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.
Kinetics of the reactions of NCO radicals with NO and NH3
Becker,Kurtenbach,Schmidt,Wiesen
, p. 128 - 133 (2007/10/03)
The rate constants for the reaction of NCO (X2∏) radicals with NO and NH3 were measured at 20 Torr total pressure in temperature ranges of 290-1098 K and 295-882 K, respectively, using C1NCO excimer laser photolysis for NCO radical formation in combination with laser-induced fluorescence detection of NCO. In the temperature range investigated the NCO + NO reaction exhibits a negative temperature dependence which is described by the following three parameter Arrhenius equation: (Equation Presented) with E0 in units of kJ/mol. For the NCO + NH3 reaction the measurements exhibit a positive temperature dependence over the temperature range investigated with a slight upwards curvature. A modified three parameters Arrhenius fit provides a good description of the experimental data: (Equation Presented) with E0 in units of kJ/mol. In addition, the rate constant of the NCO + NH3 reaction was found to be pressure independent in the range 10-193 Torr at 295 K. VCH Verlagsgesellschaft mbH, 1997.