intermediate

Moderators: Chem_Mod, Chem_Admin

FrankieClarke2C
Posts: 59
Joined: Fri Sep 28, 2018 12:28 am

intermediate

Postby FrankieClarke2C » Sun Mar 17, 2019 9:04 am

How are you able to tell what the intermediate is and why can't it exist in the rate law?

Matthew Tran 1H
Posts: 165
Joined: Fri Sep 28, 2018 12:16 am

Re: intermediate

Postby Matthew Tran 1H » Sun Mar 17, 2019 9:17 am

An intermediate is a species that is formed and subsequently used up in a reaction mechanism. It can't appear in the rate law because it is not part of the overall reaction.

Henry_Phan_4L
Posts: 68
Joined: Fri Sep 28, 2018 12:24 am

Re: intermediate

Postby Henry_Phan_4L » Sun Mar 17, 2019 9:38 am

The intermediate can't exist in the rate law because something was used to form it. So since it came from something, you gotta trace it back to the original components.

Gillian Ward 1F
Posts: 61
Joined: Fri Sep 28, 2018 12:27 am

Re: intermediate

Postby Gillian Ward 1F » Sun Mar 17, 2019 4:23 pm

Intermediates are produced in one elementary step and consumed in the next. They are not part of the overall reaction so they will not appear in the rate law.

Aili Ye 4L
Posts: 58
Joined: Fri Sep 28, 2018 12:16 am

Re: intermediate

Postby Aili Ye 4L » Mon Mar 18, 2019 9:35 am

Intermediates are form and then used up so they are not part of the overall reaction and therefor rate law as well

Emily Burghart 1k
Posts: 50
Joined: Wed Sep 18, 2019 12:17 am

Re: intermediate

Postby Emily Burghart 1k » Tue Feb 18, 2020 9:56 pm

If an intermediate is formed during a reaction, and then used, do non-state functions include those changes and quantities?

CameronDis2K
Posts: 51
Joined: Wed Feb 20, 2019 12:18 am

Re: intermediate

Postby CameronDis2K » Fri Feb 28, 2020 11:21 am

The intermediate in a series of reactions can be identified by seeing which element is both in the products of one reaction and reactants of another (it will cancel out as they are on opposite sides). Since it is not written in the overall reaction (as it is cancelled out), it is not included in the rate law equation.

805291863
Posts: 100
Joined: Sat Sep 14, 2019 12:16 am

Re: intermediate

Postby 805291863 » Sun Mar 01, 2020 2:59 pm

Intermediates are easily recognizable in a reaction mechanism, which is the sequence of elementary reactions to go from reactants to products. The molecules that are formed and consumed in these elementary reactions are intermediates

Louise Lin 2B
Posts: 97
Joined: Sat Aug 17, 2019 12:15 am

Re: intermediate

Postby Louise Lin 2B » Sun Mar 01, 2020 4:08 pm

Intermediates ultimately get canceled out when you write out chemical equations in the full, so they will not show up in the rate law because only the initial reactants and final products have an influence on the rate law.

Jasmine W 1K
Posts: 49
Joined: Sat Sep 07, 2019 12:18 am

Re: intermediate

Postby Jasmine W 1K » Sun Mar 01, 2020 5:03 pm

An intermediate is formed and used up during the reaction, so it will not be included in the rate law because it isn't part of the overall reaction.

Andres Merlos 2L
Posts: 46
Joined: Wed Sep 18, 2019 12:17 am

Re: intermediate

Postby Andres Merlos 2L » Sun Mar 01, 2020 5:21 pm

Intermediates are produced then consumed, during some part of the reaction. It cannot exist in rate law because they are not a part of the overall equation.

Alfred Barrion 2H
Posts: 100
Joined: Sat Jul 20, 2019 12:16 am

Re: intermediate

Postby Alfred Barrion 2H » Sun Mar 01, 2020 11:44 pm

An intermediate is formed and then used up during a reaction, so it cant be used in rate law.

Megan Kirschner
Posts: 46
Joined: Wed Feb 20, 2019 12:17 am

Re: intermediate

Postby Megan Kirschner » Sun Mar 08, 2020 6:36 pm

The intermediate can't exist in the rate law because something was used to form it.

Nare Nazaryan 1F
Posts: 101
Joined: Fri Aug 09, 2019 12:17 am

Re: intermediate

Postby Nare Nazaryan 1F » Sun Mar 08, 2020 9:31 pm

It is not in the rate law because it was formed then used and does not appear in the overall reaction.

Michelle Song 1I
Posts: 102
Joined: Thu Jul 11, 2019 12:17 am

Re: intermediate

Postby Michelle Song 1I » Sun Mar 08, 2020 11:08 pm

An intermediate was formed (and then used up) by the reaction, so it doesn't show up in the rate law.

SimranSangha4I
Posts: 99
Joined: Sat Sep 14, 2019 12:17 am

Re: intermediate

Postby SimranSangha4I » Sun Mar 08, 2020 11:10 pm

Since it was formed by the actual reaction, it isn't part of the rate law.

kristi le 2F
Posts: 102
Joined: Thu Jul 11, 2019 12:15 am

Re: intermediate

Postby kristi le 2F » Tue Mar 10, 2020 12:50 am

The intermediate is both formed and consumed in the reaction but does not appear in the overall chemical equation.

Nawal Dandachi 1G
Posts: 102
Joined: Sat Sep 28, 2019 12:16 am

Re: intermediate

Postby Nawal Dandachi 1G » Tue Mar 10, 2020 12:55 am

Intermediates are formed in one reaction and then consumed in the other, so they do not show up in rate laws.

vibha gurunathan 1h
Posts: 51
Joined: Mon Oct 07, 2019 12:15 am

Re: intermediate

Postby vibha gurunathan 1h » Wed Mar 11, 2020 4:08 am

The intermediate is formed and used up, and it doesn't appear in the overall chemical equation

Max Madrzyk Dis 4G
Posts: 102
Joined: Wed Sep 18, 2019 12:21 am

Re: intermediate

Postby Max Madrzyk Dis 4G » Wed Mar 11, 2020 7:54 am

An intermediate shows up in the products of step one but the reactants of step two and therefore is used up in the second reaction so none will remain after the whole thing is over. The reason this does not affect the rate law is because the rate law is determined by the reactants of the slow step and the intermediate has no effect on this.

William Chan 1D
Posts: 102
Joined: Sat Sep 14, 2019 12:15 am

Re: intermediate

Postby William Chan 1D » Wed Mar 11, 2020 9:32 pm

An intermediate will appear in one of the step and be used up in a subsequent step. It will not show up in the overall reaction.

CameronDis2K
Posts: 51
Joined: Wed Feb 20, 2019 12:18 am

Re: intermediate

Postby CameronDis2K » Sat Mar 14, 2020 11:58 am

The intermediate cancels out in the rate determining step (before the final overall equation), and is not present in the overall reaction --> as its presence in the reactant of one reaction and the product of another reaction, makes itself cancel out.

Abigail_Hagen2G
Posts: 107
Joined: Fri Aug 09, 2019 12:17 am

Re: intermediate

Postby Abigail_Hagen2G » Sun Mar 15, 2020 10:06 pm

Since an intermediate cancels out, you wouldn't write it in the final balanced equation.


Return to “Kinetics vs. Thermodynamics Controlling a Reaction”

Who is online

Users browsing this forum: No registered users and 2 guests