# Thermal Decomposition of Nitrated Tri-n-Butyl Phosphate in a Flow Reactor

Authors: Lalit K. Patil; Vilas G. Gaikar; Shekhar Kumar; U. Kamachi Mudali; R. Natarajan
Journal: ISRN Chemical Engineering
 (2012)

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## Abstract

Tri-n-butyl phosphate (TBP) is a universal nuclear extractant, commercially used in the PUREX process for the last 60 years. However, it is prone to nitration and thermal degradation, and as a consequence a red-oil event may be initiated under several operating conditions resulting in severe pressurization of vessel/cell if venting is inadequate. In this work, an attempt was made to understand the reaction pathway of thermal decomposition of nitrated TBP in a flow reactor at atmospheric pressure. Many reaction products were identified and quantified by instrumental methods like HPLC-RI and GC-TCD. The experimental data was analysed with a power law model and the apparent rate constants were estimated. The activation energy for thermal decomposition of nitrated TBP, assuming an Arrhenius type of temperature dependency, was estimated to be 47.39±0.25 kJ·mol−1. The effect of both varying temperature and concentration of nitric acid on conversion of TBP into degradation products and products distribution was experimentally studied. Based on the experimental observations, a reaction mechanism framework for thermal decomposition of nitrated TBP is proposed.


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## Body

## 1. Introduction

In nuclear fuel reprocessing industry, solvent extraction is a cost-effective process for separation of unused uranium and bred plutonium from the complex fuel matrix [1]. There are many solvents which can effectively extract uranium, plutonium, or thorium from nitric acid solutions but tri-n-butyl phosphate (TBP) is one of the important organic solvents utilized during the acid extraction step in separation process at reprocessing facilities [2, 3]. This is because of its overall superiority in operation, safety, physical properties, radiation resistance, and economics. One of the most desirable attributes of TBP is its high flash point, 146°C, compared with other solvents. The reported boiling point and the density of TBP at 25°C is 289°C and 0.973 g/mL, respectively [4–6]. Most solvent extraction operations are conducted at ambient conditions without heating TBP and have been performed safely for decades. After the extraction process, raffinate containing fission products and dissolved TBP remains as highly active rad-waste which needs to be concentrated in the evaporator for storage and further management. During the evaporation process, water is evaporated continuously which results in separation of dissolved TBP from aqueous layer. At 130°C, “red oil” (complexes of TBP and HNO3) is formed which further undergoes exothermic reactions. With continual concentration of aqueous phase, the rate of generation of gases overcomes the rate of its remove which increases the pressure of the evaporator and reaction goes in runaway condition resulting to explosion [7, 8]. So far the history has registered several explosions occurring due to the decomposition of red oil [9–13].The controls for temperature, pressure, mass, and concentration are the important factor for mitigation of red oil explosion. Maintaining the temperature below 130°C is generally accepted as a safe limit to prevent red oil explosion. Sufficient venting serves to keep pressure in control from destroying the process vessel, while, also, providing the means for evaporative cooling to keep red oil from reaching the runaway temperature. Mass control involves washing with a diluent or kerosene followed by enhanced settling in decanters to remove organics from the feed stream which are capable of producing red oil. Limiting the total available TBP is an alternate mass control technique that mitigates the consequence of a red oil explosion by controlling its maximum available explosive energy. Finally, concentration control involves keeping the concentration of nitric acid below the 10 mol·dm−3. Controlling parameters should be used alone; rather, they should be used together to provide effective defence in depth for the prevention of a red oil explosion [14].In order to effectively use the above mention control parameters, separation of TBP from aqueous raffinate and quantifying it up to sub-ppm level plays an important role from environmental safety perspectives [15]. In the PUREX process, where TBP exposed to acidic conditions (nitric acid-aqueous phase) and gamma radiation (U, Th, and fission products), undergoes hydrolytic and radiolytic reactions resulting into formation of some undesired components mainly dibutyl phosphate (DBP) and to a lesser extent monobutyl phosphate (MBP). Numerous analytical methods like GC-FID [16–19], titrimetry [20], complex-gravimetry [21], ion pair chromatography [22–24], colorimetry [25, 26], IR, UV-VIS, NMR spectroscopy [7, 22], and AAS [27] exist to determine TBP at higher concentration level. High speed isotachophoresis [28] was successfully used to analyze degradation mixture of TBP.In this report, equilibrations of pure TBP and aqueous nitric acid solutions have been studied and solubility of TBP in different concentrations of nitric acid solution was determined. The equilibrated TBP further undergoes decomposition in continuous plug flow reactor. The continuous flow reactor was specially selected for the studies, from the safety point of view. The effect of concentration and temperature on the decomposition of equilibrated TBP has been studied. A detailed reaction mechanism for thermal decomposition of TBP-nitric acid was proposed on the basis of reaction products profile [29–35]. The data generated in these experiments can be useful to analyse pitfalls of vitrification process of radioactive waste after extraction process, namely, UREX, PUREX.


