Determine the overall orders of the reactions to which the following rate laws apply:

a) rate= k[NO2]^2
b) rate = k
c) k [H2][Br2]^1/2
d) k [NO]^2[O2]

is it..
a. 2
b. 0
c. 1 1/2
d. 3

All are correct. Very good.

To determine the overall orders of the reactions, you need to sum up the individual orders of each reactant in the rate law. The overall order represents the sum of all the individual orders.

a) rate = k[NO2]^2
In this case, the rate law indicates that the reaction is second order with respect to the reactant NO2. Therefore, the overall order of this reaction is 2.

b) rate = k
The rate law is independent of the concentration of any reactants and only depends on the rate constant k. Thus, the reaction is zero order overall.

c) rate = k[H2][Br2]^1/2
This rate law shows that the reaction is first order with respect to the reactant H2 and the square root of the concentration of Br2.

As for the Br2 concentration, since it is raised to the power of 1/2 or square root, it contributes only 1/2 order.

So, the overall order of this reaction is 1 + 1/2 = 1 1/2.

d) rate = k[NO]^2[O2]
The rate law indicates that the reaction is second order with respect to the reactant NO and first order with respect to O2.

Summing up the individual orders, the overall order of this reaction is 2 + 1 = 3.

Therefore, the correct answers are:
a) 2
b) 0
c) 1 1/2
d) 3