state molecules.Hence, an optimum catalyst has to be added in order to avoid unnecessary excess catalyst and also to ensure total absorption of solar light photons for efficient photomineralisation.


#### 3.3.4. Effect of Light Intensity

The effect of light intensity on the rate of reaction was also studied. The observations are summarized in Figure7. It was observed that the rate constant increased with increasing light intensity from 200 up to 600 Wm−2 because on increasing the light intensity, the number of photons striking per unit area of reaction mixture will also increase. This will result in a corresponding increase in the rate of degradation of malachite green. Small decrease in the rate on further increasing light intensity may be due to some thermal or side reactions.Figure 7
Effect of light intensity on degradation of malachite green. Reaction conditions: dye concentration = 2.50 × 10−5M, pH = 8, cerium-cadmium oxide = 0.03 g in 50 mL dye solution.Mechanism. On the basis of these observations, a tentative mechanism for photocatalytic degradation of malachite green may be proposed as(1)
1
M
G
0
→
h
ν
M
G
1;
(2)
1
M
G
1
→
ISC
M
G
1
3;
(3)
SC
→
h
ν
e
-
(
CB
)
+
h
+
(
VB
);
(4)
e
-
+
O
2
⟶
O
2
-
•;
(5)
O
2
-
•
+
M
G
1
3
⟶
Leuco  MG;
(6)
Leuco  MG
⟶
Products.Malachite green (MG) absorbs radiations of suitable wavelength and gives rise to its first excited singlet state. Then it undergoes intersystem crossing (ISC) to give the triplet state of the dye. On the other hand, the semiconducting cerium-cadmium oxide (SC) also utilizes the radiant energy to excite its electron from the valence band to the conduction band. This electron will be abstracted by an oxygen molecule (dissolved oxygen) generating superoxide anion radical (O
2
-
•). This anion radical will reduce the dye malachite green to its leuco form, which may ultimately degrade to products. It was also confirmed that this degradation proceeds through reduction and not oxidation as the rate of degradation was not affected appreciably in the presence of hydroxyl radical scavenger (2-propanol).


## 3.1. Characterization of the Synthesized Bimetal Cerium-Cadmium Oxide

The XRD pattern of cerium-cadmium oxide is shown in Figure2. The graph has been plotted between intensity (cycles per second) and 2
θ values (in degrees). For general consideration, 2
θ values range from 20 to 80°, as the characteristic peaks for ternary oxides of cerium and lanthanum with transition metals appear in the same range. The synthesized catalyst is in nanoform (28.43 nm) as determined by the Scherrer equation.Figure 2
X-ray powder diffraction pattern of cerium-cadmium oxide.


## 3.2. Photocatalytic Degradation of Dye Using Nanosized Bimetal Oxide

A 2.0 mL of the solution was taken out from the reaction mixture, which contains dye and cerium-cadmium oxide at regular time interval and absorbance was measured spectrophotometrically atλ
max
⁡
=
620 nm. It was observed that the absorbance of the solution decreases with increasing time intervals showing thereby that the concentration of the dye decreases with increasing time of exposure. A plot of 2 + log O.D. versus time was linear and follows first-order kinetics. The rate constant was calculated by using the expression, k
=
2.303
×
Slope. The rate constant for the reaction was 7.67 × 10−4 s−1.The typical run for dye degradation is given in Table1 and graphically represented in Figure 3.Table 1
A typical run of malachite green dye degradation using cerium-cadmium oxidea.
Time (min.)
Optical Density (O.D.)
2
+
log
⁡
⁡
O.D.
0.00
1.240
2.0934
20.00
0.560
1.7482
40.00
0.213
1.3284
60.00
0.077
0.8865
80.00
0.036
0.5563
k
=
7.67
×
10
-
4
s
-
1
aReaction conditions: dye concentration = 2.50
×
10
-
5 M, light intensity = 600 W
m
-
2, cerium-cadmium oxide = 0.03 g in 50 mL dye solution, and pH = 8.Figure 3
Plot of 2 + log O.D. verses time for a typical run.


## 3.3. Effect of Different Variables on Photocatalytic Degradation of Dye

### 3.3.1. Effect of pH

Attempts have been made to study the effect of pH on the rate of dye degradation under visible light irradiation as pH plays an important role both in the characteristics of textile wastewater and the generation of hydroxyl radicals. Hence, photodegradation process was examined at pH values from 6 to 10. The effect of pH on the rate of dye degradation is reported in Figure4.Figure 4
Effect of pH on degradation of malachite green. Reaction conditions: dye concentration = 2.50 × 10−5M, light intensity = 600 Wm−2, and cerium-cadmium oxide = 0.03 g in 50 mL dye solution.In both acidic and alkaline pH, it seems to increase the percentage degradation of the dye. As observed, the rate of reaction increased with increasing pH of the solution up to pH 8.0. However, a further increase in pH of solution resulted in a decreased reaction rate. An increase in the rate of photocatalytic degradation of malachite green with increase in pH may be due to the generation of moreOH
• radicals, which are produced from the reaction between −OH ions and hole (h+) of the semiconductor. Above pH 8.0, a decrease in the rate of photocatalytic degradation of the dye was observed, which may be due to the fact that the cationic form of malachite green converts in its natural form, which faces no attraction towards the negatively charged semiconductor surface due to adsorption of OH
- ions.


