# Polyethylene Glycol Mediated Kinetic Study of  Nitro Decarboxylation ofα,β-Unsaturated Acids by Blau’s Fe(III) Phen Complex

Authors: K. Ramesh; S. Shylaja; K. C. Rajanna; P. Giridhar Reddy; P. K. Saiprakash
Journal: Journal of Chemistry
 (2013)

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## Abstract

Polyethylene glycol (PEG) mediated kinetic study of nitro decarboxylation ofα,β-unsaturated acids (USA) has been taken up by Blau’s [Fe(III) nitrate-Phen] yellow complex in acetonitrile medium. Kinetics of the reactions indicated Michaelis-Menton type of mechanism and rate law. Reaction rates are significantly influenced by the structural variation and concentration of PEG. Catalysis of PEG was explained on the lines of nonionic micelles such as TX-100 because of their structural resemblance and also due to a slight negative charge developed on polyoxyethylene and cationic form(s) of Fe(III) chelates in the intermediate stages.


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## Body

## 1. Introduction

The concept of atom efficiency has proven to be a popular tool in the evaluation of the “greenness” of a chemical process [1], which revealed a comparison between various sectors of chemical manufacturing. In pharmaceutical and fine chemicals manufacturing, the high value of the product has been particularly a significant feature in the establishment of many highly (atom) inefficient processes. Thus, the creation and use of green chemical conditions are more important in pharmaceutical and fine chemicals manufacturing. In the direction of achieving green chemical processes, catalysis not only helps in replacing reagents or enabling more efficient processes, but the demonstration of their value in reducing the environmental hazardness impact and the costs of the processes. The cost reduction of the processes will also catalyze the greening of chemistry [2, 3]. In view of the above striking features, there has been an upsurging interest in the search of eco-friendly catalysts, which satisfy the conditions of green chemistry or at least improve the greenery of reaction conditions. The most significant alternatives include (a) the use of eco-friendly materials as catalysts, (b) environmentally benign solvents such as water and polyethylene glycols (PEGs) [4–6], (c) the use of nonconventional energy sources such as sonication (by using ultrasonic waves) and microwave (MW) irradiation [7]. A special attention has also been focused on conducting the reactions under solvent free conditions by grinding the reactants in a mortar with a pestle or by microwave irradiation to achieve greenery conditions [8]. For the past few decades our group has also been actively engaged in exploiting the use of the above cited tools to assist various organic transformations such as Vilsmeier-Haack, Hunsdiecker [9–11], and nitration reactions [12–14].It is customary to measure the efficiency of a catalyst by the number of reusable cycles. Similarly, the value of a new solvent medium basically depends on its environmental impact, the ease with which it could be recycled, and solvent properties, namely, low vapor pressure, nonflammability, and high polarity for solubilization. In performing the majority of organic transformations, solvents also play an important role in mixing the ingredients to make the system homogeneous and allow molecular interactions to be more efficient. Polyethylene glycol (PEG) is a neutral, hydrophilic polyether and is less expensive. The use of PEG avoids the use of acid or base catalysts, and moreover PEG can be recovered and reused. Thus, it offers a convenient, inexpensive, nonionic, nontoxic, and recyclable reaction medium for the replacement of volatile organic solvents. This protocol also offers a rapid and clean alternative and reduces reaction times; see Scheme1.Scheme 1On the other hand, it is unreasonable to note that over the years, transition metal ions or their complexes with different environments have been used as catalysts, probably because they are economically cheap and available in any laboratory desk. Ferric salts or the complexes of Fe(III) have also been in the forefront as efficient catalysts under homogeneous as well as heterogeneous conditions. Earlier reports show that Fe(III) oxidation reactions are sluggish in acidic media and do not proceed in highly concentrated solutions. However, the addition of even trace amounts of Phenanthroline (Phen) to the reaction medium increases the formal potential of Fe(II)/Fe(III) couple, rendering the reaction thermodynamically feasible by forming yellow colored Fe(III) chelates [15–18]. Phenanthroline functions as a typical bidentate chelate molecule which interacts with metal ion through the nitrogen atoms with the formation of five-membered rings. Further, it is interesting to note that the above mentioned yellow complexes of Fe(III) are isolated as crystalline solids and well-characterized by Blau [15]. These complexes are reported to be substitution labile and entirely different from ferroin (blue complexes of Fe(III) with Phen), which could not be obtained by direct mixing but only by the oxidation of ferroin and were also found to be substitution inert.Borodin [19] was the first to report the classical Hunsdiecker-Borodin reaction (HBR) in the year 1861. Hunsdiecker et al. [20, 21] later on developed this reaction in 1942. It is one of the most versatile reactions in organic synthesis for the conversion of α,β-unsaturated aromatic carboxylic acids to β-bromostyrenes. The reaction also depicted that silver carboxylates when treated with molecular bromine at reflux temperatures underwent facile bromo decarboxylation to afford the corresponding alkyl bromides. Over a period of years, this reaction underwent several modifications as evidenced from quite a few number of publications [22–28]. In view of these striking features, the author has taken up nitration of α,β-unsaturated acids in this chapter using Blau’s yellow complexes of Fe(III) (ferric nitrate and Phen) in PEG media by avoiding mineral acids completely. In order to throw light on the most effective PEG, we have used an array of PEGs in this study.


## 2. Experimental

All theα,β-unsaturated acids used in the present study are AnalaR grade and obtained from BDH, Merck, Aldrich, Fluka, or Loba chemicals. The rest of the chemicals are procured from BDH-Merck, India. Polyethylene glycols (PEGs) were used as such which were procured from the suppliers. HPLC grade Acetonitrile was used throughout the study.


