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?
3 answers
No data.
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
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
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])
[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])
0 answers