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the intermediate in a reaction

Posted: Sat Mar 07, 2020 3:56 pm
by 105311039
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 !

Re: the intermediate in a reaction

Posted: Sat Mar 07, 2020 5:21 pm
by VLi_2B
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

Re: the intermediate in a reaction

Posted: Sat Mar 07, 2020 5:21 pm
by Andrew Pfeiffer 2E
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.

Re: the intermediate in a reaction

Posted: Sat Mar 07, 2020 6:15 pm
by Catherine Daye 1L
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.

Re: the intermediate in a reaction

Posted: Sat Mar 07, 2020 6:39 pm
by 205405339
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.

Re: the intermediate in a reaction

Posted: Sat Mar 07, 2020 6:43 pm
by Sally Qiu 2E
intermediates do not show up in the rate law or overall reaction because they will cancel out on the reactants and products side.

Re: the intermediate in a reaction

Posted: Sat Mar 07, 2020 9:33 pm
by Jamie Lee 1F
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.

Re: the intermediate in a reaction

Posted: Sat Mar 07, 2020 10:11 pm
by JChen_2I
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.

Re: the intermediate in a reaction

Posted: Sun Mar 08, 2020 1:04 am
by HuyHa_2H
Intermediates aren't included in the expression due to how it's produced in one step to be entirely consumed upon the next.

Re: the intermediate in a reaction

Posted: Sun Mar 08, 2020 9:41 am
by Rebekah Alfred 1J
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.

Re: the intermediate in a reaction

Posted: Sun Mar 08, 2020 4:48 pm
by Simon Dionson 4I
Intermediates are included in the elementary rate laws but not the overall rate-law since they cancel out.