Concept


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CaminaB_1D
Posts: 63
Joined: Fri Sep 28, 2018 12:16 am

Concept

Postby CaminaB_1D » Mon Mar 11, 2019 12:01 pm

Is there a conceptual meaning behind a zero order reaction?

Grace Kim 1J
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Joined: Fri Sep 28, 2018 12:18 am
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Re: Concept

Postby Grace Kim 1J » Mon Mar 11, 2019 12:27 pm

A zero-order reaction occurs when the rate of the reaction in unaffected by the concentration of the reactants. Rather, it could depend on another variable like enzymes or catalysts. Zero-order reactions are typically found when a material that is required for the reaction to proceed, such as a surface or a catalyst, is saturated by the reactants.

Hope this helped!

mcredi
Posts: 63
Joined: Fri Sep 28, 2018 12:16 am

Re: Concept

Postby mcredi » Mon Mar 11, 2019 12:53 pm

Zero-order reactions are typically found when a material that is required for the reaction to proceed, such as a surface or a catalyst, is saturated by the reactants. For example a constant amount of drug is eliminated per unit time; 10mg a drug may be eliminated per hour, this rate of elimination is constant and is independent of the total drug concentration in the plasma

Sophia Ding 1B
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Joined: Fri Sep 28, 2018 12:16 am

Re: Concept

Postby Sophia Ding 1B » Wed Mar 13, 2019 3:15 pm

Yeah if you think about the general rate law, k[A]^n, for a zero order reaction n would equal 0. By doing that, the rate = -kt, where it can be seen that the concentration of the reactant, [A], has no effect on the rate. Thus, it can be conceptually inferred that for zero order reaction, the rate is unaffected by the concentration of the reactant and would depend on other variables, such as a catalyst like other students said.

Nina Do 4L
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Joined: Fri Sep 28, 2018 12:27 am

Re: Concept

Postby Nina Do 4L » Wed Mar 13, 2019 10:10 pm

Zero order means that the rate constant is independent from the concentration so therefore the concentration is to the zeroth power ie the rate law being rate= k[A]^0 which will just be rate=k.
Same applies for first and second orders.
Hope that helps!


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