NO can be oxidized into NO2 in air as: 2NO+O2 ? 2NO2. The...

NO can be oxidized into NO2 in air as: 2NO+O2 ? 2NO2. The mechanism of this reaction is following: 2NO ? N2O2 (fast) (with k1 over k-1) N2O2 + O2 ? 2NO2 (slow) (with k2) (a) Derive the rate law of this reaction. (b) In most reactions, the reaction speed is increased at higher temperature. However, this reaction is faster at lower temperatures. Give possible explanation.

Given the overall reaction: 2NO2 (g) → 2NO (g) + O2 (g) and reaction mechanism: NO2 (g) → N (g) + O2 (g) N (g) + NO2 (g) → N2O2 (g) N2O2 (g) → 2NO (g) Pick the two true statements below.: 1. If the first elementary step is the slowest step, the reaction rate is first order in terms of nitrogen dioxide. 2. The nitrogen atoms in the reaction mechanism are an example of a homogeneous catalyst. 3. The reaction mechanism is not valid because the elementary steps do not sum to produce the overall reaction. 4. From the overall reaction equation, we know that the rate must be second order in terms of nitrogen dioxide. 5. There is one reaction intermediate in the reaction mechanism. 6. If the second step is the slowest step, the reaction is first order in terms of oxygen. 7. Even if the elementary reactions sum to produce the overall reaction and the observed rate equals the predicted rate (from the reaction mechanism), the reaction mechanism may still not be valid.

Adi S.

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