The following mechanism for the gas phase reaction of nitrogen dioxide with carb
ID: 1020970 • Letter: T
Question
The following mechanism for the gas phase reaction of nitrogen dioxide with carbon monoxide at temperatures above 225 degree C is consistent with the observed rate law. step 1 fast:NO_2 + CO doubleheadarrow ONOCO step 2 slow:ONOCO rightarrow NO + CO_2 What is the equation for the overall reaction? Use the smallest integer coefficients possible. If a box is not needed, leave it blank. Enter the formula of any species that acts as a reaction intermediate? If none leave box blank: Complete the rate law for the overall reaction that is consistent with this mechanism. Use the form k[A]^m[B]^n..., where '1' is understood (so don't write it if it's a '1') for m, n etc. Rate =Explanation / Answer
1) overall reaction
NO2 + CO ---------------> NO + CO2
2)
intermediate = ONOCO
3)
rate depends on slowest step in the mechanism
so
rate = k [ONOCO] ------------------>1
but ONOCO is not reactant , it is intermediate.
so we have to do more for getting rate law
from fast step
keq = [ONOCO] / [NO2] [CO]
Keq[NO2] [CO] = [ONOCO] ----------------->2
from 1 and 2
rate = k keq [NO2][CO]
rate = k [NO2][CO] -----------------------> answer
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