The following mechanism has been proposed for the reaction between nitrogen mono
ID: 1059094 • Letter: T
Question
The following mechanism has been proposed for the reaction between nitrogen monoxide and oxygen in the gas phase. step 1 fast: 2 NO N_2O_2 step 2 slow: N_2O_2 + O_2 rightarrow 2 NO_2 What is the equation for the overall reaction? Use the smallest integer coefficients possible. If a box is not needed, leave it blank. + rightarrow + 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)
Add both the steps:
2NO + N2O2 + O2 ---> 2NO2 + N2O2
remove intermediates
2NO + O2 ---> 2NO2
2)
N2O2 is intermediate
3)
rate depends on slowest step
so,
rate = k2 * [N2O2] [O2]
from step 1:
Kc= [N2O2] / [NO]^2
[N2O2] = Kc * [NO]^2
rate = k2 * [N2O2] [O2]
= k2* Kc * [NO]^2 [O2]
lets write k2*kc as k
rate = k [NO]^2 [O2]
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