Nitramide, NO 2 NH 2 , decomposes slowly in aqueous solution according to the following reaction: The

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Nitramide, NO2NH2, decomposes slowly in aqueous solution according to the following reaction:NONH(aq)  NO(g) + HO(l)

The reaction follows the experimental rate lawRate k[NONH] [H3O+]

(a) What is the apparent order of the reaction in a pH buffered solution? (In a pH buffered solution, the concentration of H3O+ is a constant.)
(b) Which of the following mechanisms is the most appropriate for the interpretation of this rate law? Explain.
Mechanism 1

NO,NH, k N2O + H2O

Mechanism 2R NONH + H3O+NONH3+ k' NONH3 + k3 NO + H3O+ + HO (rapid equilibrium) (rate-limiting step)

Mechanism 3k4 NO,NH, + H,O

(c) Show the relationship between the experimentally observed rate constant, k, and the rate constants in the selected mechanism.
(d) Based on the experimental rate law, will the reaction rate increase or decrease if the pH of the solution is increased?

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Chemistry And Chemical Reactivity

ISBN: 9780357001172

10th Edition

Authors: John C. Kotz, Paul M. Treichel, John Townsend, David Treichel

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