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Use the References to access important values if needed for this question. A proposed mechanism for the gas phase reaction between nitrogen monoxide and oxygen is as follows step 1 fast: NO+02 NO3 step 2 slow: NO3 + NO ? 2 NO2 (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 klA]"[B]"... where'' is understood (so don't write it if it's a '1') 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:
NO + O2 + NO3 + NO —> NO3 + 2 NO2
which becomes:
2 NO + O2 —> 2 NO2

Answer: 2 NO + O2 —> 2 NO2

2)
NO3 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[NO3][NO]

We need to remove intermediate which is NO3
we will use 1st step:
Kc = [NO3]/[NO][O2]
[NO3] = Kc[NO][O2]

put this in rate law expression above:
rate = k2[NO3][NO]
rate = k2Kc[NO][O2][NO]

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

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