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Unformatted text preview: 6. The experimentally determined rate law for the high temperature reduction reaction: 2 NO(g) + 2 H 2 (g) N 2 (g) + 2 H 2 O(g) was found to be Rate = k[NO] 2 [H 2 ]. A proposed reaction mechanism for this reaction is Elementary step 1 2 NO(g) + H 2 (g) N 2 O(g) + H 2 O(g) Elementary step 2 N 2 O(g) + H 2 (g) N 2 (g) + H 2 O(g) Is this mechanism consistent with the stoichiometry of the reaction and with the rate law? If so, what is the rate determining step? 7. A reaction that contributes to smog formation is the combination of oxygen with NO from automobile exhaust.: 2 NO (g) + O 2 (g) 2NO 2 (g) Show that the observed rate law: rate = k [NO] 2 [O 2 ] is consistent with the following proposed mechanism. NO (g) + O 2 (g) NO 3 (g) NO 3 (g) + NO (g) 2NO 2 (g) k 1 k-1 k 2 1 2 (fast) (slow)...
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This document was uploaded on 03/29/2012.
- Spring '10