### 2.1. General Procedure for Solvent Mediated Synthesis ofβ-Nitro Styrene

In this procedure, reactions are conducted using DCE and MeCN as solvents. Cinnamic acid (0.001 mol) dissolved in DCE/MeCN and 0.001 moles of Blau’s complex (mixture of equimolar mixture of Fe(III) nitrate and 1,10-Phenanthroline (Phen) ligand) were suspended in a three necked round bottomed flask. The flask is equipped with a mechanical stirrer and reflux condenser. The reaction mixture is stirred for some time until the evolution of CO2 completely ceases. The mixture is cooled in an ice bath and the precipitate is removed by filtration. The residue is washed with CCl4 and the filtrates are combined. The solvent is removed by distillation using a modified Claisen distillation apparatus with a 6 cm condenser. After completion of the reaction as indicated by TLC, the reaction mixture is quenched with 2% sodium carbonate solution, and the organic layer was separated, dried over Na2SO4, evaporated under vacuum, and purified with column chromatography using ethylacetate : hexane (3 : 7) as eluent to get pure product. Table 1 shows the reaction times, and under kinetic conditions also, the product of the reaction was found to be β-nitro styrene as characterized by spectroscopic methods (Table 2). But the reactions are too sluggish with long reaction times even at elevated temperatures, and the yields are too low under these conditions.Table 1
Effect of different PEGs on Fe (III)-Phen triggered nitro Hunsdiecker reactions with unsaturated carboxylic acids.
Entry
Substrates
Without PEG
PEG-200
PEG-300
PEG-400
PEG-600
PEG-6000
RT(hr)
Yield(%)
RT(hr)
Yield(%)
RT(hr)
Yield(%)
RT(hr)
Yield(%)
RT(hr)
Yield(%)
RT(hr)
Yield(%)
1
CA
26
55
2.50
78
1.75
86
1.75
82
1.75
80
3.0
75
2
4-ClCA
28
60
3.0
75
2.00
85
2.50
80
2.75
80
3.75
78
3
4-OMeCA
24
70
1.75
80
1.50
94
1.50
84
1.75
82
2.75
80
4
4-MeCA
24
60
2.0
80
1.50
90
1.75
84
2.0
80
2.75
78
5
4-NO2CA
28
55
3.0
70
2.00
82
2.75
78
3.0
75
4.0
65
6
4-OHCA
24
65
2.0
78
1.50
90
1.75
86
1.75
82
2.75
80
7
AA
26
63
2.0
76
1.50
92
1.75
88
2.0
86
2.75
82
8
CRA
28
65
3.0
75
2.00
85
2.75
80
3.0
78
4.0
70
9
3-PhCRA
26
70
2.75
76
1.50
90
1.50
85
2.0
78
2.75
72
10
2-ClCA
28
60
3.0
80
2.00
86
2.00
82
2.75
80
4.0
78
11
2-MeCA
25
55
2.0
78
1.50
88
1.50
82
1.75
80
2.75
75Table 2
NMR and mass spectral data for selected reaction products.
Entry
Substrates
Product
Spectral data
m
/
z
1H NMR
1
CA
β-Nitro styrene
149
δ 6.4 (d 1H, β-CH); δ 7.3–7.65 (m 5H, Ar-H) δ7.8(d 1H, α-CH)
2
4-ClCA
4-Chloroβ-nitro styrene
184
δ 6.6 (d 1H, β-CH);δ 7.2 (d 2H, Ar-H) δ 7.6 (d 2H, Ar-H); δ 8.3 (d 1H, α-CH)
3
4-OmeCA
4-Methoxyβ-nitro styrene
179
δ 3.8 (s 3H, OCH3); δ 6.4 (d 1H, β-CH) δ 7.32–7.7 (m 4H, Ar-H) δ 7.9 (d 1H, α-CH)
4
4-MeCA
4-Methylβ-nitro styrene
163
δ 3.0 (s 3H, CH3); δ 6.6 (d 1H, β-CH)δ 7.4–7.7 (m 4H, Ar-H);δ 7.9 (d 1H, α-CH)
5
4-NO2CA
4-Nitroβ-nitro styrene
194
δ 6.6 (d 1H, β-CH); δ 7.4 (d 2H, Ar-H) δ 7.8 (d  2H, Ar-H); δ8.2 (s 1H, α-CH)
6
4-OHCA
4-Hydroxyβ-nitro  styrene
165
δ 6.5 (d 1H, β-CH); δ 7.3 (d 2H, Ar-H) δ 7.8 (d 2H, Ar-H); δ 8.1 (d 1H, α-CH)δ 10.5 (s 1H, Ar-OH)
7
AA
1-Nitro ethene
73
δ 5.92 (d 1H, β-CH); δ 6.6 (d 1H, trans β-CH);δ 7.25 (q 1H, α-CH)
8
CRA
1-Nitro propene
87
δ 2.12 (d 3H, CH3); δ 7.0 (d 1H, α-CH) δ 7.15 (m 1H, β-CH)
9
3-PhCRA
3-Phenyl  1-nitro propene
163
δ 3.3 (d 2H, CH2); δ 7.23–7.33 (m 5H, Ar-H) δ 8.2 (d 1H,  α-C-H)
10
2-ClCA
2-Chloroβ-nitro styrene
183
δ 6.6 (d 1H, β-CH); δ 7.3–7.7 (m 4H, Ar-H) δ 8.2 (d 1H, α-C-H)
11
2-MeCA
2-Methylβ-nitro styrene
163
δ 2.9 (s 3H, CH3); δ 6.7 (d 1H, β-CH) δ 7.1–7.8 (m 4H, Ar-H); δ 8.2 (d 1H, α-CH)


### 2.2.  Kinetic Measurements

Progress of the reaction was followed by recording the absorbance values of the product of oxidation [Fe(II)-(Phen) complex] produced as a function of time at 510 nm (molar absorptivity −ε  = 1.11 × 104 dm3mol−1cm−1) on a Beckman-DU model spectrophotometer (equipped with thermostatic cell compartments). Control experiments revealed that the products of oxidation, that is, Fe(II) chelates are quite stable under the experimental conditions.


