Chemical Forums
Chemistry Forums for Students => Undergraduate General Chemistry Forum => Topic started by: kelvinLTR on March 13, 2013, 02:20:44 PM
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In the reaction 2C :rarrow:D, the following mechanism is suggested:
2C ::equil:: C + C* (forward rate constant k1 and backward rate constant k2) C* is a reactive intermediate
C* :rarrow: D (rate constant k3)
two questions are asked
1. What is the condition for the reaction to be pseudo-first order
2. What is the condition for the reaction to be 2nd order
I found d[D]/dt=k1k3[C]/k2 using the steady state approximation for [C*]
But got stuck at those two questions.
My argument is for the reaction to be pseudo first order, [C*] formed must disappear much faster than it is formed, thus k2>>k1
am I right? and can someone help me with the 2nd part
thanks in advance :)
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I found d[D]/dt=k1k3[C]/k2 using the steady state approximation for [C*]
Granted, it's been quite a while since I solved rate law problems, but I believe your difficulty may be related to this.
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in the question, in an earlier part, it is asked to derive the rate of formation of [D] in terms of [C]
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And I'm saying I didn't get the same answer you did. ;)
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mmm I got :
d[D]/dt = k3[C*]
d[C*]/dt=k1[C]2-k2[C][C*]=0 in steady state
therefore [C*]=k1[C]/k2
substituting d[D]/dt=k1k3[C]/k2
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d[C*]/dt=k1[C]2-k2[C][C*]=0 in steady state
You are forgetting to include the loss of the intermediate C* to form your final product via rate k3.
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oh silly me :) thanks a lot. I'll try again
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figured it out. Thank you very much :)
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No problem. Should be easy to find the conditions of your limits now.