17778-88-0Relevant articles and documents
Ultralow temperature kinetics of neutral-neutral reactions. The technique and results for the reactions CN+O2 down to 13 K and CN+NH3 down to 25 K
Sims, I. R.,Queffelec, J.-L.,Defrance, A.,Rebrion-Rowe, C.,Travers, D.,et al.
, p. 4229 - 4241 (1994)
An entirely new experimental method is described which enables the rate constants of neutral-neutral gas-phase reactions to be measured at ultralow temperatures.The measurements are made by applying the pulsed laser photolysis (PLP), laser-induced fluorescence (LIF) technique of studying the kinetics of free radical reactions in the ultracold environment provided by the gas flow in a Cinetique de Reaction en Ecoulement Supersonique Uniforme (CRESU) apparatus.The experimental method is described in some detail and its application and limitations are discussed.Results are reported for the reactions of CN radicals with O2 and NH3.For reaction (1) between CN and O2 data are reported for the temperature range T=13-295 K and the rate constants are well-matched by the expression k1(T)=(2.49+/-0.17)*10-11 (T/298)(-0.63+/-0.04) cm3 molecule-1 s-1.For reaction (2) between CN and NH3, rate constants in the temperature range T=25-295 K fit the expression k2(T)=(2.77+/-0.67)*10-11 (T/298)(-1.14+/-0.15) cm3 molecule-1 s-1.The kinetic data are discussed in terms of the latest quantum chemical and reaction rate theories for these systems.
Formation and characterization of VUV photolytically-induced (NH 2)(NH3)n aggregates, 0 ≤ n ≤ 3
Zins,Krim
, p. 10285 - 10295 (2013/09/02)
The formation of amidogen radical may be an important precursor toward the formation of prebiotic molecules on the surface of ice grains in interstellar clouds. Many laboratory experiments aimed at characterizing the photolysis of ammonia. Wide shifts wer
Radiolytic Reactions of Monochloramine in Aqueous Solutions
Poskrebyshev,Huie,Neta
, p. 7423 - 7428 (2007/10/03)
Monochloramine reacts with hydrated electrons very rapidly, k(NH 2Cl+eaq-) = (2.2 ± 0.3) × 10 10 L mol-1 s-1, to produce .NH 2 radicals. It reacts with .OH radicals more slowly, k(NH2Cl+.OH) = (5.2 ± 0.6) × 108 L mol-1 s-1, to produce .NHCl radicals. While .NH2 exhibits an absorption peak at 530 nm, with a molar absorption coefficient ε530 = 80 L mol-1 cm -1, .NHCl exhibits two peaks at 330 and 580 nm, ε330 = (85 ± 30) L mol-1 cm-1 and ε580 = (56 ± 30) L mol-1 cm-1. The .NHCl radical undergoes self-decay and can react also with O 2 to form a peroxyl radical. It is suggested that the peroxyl radical exists in equilibrium NHClO2? NHCl + O2 with an estimated equilibrium constant of (3 ± 2) × 10 -3 mol L-1. The reaction of chloramine with the carbonate radical is suggested to form a complex [CO3NH2Cl] .- with kf = 2.5 × 105 L mol-1 s -1 and kr = 4 × 102 s-1, and this complex decomposes with k = 7 × 102 s-1 to form .NHCl.
Product branching ratios of the NH2(X2B1) + NO2 reaction
Lindholm, Ned,Hershberger, John F.
, p. 4991 - 4995 (2007/10/03)
The reaction of NH2(X2B1) with NO2 was studied at 298 K using time-resolved infrared diode laser spectroscopy to detect N2O and NO products. The N2O + H2O channel was confirmed to be a rather minor contribution to the overall reaction, with a branching ratio of 0.24 ± 0.04. The branching ratio of the NO + H2NO channel was measured to be 0.76 ± 0.1.
