Rate predictions

Although the Arrhenius equation does not predict rate constants without parameters obtained from another source, it does predict the temperature dependence of reaction rates. The Arrhenius parameters are often obtained from experimental kinetics results since these are an easy way to compare reaction kinetics. The Arrhenius equation is also often used to describe chemical kinetics in computational fluid dynamics programs for the purposes of designing chemical manufacturing equipment, such as flow reactors. Many computational predictions are based on computing the Arrhenius parameters. [Pg.164]

To a first approximation, the activation energy can be obtained by subtracting the energies of the reactants and transition structure. The hard-sphere theory gives an intuitive description of reaction mechanisms however, the predicted rate constants are quite poor for many reactions. [Pg.166]

UFF (universal force field) a molecular mechanics force field unrestricted (spin unrestricted) calculation in which particles of different spins are described by different spatial functions VTST (variational transition state theory) method for predicting rate constants... [Pg.369]

Both Eqs. (5.9) and (5.10) predict rate laws which are first order with respect to the concentration of each of the reactive groups the proportionality constant has a different significance in the two cases, however. The observed rate laws which suggest a reactivity that is independent of molecular size and the a priori expectation cited in item (5) regarding the magnitudes of different kinds of k values lend credibility to the version presented as Eq. (5.9). [Pg.282]

The coordinates of thermodynamics do not include time, ie, thermodynamics does not predict rates at which processes take place. It is concerned with equihbrium states and with the effects of temperature, pressure, and composition changes on such states. For example, the equiUbrium yield of a chemical reaction can be calculated for given T and P, but not the time required to approach the equihbrium state. It is however tme that the rate at which a system approaches equihbrium depends directly on its displacement from equihbrium. One can therefore imagine a limiting kind of process that occurs at an infinitesimal rate by virtue of never being displaced more than differentially from its equihbrium state. Such a process may be reversed in direction at any time by an infinitesimal change in external conditions, and is therefore said to be reversible. A system undergoing a reversible process traverses equihbrium states characterized by the thermodynamic coordinates. [Pg.481]

To test the model, first check against experimental values within the design. Second, check against rates not involved in the design. Third, predict rates and execute experiments to check the results. [Pg.142]

These examples illustrate the relationship between kinetic results and the determination of reaction mechanism. Kinetic results can exclude from consideration all mechanisms that require a rate law different from the observed one. It is often true, however, that related mechanisms give rise to identical predicted rate expressions. In this case, the mechanisms are kinetically equivalent, and a choice between them is not possible on the basis of kinetic data. A further limitation on the information that kinetic studies provide should also be recognized. Although the data can give the composition of the activated complex for the rate-determining step and preceding steps, it provides no information about the structure of the intermediate. Sometimes the structure can be inferred from related chemical experience, but it is never established by kinetic data alone. [Pg.199]

The complex directive effects in radical addihons have been reviewed, and rules for predicting rates and regiochcmistry have been developed [154 755]... [Pg.1000]

So far in this chapter we have approached reaction rate from an experimental point of view, describing what happens in the laboratory or the world around us. Now we change emphasis and try to explain why certain reactions occur rapidly while others take place slowly. To do this, we look at a couple of models that chemists have developed to predict rate constants for reactions. [Pg.298]

The most popular methods are the Q-e (Section 7.3.4.1) and Patterns of Reactivity schemes (Section 7.3.4.2). Both methods may also be used to predict transfer constants (Section 6.2.1). For furtherdiscussionontheapplicationofthe.se and other methods to predict rate constants in radical reactions, see Section 2.3.7. [Pg.363]

Finally the success of the model can be judged from Figures 6.25a and b which show the experimental and model-predicted rate dependence on pCo and work function during CO oxidation on Pt/pM-Al203.71 Note the transition from a classical Langmuir-Hinshelwood to a positive order rate dependence on pco with decreasing work function. Also notice that on every point of the experimental or model predicted rate dependence, the basic promotional mle ... [Pg.326]

The goal is to determine a functional form for (a, b,. .., T) that can be used to design reactors. The simplest case is to suppose that the reaction rate has been measured at various values a,b,..., T. A CSTR can be used for these measurements as discussed in Section 7.1.2. Suppose J data points have been measured. The jXh point in the data is denoted as S/t-data aj,bj,..., Tj) where Uj, bj,..., 7 are experimentally observed values. Corresponding to this measured reaction rate will be a predicted rate, modeii p bj,7 ). The predicted rate depends on the parameters of the model e.g., on k,m,n,r,s,... in Equation (7.4) and these parameters are chosen to obtain the best fit of the experimental... [Pg.210]

Predicting Rates of Decomposition of Free-Radical Initiators... [Pg.416]

