Last edited by a moderator: May 3, 2017

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The discussion centers on solving a second-order reaction problem involving the concentration of A decreasing from 0.159 mol/L to 6.07 x 10^-3 mol/L with a rate constant of 0.169 L/(mol s). Participants emphasize the importance of showing work and understanding the problem rather than simply asking for answers. There is frustration expressed over unhelpful comments and a lack of constructive guidance. Key questions include identifying the necessary equation for a second-order reaction and the relevant concentration values. Overall, the thread highlights the need for collaborative learning and adherence to forum etiquette.
kittymaniac84
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A reaction of the form aA = products is second order with a rate constant of 0.169
L/(mol s). If the initial concentration of A is 0.159 mol/L, how many seconds would it
take for the concentration of A to decrease to 6.07 x 10^-3 mol/L ?

how to solve these
 
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do your own hw
 
If your not going to help, don't bother to post any rude comments. That is not how you help someone learn.
 
kittymaniac84 said:
If your not going to help, don't bother to post any rude comments. That is not how you help someone learn.

NO that is what the HOMEWORK forum is for. And no one is going to help you there either because you haven't even shown that you have tried any work on your own.
 
I don't know how to attempt this. I will find other places who can help.
 
gravenewworld said:
do your own hw
Ok jackass. Next time, just refer them to the Forum rules.

FAQ: Why hasn't anybody answered my question? - https://www.physicsforums.com/showthread.php?t=94384

Anyways Kitty ...

1) What is the equation you will need for a 2nd order reaction?
2) What values do you have? Initial/Final concentration ... etc?

Refer to the image for equations:

http://alt1.mathlinks.ro/Forum/latexrender/pictures/1/b/a/1bacaba62a260d46b7600cc644b6bba500f54b3b.gif
 
Last edited by a moderator:
Thread 'Confusion regarding a chemical kinetics problem'

Thread 'Confusion regarding a chemical kinetics problem'

TL;DR Summary: cannot find out error in solution proposed. [![question with rate laws][1]][1] Now the rate law for the reaction (i.e reaction rate) can be written as: $$ R= k[N_2O_5] $$ my main question is, WHAT is this reaction equal to? what I mean here is, whether $$k[N_2O_5]= -d[N_2O_5]/dt$$ or is it $$k[N_2O_5]= -1/2 \frac{d}{dt} [N_2O_5] $$ ? The latter seems to be more apt, as the reaction rate must be -1/2 (disappearance rate of N2O5), which adheres to the stoichiometry of the...
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