Iodine oxidation by hydrogen peroxide and Bray–Liebhafsky oscillating reaction: effect of the temperature

Chemical Physics Letters

2019

Section: Introductionmentioning

confidence: 56%

I2O in solution and volatility

Furrow

Chemical Physics Letters

2019

“…We now discuss the consequences of this assumption on the model of the Bray–Liebhafsky (BL) oscillating reaction . This model contains the following reactions:

{2 IO}_{2} H ⇌ {normalI}_{2} {normalO}_{3} + {normalH}_{2} O

{normalI}_{2} {normalO}_{3} + {normalH}_{2} {normalO}_{2} \to {IO}_{3}^{-} + H^{+} + {IO}_{2} H

{normalI}_{2} {normalO}_{3} + {normalH}_{2} O \to {IO}_{3}^{-} + H^{+} + IOH

…”

Section: Discussionmentioning

confidence: 99%

“…The rate constants of reactions (R2)–(R4) are taken from previous works : k 2 = 200 M −1 s −1 , k –2 = 1300 M −3 s −1 , k 3 = 4 × 10 9 M −2 s −1 , k –3 = 25 M −1 s −1 , k 4 = 1.8 × 10 9 M −1 s −1 , and k –4 = 1.7 × 10 −3 M s −1 . Reaction (R1) is the sum of (R2) and (R3), so that K 1 = K 2 K 3 and k –1 / k 1 = k –2 k –3 / k 2 k 3 (see discussion in the Supporting Information).…”

Section: Numerical Integrationsmentioning

confidence: 99%

Kinetics of Iodous Acid Disproportionation

Int J of Chemical Kinetics

Furrow

2013

Self Cite

The iodous acid disproportionation is autocatalytic, and it is not easy to measure the rate constant of the step 2IO 2 H → IO 3 − + IOH + H + separately. Hg(II) was used previously to suppress the autocatalytic pathway, but this method presents difficulties discussed in this work. A more effective method is the use of crotonic acid, an effective IOH scavenger. It suppresses side reactions, and a purely second-order rate law is obtained. The rate constant decreases from 5 to 0.2 M −1 s −1 when the sulfuric acid concentration increases from 0.08 to 0.60 M. The observed decrease could be explained if IO 2 − reacts faster than IO 2 H. This may have consequences for the mechanism of the oscillating Bray-Liebhafsky reaction. C 2013

“…During the oscillating Bray-Liebhafsky reaction, reactions (7)(8)(9) can occur alternately in one direction then in the other [16][17][18][19]. Their sum is the reversible quasi-elementary reaction (12).…”

Section: Consider Now a Quasi-element Ar Y Reactionmentioning

confidence: 99%

Fundamental concepts in chemical kinetics

Lente

2019

ChemTexts

Self Cite

Students and young researchers will find in this article a clear and accurate presentation of fundamental concepts in chemical kinetics: reaction rates, elementary reactions and mechanisms, kinetic constants and relation to thermodynamics, and energies of activation. The discussions are based on specialized literature without going into detail and avoid misunderstandings and sometimes errors found in the general literature and on the Internet. With this aim, an original approach is sometimes adopted.