## Identifying zero order

$\frac{d[R]}{dt}=-k; [R]=-kt + [R]_{0}; t_{\frac{1}{2}}=\frac{[R]_{0}}{2k}$

Glendy Gonzalez 1A
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### Identifying zero order

How can you identify a zero order reactant based on a table? Is there a "shortcut"?

Caroline LaPlaca
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### Re: Identifying zero order

There is no change in rate

Sara Sasaki 1K
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### Re: Identifying zero order

https://chem.libretexts.org/Core/Physic ... _Reactions

Kathleen Vidanes 1E
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### Re: Identifying zero order

You have to fully calculate the kinetic law. This can only be done if you know all of the elementary reactions involved.

Varsha Sivaganesh 1A
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### Re: Identifying zero order

Yes, when looking at a table you would first make sure the concentration of the reactant you are looking for is the only one changing between two experiments. If the concentration of the reactant changes and the rate does not change, then you know it is 0 order because the concentration of that particular reactant does not affect the rate of reaction.

Virpal Gill 1B
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Joined: Thu Jul 27, 2017 3:00 am

### Re: Identifying zero order

If all other reactant concentrations remain the same and you change the concentration of the reactant of interest without changing the rate, then that reactant is zero order.

AtreyiMitra2L
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### Re: Identifying zero order

You need the table to identify 0 order reactions