## 2. Materials and Methods

### 2.1. Material

Nitric acid (69%–72%), TBP (99% purity), butanol (99.6%, purity), phosphoric acid (>97% purity), and acetonitrile (HPLC grade) were procured from SD Fine-Chem limited, Mumbai, India. A standard Mixture of MBP-DBP (46%–54%) was obtained from Indira Gandhi Centre for Atomic Research, Kalpakkam. Standard gases like O2, CO, H2, CO2 and C1–C4 hydrocarbons were purchased from Alchemie gases, and other gases like NO, NO2, and N2O were purchased from Amol gases and chemicals Pvt., Ltd., Mumbai, India.


### 2.2. Experimental Set Up for Runaway Reaction

The runaway reaction between TBP and HNO3 was conducted in a continuous flow tubular reactor SS 316 (125 cm in length and 4 mm ID volumes). The reactor was placed in a ceramic furnace which can be electrically heated up to 575°C. The temperature of the furnace was controlled by a temperature controller with K-type thermocouple. A peristaltic pump was used to charge TBP equilibrated with nitric acid into the reactor. Temperature indicator and pressure indicator were placed at the end of reactor using a four-way valve. The reactor was equipped with a metal condenser along with a water cooled jacket and a phase separator. The gaseous products were passed through to a digital gas flow meter for flow measurements of evolved gases. A schematic view of the experimental setup is shown in Figure 1.Figure 1
Schematic view of experimental setup for runaway reaction. (1) peristaltic pump, (2) non-return valve, (3) coiled reactor, (4) ceramic heater, (5) temperature controller, (6) pressure gauge, (7) condenser, (8) gas-Liquid separator, (9) digital flow meter, (10) gas sampling tube, (11) gas bladder.


### 2.3. Method of Analysis

The concentration of nitric acid in organic phase was measured by titration with aqueous 1.011 mol·dm−3 NaOH solution. The amount of water in the organic phase was estimated by Karl-Fischer titration. The liquid products were analysed using a high performance liquid chromatography (HPLC) with refractive index detector using 5 μm Hypersil C18 column of length 250 mm. The column was mounted on a JASCO PU-980 HPLC chromatograph equipped with a 20 microlitre loop injector and a refractive index detector (Jasco RI-2031 plus). The column was equilibrated with 70% of acetonitrile and 30% de-ionized water as a mobile phase at a flow rate of 0.5 mL/min.HPLC chromatograph showing all the liquid products is labelled in Figure 2.Figure 2
HPLC chromatogram showing liquid products, formed during thermal decomposition of equilibrated TBP, HPLC-RI method.The qualitative and quantitative analysis of gaseous products was performed on a Chemito GC 8610 gas chromatograph equipped with a thermal conductivity detector (TCD). Gases evolved were separated on a Haysep D stainless steel packed column (25 feet in length, ID 2.4 mm). The oven temperature and TCD’s temperature were maintained constant at 35°C and 100°C, respectively. Injector port’s temperature was maintained at 35°C. In GC-TCD method, nitrogen was used as a carrier gas to detect H2, O2, CO2, NO, and N2O, whereas hydrogen was used as a carrier gas to analyse N2. Flow rate of both carrier gases was maintained at 15 mL/min. GC chromatograph showing all the gaseous product is labelled in Figure 3.Figure 3
Gas chromatogram showing gaseous products of runaway reaction of TBP and nitric acid by GC-TCD method.


### 2.4. Equilibrations of TBP with Different Concentration of Nitric Acid

The nitric acid solutions of 2, 4, 6, 8, 10, 12, and 14 mol/L concentrations were prepared from 15.6 mol/L stock solution of concentrated AR grade nitric acid and de-mineralized water of 18.2 MΩ cm resistivity. These solutions were analyzed by titrating against a standard solution of 1.011 mol/L NaOH solution. Equilibration of TBP was performed by mixing one volume of 100% TBP and five volumes of nitric acid of different concentrations in a shaker for 24 hours. After equilibration, aqueous and organic phases were separated in a glass separating funnel. Acidity of both phases was analyzed using acid-base titration with 1.011 mol/L NaOH solutions.


### 2.5. Decomposition of Nitrated TBP in Continuous Tubular Reactor

Complete evacuation of reactor was implemented to study the effect of concentration. The temperature of outer wall of reactor was set to 158°C by heater which results in an inside temperature of reactor at 150°C under flow condition; for temperature studies it was varied from 140 to 180°C, accordingly. Nitrated TBP was pumped through the reactor using peristaltic pump through nonreturn valves by means of silicon tubing at a flow rate of 0.5 mL/min. The reaction products were passed through chilled condenser and finally separated into liquid and gaseous phases. The gases were passed from the digital gas flow meter to measure the total volume of the gas produced. The gaseous products and liquid phase were collected and analyzed by gas chromatography and high pressure liquid chromatography respectively. These results are listed in Tables4 and 5.


