Solved: Determining the Rate Law for a Multistep

Chapter , Problem 2PE

(choose chapter or problem)

Problem 2PE

Determining the Rate Law for a Multistep Mechanism

The decomposition of nitrous oxide. N20. is believed to occur by a two-step mechanism:

N20(g)→N2(g) + O(g) (slow)

N20(g) + O(g)→N2(g) + O2(g) (fast)

(a) Write the equation for the overall reaction, (b) Write the rate law for the overall reaction.

Ozone reacts with nitrogen dioxide to produce dinitrogen pentoxide and oxygen:

O3(g) + 2 NO2(g)→N2O5(g) + O2(g)

The reaction is believed to occur in two steps:

O3(g) + NO2(g) →NO3(g) + O2(g)

NO3(g) + NO2(g)→N2O5(g)

The experimental rate law is rate = k[O3][NO2]. What can you say about the relative rates of the two steps of the mechanism?