Gh. Duca et al./Chem.J. Mold.. 2008, 3 (1), 22-30The reaction rate can be expressed as follows: w = d[C 2H 4] / dt = w 0– w 2– 2w 4.A wide variety <strong>of</strong> consecutive and consecutive-parallel reactions as such are known. For instance, photochemicalreactions are a significant group <strong>of</strong> reaction that can be related to this mechanism. No more than one particle <strong>of</strong> reactionproduct is formed per one adsorbed light quantum during these reactions.Cyclic reactions proceed according to type II and type III mechanisms. A particular feature <strong>of</strong> such reactions isthe formation <strong>of</strong> a particle in addition to the products. This particle then participates in one <strong>of</strong> the reactions that leadto the formation <strong>of</strong> the product. There are two types <strong>of</strong> cyclic transformations: chain and catalytic. It is important thatreaction rates <strong>of</strong> chain transformations are higher than the rate <strong>of</strong> active particles formation:w = dP/dt = w 0,where is the chain length, shows how many particles <strong>of</strong> P product are formed per active particle which are formedduring the activation stage (0). Reactions are known with 10 5 , but usually 10 - 10 3 .The photolysis <strong>of</strong> H 2O 2in aqueous solutions is one <strong>of</strong> the many examples <strong>of</strong> chain transformations:*0. H 2O 2 H 2O 2 2OH *1. H 2O 2* H 2O 22. OH• + H 2O 2 H 2O + HO 2•3. HO 2• + H 2O 2 H 2O + O 2+ OH•4. HO 2• + HO 2• H 2O 2+ O 2.For the wide majority <strong>of</strong> the studied chain processes, the active particles are atoms and free radicals, and theprocesses are called radical-chain. The lifetime <strong>of</strong> active particles such as OH•, CH 3•, etc. is short due to their highreactivity, and low concentrations, compared to the typical reaction time and reagents’ concentrations. The nonstationaryperiod, where the concentrations <strong>of</strong> active particles increase from zero to stationary values, is usually aroundmilliseconds. The method <strong>of</strong> quasi-stationary concentrations can be applied for most reactions, with regard to activeparticles.The second type <strong>of</strong> cyclic reactions is represented by catalytic reactions, when the activation <strong>of</strong> the reagentproceeds not as a result <strong>of</strong> thermal, photochemical or other influence, but as a result <strong>of</strong> its interaction with the introducedsubstance-catalyst [1]. Due to the fact that the cycle is closed on the link preceding the activation stage, the rate <strong>of</strong> acatalytic reaction cannot be higher than the activation rate <strong>of</strong> the interaction between A and E.Catalytic reactions are similar to chain reactions, considering their cyclic mechanism, and are similar to “simple”fast-reactions <strong>of</strong> type I for the reaction rate does not exceed the rate <strong>of</strong> the reagents activation on their interaction withthe catalyst.The limiting stage for catalytic cycle reactions is the share <strong>of</strong> the catalyst present in the (EA)’ complex; the initialactivation <strong>of</strong> the reagent – EA complex formation – is seldom a limiting stage, in contrast to radical-chain reactions,where the rate <strong>of</strong> the process depends on the initial formation <strong>of</strong> atoms or radicals from the reagent molecules.Taking into account that the most important fast reactions with relevance to chemical and biological systemstake place in liquid media, there are three general factors that are to be considered in case <strong>of</strong> investigating the reactionrates in solution [2,3]:The rate at which initially separated reactant molecules come together and become neighbours, i.e. the rate <strong>of</strong>encounters.The time that two reactants spend as neighbours before moving away from each other, i.e. the duration <strong>of</strong> anencounter. During this time, the reactants may collide with each other hundreds <strong>of</strong> times.The requirement <strong>of</strong> energy and orientation which two neighbouring reactant molecules must satisfy in orderto react.Any one <strong>of</strong> these three factors may dominate in governing the reaction rate.Many chemical reactions occur as soon as the reactant molecules come together and thus, for these fast reactions,the activation energy and orientation requirements are negligible. The reaction rate is limited only by the first factor(i.e., the rate at which encounters occur), which makes it diffusion-controlled.A simple mechanism for these diffusion controlled reactions may be given by the following kinetic scheme:where k dis the rate constant for diffusion <strong>of</strong> A and B towards each other, k -dis the rate constant for diffusion <strong>of</strong> A andB away from each other, and k cis the rate constant for the conversion <strong>of</strong> the complex (AB) to product R (i.e., the rateconstant with out diffusive effects).23
