Chemical Engineering

Download Chemical Reactor Design by Peter Harriott PDF

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By Peter Harriott

Analyzes rules and strategies for the review, evaluation, and optimization of reactors within the production, chemical, petrochemical, and meals processing industries. Illustrates useful layout systems, expense equations, and analytical versions for better reactor functionality.

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C s ! C þ s kPA KA PB r ¼ kA PB ¼ 1 þ PA KA þ PC KC ð2:26Þ This model was proposed by Rideal and Eley [4,5] as an alternative to the Langmuir–Hinshelwood models. 6. 6 Reaction rates for Eley–Rideal kinetics. a Langmuir–Hinshelwood reaction between adsorbed reactants. Going back to Eq. 24), if B and D are very weakly adsorbed and A and C are moderately adsorbed, the rate equation becomes rffi kKA PA KB PB ð1 þ KA PA þ KC PC Þ2 ð2:27Þ If the values of PA are not large enough to make the rate go through a maximum, the kinetic data could probably be fitted with either Eq.

Typical data for hydrogenation of olefins or aromatics can often be fitted quite well by several different models. When data are available from a differential reactor, the models can be tested using reciprocal plots similar to those used for Langmuir isotherms. 1 The kinetics of benzene hydrogenation to cyclohexane over a Ni=SiO2 catalyst were studied using a small fixed-bed reactor [7]. 2 g of glass beads. 1. What reaction models give good fit to these data? Solution. 85-fold increase in PH2 increases the rate only 18%, and a four-fold increase in PB increases the rate about 40%.

From the intercept, 1=Vm ¼ 14:5  103 , Vm ¼ 6:9  10À5 mol=L-sec. 25). Testing for Michaelis–Menton kinetics: (a) Eq. 24); (b) Eq. 5 are initial rate data obtained at different substrate concentrations. If only batch data are available, an integrated form of the rate equation is needed. For a batch reaction with initial concentration [S0] and [E0], the reaction rate is the rate of change of concentration: d½SŠ Vm ½SŠ ¼ r¼À dt Km þ ½SŠ ð ð Àd½SŠðKm þ ½SŠÞ ¼ Vm dt ½SŠ ½S0 Š þ ½S0 Š À ½SŠ ¼ Vm t Km ln ½SŠ ð1:26Þ ð1:27Þ ð1:28Þ Dividing by t and Km gives a convenient form for plotting: 1 ½S0 Š ½S0 Š À ½SŠ Vm ¼ ln þ Km t ½SŠ K t  m  1 1 V S ln ¼ mÀ 0 Km Km t t 1Àx ð1:29Þ ð1:30Þ Chain Reactions Chain reactions take place via a series of steps involving intermediates that are continually reacting and being regenerated in a cyclical process.

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