### 3.3.2. Effect of Concentration of Dye

The effect of dye concentration on the rate of dye degradation was studied by varying the concentration of dye from1.50
×
10
-
5 to 4.50
×
10
-
5 M (Figure 5). It can be seen that rate of dye degradation increased with increasing the dye concentration up to 2.50
×
10
-
5 M; after that the rate of photodegradation decreased with further increase in the dye concentration. The possible explanation for this behavior is that as the concentration of dye was increased, more dye molecules were available for excitation and energy transfer and, hence, an increase in the rate was observed, but, on further increase in concentration, dye starts acting as a filter for the incident light and will not permit the light intensity to reach the semiconductor surface.Figure 5
Effect of dye concentration on degradation of malachite green. Reaction conditions: cerium-cadmium oxide = 0.03 g in 50 mL dye solution, pH = 8, and light intensity = 600 Wm−2.


### 3.3.3. Effect of Semiconductor Amount

The effect of nanophotocatalyst loading on the rate of dye degradation has been examined by varying its amount from 0.02 to 0.08 g/50 mL of the dye solution. The results are presented in Figure6.Figure 6
Effect of amount of cerium-cadmium oxide on degradation of malachite green. Reaction conditions: dye concentration =2.50
×
10
-
5 M, light intensity = 600 Wm−2, pH = 8.It was observed that the rate of dye degradation increases rapidly with the increase in the amount of photocatalyst from 0.02 to 0.03 g/50 mL of the dye. With further increase in the amount of photocatalyst from 0.03 to 0.08 g, the rate of dye degradation decreases. This can be rationalized in terms of availability of active sites on catalyst surface and light penetration of photo activating substance into the suspension. The decreased degradation rate at higher catalyst loading may be due to deactivation of activated molecules by collision with ground state molecules.Hence, an optimum catalyst has to be added in order to avoid unnecessary excess catalyst and also to ensure total absorption of solar light photons for efficient photomineralisation.


### 3.3.4. Effect of Light Intensity

The effect of light intensity on the rate of reaction was also studied. The observations are summarized in Figure7. It was observed that the rate constant increased with increasing light intensity from 200 up to 600 Wm−2 because on increasing the light intensity, the number of photons striking per unit area of reaction mixture will also increase. This will result in a corresponding increase in the rate of degradation of malachite green. Small decrease in the rate on further increasing light intensity may be due to some thermal or side reactions.Figure 7
Effect of light intensity on degradation of malachite green. Reaction conditions: dye concentration = 2.50 × 10−5M, pH = 8, cerium-cadmium oxide = 0.03 g in 50 mL dye solution.Mechanism. On the basis of these observations, a tentative mechanism for photocatalytic degradation of malachite green may be proposed as(1)
1
M
G
0
→
h
ν
M
G
1;
(2)
1
M
G
1
→
ISC
M
G
1
3;
(3)
SC
→
h
ν
e
-
(
CB
)
+
h
+
(
VB
);
(4)
e
-
+
O
2
⟶
O
2
-
•;
(5)
O
2
-
•
+
M
G
1
3
⟶
Leuco  MG;
(6)
Leuco  MG
⟶
Products.Malachite green (MG) absorbs radiations of suitable wavelength and gives rise to its first excited singlet state. Then it undergoes intersystem crossing (ISC) to give the triplet state of the dye. On the other hand, the semiconducting cerium-cadmium oxide (SC) also utilizes the radiant energy to excite its electron from the valence band to the conduction band. This electron will be abstracted by an oxygen molecule (dissolved oxygen) generating superoxide anion radical (O
2
-
•). This anion radical will reduce the dye malachite green to its leuco form, which may ultimately degrade to products. It was also confirmed that this degradation proceeds through reduction and not oxidation as the rate of degradation was not affected appreciably in the presence of hydroxyl radical scavenger (2-propanol).


## 3.3.1. Effect of pH

Attempts have been made to study the effect of pH on the rate of dye degradation under visible light irradiation as pH plays an important role both in the characteristics of textile wastewater and the generation of hydroxyl radicals. Hence, photodegradation process was examined at pH values from 6 to 10. The effect of pH on the rate of dye degradation is reported in Figure4.Figure 4
Effect of pH on degradation of malachite green. Reaction conditions: dye concentration = 2.50 × 10−5M, light intensity = 600 Wm−2, and cerium-cadmium oxide = 0.03 g in 50 mL dye solution.In both acidic and alkaline pH, it seems to increase the percentage degradation of the dye. As observed, the rate of reaction increased with increasing pH of the solution up to pH 8.0. However, a further increase in pH of solution resulted in a decreased reaction rate. An increase in the rate of photocatalytic degradation of malachite green with increase in pH may be due to the generation of moreOH
• radicals, which are produced from the reaction between −OH ions and hole (h+) of the semiconductor. Above pH 8.0, a decrease in the rate of photocatalytic degradation of the dye was observed, which may be due to the fact that the cationic form of malachite green converts in its natural form, which faces no attraction towards the negatively charged semiconductor surface due to adsorption of OH
- ions.


