The following mechanism has been proposed for the reaction between nitrogen mono

Question

The following mechanism has been proposed for the reaction between nitrogen monoxide and oxygen in the gas phase. step 1 fast: 2 NON202 step 2 slow: N202+02>2NO2 (1) What is the equation for the overall reaction? Use the smallest integer coefficients possible. If a box is not needed, leave it blank (2) Enter the formula of any species that acts as a reaction intermediate? If none leave box blank: (3) Complete the rate law for the overall reaction that is consistent with this mechanism. Use the form k?Alml Bln , where 'l' is understood (so don't write it if it's a 'i') for m, n etc. Rate = Submit Answer Retry Entire Group 8 more group attempts remaining

Explanation / Answer

1)
Overall reaction can be obtained by adding both the steps
After adding:
2 NO + N2O2 + O2 —> N2O2 + 2 NO2
which becomes:
2 NO + O2 —> 2 NO2

Answer: 2 NO + O2 —> 2 NO2

2)
N2O2 is intermediate as this is produced in step 1 and used up in next step

3)
rate depends on the slowest step
Here 2nd step is slowest
So, rate law is:
rate = k2[N2O2][O2]

We need to remove intermediate which is NO3
we will use 1st step:
Kc = [N2O2]/[NO]^2
[N2O2] = Kc[NO]^2

put this in rate law expression above:
rate = k2[N2O2][O2]
rate = k2Kc[NO]^2[O2]

let k2Kc be k
so,
rate law becomes:
rate = k[NO]^2[O2]

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