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Slow Reaction

Posted: Fri Feb 24, 2017 12:03 am
by Maggie Elgin 2A
Im still having a hard time determining which step is the slow reaction which I understand is the reaction rate of the overall reaction. Could someone please explain how determine which is the slow and which is the fast reaction?

Re: Slow Reaction

Posted: Fri Feb 24, 2017 12:22 am
by edward_qiao_3I
Usually, if I'm not mistaken, this will be given to you

Re: Slow Reaction

Posted: Sat Feb 25, 2017 10:51 am
by samuelkharpatin2b
When given a mechanism, it should provide you with which step is the slow step and which is the fast step. The slow step, sometimes called the rate limiting step, is what determines the overall rate law.

Re: Slow Reaction

Posted: Sat Feb 25, 2017 12:32 pm
by Michael Lesgart 1H
I believe that the fast step is at equilibrium and the slow step is not at equilibrium. Also do you know if you use the pre-equilibrium approach if the fast step comes before the slow step or after the slow step?

Re: Slow Reaction

Posted: Sat Feb 25, 2017 10:02 pm
by Cobie_Allen_1H
I believe you use the pre-equilibrium approach only when the fast step is first!

Re: Slow Reaction

Posted: Sun Feb 26, 2017 2:02 pm
by Mana_Sheykhsoltan_1A
I think Professor Lavelle mentioned in Friday's lecture how the question will explicitly state which step is slow and which is fast or k, the rate constant, for each step will be given to you. By comparing the rate constants of the two steps, you can determine which step is faster and which is slower. The slowest step is the rate determining step, and thus it determines the speed at which the overall reaction proceeds. When coming up with your rate equation, you only have to look at the slowest step's reactants. Hope this helps!

Re: Slow Reaction

Posted: Sun Feb 26, 2017 10:38 pm
by Wenqian_Deng_1L
When given a two chemical reactions, and we know that one is slow and the other is fast, the problem should either give us clues to determining which is which. For example, the problem could say that the equilibrium constant (k1) of one reaction is slower than the equilibrium constant (k2) of the other reaction. If this was the case, then k1 should be smaller k2.

Re: Slow Reaction

Posted: Sun Feb 26, 2017 11:11 pm
by Zulfiqar Lokhandwala 1H
When it comes to the slow step reaction is the reaction that is reversible also the slow step reaction? So if it states that the reaction is reversible k and k(prime) would be included in the slow step reaction as well?

Re: Slow Reaction

Posted: Fri Mar 03, 2017 12:49 pm
by Xiaoman_Kang_2J
Zulfiqar Lokhandwala 1H wrote:When it comes to the slow step reaction is the reaction that is reversible also the slow step reaction? So if it states that the reaction is reversible k and k(prime) would be included in the slow step reaction as well?


If the forward the reaction is slow, then its reverse reaction should be fast.

Re: Slow Reaction

Posted: Sat Mar 04, 2017 11:07 am
by Michael Lesgart 1H
When the question asks you to find the rate equation, what do you do when your equation requires you to know the concentration of an intermediate species? Are you supposed to replace it by looking at the fast reaction and setting the forward rate equal to the reverse rate? Or is there another method of replacing the intermediate in the equation?

Re: Slow Reaction

Posted: Sat Mar 04, 2017 12:20 pm
by Helen_Onuffer_1A
Michael Lesgart 1H wrote:When the question asks you to find the rate equation, what do you do when your equation requires you to know the concentration of an intermediate species? Are you supposed to replace it by looking at the fast reaction and setting the forward rate equal to the reverse rate? Or is there another method of replacing the intermediate in the equation?


My TA told us that intermediates are not included in rate equations, and this is so because the rate law is determined by experiment and intermediates aren't really observable. If the first step is fast and the second step is slow, you go back to the first (fast) step which involves an equilibrium. At equilibrium, the forward reaction rate is equal to the reverse reaction rate (k[R] = k'[P]) and you solve for the concentration of the intermediate (it'll be an expression). You then substitute in this expression for the concentration of the intermediate in your slow step rate law. Hope this helps!

Re: Slow Reaction

Posted: Sat Mar 04, 2017 1:07 pm
by Stephanie_Martinez3E
It should usually be given, because that rate of a reaction is usually experimentally found.