The rates of radical-forming thermal decomposition of four families of free radical initiators can be predicted from a sum of transition state and reactant state effects. The four families of initiators are trarw-symmetric bisalkyl diazenes,trans-phenyl, alkyl diazenes, peresters and hydrocarbons (carbon-carbon bond homolysis). Transition state effects are calculated by the HMD pi- delocalization energies of the alkyl radicals formed in the reactions. Reactant state effects are estimated from standard steric parameters. For each family of initiators, linear energy relationships have been created for calculating the rates at which members of the family decompose at given temperatures. These numerical relationships should be useful for predicting rates of decomposition for potential new initiators for the free radical polymerization of vinyl monomers under extraordinary conditions. [Pg.416]

Working with rats, Lntz et al. (1977) compared the rates of loss from blood of 4,-CB (rapidly metabolized) with that of 2,2, 4,4, 5 -HCB (slowly metabolized). Both showed biphasic elimination, with the former disappearing much more rapidly than the latter. Estimations were made of the rates of hepatic metabolism in vitro, which were then incorporated into toxicokinetic models to predict rates of loss. The predictions for HCB were very close to actual rates of loss for the entire period of... [Pg.139]

We now study the consequences of these BEP choices to the dependence of predicted rate of methane production on Eads- Making the additional simplifying assumption that the adsorption energy parameters in Eqs. (1.9b) and (1.9c) are the same, one finds for the rate of methane production an expression... [Pg.11]

The first step in Mechanism I is the unimolecular decomposition of NO2. Our molecular analysis shows that the rate of a unimolecular reaction is constant on a per molecule basis. Thus, if the concentration of NO2 is doubled, twice as many molecules decompose in any given time. In quantitative terms, if NO2 decomposes by Mechanism I, the rate law will be Predicted rate (Mechanism I) = [N02 ] Once an NO2 molecule decomposes, the O atom that results from decomposition very quickly reacts with another NO2 molecule. [Pg.1063]

The rate-determining step of Mechanism II is a bimolecular collision between two identical molecules. A bimolecular reaction has a constant rate on a per collision basis. Thus, if the number of collisions between NO2 molecules increases, the rate of decomposition increases accordingly. Doubling the concentration of NO2 doubles the number of molecules present, and it also doubles the number of collisions for each molecule. Each of these factors doubles the rate of reaction, so doubling the concentration of NO2 increases the rate for this mechanism by a factor offour. Consequently, if NO2 decomposes by Mechanism II, the rate law will be Predicted rate (Mechanism n) = < [N02][N02] = J [N02] ... [Pg.1063]

The two proposed mechanisms for this reaction predict different rate laws. Whereas Mechanism I predicts that the rate is proportional to NO2 concentration. Mechanism II predicts that the rate is proportional to the square of NO2 concentration. Experiments agree with the prediction of Mechanism II, so Mechanism II is consistent with the experimental behavior of the NO2 decomposition reaction. Mechanism I predicts rate behavior contrary to what is observed experimentally, so Mechanism I cannot be correct. [Pg.1063]

When the first step of a mechanism is rate-determining, the predicted rate law for the overall reaction is the rate law for that first step. [Pg.1083]

The predicted rate law is first order for a reaction whose first step is unimolecular and rate-determining. The predicted rate law is second order overall for a reaction whose first step is bimolecular and rate-determining. For example, the first step of the mechanism for the C5 Hi 1 Br reaction is unimolecular and slow, so the rate law... [Pg.1083]

What is the predicted rate law for each of these mechanisms ... [Pg.1084]

Mechanism I is a three-step process in which the first step is rate-determining. When the first step of a mechanism is rate-determining, the predicted rate law is the same as the rate expression for that first step. Here, the rate-determining step is a bimolecular collision. The rate expression for a bimolecular collision is first order in each collision partner Rate = j i[03 ][N0 j Mechanism I is consistent with the experimental rate law. If we add the elementary reactions, we find that it also gives the correct overall stoichiometry, so this mechanism meets all the requirements for a satisfactory one. [Pg.1089]

Mechanism III is a simple one-step bimolecular collision. Its predicted rate law is as follows ... [Pg.1089]

Derive the predicted rate law for the general mechanism for enzyme catalysis, assuming that the distortion... [Pg.1114]

In SIMCA, we can determine the modelling power of the variables, i.e. we measure the importance of the variables in modelling the elass. Moreover, it is possible to determine the discriminating power, i.e. which variables are important to discriminate two classes. The variables with both low discriminating and modelling power are deleted. This is more a variable elimination procedure than a selection procedure we do not try to select the minimum number of features that will lead to the best classification (or prediction rate), but rather eliminate those that carry no information at all. [Pg.237]

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