## 2.1. General Procedure for Solvent Mediated Synthesis ofβ-Nitro Styrene

In this procedure, reactions are conducted using DCE and MeCN as solvents. Cinnamic acid (0.001 mol) dissolved in DCE/MeCN and 0.001 moles of Blau’s complex (mixture of equimolar mixture of Fe(III) nitrate and 1,10-Phenanthroline (Phen) ligand) were suspended in a three necked round bottomed flask. The flask is equipped with a mechanical stirrer and reflux condenser. The reaction mixture is stirred for some time until the evolution of CO2 completely ceases. The mixture is cooled in an ice bath and the precipitate is removed by filtration. The residue is washed with CCl4 and the filtrates are combined. The solvent is removed by distillation using a modified Claisen distillation apparatus with a 6 cm condenser. After completion of the reaction as indicated by TLC, the reaction mixture is quenched with 2% sodium carbonate solution, and the organic layer was separated, dried over Na2SO4, evaporated under vacuum, and purified with column chromatography using ethylacetate : hexane (3 : 7) as eluent to get pure product. Table 1 shows the reaction times, and under kinetic conditions also, the product of the reaction was found to be β-nitro styrene as characterized by spectroscopic methods (Table 2). But the reactions are too sluggish with long reaction times even at elevated temperatures, and the yields are too low under these conditions.Table 1
Effect of different PEGs on Fe (III)-Phen triggered nitro Hunsdiecker reactions with unsaturated carboxylic acids.
Entry
Substrates
Without PEG
PEG-200
PEG-300
PEG-400
PEG-600
PEG-6000
RT(hr)
Yield(%)
RT(hr)
Yield(%)
RT(hr)
Yield(%)
RT(hr)
Yield(%)
RT(hr)
Yield(%)
RT(hr)
Yield(%)
1
CA
26
55
2.50
78
1.75
86
1.75
82
1.75
80
3.0
75
2
4-ClCA
28
60
3.0
75
2.00
85
2.50
80
2.75
80
3.75
78
3
4-OMeCA
24
70
1.75
80
1.50
94
1.50
84
1.75
82
2.75
80
4
4-MeCA
24
60
2.0
80
1.50
90
1.75
84
2.0
80
2.75
78
5
4-NO2CA
28
55
3.0
70
2.00
82
2.75
78
3.0
75
4.0
65
6
4-OHCA
24
65
2.0
78
1.50
90
1.75
86
1.75
82
2.75
80
7
AA
26
63
2.0
76
1.50
92
1.75
88
2.0
86
2.75
82
8
CRA
28
65
3.0
75
2.00
85
2.75
80
3.0
78
4.0
70
9
3-PhCRA
26
70
2.75
76
1.50
90
1.50
85
2.0
78
2.75
72
10
2-ClCA
28
60
3.0
80
2.00
86
2.00
82
2.75
80
4.0
78
11
2-MeCA
25
55
2.0
78
1.50
88
1.50
82
1.75
80
2.75
75Table 2
NMR and mass spectral data for selected reaction products.
Entry
Substrates
Product
Spectral data
m
/
z
1H NMR
1
CA
β-Nitro styrene
149
δ 6.4 (d 1H, β-CH); δ 7.3–7.65 (m 5H, Ar-H) δ7.8(d 1H, α-CH)
2
4-ClCA
4-Chloroβ-nitro styrene
184
δ 6.6 (d 1H, β-CH);δ 7.2 (d 2H, Ar-H) δ 7.6 (d 2H, Ar-H); δ 8.3 (d 1H, α-CH)
3
4-OmeCA
4-Methoxyβ-nitro styrene
179
δ 3.8 (s 3H, OCH3); δ 6.4 (d 1H, β-CH) δ 7.32–7.7 (m 4H, Ar-H) δ 7.9 (d 1H, α-CH)
4
4-MeCA
4-Methylβ-nitro styrene
163
δ 3.0 (s 3H, CH3); δ 6.6 (d 1H, β-CH)δ 7.4–7.7 (m 4H, Ar-H);δ 7.9 (d 1H, α-CH)
5
4-NO2CA
4-Nitroβ-nitro styrene
194
δ 6.6 (d 1H, β-CH); δ 7.4 (d 2H, Ar-H) δ 7.8 (d  2H, Ar-H); δ8.2 (s 1H, α-CH)
6
4-OHCA
4-Hydroxyβ-nitro  styrene
165
δ 6.5 (d 1H, β-CH); δ 7.3 (d 2H, Ar-H) δ 7.8 (d 2H, Ar-H); δ 8.1 (d 1H, α-CH)δ 10.5 (s 1H, Ar-OH)
7
AA
1-Nitro ethene
73
δ 5.92 (d 1H, β-CH); δ 6.6 (d 1H, trans β-CH);δ 7.25 (q 1H, α-CH)
8
CRA
1-Nitro propene
87
δ 2.12 (d 3H, CH3); δ 7.0 (d 1H, α-CH) δ 7.15 (m 1H, β-CH)
9
3-PhCRA
3-Phenyl  1-nitro propene
163
δ 3.3 (d 2H, CH2); δ 7.23–7.33 (m 5H, Ar-H) δ 8.2 (d 1H,  α-C-H)
10
2-ClCA
2-Chloroβ-nitro styrene
183
δ 6.6 (d 1H, β-CH); δ 7.3–7.7 (m 4H, Ar-H) δ 8.2 (d 1H, α-C-H)
11
2-MeCA
2-Methylβ-nitro styrene
163
δ 2.9 (s 3H, CH3); δ 6.7 (d 1H, β-CH) δ 7.1–7.8 (m 4H, Ar-H); δ 8.2 (d 1H, α-CH)


## 2.2.  Kinetic Measurements

Progress of the reaction was followed by recording the absorbance values of the product of oxidation [Fe(II)-(Phen) complex] produced as a function of time at 510 nm (molar absorptivity −ε  = 1.11 × 104 dm3mol−1cm−1) on a Beckman-DU model spectrophotometer (equipped with thermostatic cell compartments). Control experiments revealed that the products of oxidation, that is, Fe(II) chelates are quite stable under the experimental conditions.


