By Peter Harriott
Analyzes rules and strategies for the evaluate, review, and optimization of reactors within the production, chemical, petrochemical, and meals processing industries. Illustrates functional layout strategies, fee equations, and analytical versions for better reactor functionality.
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Additional info for Chemical Reactor Design
B. Determine the reaction order from the initial reaction rates. c. What type of equation is needed to ﬁt these data? What is the signiﬁcance of the different orders? 12) . How well can the decrease in rate constant be accounted for using the simple activation theory of Lindemann? Determine this value of k1 , and compare with the author’s value of 8:88 Â 10À3 secÀ1 . C2 H5 Cl ! 5 The thermal reaction H2 þ Br2 ! 2HBr is thought to proceed by the chain mechanism given here, with appropriate rate constants at 800 K.
For an irreversible bimolecular reaction between molecules that are competitively adsorbed on the same type of sites, the reaction rate depends on the probability that the molecules are on adjacent sites. This probability is approximately proportional to the product of the fractional coverages: As þ Bs ! 23) can also be obtained by considering surface migration of adsorbed species. The reaction rate then depends on the rate of collisions, which is proportional to the product of the surface concentrations.
The rate of recombination of nitrogen atoms and the reaction of nitrogen and oxygen atoms are negligible because of the very low concentration of nitrogen atoms. The initiation and termination are assumed to be very rapid compared to the propagation step, so a pseudo-steady-state concentration is reached: k1 ½M½O2 ¼ k2 ½M½O2 sﬃﬃﬃﬃﬃﬃﬃﬃﬃﬃﬃﬃﬃﬃ k1 ½O ¼ ½O k2 2 Combining Eqs. 33) gives Copyright © 2003 by Taylor & Francis Group LLC ð1:32Þ ð1:33Þ Homogeneous Kinetics ri;NO ¼ 2k3 1=2 k1 ½O2 1=2 ½N2 k2 33 ð1:34Þ Experiments show that Eq.
Chemical Reactor Design by Peter Harriott