Question

5. Ozone in the atmosphere decomposes by the following reaction: The experimentally observed rate law is Show that this proposed mechanism is consistent with the experimenta 203() 30200) Os)02)+ 0 (a) Os(a)+Oa) 200) Fast Slow

Answer 1

rate depends on the slowest step

Here 2nd step is slowest

So, rate law is:

rate = k2[O3][O]

We need to remove intermediate which is O

we will use 1st step:

Kc = [O2][O]/[O3]

[O] = Kc[O3][O2]-1

put this in rate law expression above:

rate = k2[O3][O]

rate = k2[O3]Kc[O3][O2]^-1

let k2Kc be k

so,

rate law becomes:

rate = k[O3]²[O2]^-1

Hence proved