intermediate

[FrankieClarke2C]

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

[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.

[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.

[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.

[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

[Emily Burghart 1k]

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

[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.

[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

[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.

[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.

[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.

[Alfred Barrion 2H]

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

[Megan Kirschner]

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

[Nare Nazaryan 1F]

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

[Michelle Song 1I]

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

[SimranSangha4I]

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

[kristi le 2F]

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

[Nawal Dandachi 1G]

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

[vibha gurunathan 1h]

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

[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.

[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.

[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.

[Abigail_Hagen2G]

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

[Xinying Wang_3C]

An intermediate is produced in the steps of reactions, but it will be the reactant for some follow-up chemical equations and is eventually canceled out after summing all the steps together to get the final formula.

[Alen Huang 2G]

An intermediate will be the product of one elementary reaction and the reactant of another.

[DPatel_2L]

They are formed and used up in the reaction, so should not be included.

[reyvalui_3g]

Intermediates are formed during the reaction and then used up, so they are not a part of the rate law.