The Reaction F + H<sub>2</sub>→ Hf + H

Anderson, James B.

doi:10.1002/9780470142608.ch4

Cited by 39 publications

(5 citation statements)

References 117 publications

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“…The multiple experimental data for k 1 at room temperature (293-300 K) [15][16][17][18][19][20][21][22][23][24] were analyzed in previous evaluations. 1,25 Persky and Kornweitz 1 considered that the most accurate results for k 1 available at that moment were those of Clyne and Hodgson, 22 Wurzberg and Houston, 8 and Stevens et al, 7 and recommended The absolute values of k 1 measured by Heidner et al 5 are by a factor of 1.4-1.7 higher than the current data, and the difference increases with temperature. The values of k 1 measured by Igoshin et al 26 at two temperatures (195 and 296 K), although considered in previous reviews as rather uncertain, 1,25 and those reported by Homann et al 27 (in a rather narrow temperature range 300-400 K) are also in a reasonable agreement with the present measurements.…”

Section: Rate Constant Of Reaction (1): Relative Measurementsmentioning

confidence: 63%

“…1,25 Persky and Kornweitz 1 considered that the most accurate results for k 1 available at that moment were those of Clyne and Hodgson, 22 Wurzberg and Houston, 8 and Stevens et al, 7 and recommended The absolute values of k 1 measured by Heidner et al 5 are by a factor of 1.4-1.7 higher than the current data, and the difference increases with temperature. The values of k 1 measured by Igoshin et al 26 at two temperatures (195 and 296 K), although considered in previous reviews as rather uncertain, 1,25 and those reported by Homann et al 27 (in a rather narrow temperature range 300-400 K) are also in a reasonable agreement with the present measurements. Ioffe et al 6 determined k 1 at T = 293-700 K in a discharge flow system with direct detection of fluorine atom decays in excess of H 2 by electron spin resonance method.…”

Section: Rate Constant Of Reaction (1): Relative Measurementsmentioning

confidence: 63%

“…The parallel shift between the two sets of kinetic data seems to support the assumption of Stevens et al 7 on the possible systematic error between their data and those of both Heidner et al 5 and Wurzberg and Houston. 8 The values of k 2 reported by Igoshin et al 26 at two temperatures, 195 and 295 K, which are significantly higher than all other data, were analyzed in the reviews of Anderson 25 and Persky and Kornweitz 1 and estimated to be highly uncertain. The Arrhenius expression k 2 = (1.06 ± 0.12) × 10 −10 exp(−635 ± 55/T) cm 3 molecule −1 s −1 (dashed line in Figure 6), recommended by Persky and Kornweitz 1 in a critical evaluation of the available kinetic data for reaction of fluorine atoms with D 2 for T = 190-376 K, provides the values of k 2 by a factor of 1.4-1.5 higher than those measured in the present work.…”

Section: Rate Constant Of Reaction (2)mentioning

confidence: 95%

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Rate constants for the reactions of F atoms with H₂and D₂over the temperature range 220‐960 K

Bedjanian

2020

Int J of Chemical Kinetics

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The kinetics of the reactions of F atoms with hydrogen and deuterium has been studied in a discharge flow reactor combined with an electron impact ionization quadrupole mass spectrometer at nearly 2 Torr total pressure of helium and in the temperature range 220-960 K. The rate constant of the reaction F + H 2 → HF + H (1) was determined using both relative rate method (using reaction F + Br 2 as a reference) and absolute measurements, monitoring the kinetics of F atom consumption in excess of H 2 : k 1 = (1.24 ± 0.09) × 10 −10 exp(−(507 ± 23)/T) cm 3 molecule −1 s −1. The rate constant of the reaction F + D 2 → DF + D (2) was measured under pseudofirst-order conditions in excess of D 2 over F atoms: k 2 = (8.47 ± 0.42) × 10 −11 exp(−(670 ± 16)/T) cm 3 molecule −1 s −1 (the uncertainties on both k 1 and k 2 represent precision at the 2σ level, the estimated total uncertainty on the rate constants being 15% at all temperatures). The kinetic isotope effect measured independently, k 1 /k 2 = (1.58 ± 0.05) × exp((131 ± 2)/T), was found to be in excellent agreement (within 7% in the temperature range of the work, T = 220-960 K) with the ratio of k 1 to k 2 calculated with the Arrhenius expressions for k 1 and k 2 determined in the study. The kinetic data from the present work are discussed in comparison with previous measurements and theoretical calculations.