## 3.3.2. Effect of Concentration of Dye

The effect of dye concentration on the rate of dye degradation was studied by varying the concentration of dye from1.50
×
10
-
5 to 4.50
×
10
-
5 M (Figure 5). It can be seen that rate of dye degradation increased with increasing the dye concentration up to 2.50
×
10
-
5 M; after that the rate of photodegradation decreased with further increase in the dye concentration. The possible explanation for this behavior is that as the concentration of dye was increased, more dye molecules were available for excitation and energy transfer and, hence, an increase in the rate was observed, but, on further increase in concentration, dye starts acting as a filter for the incident light and will not permit the light intensity to reach the semiconductor surface.Figure 5
Effect of dye concentration on degradation of malachite green. Reaction conditions: cerium-cadmium oxide = 0.03 g in 50 mL dye solution, pH = 8, and light intensity = 600 Wm−2.


## 3.3.3. Effect of Semiconductor Amount

The effect of nanophotocatalyst loading on the rate of dye degradation has been examined by varying its amount from 0.02 to 0.08 g/50 mL of the dye solution. The results are presented in Figure6.Figure 6
Effect of amount of cerium-cadmium oxide on degradation of malachite green. Reaction conditions: dye concentration =2.50
×
10
-
5 M, light intensity = 600 Wm−2, pH = 8.It was observed that the rate of dye degradation increases rapidly with the increase in the amount of photocatalyst from 0.02 to 0.03 g/50 mL of the dye. With further increase in the amount of photocatalyst from 0.03 to 0.08 g, the rate of dye degradation decreases. This can be rationalized in terms of availability of active sites on catalyst surface and light penetration of photo activating substance into the suspension. The decreased degradation rate at higher catalyst loading may be due to deactivation of activated molecules by collision with ground state molecules.Hence, an optimum catalyst has to be added in order to avoid unnecessary excess catalyst and also to ensure total absorption of solar light photons for efficient photomineralisation.


## 3.3.4. Effect of Light Intensity

The effect of light intensity on the rate of reaction was also studied. The observations are summarized in Figure7. It was observed that the rate constant increased with increasing light intensity from 200 up to 600 Wm−2 because on increasing the light intensity, the number of photons striking per unit area of reaction mixture will also increase. This will result in a corresponding increase in the rate of degradation of malachite green. Small decrease in the rate on further increasing light intensity may be due to some thermal or side reactions.Figure 7
Effect of light intensity on degradation of malachite green. Reaction conditions: dye concentration = 2.50 × 10−5M, pH = 8, cerium-cadmium oxide = 0.03 g in 50 mL dye solution.Mechanism. On the basis of these observations, a tentative mechanism for photocatalytic degradation of malachite green may be proposed as(1)
1
M
G
0
→
h
ν
M
G
1;
(2)
1
M
G
1
→
ISC
M
G
1
3;
(3)
SC
→
h
ν
e
-
(
CB
)
+
h
+
(
VB
);
(4)
e
-
+
O
2
⟶
O
2
-
•;
(5)
O
2
-
•
+
M
G
1
3
⟶
Leuco  MG;
(6)
Leuco  MG
⟶
Products.Malachite green (MG) absorbs radiations of suitable wavelength and gives rise to its first excited singlet state. Then it undergoes intersystem crossing (ISC) to give the triplet state of the dye. On the other hand, the semiconducting cerium-cadmium oxide (SC) also utilizes the radiant energy to excite its electron from the valence band to the conduction band. This electron will be abstracted by an oxygen molecule (dissolved oxygen) generating superoxide anion radical (O
2
-
•). This anion radical will reduce the dye malachite green to its leuco form, which may ultimately degrade to products. It was also confirmed that this degradation proceeds through reduction and not oxidation as the rate of degradation was not affected appreciably in the presence of hydroxyl radical scavenger (2-propanol).


## 4. Conclusion

Easy, simple, fast, and low cost synthesis of novel nanosized cerium-cadmium oxide and its characterization by XRD were studied in this research paper. The particle size of the synthesized bimetal oxide is 28.43 nm. From the nanotechnology point of view, this is a significant advancement to synthesize nanosized cerium-cadmium bimetal oxide. Based on this study, some other nanophotocatalysts may be synthesized in the future. Also, in this paper, we reported the photocatalytic activity of the synthesized nanoparticles. The optimum reaction conditions of dye degradation with cerium-cadmium oxide were experimentally determined. The photochemical degradation of dye follows first-order kinetics. The synthesized bimetal oxide may be used for the degradation of some other dyes.



---

*Source: 480107-2014-04-30.xml*