DatLemonDoe

Yes, that makes a lot of sense. Thank you very much, have a great day

Hi There is a big hole in my understanding of integrated rate laws, and I've been having a hard time finding what it is that i'm not understanding. I would assume that it's a very small idea that i'm missing. Anyway, here's my problem, I would assume that I will say some false statement at some point, hence me getting weird results. Say you have the reaction A + B --) C And let's assume that the global order of the reaction is 2. We are also given the initial concentration of A aswell as the contentration of A at a certain point in time (t) The integrated rate law would be 1/[A]=1/[A]0+kt. We can use that equation to find a value for k, since we know every other variable. Now, here's where I get lost. Say we do a second experiment where the intial concentration of B is different, but the initial concentration of A remains the same. We once again find the concentration of A at the sime point in time (t) If we once again find the value of k in the integrated rate law, won't it's value be different? Changing the initial concentration of B has had for effect to change the rate of the reaction, and therefore the concentration of A at the same point in time is no longer the same. However, t and [A]0 are still the same. Now I know that the value of k doesn't change if you change the concentration of a reactant, so I'm confused as to why I get those results. Hopefully It wasn't too confusing. If it was, ask me questions and I will gladly clarify. Thanks a lot, I appreciate your time and kindness.