15.29

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Miranda 1J
Posts: 51
Joined: Fri Sep 29, 2017 7:06 am

15.29

Postby Miranda 1J » Wed Mar 07, 2018 12:24 am

Although I get the working out, I don't get which equation is being used in part (a) where we're asked to find the rate constant for the reaction given

Samantha Kan 2L
Posts: 30
Joined: Sat Jul 22, 2017 3:00 am

Re: 15.29

Postby Samantha Kan 2L » Wed Mar 07, 2018 9:48 am

You are using the equation ln[A] = -kt + ln[A]0 to find k. However, first you must use stoichiometry to find the concentration of A used up to form the given mols of B. Then you subtract the concentration of A used up from the initial concentration of A to find the final concentration of A. After you have all these components, you use the equation. Hope this helps!

Jessica Wakefield 1H
Posts: 58
Joined: Thu Jul 27, 2017 3:00 am

Re: 15.29

Postby Jessica Wakefield 1H » Wed Mar 07, 2018 10:35 pm

because depletion of A is proportional to generation of B, we use the increase in B given and convert it to moles of A by multiplying .018 by 1/3 (because the ratio of A/B is 1 mole to 3 moles). After doing this we subtract this value from the initial to get the new value of [A] or [A]t.
then you just plug your values into the integrated rate law equation and solve for k


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