Topic: Derive the rate law and k for the reaction? (Read 4972 times)

kaywalker · « **on:** January 30, 2008, 11:24:11 PM »

the fallowing three-step mechanism has been proposed:
Cl2 --><-- 2Cl (reversible) k1 and k-1
Cl+CHCl3 --> HCL +CCl3 k2
CCl3+Cl-->CCl4 k3

k1=4.8 * 10 ^ 3
k-1= 3.6 * 10 ^ 3
k2=1.3 * 10 ^ -2
k3=2.7 * 10 ^ 2

I have no idea how to tackle this. very confusing. someone please help me. thanks in advance.

Yggdrasil · « **Reply #1 on:** January 30, 2008, 11:34:36 PM »

Do you notice anything about the rates of each step? Does this allow you to make any assumptions that greatly simplify the problem?

kaywalker · « **Reply #2 on:** January 30, 2008, 11:49:05 PM »

Quote from: Yggdrasil on January 30, 2008, 11:34:36 PM

Do you notice anything about the rates of each step? Does this allow you to make any assumptions that greatly simplify the problem?

not really. I'm ok with writing the rest of it. I just can't find K.

Borek · « **Reply #3 on:** January 31, 2008, 03:20:21 AM »

Do you know what a limiting step is?

champ · « **Reply #4 on:** January 31, 2008, 08:24:08 PM »

first u have to know the intermediates and then the rate determing reaction..

Topic: Derive the rate law and k for the reaction? (Read 4972 times)

kaywalker

Derive the rate law and k for the reaction?

Yggdrasil

Re: Derive the rate law and k for the reaction?

kaywalker

Re: Derive the rate law and k for the reaction?

Borek

Re: Derive the rate law and k for the reaction?

champ

Re: Derive the rate law and k for the reaction?

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