Question

The following initial rate data are for the reaction of nitrogen monoxide with ozone at 25 ^oC:

NO + O₃ ---->NO₂ + O₂

Experiment	[NO]o, M	[O3]o, M	Initial Rate, Ms-1
1	0.164	2.56×10-2	0.395
2	0.164	5.12×10-2	0.789
3	0.327	2.56×10-2	0.787
4	0.327	5.12×10-2	1.57

Complete the rate law for this reaction in the box below.
Use the form k[A]^m[B]ⁿ , where '1' is understood for m or n and concentrations taken to the zero power do not appear. Don't enter 1 for m or n

Rate =

From these data, the rate constant is M^-1s^-1.

Answer 1

As we can see when [no] is kept constant and [O3] is doubled the rate is increased by two fold and when the [O3] is kept constant and [NO] is doubled the rate is again increased by two fold But when botht the concentrations are doubled the rate incresed by four fold.

Hence it indicates that the reaction is overall second order and first order in NO and O3. The rate equation is

Rate = k[NO] k[O3]

and the unit of overall rate constant for second order rate equation is M-1s-1