The following mechanism has been proposed for the gas phase reaction of nitrogen

Question

The following mechanism has been proposed for the gas phase reaction of nitrogen monoxide with bromine. step 1 fast: NO+Br--NOBr, step 2 slow: NOBrNO2 NOBr a) what is the equation for the overall reaction? Use the smallest integer coefficients possible lf 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 m Use the form k[A] [B]"... where '1'is understood (so don't write it if it's a '1') for m, n etc. Rate

Explanation / Answer

1)

overall reaction can be obtained by adding both steps

2 NO + Br2 —> 2 NOBr

2)

NOBr2 is produced in step 1 and used up in step 2

So, NOBr2 is an intermediate

3)

rate depends on the slowest step

Here 2nd step is slowest

So, rate law is:

rate = k2 [NOBr2][NO]

NOBr2 is an intermediate. We need to remove it.

we will use 1st step:

Kc = [NOBr2]/[NO][Br2]

[NOBr2] = Kc*[NO][Br2]

Rate law thus is:

rate = k2 [NOBr2][NO]

rate = k2Kc*[NO][Br2][NO]

rate = k2Kc*[NO]^2[Br2]

k2*Kc can be written as k

so,

rate law is:

rate = k[NO]2[Br2]

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