Gh. Duca et al./Chem.J. Mold.. 2008, 3 (1), 22-30Using the Steady-State Approximation on (AB):d[(AB)] 0 kd[ A][B] kdtd[( AB)] k [( AB)] [( AB)](kkrkThus, the reaction velocity is given by the equation: r kr[(AB)]kcdkd[ A][B] kc) kd[ A][B];[( AB)]k kdd[ A][B] kkr kThus, the rate constant <strong>of</strong> the bimolecular reaction A + B 2rkdproducts, is given by: k2 [ A][B]kd krIn this case, two limiting cases should be considered:(i) diffusion-controlled reaction: k r»k -d, separation <strong>of</strong> A and B is relatively difficult, e.g., the solvent has alarge viscosity , or the reaction has a small activation energy, so the rate-determining step is the diffusiveapproach <strong>of</strong> the reactants; once they are in the solvent reaction cage, reaction is assured, k 2= k d(where foraqueous solutions at room temperature, k d 10 9 – 10 10 M -1 s -1 , and a value <strong>of</strong> k d> 10 9 M -1 s -1 usually indicatesthat the aqueous solution reaction is diffusion controlled).(ii) activation-controlled reaction: k r « k -d , reactions with large activation energies, E a 20 kJ mol -1 for reactionskdin water k k2r kdwhere the second factor is the equilibrium constant K ABfor the formation <strong>of</strong> the encounter pair; thus k 2= k rK AB, andthe reaction rate is determined by the equilibrium concentration <strong>of</strong> encounter pairs and the rate <strong>of</strong> passage over theactivation energy barrier.One way to assess the validity <strong>of</strong> the assumption <strong>of</strong> fast <strong>chemistry</strong> is to estimate the Damkohler number [3], animportant dimensionless parameter that quantifies whether a process is kinetically or diffusion controlled. Damkohlernumber is defined as Da mix/ react. Here, mixis a characteristic mixing time for the system, while reacis a characteristictime for the chemical reaction. If the Damkohler number has a value much larger than unity, the process is diffusionallycontrolled, while a value much lower than unity indicates a kinetically controlled process.Another factor which affects the rate <strong>of</strong> reactions in solution involves the effects <strong>of</strong> solvent molecules on themotions <strong>of</strong> reactant molecules.Once two reactant molecules diffuse together, their first collision may not satisfy the energy and orientationrequirements for reaction. The surrounding solvent molecules create a “solvent cage” which inhibits the separation <strong>of</strong>the reactant molecules.This solvent “cage effect” provides the opportunity for the molecules to undergo many more collisions beforefinally either reacting or diffusing away from each other.The duration <strong>of</strong> such an encounter may be 10 -10 s, during which the reactant molecules may collide hundreds <strong>of</strong>times. The cage effect tends to increase the reaction rate by increasing the opportunity for reactant molecules to find therequired energy and/or orientation to react during the caged encounter.However, there are a large number <strong>of</strong> reactions that are initiated by the formation <strong>of</strong> a reactive species in theinvestigated solution, rather than by mixing the reagents. In the case <strong>of</strong> such chemical reactions it has to be taken intoconsideration that the duration <strong>of</strong> the initiation process has to be a lot shorter than the reaction time and it has to beperformed by techniques that would not alter the solution’s homogeneity.The main physical methods that are currently used in the investigation <strong>of</strong> rapid reactions are reviewed below.Basic concepts <strong>of</strong> the methods that are used to study fast reactionsFlow-based MethodsFlow analysis comprises all analytical methods that are based on the introduction and processing <strong>of</strong> test samplesin flowing media. A primary classification can be based on two aspects [4]:- the way the test portion is introduced, i. e. continuously or intermittently/discretely,- the basic character <strong>of</strong> the flowing media, i.e. either segmented, unsegmented or monosegmented wheresegmentation is primarily considered as being applied for the purpose <strong>of</strong> preventing intermixing <strong>of</strong> successive analytezones.However, among all the flow methods used for the study <strong>of</strong> fast reactions the most popular seems to be thestopped-flow method. Due to the short analysis time and feasibility, flow based systems have become one <strong>of</strong> the mostpowerful analytical tools used for studying fast reactions. This can also be explained by the possibility <strong>of</strong> employingmost various detection systems.The apparatus [5] is made <strong>of</strong> 2 reservoir syringes that are loaded with the desired species. A pneumatic syringe pushrdc24
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