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15.63 (6th addition)

Posted: Fri Mar 15, 2019 2:54 pm
by melodyzaki2E
The rate constant of the reaction between CO2 and OH in aqueous solution to give the HCO3- ion is 1.5 *10^10 L/mol*s at 25 C. Determine the rate constant at blood temperature (37 C), given that the activation energy for the reaction is 38 kJmol-1.

Re: 15.63 (6th edition)

Posted: Fri Mar 15, 2019 4:39 pm
by Karyn Nguyen 1K
I'm getting stuck on this question too. I was looking at the solution and I was wondering where 0.59 came from.

Re: 15.63 (6th edition)

Posted: Fri Mar 15, 2019 4:51 pm
by Karyn Nguyen 1K
Karyn Nguyen 1K wrote:I'm getting stuck on this question too. I was looking at the solution and I was wondering where 0.59 came from.


This is the solution:

ln(k'/k) = (38 kJ/mol)/(0.08314 kJ/molK)


Re: 15.63 (6th addition)

Posted: Fri Mar 15, 2019 7:11 pm
by Maddy Mackenzie
Can anyone explain where the .59 comes from? Additionally, isn't the equation ln (k2/K1) = -Ea/R (1/T2 - 1/T1)? So why would the temperature corresponding to T2 come second in the solutions maual?