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Section: Rate Constant Of Reaction (1): Relative Measurementsmentioning

confidence: 63%

Section: Rate Constant Of Reaction (1): Relative Measurementsmentioning

confidence: 63%

Section: Rate Constant Of Reaction (2)mentioning

confidence: 95%

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Rate constants for the reactions of F atoms with H₂and D₂over the temperature range 220‐960 K

Bedjanian

2020

Int J of Chemical Kinetics

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“…The study adds weight to, or challenges some of the propositions that have been developed by Anderson andTaylor (2007) on the matter of cultural diversity as concerns the socialization of girls. The present study is to be understood together with study conducted by Anderson and Taylor (2007), which have attempted a comparative analysis of girls in different societies. By providing a comparative analysis of the situation, the present study develops a body of information on the similarities and differences with regard to the informal social activities of English girls and Indian girls.…”

Section: Introductionmentioning

confidence: 99%

A comparative study of British and Indian informal activities of girls.

Sukare¹

2021

TURCOMAT

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This research study aims to investigate the informal social activities of youth age girls in England and in India . Culture has been perceived to be the pivot point on which human beings peg their socialization orientation and characterization (Piranha, 2009). However, with the current trends, including globalization and technological advances, it is hypothesized that the world’s youths engage in similar informal activities. This research therefore, tries to prove the hypothesis of whether girls informal activities are the same in a secular society and a closed society; England and India respectively. The aim of this study is to critically examine the similarities and differences between Indian and English young girls with regard to how they spend their free time in their respective countries. It aims to address these issues from a historical as well as current view points and tries to postulate how long the activities will still be pegged on regions and cultural orientations of the society. The research will examine these trends and endeavor to explain the reasons why the differences still exist or what has made them erode. India and England have unique differences in terms of their histories, economic power, level and type of education, cultural orientation, population and lifestyles (Piranha, 2009). This research therefore, attempts to investigate how these themes constitute the development of policies for the young girl. The way children, and girls in particular, are raised in Indian and English societies will be investigated to establish a link between the upbringing and the girls’ future development.

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“…The chemical reaction networks can be considered as Birth-and-Death processes without memory, which are Markov processes in a multidimensional space, this point of view was studied by Anderson [ 9 ] and Van Kampen [ 8 ]. While the roots to formulate properly the CME based on microphysical principles were established by Gillespie [ 6 , 7 ].…”

Section: Introductionmentioning

confidence: 99%

Chemical Kinetics Roots and Methods to Obtain the Probability Distribution Function Evolution of Reactants and Products in Chemical Networks Governed by a Master Equation

Muñoz-Cobo

Berna

2019

Entropy

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In this paper first, we review the physical root bases of chemical reaction networks as a Markov process in multidimensional vector space. Then we study the chemical reactions from a microscopic point of view, to obtain the expression for the propensities for the different reactions that can happen in the network. These chemical propensities, at a given time, depend on the system state at that time, and do not depend on the state at an earlier time indicating that we are dealing with Markov processes. Then the Chemical Master Equation (CME) is deduced for an arbitrary chemical network from a probability balance and it is expressed in terms of the reaction propensities. This CME governs the dynamics of the chemical system. Due to the difficulty to solve this equation two methods are studied, the first one is the probability generating function method or z-transform, which permits to obtain the evolution of the factorial moment of the system with time in an easiest way or after some manipulation the evolution of the polynomial moments. The second method studied is the expansion of the CME in terms of an order parameter (system volume). In this case we study first the expansion of the CME using the propensities obtained previously and splitting the molecular concentration into a deterministic part and a random part. An expression in terms of multinomial coefficients is obtained for the evolution of the probability of the random part. Then we study how to reconstruct the probability distribution from the moments using the maximum entropy principle. Finally, the previous methods are applied to simple chemical networks and the consistency of these methods is studied.

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The Reaction F + H₂→ Hf + H

Cited by 39 publications

References 117 publications

Rate constants for the reactions of F atoms with H₂and D₂over the temperature range 220‐960 K

Rate constants for the reactions of F atoms with H₂and D₂over the temperature range 220‐960 K

A comparative study of British and Indian informal activities of girls.

Chemical Kinetics Roots and Methods to Obtain the Probability Distribution Function Evolution of Reactants and Products in Chemical Networks Governed by a Master Equation

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The Reaction F + H2→ Hf + H

Cited by 39 publications

References 117 publications

Rate constants for the reactions of F atoms with H2and D2over the temperature range 220‐960 K

Rate constants for the reactions of F atoms with H2and D2over the temperature range 220‐960 K

A comparative study of British and Indian informal activities of girls.

Chemical Kinetics Roots and Methods to Obtain the Probability Distribution Function Evolution of Reactants and Products in Chemical Networks Governed by a Master Equation

Contact Info

Product

Resources

About

The Reaction F + H₂→ Hf + H

Rate constants for the reactions of F atoms with H₂and D₂over the temperature range 220‐960 K

Rate constants for the reactions of F atoms with H₂and D₂over the temperature range 220‐960 K