Irreversible Second-Order Reaction In the case where the reactants A and B are [Pg.34]

Irreversible second-order reactions A + B C + D, small scale [Pg.127]

Irreversible second-order reaction A - - B large scale [Pg.129]

An irreversible second-order reaction in the liquid phase 2A P [Pg.43]

Slow irreversible second-order reaction in the bulk liquid, with C o 0 (Section II,B,2) [Pg.19]

For an irreversible second-order reaction to which eqn. (13) applies, integration of the design equation, again assuming isothermal conditions, yields [Pg.68]

For an irreversible second-order reaction, the optimization of the reaction temperature and feed rate can be performed by using the following equation [14] [Pg.172]

Application 8.1. Irreversible second-order reactions, small scale [Pg.127]

Another class of irreversible second-order reactions obeys the rate law r = k[A][B] [Pg.51]

Application 8.2. Irreversible second-order reaction, large scale [Pg.129]

For a graph of an irreversible second order reaction with a single reactant of the form 2A —> products rate = kJiA]2 [Pg.32]

We again consider the irreversible second-order reaction [Pg.50]

Other Correlations for an Irreversible Second-Order Reaction [Pg.16]

Solutions for two types of irreversible second-order reaction are presented in Table 9.5. The first (second-order reaction (a)) is a [Pg.321]

This discussion applies to an irreversible second-order reaction. For reversible reactions the relationships are more complex and are discussed in the texts by Sherwood et al. (1975) and by Danckwerts (1970). [Pg.12]

If the rate-limiting step in an irreversible second-order reaction to produce P from reactants A and B is the collision of single molecules of A and B, then the reaction rate should be proportional to the concentrations (C) of A and B that is, (kmolm 3) and Cg (kmolm ). The rate of reaction can be given as [Pg.28]

Transient absorption of gas, followed by irreversible second-order reaction, has been studied extensively by Brian et al. (B26) and Danckwerts (Dl). The average rate of absorption for a contact time d is also given in terms of the enhancement factor [Pg.15]

T iming to Danckwerts model, we observe that irreversible second-order reactions are not conveniently dealt with except where the reaction is pseudo-first-order based on component A. In this case (D2), it is found for [Pg.15]

Derive an integrated rate equation similar to Equation 3.22 for the irreversible second-order reaction, when reactants A and B are introduced in the stoichiometric ratio [Pg.43]

Let s calculate the time necessary to achieve a giwn conversion X for the irreversible second-order reaction [Pg.149]

The use of the PDF is best illustrated by use of a simple example for a single irreversible second order reaction at isotherm conditions, defined by [Pg.712]

Figure 5 shows concentration profiles that commonly occur when solute A undergoes an irreversible second-order reaction with component B, dissolved in the liquid, to give product C, [Pg.11]

In a previous work ( 5), the film theory was used to analyze special cases of gas absorption with an irreversible second-order reaction for the case involving a volatile liquid reactant. Specifically, fast and instantaneous reactions were considered. Assessment of the relative importance of liquid reactant volatility from a local (i.e., enhancement) and a global (i.e., reactor behavior) viewpoint, however, necessitates consideration of this problem without limitation on the reaction regime. [Pg.96]

The type of chemical system that has received the most attention is the one in which the dissolved gas (component A) undergoes an irreversible second-order reaction with a reactant (component B) dissolved in the liquid. For the present, the gas will be taken as consisting of pure A, so that complications arising from gas film resistance can be avoided. The stoichiometry of the reaction is represented by [Pg.7]

The occurrence of steady-state multiplicity in gas-liquid CSTRs has been demonstrated in experimental (9) and theoretical investigations (cf., 10). The irreversible second-order reaction system, in particular, has been treated extensively in several theoretical studies (10-15). These studies are however based on neglecting energy and material losses which result from evaporation of the liquid. [Pg.99]

Section 5.1 shows how nonlinear regression analysis is used to model the temperature dependence of reaction rate constants. The functional form of the reaction rate was assumed e.g., St = kab for an irreversible, second-order reaction. The rate constant k was measured at several temperatures and was fit to an Arrhenius form, k = ko exp —Tact/T). This section expands the use of nonlinear regression to fit the compositional and temperature dependence of reaction rates. The general reaction is [Pg.209]

There are two other limiting forms of these equations that are also of interest. If k 1 k2, the first step is very rapid compared to the second, so that it is essentially complete before the latter starts. The reaction may then be treated as a simple irreversible second-order reaction with the second step being rate limiting. On the other hand, if k2 ku the first step controls the reaction so the kinetics observed are those for a single second-order process. However, the analysis must take into account the fact that in this case 2 moles of species A will react for each mole of B that is consumed. [Pg.156]

Some specific aspects in the modeling of gas-liquid continuous-stirred tank reactors are considered. The influence of volatility of the liquid reactant on the enhancement of gas absorption is analyzed for irreversible second-order reactions. The impact of liquid evaporation on the behavior of a nonadiabatic gas-liquid CSTR where steady-state multiplicity occurs is also examined. [Pg.96]

The simplest case of parallel second-order steps is that of formation of two different dimers of a reactant A, corresponding to the network 5.23 and rate equations 5.24 (see next page). At all times, both products are formed in the same ratio rP rQ = kAP kAQ, so that the decay of A is an ordinary second-order reaction with rate coefficient k = kAP + kAQ. Likewise, the product formations are ordinary second-order reactions. (One could think of the initial amount of A as divided into two portions in the ratio kAP.kAQ that react independently of one another, one to P and the other to Q.) All equations and plots for irreversible second-order reactions thus are valid (see Section 3.3.1). [Pg.105]

See also in sourсe #XX -- [ Pg.317 ]

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