66291-19-8

Upstream product

• 766-76-7 benzoate 
• 1610-26-0 1-nitro-4-(nitromethyl)benzene 
• 102-82-9 tributyl-amine 

Downstream Products

• 1610-26-0 1-nitro-4-(nitromethyl)benzene 
• 766-76-7 benzoate 

Relevant academic research and scientific papers

Kinetic Isotope Effect and Tunnelling in the Reaction between 4-Nitrophenylnitromethane in Acetonitrile and Toluene

Rates and activation parameters for the proton and deuteron transfer reaction of 4-nitrophenylnitromethane with pentamethylguanidine in acetonitrile have been determined.The isotope effect and differences in activation parameters are larger than the semic

The Kinetics and Mechanism of Proton Transfer from 4- Nitrophenylnitromethane to Triethylamine

The rate constants for the forward and back proton transfer reactions between 4-nitropehenylnitromethane and triethylamine in aprotic solvents, whose permittivities varied in a wide range, were determined by the stopped flow method. A quantum-chemical stu

Kinetic study of the reactions of various types of C-acids with amine bases in acetonitrile. An unusual effect of common BH+ cation on the rate constants

The rates of proton transfer reactions between C-acids of different types such as 1-(4-nitrophenyl)-1-nitroalkanes, 4-nitrophenylcyanomethanes, and 2,4,6-trinitrotoluene, and organic bases such as 1,1,3,3-tetrametylguanidine, 7-methyl-1,5,7-triazabicyclo[4.4.0]dec-5-ene (MTBD), and tri-n-butylamine have been measured in acetonitrile at pseudo-first-order conditions. A general equation for the rates of proton transfer reactions between C-acids and bases with product existing in two forms, ions and ion pairs, has been derived and its applicability tested. The equation works well except for reactions of 1-(4-nitrophenyl)-1-nitroalkanes with guanidines for which the second-order rate constant is diminished with concentration of guanidinium cation, while tetrabutylammonium salts accelerate the reactions. Possible reasons for this are discussed.

Solvent Effects on Proton Transfer Reactions: Benzoate Ion Promoted Deprotonation Reactions of Arylnitromethanes in Methanol Solution

Second-order rate constants and equilibrium constants have been determined for the benzoate ion promoted deprotonation reactions of (m-nitrophenyl)nitromethane, (p-nitrophenyl)nitromethane, and (3,5-dinitrophenyl)nitromethane in methanol solution. The pK

Hydrolysis of substituted α-nitrostilbenes: Dissection of rate coefficients for individual steps in the four-step mechanism. Estimates of intrinsic rate constants and transition-state imbalances

A kinetic study of the hydrolysis of substituted α-nitrostilbenes (NS-Z with Z = 4-Me, H, 4-Br, 3-NO2, and 4-NO2) in 50% Me2SO-50% water (v/v) at 20 °C is reported. The mechanism consists of four steps: nucleophilic addition to NS-Z of water (k1H2O) and OH- (k1OH) to form PhCH(OH)C(Ar)NO2- (TOH-); carbon protonation of TOH- by water (k2H2O), H3O+ (k2H), and buffer acids (k2BH) to form PhCH(OH)CH(Ar)NO2 (TOH0); rapid oxygen deprotonation of TOH0 (KaOH) to form PhCH(O-)CH(Ar)NO2 (TO-); collapse of TO- (k4) into benzaldehyde and arylnitromethane anion. The aci-form of TOH0, PhCH(OH)CH(Ar)NO2H (TOH,aci0), can also be generated as a transient by reaction of TOH- with strong acid. A combination of kinetic experiments involving the reaction of the olefin with water and OH-, the reaction of TOH- with acid, and the reaction of independently synthesized TOH0 with base allowed the dissection of the rate coefficients of most of the individual steps. From the substituent dependence of these rate coefficients, it is concluded that water and OH- addition to NS-Z (k1H2O and k1OH) as well as the collapse of TO- to benzaldehyde and ArCH=NO2- (k4) is characterized by substantial transition-state imbalances, reminiscent of the imbalance observed in the deprotonation of ArCH2NO2. It is also shown that the intrinsic rate constants for the k1OH and k4 steps are low compared to those for the corresponding steps in the hydrolysis of other olefins of the type PhCH=CXY (XY = (H, NO2), (CO)2C6H4, (COO)2C(CHj)2, and (CN)2). This again parallels the behavior in the deprotonation of ArCH2NO2.

