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Unformatted text preview: Consider the gas phase reaction of nitric oxide with chlorine to form nitrosyl chloride, NOCl: 2 NO ( g ) + Cl 2 2 NOCl ( g ) The experimentally determined rate law for this reaction is: rate = k [NO] 2 [Cl 2 ]. Although this rate law is consistent with a one-step, termolecular (three molecule) reaction, a simultaneous collision among three molecules is not very probable. An alternative pathway has been proposed where the first step is: NO ( g ) + Cl 2 NOCl 2 ( g ) a fast equilibrium (note the product is NOCl 2 , not NOCl) a) Propose a second, rate-limiting step that is consistent with the overall stoichiometry of the reaction. b) What overall rate law would be predicted for your new, two-step pathway? Explain why. c) Describe an experiment that would allow you distinguish between the one-step pathway (rate law) and your proposed two-step pathway? (How could you differentiate between the two in lab?) 1....
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This note was uploaded on 05/15/2011 for the course CHM 116 taught by Professor Matchett during the Fall '11 term at Grand Valley State University.
- Fall '11