Question

The data below were collected for the following reaction:
2NO2 (g) + F2 (g) ->2NO2F(g)

A: Calculate the value of the rate constant, k.

B: What is the overall order of the reaction?

Answer 1

No data.

Answer 2

Here is the data. I am sorry that I forgot to list it:

Initial Rate
[NO2](M) [F2](M) Initial Rate (M/s)
0.100 0.100 0.026
0.200 0.100 0.051
0.200 0.200 0.103
0.400 0.400 0.411

Answer 3

Initial Rate
[NO2](M) [F2](M) Initial Rate (M/s)
0.100 0.100 0.026
0.200 0.100 0.051
0.200 0.200 0.103
0.400 0.400 0.411


When the concentration of NO2 is doubled from line 1 to line 2, the rate doubles. When the concentration of F2 doubles from line 2 to line 3, the rate doubles, so 2^n=2 and 2^m=2

So, n=1 and m=1

rate=k[NO2][F2]

Taking the data from line 1, solve for k

0.026=k[0.1][0.1]

k=(0.026)/([0.1][0.1])