## Finding the intermediate(s)

$K = \frac{k_{forward}}{k_{reverse}}$

Silvino Jimenez 1A
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### Finding the intermediate(s)

How do we determine when a reactant is an intermediate?

Kaylin Krahn 1I
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### Re: Finding the intermediate(s)

If it is produced in a step and a product in another, therefore being cancelled out of the overall reaction, then it is an intermediate

kaushalrao2H
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### Re: Finding the intermediate(s)

you should be able to add all of the reaction mechanism (step) reactions together in a Hess's law type manner in order to get the final chemical equation.

Wayland Leung
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### Re: Finding the intermediate(s)

Why do we not include any intermediates in the overall rate law when the intermediates are a part of the slow step?

Dang Lam
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### Re: Finding the intermediate(s)

Wayland Leung wrote:Why do we not include any intermediates in the overall rate law when the intermediates are a part of the slow step?

From my understanding, we don't include the intermediate in the rate equation because we cancel the it out when we combined the elementary equations to get the overall equation.

Julia Cheng 2J
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### Re: Finding the intermediate(s)

An intermediate is produced in an earlier step and then used in a later step. It isn't an intermediate if it is used in an early step and produced in a later step.