Homework 15.63

Arrhenius Equation:

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arif_latif_2G
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Joined: Fri Sep 28, 2018 12:23 am

Homework 15.63

Postby arif_latif_2G » Sun Mar 10, 2019 6:41 pm

Can someone help me through this question:
The rate constant of the reaction between CO2 and OH- in aqueous solution to give the HCO3- ion is 1.5 x 10^10 Lmol^-1s^-1 at 25C. Determine the rate constant at blood
temperature (37 C), given that the activation energy for the reaction is 38 kJmol^-1.
.

Tam To 1B
Posts: 72
Joined: Fri Sep 28, 2018 12:25 am

Re: Homework 15.63

Postby Tam To 1B » Mon Mar 11, 2019 4:17 pm

You use the Arrhenius equation for this problem. ln(k2/k1) = Ea/R(1/T1-1/T2)
Given:
Ea = 38 kj/mol
k1 = 1.5E10 L/mols
T1 = 298 K
k2 = ?
T2 = 310 K
lnk2 = ln(1.5E10) + (38/.008314)(1/298 - 1/310)
k2 = e^24 = 2.7E10 L/mols

Kimberly 1H
Posts: 63
Joined: Fri Sep 28, 2018 12:17 am
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Re: Homework 15.63

Postby Kimberly 1H » Tue Mar 12, 2019 4:06 pm

Don't forget that in the form ln()=()-)


to use T1-T2 not T2-T1


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