## 2.1. Material

Nitric acid (69%–72%), TBP (99% purity), butanol (99.6%, purity), phosphoric acid (>97% purity), and acetonitrile (HPLC grade) were procured from SD Fine-Chem limited, Mumbai, India. A standard Mixture of MBP-DBP (46%–54%) was obtained from Indira Gandhi Centre for Atomic Research, Kalpakkam. Standard gases like O2, CO, H2, CO2 and C1–C4 hydrocarbons were purchased from Alchemie gases, and other gases like NO, NO2, and N2O were purchased from Amol gases and chemicals Pvt., Ltd., Mumbai, India.


## 2.2. Experimental Set Up for Runaway Reaction

The runaway reaction between TBP and HNO3 was conducted in a continuous flow tubular reactor SS 316 (125 cm in length and 4 mm ID volumes). The reactor was placed in a ceramic furnace which can be electrically heated up to 575°C. The temperature of the furnace was controlled by a temperature controller with K-type thermocouple. A peristaltic pump was used to charge TBP equilibrated with nitric acid into the reactor. Temperature indicator and pressure indicator were placed at the end of reactor using a four-way valve. The reactor was equipped with a metal condenser along with a water cooled jacket and a phase separator. The gaseous products were passed through to a digital gas flow meter for flow measurements of evolved gases. A schematic view of the experimental setup is shown in Figure 1.Figure 1
Schematic view of experimental setup for runaway reaction. (1) peristaltic pump, (2) non-return valve, (3) coiled reactor, (4) ceramic heater, (5) temperature controller, (6) pressure gauge, (7) condenser, (8) gas-Liquid separator, (9) digital flow meter, (10) gas sampling tube, (11) gas bladder.


## 2.3. Method of Analysis

The concentration of nitric acid in organic phase was measured by titration with aqueous 1.011 mol·dm−3 NaOH solution. The amount of water in the organic phase was estimated by Karl-Fischer titration. The liquid products were analysed using a high performance liquid chromatography (HPLC) with refractive index detector using 5 μm Hypersil C18 column of length 250 mm. The column was mounted on a JASCO PU-980 HPLC chromatograph equipped with a 20 microlitre loop injector and a refractive index detector (Jasco RI-2031 plus). The column was equilibrated with 70% of acetonitrile and 30% de-ionized water as a mobile phase at a flow rate of 0.5 mL/min.HPLC chromatograph showing all the liquid products is labelled in Figure 2.Figure 2
HPLC chromatogram showing liquid products, formed during thermal decomposition of equilibrated TBP, HPLC-RI method.The qualitative and quantitative analysis of gaseous products was performed on a Chemito GC 8610 gas chromatograph equipped with a thermal conductivity detector (TCD). Gases evolved were separated on a Haysep D stainless steel packed column (25 feet in length, ID 2.4 mm). The oven temperature and TCD’s temperature were maintained constant at 35°C and 100°C, respectively. Injector port’s temperature was maintained at 35°C. In GC-TCD method, nitrogen was used as a carrier gas to detect H2, O2, CO2, NO, and N2O, whereas hydrogen was used as a carrier gas to analyse N2. Flow rate of both carrier gases was maintained at 15 mL/min. GC chromatograph showing all the gaseous product is labelled in Figure 3.Figure 3
Gas chromatogram showing gaseous products of runaway reaction of TBP and nitric acid by GC-TCD method.


## 2.4. Equilibrations of TBP with Different Concentration of Nitric Acid

The nitric acid solutions of 2, 4, 6, 8, 10, 12, and 14 mol/L concentrations were prepared from 15.6 mol/L stock solution of concentrated AR grade nitric acid and de-mineralized water of 18.2 MΩ cm resistivity. These solutions were analyzed by titrating against a standard solution of 1.011 mol/L NaOH solution. Equilibration of TBP was performed by mixing one volume of 100% TBP and five volumes of nitric acid of different concentrations in a shaker for 24 hours. After equilibration, aqueous and organic phases were separated in a glass separating funnel. Acidity of both phases was analyzed using acid-base titration with 1.011 mol/L NaOH solutions.


## 2.5. Decomposition of Nitrated TBP in Continuous Tubular Reactor

Complete evacuation of reactor was implemented to study the effect of concentration. The temperature of outer wall of reactor was set to 158°C by heater which results in an inside temperature of reactor at 150°C under flow condition; for temperature studies it was varied from 140 to 180°C, accordingly. Nitrated TBP was pumped through the reactor using peristaltic pump through nonreturn valves by means of silicon tubing at a flow rate of 0.5 mL/min. The reaction products were passed through chilled condenser and finally separated into liquid and gaseous phases. The gases were passed from the digital gas flow meter to measure the total volume of the gas produced. The gaseous products and liquid phase were collected and analyzed by gas chromatography and high pressure liquid chromatography respectively. These results are listed in Tables4 and 5.


