rate laws are quite simple...
you need to set the up equal to rate, like you did
rate=k[O3] thats it... if you need to calculate it, then you need the mol/L of O3
someone correct me if im wrong.. (thank God i had my notebook next to me)
to find the order of reactants you would need the data of the reaction....
for example, if
initial [O3] is .010 and initial [O1] is .010 and the rate is 1.20x10E-3, then
in another experiment,
initial [O3] is .020 and initial [O1] is .010 and the rate is 2.40x10E-3....
O3 is order 1, and O is order 2.
Hope this helps
sorry for the [O1] thing, but if i put [ O ] it looks like this (look below)