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Rate Law Question


Hello all,
I know I did some things wrong in this problem. Could I have some help understanding where I went wrong? The numbers seem a bit too big and unwieldy to make sense in the context of the problem.
Here is the text of the problem

Thank you

I think that this reaction cannot give FO and ClO as products !!!!

Experiments 2 and 3 show that with equal concentration of CF2Cl2 reaction speed is proportional to concentration of O3 (it drops with the same rate).

Experiments 1 and 4 give us information about dependence of rate vs. concentration of CF2Cl2 (according to my calculations it is V ~ [CF2Cl2]3).

Here is the problem, as this data gives conflicted results about rate constant (different constant for experiment 1 and 4, and different for 2 and 3).

I don't know is it error in this test or did I went wrong ???

I can't see your attachment.
The equation isn't balanced, so it must be wrong.
The data are inconsistent. Experiments 2, 3 and 4 are consistent with rate ≈ 10[O2][CF2Cl2], but experiment 1 is not. I don't think this question can be answered.


--- Quote ---Experiments 2, 3 and 4 are consistent with rate ≈ 10[O2][CF2Cl2]
--- End quote ---

I think that this answer would be too easy.

But you are right. Is it V = k [O3] x [CF2Cl2] or V = k [O3] x [CF2Cl2]3, presented data are wrong.


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