D
d_remeday86
Guest
Consider the following mechanism:
Step 1: X + Y2 ---> XY2 (slow) (k1)
Step 2: XY2 ---> XY + Y (fast) (k2)
Overall: X + Y2 ---> XY + Y
Use the above mechanism to propose a rate law for the overall reaction.
--The answer is:
rate = k1 [X][Y2]
I dont know how they got that answer??? Please explain.
Also, the molecularity of the rate-determining step is bimolecular (molecularity of 2) and the intermediates of this reaction is XY2 only. But can you please explain why it is so. I really want to understand this problem so pleasee help. THANKS IN ADVANCEE!
Step 1: X + Y2 ---> XY2 (slow) (k1)
Step 2: XY2 ---> XY + Y (fast) (k2)
Overall: X + Y2 ---> XY + Y
Use the above mechanism to propose a rate law for the overall reaction.
--The answer is:
rate = k1 [X][Y2]
I dont know how they got that answer??? Please explain.
Also, the molecularity of the rate-determining step is bimolecular (molecularity of 2) and the intermediates of this reaction is XY2 only. But can you please explain why it is so. I really want to understand this problem so pleasee help. THANKS IN ADVANCEE!