## 3. Results and Discussion

### 3.1. Equilibrium Studies

From the equilibration studies, it is clear that as concentration of nitric acid in aqueous phase increases, the ability of TBP to extract the nitric acid decreases. Acid uptake of the organic phase is listed in Table1. In case of the 2 mol/L nitric acid, 60% nitric acid is extracted into organic phase whereas for concentrated nitric acid (15.6 mol/L), 35% of nitric acid is extracted into organic phase. The distribution ratio of nitric acid in water and TBP decreases as concentration of nitric acid increases but it was found to be constant at concentration of nitric acid ≥10 mol/L. Hence at higher concentration of nitric acid (≥10 mol/L), the distribution ratio of nitric acid in water and TBP is 0.36. As the concentration of nitric acid in aqueous phase increases, the solubility of TBP decreases and it was found that at higher concentration of nitric acid (≥10 mol/L) TBP has no solubility in aqueous phase. The aqueous solubility of TBP was estimated by HPLC method and the results are listed in Table 2.Table 1
Acid uptake by TBP: analytical results.
Initial conc. of nitric acid in aqueous phase (mol/L)
Conc. of nitric acid in equilibrated  aqueous phase (mol/L)
Conc. of nitric acid in equilibrated TBP phase (mol/L)
Distribution ratio
2
1.76
1.19
0.67
4
3.53
2.18
0.61
6
5.35
2.85
0.53
8
7.45
3.14
0.42
10
9.31
3.63
0.39
12
11.46
4.12
0.36
14
13.40
4.80
0.35
15.6
15.10
5.49
0.35Table 2
Aqueous solubility of organic phase during experiment.
Aqueous nitric acid conc. (mol/L)
TBP content of aqueous phase (ppm)
2
326
4
276
6
182
8
94


### 3.2. Product Composition

Decomposition of nitrated TBP was carried out in a continuous plug flow reactor. The reaction mass was passed through ice cooled condenser so that condensable vapors can be condensed and further separated by phase separator. Liquid products were analyzed by HPLC-RI method which shows the presence of MBP, DBP, butanol, and unreacted TBP. It was expected that nitric acid will lead to complete hydrolysis of  TBP, but HPLC-RI method confirmed the absence of phosphoric acid. Gaseous products were transferred to digital gas flow meter which measured the total amount of gas generated during the reaction and collected in gas sampling tube with gas bladder and analyzed by GC-TCD method. The results showed that the presence of H2, O2, N2, CO2, NO, and N2O. Although the gas produced initially was orange brown, which suggests the presence of NO2, GC-TCD method confirmed the absence of NO2 in the gaseous products. All the products were identified by comparing their retention indices with those of standard components.


### 3.3. Effect of Operating Variables on Thermal Decomposition of Nitrated TBP

The effect of operating variables on the single-phase thermal decomposition of nitrated TBP was studied by varying the temperature from 140°C to 180°C along with the concentration of nitric acid. For this study, three solutions of nitric acid in TBP with the respective concentrations of 2.85, 3.14, and 4.12 mol/L were prepared by mixing respective aqueous nitric acid solutions of 6, 8 and 12 mol/L concentration with pure TBP for 24 hours. Effect of temperatures on gas generation during thermal decomposition of TBP equilibrated with 6, 8, and 12 mol/L of nitric acid is depicted in Figure4. It was also observed the increase of concentration of nitric acid enhanced gas yield as well as the rate of hydrolysis of TBP. Effect of temperatures on composition of gaseous products formed during thermal decomposition of TBP, equilibrated with 6, 8, and 12 mol/L of nitric acid, is shown in Table 3 and Figures 5, 7, and 9, respectively. It suggests that large amount of nitrous oxide (N2O) was formed but concentration of nitrous oxide was found to decrease as the temperature was increased. With the increase in temperature, the decomposition of nitric acid increases which results in the increase in formation of nitrogen. The yield of hydrogen increased drastically at elevated temperatures (160 