## 3. Results and Discussion

### 3.1. Salient Kinetic Features

(1) Under pseudo first order conditions, namely, (i) [Phen] ≫ [Fe(III)], [USA] ≫ [Fe(III)]; in the case of Blau’s yellow complexes the plots ofln(a/(a-x)) or [ln(A∞-A0)/(A∞-At)] versus time were found to be linear with negative gradients in all the systems studied. First order rate constant (k′) could be obtained either by point-wise calculation using first order rate expression or from the slopes of linear plots cited (k′). Both the values agreed with each other. This observation indicates first order with respect to [Fe(III) Phen] in all the systems. Similar observations were noticed when the reactions were studied in all PEG media (Figures 1 and 2).Figure 1
Pseudo first order kinetic plot of cinnamic acid (ln(A∞-At) versus time)  at 313 K. [CA] = 6.25 × 10−3mol dm−3; [Phen] = 3.75 × 10−3mol dm−3; [Fe(III)] = 1.25 × 10−3mol dm−3; [PEG-200] = 9.37 × 10−1mol dm−3.Figure 2
Pseudo first order kinetic plot of acrylic acid (ln(A∞-At) versus time) at 313 K. [AA] = 6.25  × 10−3mol dm−3; [Phen] = 3.75 × 10−3mol dm−3; [Fe(III)] = 1.25  × 10−3mol dm−3; [PEG-300] = 6.24 × 10−1mol dm−3.(2) This reaction is also conducted under second order conditions with equal concentrations of[Phen]≫[Fe(III)]o=[S]o. Kinetic plots of [1/(a-x)] or [1/(A∞-At)] versus time have been found linear with a positive gradient and definite intercept on ordinate vertical axis, indicating overall second order kinetics (Figures 3 and 4). Since the order with respect to [Fe(III)] is one under pseudo conditions, this observation suggests that order in [S] is also one. Thus, from the foregoing process of kinetic results, we conclude that [Fe(III) Phen] mediated Hunsdiecker-Borodin reaction follows an overall second order kinetics.Figure 3
Second order kinetic plots of cinnamic acid1/At versus time at 323 K. [CA] = 6.25 × 10−3mol dm−3; [Phen] = 6.25 × 10−3mol dm−3; [Fe(III)] = 1.25 × 10−3mol dm−3; [PEG-200] = 9.37 × 10−1mol dm−3.Figure 4
Second order kinetic plots of acrylic acid1/At versus time at 313 K. [AA] = 6.25 × 10−3mol dm−3; [Phen] = 6.25 × 10−3mol dm−3; [Fe(III)] = 1.25 × 10−3 mol dm−3 [PEG-200] = 6.24 × 10−1mol dm−3.(3) Even though the plots of1/k′ versus 1/[Phen] as well as 1/k′ versus 1/[Phen]2 were found linear with positive slope and intercept on 1/k′-axis, the plots between (1/k′) and 1/[Phen] indicated better correlation coefficients (R2>0.990) than those obtained from 1/k′ versus 1/[Phen]2 plots. These observations probably suggest the formation of a precursor (formation of 1 : 1 Fe(III)-Phen complex) between Fe(III) and Phen. Similar observations were recorded in all PEG media and the representative data are presented in Figure 5.Figure 5
Effect of variation of [Phen] on first orderk′ of cinnamic acid in PEG-300, medium at 320 K.(4) All the reactions have been studied in different PEG media and significant rate enhancements were observed.


### 3.2. Reactive Species

Although reactive Fe(III) species are complicated, Whiteker and Davidson [17] were the first to give a clear picture regarding the formation and analysis of various types of Fe(III) species in aqueous sulphuric acid medium. On similar lines various forms of Fe(III) nitrate species such as Fe(NO3)3, Fe+(NO3)2, Fe2+(NO3), Fe3+(aq), and Fe(OH)2+ could be formulated. Fe3+(aq) forms Fe(OH)2+ upon hydrolysis, (1)Fe3++H2O⇆KhFe(OH)2++H+Kh value for this reaction was reported as 2.0×10-3 at 27°C. Fe3+ readily forms various types of nitrate species in nitric acid according to the following equilibria:
(2)Fe(OH)2++H2O⇆Fe(OH)2++H+(3)Fe3+(aq)+HNO3⇆Fe(NO3)2++H+(4)Fe(NO3)2++HNO3⇆Fe(NO3)2++H+(5)Fe(NO3)2++HNO3⇆Fe(NO3)3+H+In a reaction occurring in solution phase the reactive species partaking in a rate limiting step are considered mainly on the basis of results obtained from (i) acidity (pH), (ii) ionic strength (μ), and (iii) dielectric constant (solvent) variations on the rate of the reaction. But in the present investigation the reactions are conducted in nonaqueous (MeCN) media containing PEG and Lewis bases (L) such as Phenanthroline (L=Phen). Literature reports show that Gaines Jr. et al. [18] earlier synthesized the solid crystalline complexes by direct mixing of the ligand to an aqueous solution of Fe(III) containing sulphate ions. From magnetic susceptibility data, it has been substantiated that the resultant complexes exhibited the composition of [Fe(III)]/[Phen] = 1/2. They also mentioned that a greater stability of these [Fe(III)L2] complexes is achieved when direct mixing is done in solution. If this contention has been more probable, the reciprocal plot of 1/k′ versus 1/[Phen]2 should have indicated a better linearity over 1/k′ versus 1/[Phen] plots. (Supplementary Tables S.12 to S.20 depict detailed kinetic data related to these plots. The plots are linear with very good to excellent correlation coefficients, see Tables S.12 to S.20 in Supplementary Material available online at http://dx.doi.org/10.1155/2013/703271). It is therefore reasonable to consider that Fe(III) nitrate binds with one unit of Phen to form 1 : 1 complex (i.e., [Fe(III)]/[Phen] = 1 rather than 1/2). Further, the reactions are conducted under PEG environment in addition to Phen. It is also important to consider that structural variation of PEG affected the rate of reaction considerably from PEG-200 to PEG-600 with a maximum activity with PEG-300. This observation probably supports the idea of PEG bound Fe(III) as reactive species in the present study.


