A gas phase reaction between nitrogen dioxide and fluorine is proposed to occur

Question

A gas phase reaction between nitrogen dioxide and fluorine is proposed to occur by the following mechanism: step 1 slow: NO_2 + F_2 rightarrow NO_2F + F step 2 fast: F + NO_2 rightarrow NO_2F What is the equation for the overall reaction? Use the smallest integer coefficients possible. If a box is not needed, leave it blank. Which species acts as a catalyst? Enter formula. If none, leave box blank: Which species acts as a reaction intermediate? Enter formula. If none, leave box blank: Complete the rate law for the overall reaction that is consistent with this mechanism. (Use the form k[A]^m[B]^n ..., where '1' is understood (so don't write it) for m, n etc.)

Explanation / Answer

1. 2NO2 + F2 2NO2F
2. There is no catalyst in the reaction.
3. F is the reaction intermediate.
4. rate = k[NO2][F2]

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