Consider this initial-rate data at a certain temperature for the reaction described by N2O3 (

g. - > NO (

g. + NO2 (

g. N2O3 (M) =.1 (initial rate =.66) =.2 (initial rate = 1.32) =.3 (initial rate = 1.98) find k?

N2 O3 (g) →NO (g) + NO2 (g)

[ N2 O3 ] Initial Rate

0.1 M r (t) = 0.66 M/s

0.2 M r (t) = 1.32 M/s

0.3 M r (t) = 1.98 M/s

We can have the relationship:

([ N2 O3 ] / [ N2 O3 ] 0) ^m = r (t) / r0 (t)

However,

([N2O3]/[N2O3]0) = 2

Also, we assume m=1 which is the order of the reaction.

Thus, the relationship is simplified to,

r (t) / r0 (t) = 2

r (t) = k [ N2 O3 ]

0.66 M/s=k*0.1 M

k=6.6 s - 1