Without doing any calculations prove that you have

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Unformatted text preview: ithout doing any calculations, prove that you have enough information about the process to determine these quantities. (b) Perform the calculations. (c) Why would benzene be fed in excess and the fractional conversion kept low? (d) What might be done with the gaseous effluent? (e) It is possible to use 99.9% pure (“reagent-grade”) chlorine instead of the technical grade actually used in the process. Why is this probably not done? Under what conditions might extremely pure reactants be called for in a commercial process? (Hint: Think about possible problems associated with the impurities in technical grade chemicals.) SOLUTION (a) The answers to these questions can only be done in terms of the number of moles, so we will need to convert all of the mass units to molar units. To do this use the following molecular weights: MWC6H6 = 78,MWC6H5Cl = 112.5, MWC6H4Cl2 = 146.9, and MWC6H3Cl3 = 181.5. Using this information we can convert to mole fractions via the table shown below. Com...
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This note was uploaded on 03/01/2013 for the course CHEME 2171 taught by Professor Benton during the Spring '12 term at LSU.

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