Ans: C
Please explain why the answer is C. Thank you.
activation energy is larger for 2nd step
So, 2nd step is rate determining step
From 2nd step:
rate law is:
rate = k2[Cl2O2][N2]
since [Cl2O2] is intermediate, we will use step 1
using steady state approximation for step 1
rate forward = rate backward
k1[Cl2][O2] = k-1 [Cl2O2]
So,
[Cl2O2] = (k1/k-1)[Cl2][O2]
put this in rate law expression:
rate = k2[Cl2O2][N2]
rate = k2(k1/k-1)[Cl2][O2][N2]
let k2(k1/k-1) = kobs
so,
rate law is:
rate = kobs[Cl2][O2][N2]
Answer: C
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