### 3.3. Mechanism of Nitrodecarboxylation

The foregoing salient kinetics features, namely, first order in oxidant, first order dependence in, USA, and linearity of the plots of1/k′ versus 1/[Phen] may probably indicate the formation of a precursor prior to the rate limiting decomposition step. According to Gaines Jr. et al. [18], when polynuclear heterocyclic bases such as Phenanthroline are directly added to Fe(III) solutions, substitution liable yellow complexes of the type [L2Fe-O-FeL2]4+ and [Fe(III)L2]3+ resulted. However, in solution state [Fe(III)L2]3+ is more likely to exist. Dimeric species of Fe(III) reactive species could be ruled out because of very low concentrations of Fe(III) (~10−4mol dm−3) used in the present study. On the basis of foregoing discussions a most plausible mechanism for nitrodecarboxylation of unsaturated acids could be written as a sequence of reaction steps shown in Scheme 2.Scheme 2For the mechanism given in Scheme2, the rate law was derived according to the following sequence of steps. From the second step of Scheme 2 we have(6)Rate(ν)=k[Fe(NO3)2L(OH)(ACN)2][RCH=CH–COOH]
Considering the total concentration of ([M]tot) as the algebraic sum of free metal ion species and metal ion bound-ligand (complex) species,
(7)[M]tot=[M]+[ML]From metal ion-ligand binding equilibrium,(8)K1=[ML][M][L]or[M]=[ML]K1[L]Substitution of [M] in (7) gives
(9)[ML](K1[L])+[ML]=[M]tot[ML](1+K1[L])=[M]totK1[L][L]≈CL[ML]=[M]totK1CL(1+K1CL)=K1[Fe(III)][Phen](1+K1[Phen])Or[Fe+(NO3)2L]=[ML]=K1[M]CL1+K1[L]=K1[Fe(III)][Phen]1+K1[Phen]
Substituting this in rate limiting step (6), rate law comes out as
(10)ν=kK1[Fe(III)][Phen][USA](1+K1[Phen])This equation is in accordance with all the observed kinetic features. According to the reciprocal form of (10), plots of 1/k′ versus 1/[Phen] have been realized in the present study showing the validity of the proposed mechanism. From the observed straight line plots with positive slope (m) and intercept (C) kinetic constants K1 and k could be evaluated, where
(11)m=1kK1,C=1k,K1=Cm,k=1C.Formation constants (K1) and rate constant (k) data are presented in Tables 3 and 4 (for details, please refer to Tables S.1 to S.20 in Supplementary Material).Table 3
Activation parameters involving rate constant(k).
Substrate
PEG
k
Δ
H
#
Δ
G
#
Δ
S
#
dm3 mol−1 s−1 at 310 K
kJ/mol
J/K/mol
Cinnamic acid
200
2318
21.7
56.2
−111
300
5925
58.8
62.0
−10.2
400
1975
23.8
56.2
−104
600
2857
36.5
55.7
−62.0
Crotonic acid
200
3404
30.2
54.6
−78.6
300
5925
37.2
54.0
−54.0
400
2000
38.4
56.0
−56.6
600
2857
43.9
54.5
−34.2
Acrylic acid
200
1975
23.8
56.2
−104
300
3636
46.9
54.0
−23.1
400
3404
44.0
54.2
−33.2
600
2857
46.5
57.7
−28.6
Methoxy cinnamic acid
200
1584
18.3
56.6
−122
300
5333
34.5
66.6
4.0
400
3018
75.2
72.9
7.5
600
2857
36.5
38.8
−7.4
Nitro cinnamic acid
200
2318
21.0
56.2
−113
300
5925
54.8
55.1
−1.1
400
3404
41.3
54.3
−41.7
600
3809
38.2
54.4
−52.5Table 4
Thermodynamic parameters involving formation constant(K1).
Substrate
PEG
K
1
Δ
H
Δ
G
Δ
S
dm3 mol−1 at 310 K
kJ/mol
J/K/mol
Cinnamic acid
200
0.307
14.9
3.0
38.2
300
0.067
44.8
4.4
130
400
0.618
22.8
1.2
69.6
600
0.350
6.6
2.7
12.6
Crotonic acid
200
0.176
137
3.61
430
300
0.078
126
6.85
384
400
0.356
118
10.21
347
600
0.224
128
5.35
395
Acrylic acid
200
0.618
25.0
1.2
76.7
300
0.172
50.7
4.5
149
400
0.085
20.2
6.3
44.0
600
0.362
9.6
2.00
22.4
Methoxy cinnamic acid
200
0.284
21.7
3.2
59.7
300
0.123
44.8
4.3
130
400
0.281
30.1
3.3
86.7
600
0.350
6.6
2.7
12.6
Nitro cinnamic acid
200
0.350
14.9
3.04
38.3
300
0.470
23.5
2.0
69.6
400
0.109
52.0
5.7
149
600
0.119
69.6
5.5
206


### 3.4. Effect of [PEG] on Mechanism of Nitrodecarboxylation

Progress of the reaction has been studied in the presence of different PEGs with varied structures. Reaction rates are significantly influenced by the structural variation and concentration of PEG, which can be attributed to the electron density on polyoxyethylene moiety of PEG with an increase in methyl groups, and found that the reaction is accelerated by all the PEGs with an increasing order: PEG-200 < PEG-300 > PEG-400 > PEG-600 > PEG-6000. This could be attributed to the negative charge developed on polyoxyethylene moiety of PEG in the lines of nonionic micelles such as TX and oxidant species as mentioned above. Mechanism could probably fit into the Menger and Portnoy [29, 30] model which closely resembles that of an enzymatic catalysis. According to this model, formation of micelle-substrate complex (MS) could occur in the preequilibrium step due to the interaction of substrate (S) with micelle (M). The complex thus formed may possess higher or lower reactivity to gives products. The catalytic activity of PEG could be explained through the formation of (PEG bound Fe(III)L) by binding model.
(12)PEG+[Fe(NO3)2Phen(OH)(ACN)2]⇌[OH–CH2–(CH2–O–CH2–)n–CH2–O–Fe(NO3)2Phen(ACN)2]+H2O[PEG-Fe(NO3)2Phen(OH)(ACN)2]A general mechanism is proposed by considering the bulk phase and micellar phase reactions as shown in Scheme3.Scheme 3Data presented in Table1 show that the reactions are too sluggish with longer reaction times (>24 hrs) even under reflux conditions, while remarkable rate enhancements associated with shorter reaction times and enhanced product yields are observed in PEG mediated reactions. On the basis of these observations, mechanism of PEG mediated reactions could be explained with the participation of unsaturated acid and PEG-bound-Fe(III) nitrate species in the slow step as shown in Scheme 4.Scheme 4


