Arrhenius Equation:

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Emilie Hoffman 1E
Posts: 55
Joined: Fri Sep 29, 2017 7:04 am


Postby Emilie Hoffman 1E » Wed Mar 14, 2018 10:40 pm

I tried to solve this problem the slope way, with the activation energy over R being equal to (lnk1 - lnk2)/(1/T1 - 1/T2). Is this the correct way to set up this relationship, because I'm not getting the answer listed in the solutions manual.

Here is the problem for reference:
The rate constant of the reaction between CO2 and OH- in aqueous solution to give the HCO3- ion is 1.5 x 10^10 L/molxs at 25 C. Determine the rate constant at blood temperature (37 C), given that the activation energy for the reaction is 38 kJ/mol.

Matthew Lee 3L
Posts: 51
Joined: Fri Sep 29, 2017 7:07 am

Re: 15.63

Postby Matthew Lee 3L » Thu Mar 15, 2018 12:24 am

I believe if you set it up like that it should be ln(k1/k2) = (Ea/R)(1/T2 - 1/T1)

Posts: 58
Joined: Sat Jul 22, 2017 3:00 am

Re: 15.63

Postby allyz1F » Thu Mar 15, 2018 10:00 pm

Can someone please explain where the -.59 came from in the solution manual? I'm very confused by this

Clarisse Wikstrom 1H
Posts: 63
Joined: Fri Sep 29, 2017 7:05 am

Re: 15.63

Postby Clarisse Wikstrom 1H » Thu Mar 15, 2018 10:04 pm

FYI If you derive the Arrhenius equation yourself, you may also get ln(k2/k1) = (Ea/R)(1/T1- 1/T2), and it works as well. As long as whatever k you have on the top, you have the corresponding T second.

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