to 180°C). Small amount of nitric oxide and oxygen were observed in all cases. At higher temperature, yield of carbon dioxide was found to decrease as negligible amount of coke formation was observed at elevated temperature. Effect of temperatures on liquid product profile during thermal decomposition of TBP equilibrated with 6, 8, and 12 mole/L of nitric acid is schematically shown in Table 4 and Figures 6, 8, and 10, respectively. It was also observed that conversion of TBP to degradation products increased with increase in prevailing acidity as well as temperature. As the TBP decomposition increased, the formation of MBP, DBP, and butanol also increased but the amount of butanol was not so significant. Vapor phase decomposition of butanol under oxidizing conditions yielded carbon dioxide and hydrogen. It is confirmed that concentration of nitric acid plays an important role during nitration/decomposition reactions of TBP. Thus, it is necessary to study the effect of nitric acid concentration on decomposition of nitrated TBP. For this purpose, TBP is equilibrated with 2, 4, 6, 8, 10, and 12 mol/L nitric acid. The reactor temperature is maintained at 150°C. Figure 11 shows increasing yield of gaseous product with the concentration of nitric acid in TBP. This may be partially attributed to production of butanol and butyl nitrate as decomposition products, as butyl nitrate is highly reactive at room temperature. The effect of nitric acid concentration on yield of gaseous and liquid products is shown in Figures 12 and 13, respectively.Table 3
Composition of gaseous products, formed during thermal decomposition of equilibrated TBP at 150°C.
Equilibrated nitric acid conc. in organic phase (mol/L)
Composition in mole %
N2
H2
O2
NO
CO2
N2O
1.19
7.0
8.99
9.41
2.75
38.20
33.66
2.18
8.9
7.84
2.79
2.56
38.05
39.86
2.85
9.8
6.48
2.73
4.72
39.60
36.65
3.14
10.4
6.80
1.23
3.18
34.66
43.70
3.63
12.1
8.06
1.72
3.28
34.33
40.47
4.12
12.8
9.16
2.21
3.70
32.51
39.64Table 4
Composition of liquid products, formed during thermal decomposition of equilibrated TBP at 150°C.
Equilibrated nitric acid conc. (mol/L)
Composition in wt.%
TBP
MBP + DBP
Butanol
Nitricacid
Water
1.19
70.87
21.79
2.99
3.06
1.29
2.18
62.23
25.47
3.46
6.91
1.93
2.85
52.04
30.21
5.10
10.58
2.07
3.14
48.88
33.50
3.99
11.42
2.21
3.63
39.84
38.31
7.07
12.36
2.41
4.12
34.70
41.91
7.34
13.12
2.93Table 5
Estimation of rate constant for thermal decomposition of nitrated TBP in a flow reactor.
Temperature(K)
Initial (TBP)  (moles)
Initial (HNO3)  (moles)
Final (TBP) (moles)
Estimated rate constantk
413
0.031
0.031
0.014
0.012
423
0.031
0.031
0.013
0.013
433
0.031
0.031
0.0091
0.024
443
0.031
0.031
0.0068
0.036
453
0.031
0.031
0.0054
0.048Figure 4
Effect of temperature on gases generation during the single phase decomposition of TBP equilibrated with different concentration of nitric acid.Figure 5
Effect of temperature on gas composition during the single-phase decomposition of TBP equilibrated with 6 mol/L nitric acid.Figure 6
Effect of temperature on liquid product in weight percentage during the single-phase decomposition of TBP equilibrated with 6 mol/L nitric acid.Figure 7
Effect of temperature on gaseous products in mole percentage during the single-phase decomposition of TBP equilibrated with 8 mol/L nitric acid.Figure 8
Effect of temperature on liquid product in weight percentage during the single-phase decomposition of TBP equilibrated with 8 mol/L nitric acid.Figure 9
Effect of temperature on gaseous products in mole percentage during the single-phase decomposition of TBP equilibrated with 12 mol/L nitric acid.Figure 10
Effect of temperature on liquid product in weight percentage during the single-phase decomposition of TBP equilibrated with 12 mol/L nitric acid.Figure 11
Effect of concentration of nitric acid on gas formation.Figure 12
Effect of nitric acid concentration of TBP decomposition on gas formation in mole percentage.Figure 13
Effect of nitric acid concentration on TBP decomposition on liquid product formation.


