the intermediate in a reaction

[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 !

[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

[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.

[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.

[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.

[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.

[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.

[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.

[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.

[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.

[Simon Dionson 4I]

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