The data below were colected for the following reaction: 2NO2(g) + F2(g) --> 2NO

Question

The data below were colected for the following reaction:

2NO2(g) + F2(g) --> 2NO2F (g)

Rate= k[NO2][F2]

Calculate the value of the rate constant, k.

and

What is the overall orfer of the reaction?

[NO2] (M) [F2] (M) (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 The data below were colected for the following reaction: 2NO2(g) + F2(g) --> 2NO2F (g) Rate= k[NO2][F2] Calculate the value of the rate constant, k. and What is the overall orfer of the reaction?

Explanation / Answer

The rate determining step is the slowest step which is step 2.

Since the coefficient of N2O2 is 1 ,that is, there is a 1 before N2O2(it's not shown but you should know that N2O2 means 1N2O2 ) therefore the exponent of [N2O2] will be 1 in the rate law, and since O2 has the coefficient 1 the exponent of [O2] will also be 1 in the rate law.

Rate=k[N2O2]^1[O2]^1=k[N2O2][O2]

However we have a problem, in the net reaction there is no N2O2 so we need to get rid of N2O2 in the rate law. We do this by noting that the first step is an equilibrium which essentially means 2NO=N2O2 so we go back to step 2.

N2O2+O2?2NO2(slow)
and now we replace N2O2 with 2NO
2NO+O2?2NO2
Now because the coefficient of NO is 2, that is, there's a 2 in front of NO, [NO] will have the exponent 2 and since O2 has the coefficient 1, it will have the exponent 1.

Rate=k[NO]^2[O2]^1
Rate=k[NO][O2]

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