### 3.4. Kinetics of Decomposition of TBP, Equilibrated with Nitric Acid

Single-phase decomposition of TBP equilibrated with 6, 8, and 12 mol/L nitric acid was studied at temperatures ranging from 140°C to 180°C at atmospheric pressure. The reaction was found to follow first order with respect to TBP as well as nitric acid and overall second order. The rate equation could be written as follows:(1)-rTBP=k·CTBP·CHNO3
For a second order reaction in a plug flow reactor with an initial reactant ratio different than unity, the rate equation is derived from the above equation using power law model as follows:
(2)kτ=1CTBP0(M-1)ln(M-XTBPM(1-XTBP)),whereM≠1.
The value of rate constant k was determined from (2). For different operating temperatures, the obtained k values are listed in Table 5. Activation energy was calculated by using Arrhenius equation and it was found to be -47.39±0.25 kJ mol−1.


### 3.5. A Possible Mechanism for Thermal Decomposition of Nitrated TBP

From the analysis of reaction products observed during the thermal decomposition of TBP in presence of nitric acid, the following mechanism is proposed.Initially in the presence of acid, TBP is subjected to hydrolysis to produce DBP and butanol. DBP is further hydrolyzed to MBP and butanol [29]. MBP, however, remained in the reaction mixture and possibly undergoes decomposition as no phosphoric acid was detected as follows:(3a)(C4H9O)3PO+H2O→(C4H9O)2POOH+C4H9OH(3b)(C4H9O)2POOH+H2O→C4H9OPO(OH)2+C4H9OHIt was also suggested by Wilkinson and Williams [30] that TBP could directly react with nitric acid and form DBP via transesterification reaction. DBP formed is prone to nitration yielding MBP and butyl nitrate as
(4)(C4H9O)2POOH+HNO3→C4H9OPO(OH)2+C4H9ONO2C4H9OPO(OH)2+HNO3→PO(OH)3+C4H9ONO2
Barney and Copper [31] suggested that butanol, formed during the hydrolysis of TBP, undergoes an esterification reaction with nitric acid to yield butyl nitrate. The reaction might take place in vapor phase as prevailing temperatures (>130°C) were greater than the boiling point of butanol (117°C) and nitric acid (84–121°C) as
(5)C4H9OH+HONO2→C4H9ONO2+H2O
A simple way for thermal decomposition of nitric acid vapor has also been suggested in the literature [32, 33]
(6)4HNO3→2H2O+4NO2+O2
Butyl nitrate, formed from (4) and (5), is highly unstable even at room temperature. Therefore, it may decompose to yield butylaldehyde, nitrous acid, and hydrogen gas as follows as
(7)C4H9ONO2→C4H9O•+NO2•C4H9O•→CH3CH2CH2CHO+H•H•+H•→H2H•+NO2•→HNO2
As per Hiskey et al. [34], butylaldehyde is also highly reactive in acidic medium. It may react with nitrogen dioxide to yield carbon monoxide, nitric oxide, and water vapor as
(8)C4H8O+7NO2•→4CO+4H2O+7NO
Carbon monoxide could be oxidized to carbon dioxide in the presence of oxygen as follows:
(9)2CO+O2→2CO2
Bachman et al. [35] had proposed that nitrous acid also undergoes decomposition in the following three different ways:(10a)2HNO2→NO2+NO+H2O(10b)3HNO2→HNO3+2NO+H2O(10c)4HNO2→2HNO3+N2O+H2OThis study has shown possible mechanism of generation of large quantities of gaseous components in the thermal runaway “red oil” explosion. Thus, decomposition reactions of butyl nitrate and nitrous acid may be responsible for major yield of hydrogen gas generated during the thermal decomposition of nitrated TBP. The presence of hydrogen in large amount at higher temperature and higher nitric acid concentration is reported for the first time in this work.


## 3.1. Equilibrium Studies

From the equilibration studies, it is clear that as concentration of nitric acid in aqueous phase increases, the ability of TBP to extract the nitric acid decreases. Acid uptake of the organic phase is listed in Table1. In case of the 2 mol/L nitric acid, 60% nitric acid is extracted into organic phase whereas for concentrated nitric acid (15.6 mol/L), 35% of nitric acid is extracted into organic phase. The distribution ratio of nitric acid in water and TBP decreases as concentration of nitric acid increases but it was found to be constant at concentration of nitric acid ≥10 mol/L. Hence at higher concentration of nitric acid (≥10 mol/L), the distribution ratio of nitric acid in water and TBP is 0.36. As the concentration of nitric acid in aqueous phase increases, the solubility of TBP decreases and it was found that at higher concentration of nitric acid (≥10 mol/L) TBP has no solubility in aqueous phase. The aqueous solubility of TBP was estimated by HPLC method and the results are listed in Table 2.Table 1
Acid uptake by TBP: analytical results.
Initial conc. of nitric acid in aqueous phase (mol/L)
Conc. of nitric acid in equilibrated  aqueous phase (mol/L)
Conc. of nitric acid in equilibrated TBP phase (mol/L)
Distribution ratio
2
1.76
1.19
0.67
4
3.53
2.18
0.61
6
5.35
2.85
0.53
8
7.45
3.14
0.42
10
9.31
3.63
0.39
12
11.46
4.12
0.36
14
13.40
4.80
0.35
15.6
15.10
5.49
0.35Table 2
Aqueous solubility of organic phase during experiment.
Aqueous nitric acid conc. (mol/L)
TBP content of aqueous phase (ppm)
2
326
4
276
6
182
8
94


## 3.2. Product Composition

Decomposition of nitrated TBP was carried out in a continuous plug flow reactor. The reaction mass was passed through ice cooled condenser so that condensable vapors can be condensed and further separated by phase separator. Liquid products were analyzed by HPLC-RI method which shows the presence of MBP, DBP, butanol, and unreacted TBP. It was expected that nitric acid will lead to complete hydrolysis of  TBP, but HPLC-RI method confirmed the absence of phosphoric acid. Gaseous products were transferred to digital gas flow meter which measured the total amount of gas generated during the reaction and collected in gas sampling tube with gas bladder and analyzed by GC-TCD method. The results showed that the presence of H2, O2, N2, CO2, NO, and N2O. Although the gas produced initially was orange brown, which suggests the presence of NO2, GC-TCD method confirmed the absence of NO2 in the gaseous products. All the products were identified by comparing their retention indices with those of standard components.


