The following mechanism has been proposed for the gas phase reaction of nitrogen
ID: 1039110 • Letter: T
Question
The following mechanism has been proposed for the gas phase reaction of nitrogen monoxide with bromine. step 1 fast: NO+ Br2NOBr2 step 2 slow: NOBr2+NO2 NOBr (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[A]"[B]".. , where 'l' 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 NextExplanation / Answer
1)
Overall reaction can be obtained by adding both the steps
After adding:
NO + Br2 + NOBr2 + NO —> NOBr2 + 2 NOBr
which becomes:
2 NO + Br2 —> 2 NOBr
Answer: 2 NO + Br2 —> 2 NOBr
2)
NOBr2 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[NOBr2][NO]
We need to remove intermediate which is NOBr2.
we will use 1st step:
Kc = [NOBr2]/[NO][Br2]
[NOBr2] = Kc[NO][Br2]
put this in rate law expression above:
rate = k2[NOBr2][NO]
rate = k2Kc[NO][Br2][NO]
let k2Kc be k
so,
rate law becomes:
rate = k[NO]^2 [Br2]
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