Suppose the decomposition of nitrogen dioxide proceeds by the following mechanism:
step elementary reaction rate constant
1 NO2 (g) → NO (g) + O (g) k1
2 O (g) + NO2 (g) → O2 (g) + NO (g) k2
Suppose also k1>>k2. That is, the first step is much faster than the second.
(a) Write the balanced chemical equation for the overall chemical reaction.
(b) Write the experimentally-observable rate law for the overall chemical reaction. Note: your answer should not contain the concentrations of any intermediates.
(c) Express the rate constant k for the overall chemical reaction in terms of k1, k2, and (if necessary) the rate constants k.1 and k.2 for the reverse of the two elementary reactions in the mechanism.