Proton transfer from carbon acids to carbanions. 1. Reactions of various carbon acids with the anions of substituted benzylmalononitriles in 90% Me2SO-10% water. determination of intrinsic barriers of identity reactions from the marcus relationship

A kinetic study of the reversible deprotonation of 9-cyanofluorene (2), 1,3-indandione (3), 4-nitrophenyl-acetonitrile (4), (3-nitrophenyl)nitromethane (5), and (4-nitrophenyl)nitromethane (6) by the anions of substituted benzylmalononitrile (1-X-) in 90% Me2SO-10% water (v/v) at 20 °C is reported. Intrinsic rate constants and intrinsic barriers of these reactions have been determined by extrapolation or interpolation of Br?nsted plots whose slopes (β) are all close to 0.5. Intrinsic barriers of the identity reactions CH + C- ? C- + CH (CH = 2,3,4,and phenylnitromethane) have been estimated on the basis of the Marcus equation, coupled with either a plausible value for the identity barrier of the reaction AH+ + A ? A + AH+ (A = piperidine or morpholine) ("amine method") or a plausible value for the identity barrier of the reaction 2 + 2- ? 2- + 2 ("9-cyanofluorene method"). There are discrepancies in the identity barriers for CH + C- ? C- + CH (CH = 2, 3, 4, and phenylnitromethane) calculated by the two methods. Possible reasons for these discrepancies and the significance of the results in terms of the validity and scope of the Marcus equation are discussed.

Kinetics of deprotonation of arylnitromethanes by benzoate ions in acetonitrile solution. Effect of equilibrium and nonequilibrium transition-state solvation on intrinsic rate constants of proton transfers

Second-order rate constants for benzoate ion promoted deprotonation reactions of (3-nitropbenyl)nitromethane, (4-nitrophenyl)nitromethane, and (3,5-dinitrophenyl)nitromethane have been determined in acetonitrile solution at 25 °C. These data were obtained at low benzoate buffer concentrations (a= 21.7; (4-nitromethyl)nitromethane, pKa = 20.6; and (3,5-dinitrophenyl)nitromethane, pKa, = 19.8. A Br?nsted βB value of 0.56 and an αCHlue of 0.79 have been calculated for the benzoate, 3-bromobenzoate, and 4-nitrobenzoate ion promoted reactions of (3,5- dinitrophenyl)nitromethane and for the benzoate ion promoted reactions of (3- nitrophenyl)nitromethane and (3,5-dinitrophenyl)nitromethane, respectively; (4-nitrophenyl)nitromethane deviates negatively from the Bronsted plot due to the resonance effect of the 4-nitro group. The logarithms of the intrinsic rate constants for benzoate promoted deprotonations of (3-nitrophenyl)nitromethane, (4-nitro phenyl)nitromethane, and (3,5-dinitrophenyl)nitromethane are 4.81, 4.58, and 5.27, respectively, and these values are 1.43, 1.70, and 1.30 log units, respectively, higher in acetonitrile than in dimethyl sulfoxide. Transfer activity coefficients from dimethyl sulfoxide (D) to acetonitrile (A) solution, log DγA, for (3-nitropbenyl)nitroimethyl anion (0.28), (4-nitrophenyl)nitromethyl anion (0.56), (3-nitrophenyl)nitromethane (0.18), and (4-nitrophenyl)nitromethane (0.16) have been calculated, and log DγA for benzoic acid (～ 1.9) and the benzoate ion (～0.25) have been estimated. The solvent effects on the intrinsic rate constants are analyzed within the framework of the Principle of Nonperfect Synchronization (PNS) in terms of contributions by late solvation of the arylnitromethyl anion, late solvation of the benzoic acid (produced as a product of the reaction), early desolvation of the benzoate ion and the arylnitromethane, and by a classical solvent effect. The results are also compared with predictions by a theoretical model recently proposed by Kurz. For the comparison of intrinsic rate constants in water and dimethyl sulfoxide there is good agreement between the Kurz model and the experimental results as well as the PNS analysts, but there is a discrepancy between the results and the predictions of the Kurz model for the comparison of intrinsic rate constants in dimethyl sulfoxide and acetonitrile solutions.