Catalyst and Intermediate


Moderators: Chem_Mod, Chem_Admin

PeterTran1C
Posts: 30
Joined: Thu Jul 13, 2017 3:00 am

Catalyst and Intermediate

Postby PeterTran1C » Wed Mar 14, 2018 2:49 pm

In a mechanism reaction, can you ideally have both catalysts at the beginning and intermediates throughout the same reaction?

Cooper1C
Posts: 50
Joined: Fri Sep 29, 2017 7:07 am

Re: Catalyst and Intermediate

Postby Cooper1C » Wed Mar 14, 2018 3:09 pm

A catalyst does not change the reactants and products of a reaction - it just changes the pathway. So you should be able to have catalysts and intermediates in the same reaction.

Angel R Morales Dis1G
Posts: 50
Joined: Sat Jul 22, 2017 3:01 am

Re: Catalyst and Intermediate

Postby Angel R Morales Dis1G » Wed Mar 14, 2018 10:30 pm

Yeah, a catalyst will be used in the first step and be regenerated in the last step, whereas an intermediate is formed in the first step and used in the second step. In other words, the intermediate will be cancelled out whereas the catalyst will not. You will be able to see and use both of them.

kaushalrao2H
Posts: 63
Joined: Thu Jul 13, 2017 3:00 am
Been upvoted: 2 times

Re: Catalyst and Intermediate

Postby kaushalrao2H » Wed Mar 14, 2018 10:31 pm

catalysts are not used up in the reaction, so you will see the catalyst in BOTH the product and reactant sides of the chemical equations. intermediates, on the other hand, so not appear in the chemical reaction equation.

Joyce Gu 1E
Posts: 29
Joined: Tue Nov 24, 2015 3:00 am

Re: Catalyst and Intermediate

Postby Joyce Gu 1E » Sat Mar 17, 2018 8:37 pm

yes, they can show up in the same reaction, but just don't show up in the end product

Guangyu Li 2J
Posts: 50
Joined: Fri Sep 29, 2017 7:07 am
Been upvoted: 1 time

Re: Catalyst and Intermediate

Postby Guangyu Li 2J » Sun Mar 18, 2018 2:23 am

Yes. It is really easy to confuse these two ideas. Reaction intermediate is a molecule that plays a role in the reactions but does not appear in the overall reaction equation. On the other hand, the catalyst is a molecule that speeds up the chemical reactions by providing an optional pathway, or more specifically, decreasing the activation energy required to reach the energy barrier.

So in the realistic reactions, you will find that catalyst is always consistent with its original amount during the chemical reaction, but intermediate only appears in one or several steps in the reaction except for the overall equation.

Hope this helps! Good luck in the Final!


Return to “Reaction Mechanisms, Reaction Profiles”

Who is online

Users browsing this forum: No registered users and 1 guest