## 3.3. Effect of Operating Variables on Thermal Decomposition of Nitrated TBP

The effect of operating variables on the single-phase thermal decomposition of nitrated TBP was studied by varying the temperature from 140°C to 180°C along with the concentration of nitric acid. For this study, three solutions of nitric acid in TBP with the respective concentrations of 2.85, 3.14, and 4.12 mol/L were prepared by mixing respective aqueous nitric acid solutions of 6, 8 and 12 mol/L concentration with pure TBP for 24 hours. Effect of temperatures on gas generation during thermal decomposition of TBP equilibrated with 6, 8, and 12 mol/L of nitric acid is depicted in Figure4. It was also observed the increase of concentration of nitric acid enhanced gas yield as well as the rate of hydrolysis of TBP. Effect of temperatures on composition of gaseous products formed during thermal decomposition of TBP, equilibrated with 6, 8, and 12 mol/L of nitric acid, is shown in Table 3 and Figures 5, 7, and 9, respectively. It suggests that large amount of nitrous oxide (N2O) was formed but concentration of nitrous oxide was found to decrease as the temperature was increased. With the increase in temperature, the decomposition of nitric acid increases which results in the increase in formation of nitrogen. The yield of hydrogen increased drastically at elevated temperatures (160 to 180°C). Small amount of nitric oxide and oxygen were observed in all cases. At higher temperature, yield of carbon dioxide was found to decrease as negligible amount of coke formation was observed at elevated temperature. Effect of temperatures on liquid product profile during thermal decomposition of TBP equilibrated with 6, 8, and 12 mole/L of nitric acid is schematically shown in Table 4 and Figures 6, 8, and 10, respectively. It was also observed that conversion of TBP to degradation products increased with increase in prevailing acidity as well as temperature. As the TBP decomposition increased, the formation of MBP, DBP, and butanol also increased but the amount of butanol was not so significant. Vapor phase decomposition of butanol under oxidizing conditions yielded carbon dioxide and hydrogen. It is confirmed that concentration of nitric acid plays an important role during nitration/decomposition reactions of TBP. Thus, it is necessary to study the effect of nitric acid concentration on decomposition of nitrated TBP. For this purpose, TBP is equilibrated with 2, 4, 6, 8, 10, and 12 mol/L nitric acid. The reactor temperature is maintained at 150°C. Figure 11 shows increasing yield of gaseous product with the concentration of nitric acid in TBP. This may be partially attributed to production of butanol and butyl nitrate as decomposition products, as butyl nitrate is highly reactive at room temperature. The effect of nitric acid concentration on yield of gaseous and liquid products is shown in Figures 12 and 13, respectively.Table 3
Composition of gaseous products, formed during thermal decomposition of equilibrated TBP at 150°C.
Equilibrated nitric acid conc. in organic phase (mol/L)
Composition in mole %
N2
H2
O2
NO
CO2
N2O
1.19
7.0
8.99
9.41
2.75
38.20
33.66
2.18
8.9
7.84
2.79
2.56
38.05
39.86
2.85
9.8
6.48
2.73
4.72
39.60
36.65
3.14
10.4
6.80
1.23
3.18
34.66
43.70
3.63
12.1
8.06
1.72
3.28
34.33
40.47
4.12
12.8
9.16
2.21
3.70
32.51
39.64Table 4
Composition of liquid products, formed during thermal decomposition of equilibrated TBP at 150°C.
Equilibrated nitric acid conc. (mol/L)
Composition in wt.%
TBP
MBP + DBP
Butanol
Nitricacid
Water
1.19
70.87
21.79
2.99
3.06
1.29
2.18
62.23
25.47
3.46
6.91
1.93
2.85
52.04
30.21
5.10
10.58
2.07
3.14
48.88
33.50
3.99
11.42
2.21
3.63
39.84
38.31
7.07
12.36
2.41
4.12
34.70
41.91
7.34
13.12
2.93Table 5
Estimation of rate constant for thermal decomposition of nitrated TBP in a flow reactor.
Temperature(K)
Initial (TBP)  (moles)
Initial (HNO3)  (moles)
Final (TBP) (moles)
Estimated rate constantk
413
0.031
0.031
0.014
0.012
423
0.031
0.031
0.013
0.013
433
0.031
0.031
0.0091
0.024
443
0.031
0.031
0.0068
0.036
453
0.031
0.031
0.0054
0.048Figure 4
Effect of temperature on gases generation during the single phase decomposition of TBP equilibrated with different concentration of nitric acid.Figure 5
Effect of temperature on gas composition during the single-phase decomposition of TBP equilibrated with 6 mol/L nitric acid.Figure 6
Effect of temperature on liquid product in weight percentage during the single-phase decomposition of TBP equilibrated with 6 mol/L nitric acid.Figure 7
Effect of temperature on gaseous products in mole percentage during the single-phase decomposition of TBP equilibrated with 8 mol/L nitric acid.Figure 8
Effect of temperature on liquid product in weight percentage during the single-phase decomposition of TBP equilibrated with 8 mol/L nitric acid.Figure 9
Effect of temperature on gaseous products in mole percentage during the single-phase decomposition of TBP equilibrated with 12 mol/L nitric acid.Figure 10
Effect of temperature on liquid product in weight percentage during the single-phase decomposition of TBP equilibrated with 12 mol/L nitric acid.Figure 11
Effect of concentration of nitric acid on gas formation.Figure 12
Effect of nitric acid concentration of TBP decomposition on gas formation in mole percentage.Figure 13
Effect of nitric acid concentration on TBP decomposition on liquid product formation.


## 3.4. Kinetics of Decomposition of TBP, Equilibrated with Nitric Acid

Single-phase decomposition of TBP equilibrated with 6, 8, and 12 mol/L nitric acid was studied at temperatures ranging from 140°C to 180°C at atmospheric pressure. The reaction was found to follow first order with respect to TBP as well as nitric acid and overall second order. The rate equation could be written as follows:(1)-rTBP=k·CTBP·CHNO3
For a second order reaction in a plug flow reactor with an initial reactant ratio different than unity, the rate equation is derived from the above equation using power law model as follows:
(2)kτ=1CTBP0(M-1)ln(M-XTBPM(1-XTBP)),whereM≠1.
The value of rate constant k was determined from (2). For different operating temperatures, the obtained k values are listed in Table 5. Activation energy was calculated by using Arrhenius equation and it was found to be -47.39±0.25 kJ mol−1.


