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intermediate

Posted: Sun Mar 17, 2019 9:04 am
by FrankieClarke2C
How are you able to tell what the intermediate is and why can't it exist in the rate law?

Re: intermediate

Posted: Sun Mar 17, 2019 9:17 am
by Matthew Tran 1H
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.

Re: intermediate

Posted: Sun Mar 17, 2019 9:38 am
by Henry_Phan_4L
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.

Re: intermediate

Posted: Sun Mar 17, 2019 4:23 pm
by Gillian Ward 1F
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.

Re: intermediate

Posted: Mon Mar 18, 2019 9:35 am
by Aili Ye 4L
Intermediates are form and then used up so they are not part of the overall reaction and therefor rate law as well

Re: intermediate

Posted: Tue Feb 18, 2020 9:56 pm
by Emily Burghart 1k
If an intermediate is formed during a reaction, and then used, do non-state functions include those changes and quantities?

Re: intermediate

Posted: Fri Feb 28, 2020 11:21 am
by CameronDis2K
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.

Re: intermediate

Posted: Sun Mar 01, 2020 2:59 pm
by 805291863
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

Re: intermediate

Posted: Sun Mar 01, 2020 4:08 pm
by Louise Lin 2B
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.

Re: intermediate

Posted: Sun Mar 01, 2020 5:03 pm
by Jasmine W 1K
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.

Re: intermediate

Posted: Sun Mar 01, 2020 5:21 pm
by Andres Merlos 2L
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.

Re: intermediate

Posted: Sun Mar 01, 2020 11:44 pm
by Alfred Barrion 2H
An intermediate is formed and then used up during a reaction, so it cant be used in rate law.

Re: intermediate

Posted: Sun Mar 08, 2020 6:36 pm
by Megan Kirschner
The intermediate can't exist in the rate law because something was used to form it.

Re: intermediate

Posted: Sun Mar 08, 2020 9:31 pm
by Nare Nazaryan 1F
It is not in the rate law because it was formed then used and does not appear in the overall reaction.

Re: intermediate

Posted: Sun Mar 08, 2020 11:08 pm
by Michelle Song 1I
An intermediate was formed (and then used up) by the reaction, so it doesn't show up in the rate law.

Re: intermediate

Posted: Sun Mar 08, 2020 11:10 pm
by SimranSangha4I
Since it was formed by the actual reaction, it isn't part of the rate law.

Re: intermediate

Posted: Tue Mar 10, 2020 12:50 am
by kristi le 2F
The intermediate is both formed and consumed in the reaction but does not appear in the overall chemical equation.

Re: intermediate

Posted: Tue Mar 10, 2020 12:55 am
by Nawal Dandachi 1G
Intermediates are formed in one reaction and then consumed in the other, so they do not show up in rate laws.

Re: intermediate

Posted: Wed Mar 11, 2020 4:08 am
by vibha gurunathan 1h
The intermediate is formed and used up, and it doesn't appear in the overall chemical equation

Re: intermediate

Posted: Wed Mar 11, 2020 7:54 am
by Max Madrzyk Dis 4G
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.

Re: intermediate

Posted: Wed Mar 11, 2020 9:32 pm
by William Chan 1D
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.

Re: intermediate

Posted: Sat Mar 14, 2020 11:58 am
by CameronDis2K
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.

Re: intermediate

Posted: Sun Mar 15, 2020 10:06 pm
by Abigail_Hagen2G
Since an intermediate cancels out, you wouldn't write it in the final balanced equation.