### 3.5. Effect of Structure on Enthalpy and Entropy Changes

When a series of structurally related substrates undergo the same general reaction or when the reaction conditions for a single substrate are changed in a systematic way, a considerable variation in the enthalpies and entropies of activation is more likely. The entropy of activation (ΔS#) provides important information about the transition state and molecularity of the rate-determining step in the reaction path. Positive values for ΔS# suggest that entropy increases upon achieving the transition state, which often indicates a dissociative mechanism. Negative values for ΔS# indicate that entropy decreases upon achieving the transition state, which often indicates an associative mechanism.Eyring plots for rate constant (k) variation with temperature (Figures 6 and 7) are linear, and related activation parameters data are presented in Table 3 (more details of these plots are given in Supplementary Tables S.21 to S.25). A positive change in entropy of activation compiled in Table 3 probably indicates a more disordered transition state. Degrees of freedom are “liberated” ongoing from the ground state to the transition state and the reaction is fast. These results probably support the release of proton from PEG and nitrate from Fe(III) moieties, which readily brings about changes in the transition state and causes simultaneous association and dissociation of species, causing a greater disorderliness in the transition state leading to a chemical reaction. Similar trends are recorded in all the PEGs used in this study. The free energy of activation for all the systems is negative (i.e., ΔG#<0) indicating that the reaction is spontaneous.Figure 6
Eyring’s plot of cinnamic acid (ln(Nhk/RT) versus 103/T). Kinetic study with [PEG-300] = 6.24 × 10−1mol dm−3.Figure 7
Eyring’s plot of acrylic acid (ln(Nhk/RT) versus 103/T). Kinetic study with [Phen] = 3.75 × 10−3mol dm−3; [PEG-300] = 6.24 × 10−1mol dm−3;    [Fe(III)] = 1.25  × 10−3mol dm−3.Further, Vant Hoff’s plots (Figures8 and 9) of ln K1 versus (1/T) are also linear with negative slopes indicating the endothermic nature of the equilibrium. Related activation parameters are evaluated from these plots and the data are presented in Table 4 (more details of these plots are given in Supplementary Tables S.26 to S.30). Entropy values compiled in Table 4 of the present study are highly positive, which indicate greater instability and are prone to decompose or move towards another reactant to give products by interacting with it. Very small ΔG values support this contention, which also show the nonspontaneous and unstable equilibrium.Figure 8
Vant Hoff’s plot of cinnamic acid (ln(K) versus 103/T). Kinetic study with [PEG-300] = 6.24 × 10−1mol dm−3.Figure 9
Vant Hoff’s plot of acrylic acid (ln(K) versus 103/T). Kinetic study with [Phen] = 3.75 × 10−3mol dm−3[PEG-300] = 6.24 × 10−1mol dm−3;  [Fe(III)] = 1.25 × 10−3mol dm−3.


## 3.1. Salient Kinetic Features

(1) Under pseudo first order conditions, namely, (i) [Phen] ≫ [Fe(III)], [USA] ≫ [Fe(III)]; in the case of Blau’s yellow complexes the plots ofln(a/(a-x)) or [ln(A∞-A0)/(A∞-At)] versus time were found to be linear with negative gradients in all the systems studied. First order rate constant (k′) could be obtained either by point-wise calculation using first order rate expression or from the slopes of linear plots cited (k′). Both the values agreed with each other. This observation indicates first order with respect to [Fe(III) Phen] in all the systems. Similar observations were noticed when the reactions were studied in all PEG media (Figures 1 and 2).Figure 1
Pseudo first order kinetic plot of cinnamic acid (ln(A∞-At) versus time)  at 313 K. [CA] = 6.25 × 10−3mol dm−3; [Phen] = 3.75 × 10−3mol dm−3; [Fe(III)] = 1.25 × 10−3mol dm−3; [PEG-200] = 9.37 × 10−1mol dm−3.Figure 2
Pseudo first order kinetic plot of acrylic acid (ln(A∞-At) versus time) at 313 K. [AA] = 6.25  × 10−3mol dm−3; [Phen] = 3.75 × 10−3mol dm−3; [Fe(III)] = 1.25  × 10−3mol dm−3; [PEG-300] = 6.24 × 10−1mol dm−3.(2) This reaction is also conducted under second order conditions with equal concentrations of[Phen]≫[Fe(III)]o=[S]o. Kinetic plots of [1/(a-x)] or [1/(A∞-At)] versus time have been found linear with a positive gradient and definite intercept on ordinate vertical axis, indicating overall second order kinetics (Figures 3 and 4). Since the order with respect to [Fe(III)] is one under pseudo conditions, this observation suggests that order in [S] is also one. Thus, from the foregoing process of kinetic results, we conclude that [Fe(III) Phen] mediated Hunsdiecker-Borodin reaction follows an overall second order kinetics.Figure 3
Second order kinetic plots of cinnamic acid1/At versus time at 323 K. [CA] = 6.25 × 10−3mol dm−3; [Phen] = 6.25 × 10−3mol dm−3; [Fe(III)] = 1.25 × 10−3mol dm−3; [PEG-200] = 9.37 × 10−1mol dm−3.Figure 4
Second order kinetic plots of acrylic acid1/At versus time at 313 K. [AA] = 6.25 × 10−3mol dm−3; [Phen] = 6.25 × 10−3mol dm−3; [Fe(III)] = 1.25 × 10−3 mol dm−3 [PEG-200] = 6.24 × 10−1mol dm−3.(3) Even though the plots of1/k′ versus 1/[Phen] as well as 1/k′ versus 1/[Phen]2 were found linear with positive slope and intercept on 1/k′-axis, the plots between (1/k′) and 1/[Phen] indicated better correlation coefficients (R2>0.990) than those obtained from 1/k′ versus 1/[Phen]2 plots. These observations probably suggest the formation of a precursor (formation of 1 : 1 Fe(III)-Phen complex) between Fe(III) and Phen. Similar observations were recorded in all PEG media and the representative data are presented in Figure 5.Figure 5
Effect of variation of [Phen] on first orderk′ of cinnamic acid in PEG-300, medium at 320 K.(4) All the reactions have been studied in different PEG media and significant rate enhancements were observed.


