the intermediate in a reaction


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105311039
Posts: 107
Joined: Fri Aug 02, 2019 12:16 am

the intermediate in a reaction

Postby 105311039 » Sat Mar 07, 2020 3:56 pm

Can an intermediate always be in the rate law expression? Or is there certain instances where it cannot be placed in the rate law expression and has to be replaced with something other. Thank you !

VLi_2B
Posts: 99
Joined: Sat Sep 14, 2019 12:15 am

Re: the intermediate in a reaction

Postby VLi_2B » Sat Mar 07, 2020 5:21 pm

Intermediates are produced in one step and consumed in a later step, so they do not appear in the overall reaction equation or overall rate law

Andrew Pfeiffer 2E
Posts: 101
Joined: Sat Sep 28, 2019 12:16 am

Re: the intermediate in a reaction

Postby Andrew Pfeiffer 2E » Sat Mar 07, 2020 5:21 pm

Because intermediates are by definition produced in one step and consumed in another, they are not actually present in the overall equation or rate law of the reaction.

Catherine Daye 1L
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Joined: Wed Sep 11, 2019 12:16 am

Re: the intermediate in a reaction

Postby Catherine Daye 1L » Sat Mar 07, 2020 6:15 pm

The intermediate is never in the rate law expression because intermediates get used up in the intermediate steps. The rate law only includes substances present in the end of the reaction.

205405339
Posts: 77
Joined: Thu Jul 11, 2019 12:16 am

Re: the intermediate in a reaction

Postby 205405339 » Sat Mar 07, 2020 6:39 pm

the intermediate is a species produced in one step then consumed in the next step so the intermediate species will not appear in the overall reaction equation as it is depleted by the end of the next step.

Sally Qiu 2E
Posts: 105
Joined: Fri Aug 30, 2019 12:18 am

Re: the intermediate in a reaction

Postby Sally Qiu 2E » Sat Mar 07, 2020 6:43 pm

intermediates do not show up in the rate law or overall reaction because they will cancel out on the reactants and products side.

Jamie Lee 1F
Posts: 106
Joined: Fri Aug 09, 2019 12:16 am

Re: the intermediate in a reaction

Postby Jamie Lee 1F » Sat Mar 07, 2020 9:33 pm

Intermediates are produced in a step, then are consumed in a later step. It's kind of like when you are balancing redox reactions and cancel out the electrons from both reactions.

JChen_2I
Posts: 107
Joined: Fri Aug 09, 2019 12:17 am

Re: the intermediate in a reaction

Postby JChen_2I » Sat Mar 07, 2020 10:11 pm

Intermediates should not be a part of the rate law expression. Use the elementary reactions to find an equation you can set equal to the intermediate and plug it into the rate law equation.

HuyHa_2H
Posts: 100
Joined: Wed Sep 11, 2019 12:15 am

Re: the intermediate in a reaction

Postby HuyHa_2H » Sun Mar 08, 2020 1:04 am

Intermediates aren't included in the expression due to how it's produced in one step to be entirely consumed upon the next.

Rebekah Alfred 1J
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Re: the intermediate in a reaction

Postby Rebekah Alfred 1J » Sun Mar 08, 2020 9:41 am

The intermediate is not included in the rate law expression. You can recognize a species is an intermediate if it is in the steps, but not included in the overall reaction.

Simon Dionson 4I
Posts: 107
Joined: Sat Sep 14, 2019 12:17 am

Re: the intermediate in a reaction

Postby Simon Dionson 4I » Sun Mar 08, 2020 4:48 pm

Intermediates are included in the elementary rate laws but not the overall rate-law since they cancel out.


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