Nitrous di-oxide reacts with ozone to form nitrogen tri-oxide and oxygen. This reaction is described by the following equation:

NO2 + O3

NO3 + O2

The reaction was studied at 45^oC and the data in the table were collected.

[NO2]	[O3]	Initial rate of reaction (M sec-1)
1.17	1.16	0.0456
0.39	0.58	0.0228
0.13	0.29	0.0114
1.17	0.58	0.0228

The rate law for the reaction can be written as: rate = k[NO₂]^x.[O₃]^y

Determine the orders x and y and calculate the rate constant k. Enter these values in the boxes below and select the correct units for the rate constant.

x =

y =

k =

mol-3 L3 sec-1 mol-1 L sec-1 sec sec-1 mol-2 L2 sec-1