Question

The following mechanism has been proposed for the reaction between nitrogen monoxide and oxygen in the gas phase.

.....step 1.....fast:......2 NO ---> N₂O₂

.....step 2.....slow:....N₂O₂ + O₂ ----> 2 NO₂

(1) What is the equation for the overall reaction? Use the smallest integer coefficients possible. If a box is not needed, leave it blank.

_______ +

________

_________ + ________

(2)

Enter the formula of any species that acts as a reaction intermediate? If none leave box blank:

________

(3) 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 if it's a '1') for m, n etc.

Rate = ______

Answer 1

(ast) Step o No step N slaw) overall veacton step D step aNo ৪+ ২ NO Oveya eacon aNo intermediate Thg enea lly as PYoduct appeares and disappeaye reactant as Tn this eacdion o appeare 15 Product and disappeares as Yeactant so Tntermediate

Slow step eact Rate law depends on Teactant Concentoations .: Rate = N iSintermediate erom step k' No 2 subsiute in D k'x" No Rate Rate =k [No Rate law 3 Rate