Determining the Rate Law for a Multistep Mechanism
The decomposition of nitrous oxide, N2O, is believed to occur by a two-step mechanism:
N2O(g)→N2(g) + O(g) (slow)
N2O(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?
Chapter 1 Chemistry- known as the study of matter and changes that it undergoes Matter- is anything that occupies space You occupy space therefore you are matter Substance- is a form of matter that has a definite composition Ex: water or gold Qualitative Information- characteristics that are different from each other, mostly physical If...