## 3.2. Reactive Species

Although reactive Fe(III) species are complicated, Whiteker and Davidson [17] were the first to give a clear picture regarding the formation and analysis of various types of Fe(III) species in aqueous sulphuric acid medium. On similar lines various forms of Fe(III) nitrate species such as Fe(NO3)3, Fe+(NO3)2, Fe2+(NO3), Fe3+(aq), and Fe(OH)2+ could be formulated. Fe3+(aq) forms Fe(OH)2+ upon hydrolysis, (1)Fe3++H2O⇆KhFe(OH)2++H+Kh value for this reaction was reported as 2.0×10-3 at 27°C. Fe3+ readily forms various types of nitrate species in nitric acid according to the following equilibria:
(2)Fe(OH)2++H2O⇆Fe(OH)2++H+(3)Fe3+(aq)+HNO3⇆Fe(NO3)2++H+(4)Fe(NO3)2++HNO3⇆Fe(NO3)2++H+(5)Fe(NO3)2++HNO3⇆Fe(NO3)3+H+In a reaction occurring in solution phase the reactive species partaking in a rate limiting step are considered mainly on the basis of results obtained from (i) acidity (pH), (ii) ionic strength (μ), and (iii) dielectric constant (solvent) variations on the rate of the reaction. But in the present investigation the reactions are conducted in nonaqueous (MeCN) media containing PEG and Lewis bases (L) such as Phenanthroline (L=Phen). Literature reports show that Gaines Jr. et al. [18] earlier synthesized the solid crystalline complexes by direct mixing of the ligand to an aqueous solution of Fe(III) containing sulphate ions. From magnetic susceptibility data, it has been substantiated that the resultant complexes exhibited the composition of [Fe(III)]/[Phen] = 1/2. They also mentioned that a greater stability of these [Fe(III)L2] complexes is achieved when direct mixing is done in solution. If this contention has been more probable, the reciprocal plot of 1/k′ versus 1/[Phen]2 should have indicated a better linearity over 1/k′ versus 1/[Phen] plots. (Supplementary Tables S.12 to S.20 depict detailed kinetic data related to these plots. The plots are linear with very good to excellent correlation coefficients, see Tables S.12 to S.20 in Supplementary Material available online at http://dx.doi.org/10.1155/2013/703271). It is therefore reasonable to consider that Fe(III) nitrate binds with one unit of Phen to form 1 : 1 complex (i.e., [Fe(III)]/[Phen] = 1 rather than 1/2). Further, the reactions are conducted under PEG environment in addition to Phen. It is also important to consider that structural variation of PEG affected the rate of reaction considerably from PEG-200 to PEG-600 with a maximum activity with PEG-300. This observation probably supports the idea of PEG bound Fe(III) as reactive species in the present study.


## 3.3. Mechanism of Nitrodecarboxylation

The foregoing salient kinetics features, namely, first order in oxidant, first order dependence in, USA, and linearity of the plots of1/k′ versus 1/[Phen] may probably indicate the formation of a precursor prior to the rate limiting decomposition step. According to Gaines Jr. et al. [18], when polynuclear heterocyclic bases such as Phenanthroline are directly added to Fe(III) solutions, substitution liable yellow complexes of the type [L2Fe-O-FeL2]4+ and [Fe(III)L2]3+ resulted. However, in solution state [Fe(III)L2]3+ is more likely to exist. Dimeric species of Fe(III) reactive species could be ruled out because of very low concentrations of Fe(III) (~10−4mol dm−3) used in the present study. On the basis of foregoing discussions a most plausible mechanism for nitrodecarboxylation of unsaturated acids could be written as a sequence of reaction steps shown in Scheme 2.Scheme 2For the mechanism given in Scheme2, the rate law was derived according to the following sequence of steps. From the second step of Scheme 2 we have(6)Rate(ν)=k[Fe(NO3)2L(OH)(ACN)2][RCH=CH–COOH]
Considering the total concentration of ([M]tot) as the algebraic sum of free metal ion species and metal ion bound-ligand (complex) species,
(7)[M]tot=[M]+[ML]From metal ion-ligand binding equilibrium,(8)K1=[ML][M][L]or[M]=[ML]K1[L]Substitution of [M] in (7) gives
(9)[ML](K1[L])+[ML]=[M]tot[ML](1+K1[L])=[M]totK1[L][L]≈CL[ML]=[M]totK1CL(1+K1CL)=K1[Fe(III)][Phen](1+K1[Phen])Or[Fe+(NO3)2L]=[ML]=K1[M]CL1+K1[L]=K1[Fe(III)][Phen]1+K1[Phen]
Substituting this in rate limiting step (6), rate law comes out as
(10)ν=kK1[Fe(III)][Phen][USA](1+K1[Phen])This equation is in accordance with all the observed kinetic features. According to the reciprocal form of (10), plots of 1/k′ versus 1/[Phen] have been realized in the present study showing the validity of the proposed mechanism. From the observed straight line plots with positive slope (m) and intercept (C) kinetic constants K1 and k could be evaluated, where
(11)m=1kK1,C=1k,K1=Cm,k=1C.Formation constants (K1) and rate constant (k) data are presented in Tables 3 and 4 (for details, please refer to Tables S.1 to S.20 in Supplementary Material).Table 3
Activation parameters involving rate constant(k).
Substrate
PEG
k
Δ
H
#
Δ
G
#
Δ
S
#
dm3 mol−1 s−1 at 310 K
kJ/mol
J/K/mol
Cinnamic acid
200
2318
21.7
56.2
−111
300
5925
58.8
62.0
−10.2
400
1975
23.8
56.2
−104
600
2857
36.5
55.7
−62.0
Crotonic acid
200
3404
30.2
54.6
−78.6
300
5925
37.2
54.0
−54.0
400
2000
38.4
56.0
−56.6
600
2857
43.9
54.5
−34.2
Acrylic acid
200
1975
23.8
56.2
−104
300
3636
46.9
54.0
−23.1
400
3404
44.0
54.2
−33.2
600
2857
46.5
57.7
−28.6
Methoxy cinnamic acid
200
1584
18.3
56.6
−122
300
5333
34.5
66.6
4.0
400
3018
75.2
72.9
7.5
600
2857
36.5
38.8
−7.4
Nitro cinnamic acid
200
2318
21.0
56.2
−113
300
5925
54.8
55.1
−1.1
400
3404
41.3
54.3
−41.7
600
3809
38.2
54.4
−52.5Table 4
Thermodynamic parameters involving formation constant(K1).
Substrate
PEG
K
1
Δ
H
Δ
G
Δ
S
dm3 mol−1 at 310 K
kJ/mol
J/K/mol
Cinnamic acid
200
0.307
14.9
3.0
38.2
300
0.067
44.8
4.4
130
400
0.618
22.8
1.2
69.6
600
0.350
6.6
2.7
12.6
Crotonic acid
200
0.176
137
3.61
430
300
0.078
126
6.85
384
400
0.356
118
10.21
347
600
0.224
128
5.35
395
Acrylic acid
200
0.618
25.0
1.2
76.7
300
0.172
50.7
4.5
149
400
0.085
20.2
6.3
44.0
600
0.362
9.6
2.00
22.4
Methoxy cinnamic acid
200
0.284
21.7
3.2
59.7
300
0.123
44.8
4.3
130
400
0.281
30.1
3.3
86.7
600
0.350
6.6
2.7
12.6
Nitro cinnamic acid
200
0.350
14.9
3.04
38.3
300
0.470
23.5
2.0
69.6
400
0.109
52.0
5.7
149
600
0.119
69.6
5.5
206


