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### Example Help

Posted: Sun Mar 08, 2020 7:40 pm
Can someone walk through a zero order reaction problem step by step? Please include side information, conceptual knowledge, and graphical representations?

### Re: Example Help

Posted: Mon Mar 09, 2020 4:16 pm
Zero order does not depend on the concentration of reactants. The equation is [A]= -kt + [A]o. The graph is a negative line because the slope is -k. Zero order are common in enzymes and catalysts. Various UA sessions will cover these, and you can ask TA's for clarification.

### Re: Example Help

Posted: Thu Mar 12, 2020 10:59 am
You can identify a reactant as zero-order if changing its concentration does not affect the rate in any way.

### Re: Example Help

Posted: Thu Mar 12, 2020 11:13 am
If you see a graph of [A] v. t and it is linear with a negative slope, you know that the reaction is zero-order with respect to that reactanct. The rate constant k is equal to the negative of the slope.

### Re: Example Help

Posted: Sat Mar 14, 2020 3:39 pm
Michael Nguyen 1E wrote:If you see a graph of [A] v. t and it is linear with a negative slope, you know that the reaction is zero-order with respect to that reactanct. The rate constant k is equal to the negative of the slope.

Thank you this is very helpful.

### Re: Example Help

Posted: Sat Mar 14, 2020 5:23 pm
In a zero order reaction, the rate of the reaction does NOT depend of the concentration of the reactant; the rate remains constant throughout the entire reaction.

### Re: Example Help

Posted: Sat Mar 14, 2020 5:40 pm
In a zero order reaction, the rate of reaction does not depend on the concentration of the reactants, so the rate of reaction is constant as the concentration decreases.
If you want examples and graphs: https://chem.libretexts.org/Bookshelves/Physical_and_Theoretical_Chemistry_Textbook_Maps/Supplemental_Modules_(Physical_and_Theoretical_Chemistry)/Kinetics/Reaction_Rates/Zero-Order_Reactions