431_2 - 754 773 789 803 810 827 837 k(1/s 0.15 0.273 0.333...

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MICHIGAN STATE UNIVERSITY CHE 431 Chemical Reaction Engineering Fall 2007 Homework 2 Due Sept. 12, 2007 1. There are two reactors of equal volume available for your use: one a CSTR, the other a PFR. The reaction is second order { – r A = kC A 2 = kC A0 2 (1-X) 2 }, irreversible, and is carried out isothermally. A Æ B There are three ways you can arrange your system: (1) Reactors in series: CSTR followed by PFR (2) Reactors in series: PFR followed CSTR (3) Reactors in parallel with half the feed rate going to each reactor after which the exit streams are mixed (a) Which configuration gives the highest overall conversion? (b) Which configuration gives the lowest overall conversion? 2. For the thermal cracking of ethane in a tubular reactor, the following data were obtained for the rate coefficient at different reference temperatures: T (C) 702 725 734
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Unformatted text preview: 754 773 789 803 810 827 837 k (1/s) 0.15 0.273 0.333 0.595 0.923 1.492 2.138 2.718 4.137 4.665 Determine the corresponding activation energy and frequency factor. 3. For each of the following reactions and rate laws at low temperatures, suggest a rate law at high temperature. The reactions are highly exothermic and therefore reversible at high temperatures. (a) The reaction A Æ B is irreversible at low temperature, and the rate law is – r A = k C A (b) The reaction A + 2B Æ 2D is irreversible at low temperature, and the rate law is – r A = k C A 0.5 C B (c) The catalytic reaction A + B Æ C + D is irreversible at low temperature, and the rate law is – r’ A = k P A P B / (1 + K A P A + K B P B ) In each case, make sure that the rate laws at high temperature are thermodynamically consistent at equilibrium....
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This note was uploaded on 05/21/2008 for the course CHE 431 taught by Professor Christinachan during the Fall '07 term at Michigan State University.

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431_2 - 754 773 789 803 810 827 837 k(1/s 0.15 0.273 0.333...

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