## 3.4. Effect of [PEG] on Mechanism of Nitrodecarboxylation

Progress of the reaction has been studied in the presence of different PEGs with varied structures. Reaction rates are significantly influenced by the structural variation and concentration of PEG, which can be attributed to the electron density on polyoxyethylene moiety of PEG with an increase in methyl groups, and found that the reaction is accelerated by all the PEGs with an increasing order: PEG-200 < PEG-300 > PEG-400 > PEG-600 > PEG-6000. This could be attributed to the negative charge developed on polyoxyethylene moiety of PEG in the lines of nonionic micelles such as TX and oxidant species as mentioned above. Mechanism could probably fit into the Menger and Portnoy [29, 30] model which closely resembles that of an enzymatic catalysis. According to this model, formation of micelle-substrate complex (MS) could occur in the preequilibrium step due to the interaction of substrate (S) with micelle (M). The complex thus formed may possess higher or lower reactivity to gives products. The catalytic activity of PEG could be explained through the formation of (PEG bound Fe(III)L) by binding model.
(12)PEG+[Fe(NO3)2Phen(OH)(ACN)2]⇌[OH–CH2–(CH2–O–CH2–)n–CH2–O–Fe(NO3)2Phen(ACN)2]+H2O[PEG-Fe(NO3)2Phen(OH)(ACN)2]A general mechanism is proposed by considering the bulk phase and micellar phase reactions as shown in Scheme3.Scheme 3Data presented in Table1 show that the reactions are too sluggish with longer reaction times (>24 hrs) even under reflux conditions, while remarkable rate enhancements associated with shorter reaction times and enhanced product yields are observed in PEG mediated reactions. On the basis of these observations, mechanism of PEG mediated reactions could be explained with the participation of unsaturated acid and PEG-bound-Fe(III) nitrate species in the slow step as shown in Scheme 4.Scheme 4


## 3.5. Effect of Structure on Enthalpy and Entropy Changes

When a series of structurally related substrates undergo the same general reaction or when the reaction conditions for a single substrate are changed in a systematic way, a considerable variation in the enthalpies and entropies of activation is more likely. The entropy of activation (ΔS#) provides important information about the transition state and molecularity of the rate-determining step in the reaction path. Positive values for ΔS# suggest that entropy increases upon achieving the transition state, which often indicates a dissociative mechanism. Negative values for ΔS# indicate that entropy decreases upon achieving the transition state, which often indicates an associative mechanism.Eyring plots for rate constant (k) variation with temperature (Figures 6 and 7) are linear, and related activation parameters data are presented in Table 3 (more details of these plots are given in Supplementary Tables S.21 to S.25). A positive change in entropy of activation compiled in Table 3 probably indicates a more disordered transition state. Degrees of freedom are “liberated” ongoing from the ground state to the transition state and the reaction is fast. These results probably support the release of proton from PEG and nitrate from Fe(III) moieties, which readily brings about changes in the transition state and causes simultaneous association and dissociation of species, causing a greater disorderliness in the transition state leading to a chemical reaction. Similar trends are recorded in all the PEGs used in this study. The free energy of activation for all the systems is negative (i.e., ΔG#<0) indicating that the reaction is spontaneous.Figure 6
Eyring’s plot of cinnamic acid (ln(Nhk/RT) versus 103/T). Kinetic study with [PEG-300] = 6.24 × 10−1mol dm−3.Figure 7
Eyring’s plot of acrylic acid (ln(Nhk/RT) versus 103/T). Kinetic study with [Phen] = 3.75 × 10−3mol dm−3; [PEG-300] = 6.24 × 10−1mol dm−3;    [Fe(III)] = 1.25  × 10−3mol dm−3.Further, Vant Hoff’s plots (Figures8 and 9) of ln K1 versus (1/T) are also linear with negative slopes indicating the endothermic nature of the equilibrium. Related activation parameters are evaluated from these plots and the data are presented in Table 4 (more details of these plots are given in Supplementary Tables S.26 to S.30). Entropy values compiled in Table 4 of the present study are highly positive, which indicate greater instability and are prone to decompose or move towards another reactant to give products by interacting with it. Very small ΔG values support this contention, which also show the nonspontaneous and unstable equilibrium.Figure 8
Vant Hoff’s plot of cinnamic acid (ln(K) versus 103/T). Kinetic study with [PEG-300] = 6.24 × 10−1mol dm−3.Figure 9
Vant Hoff’s plot of acrylic acid (ln(K) versus 103/T). Kinetic study with [Phen] = 3.75 × 10−3mol dm−3[PEG-300] = 6.24 × 10−1mol dm−3;  [Fe(III)] = 1.25 × 10−3mol dm−3.


## 4. Conclusions

The observed catalytic activity of PEGs could be explained in the lines of nonionic micelles (TX). The slight negative charge developed on polyoxyethylene groups probably interact with cationic form(s) of Fe(III) chelates in the intermediate stages and enhances the rate of reaction.



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*Source: 703271-2013-10-10.xml*