## 3.5. A Possible Mechanism for Thermal Decomposition of Nitrated TBP

From the analysis of reaction products observed during the thermal decomposition of TBP in presence of nitric acid, the following mechanism is proposed.Initially in the presence of acid, TBP is subjected to hydrolysis to produce DBP and butanol. DBP is further hydrolyzed to MBP and butanol [29]. MBP, however, remained in the reaction mixture and possibly undergoes decomposition as no phosphoric acid was detected as follows:(3a)(C4H9O)3PO+H2O→(C4H9O)2POOH+C4H9OH(3b)(C4H9O)2POOH+H2O→C4H9OPO(OH)2+C4H9OHIt was also suggested by Wilkinson and Williams [30] that TBP could directly react with nitric acid and form DBP via transesterification reaction. DBP formed is prone to nitration yielding MBP and butyl nitrate as
(4)(C4H9O)2POOH+HNO3→C4H9OPO(OH)2+C4H9ONO2C4H9OPO(OH)2+HNO3→PO(OH)3+C4H9ONO2
Barney and Copper [31] suggested that butanol, formed during the hydrolysis of TBP, undergoes an esterification reaction with nitric acid to yield butyl nitrate. The reaction might take place in vapor phase as prevailing temperatures (>130°C) were greater than the boiling point of butanol (117°C) and nitric acid (84–121°C) as
(5)C4H9OH+HONO2→C4H9ONO2+H2O
A simple way for thermal decomposition of nitric acid vapor has also been suggested in the literature [32, 33]
(6)4HNO3→2H2O+4NO2+O2
Butyl nitrate, formed from (4) and (5), is highly unstable even at room temperature. Therefore, it may decompose to yield butylaldehyde, nitrous acid, and hydrogen gas as follows as
(7)C4H9ONO2→C4H9O•+NO2•C4H9O•→CH3CH2CH2CHO+H•H•+H•→H2H•+NO2•→HNO2
As per Hiskey et al. [34], butylaldehyde is also highly reactive in acidic medium. It may react with nitrogen dioxide to yield carbon monoxide, nitric oxide, and water vapor as
(8)C4H8O+7NO2•→4CO+4H2O+7NO
Carbon monoxide could be oxidized to carbon dioxide in the presence of oxygen as follows:
(9)2CO+O2→2CO2
Bachman et al. [35] had proposed that nitrous acid also undergoes decomposition in the following three different ways:(10a)2HNO2→NO2+NO+H2O(10b)3HNO2→HNO3+2NO+H2O(10c)4HNO2→2HNO3+N2O+H2OThis study has shown possible mechanism of generation of large quantities of gaseous components in the thermal runaway “red oil” explosion. Thus, decomposition reactions of butyl nitrate and nitrous acid may be responsible for major yield of hydrogen gas generated during the thermal decomposition of nitrated TBP. The presence of hydrogen in large amount at higher temperature and higher nitric acid concentration is reported for the first time in this work.


## 4. Conclusions

The idea about continuous plug flow reactor to study the violent reaction between TBP and nitric acid was successfully applied and red oil was synthesized without any runaway conditions. It can be synthesized by using 100% TBP equilibrated with 2 mol/L nitric acid at 150°C. During the decomposition of TBP equilibrated with nitric acid in a flow reactor, pressurization of reactor system to dangerous level is prevented as the decomposition is conducted at atmospheric pressure, thus it can be concluded that sufficient venting is one of the most important factors to prevent pressurization of the reactor systems. Furthermore, at higher concentration of nitric acid and temperature, that is, higher than 8 mol/L and 150°C, respectively, the rate of generation of gaseous products increases linearly. Hence the concentration of nitric acid and temperature of reactor play an important role to prevent runaway reaction. It is always necessary to keep the temperature of the reactor below its runaway initiation temperature.The thermal decomposition of TBP equilibrated with nitric acid over the temperature range 130–180°C is an irreversible, first order reaction with respect to TBP as well as nitric acid concentration. Activation energy of47.39±0.25 kJ mol−1 was estimated from experimental runs. In both that is, concentration and temperature effect, the decomposition of TBP increases to produce MBP, DBP, and butanol which further undergo decomposition to produce a large amount of gases. At higher temperature and concentration of nitric acid, the generation of gases is quite high which may lead to runaway condition. Thus, it is concluded that adequate venting has to be provided to the evaporator/concentrator so that pressurization of the system does not occur and volume reduction of waste aqueous raffinate could be carried out safely.The results obtained during decomposition of TBP equilibrated with nitric acid are useful for safety analysis of possible runaway reaction during evaporative concentration of radioactive acidic waste in nuclear fuel reprocessing facility.



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*Source: 193862-2012-12-27.xml*