Arrhenius Equation: $\ln k = - \frac{E_{a}}{RT} + \ln A$

melodyzaki2E
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Joined: Fri Sep 28, 2018 12:18 am

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.

Karyn Nguyen 1K
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### Re: 15.63 (6th edition)

I'm getting stuck on this question too. I was looking at the solution and I was wondering where 0.59 came from.

Karyn Nguyen 1K
Posts: 72
Joined: Fri Apr 06, 2018 11:04 am

### Re: 15.63 (6th edition)

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)$ln(\frac{k'}{k}) = \frac{38 kJ/mol}{0.08314 kJ/molK}(\frac{1}{298 K}-\frac{1}{310 K}) - 0.59$
$\frac{k'}{k} = 1.8$
$k' = 1.8(1.5\times 10^{10} L/mol\cdot s)=2.7\times 10^{^{10}} L/mol\cdot s$

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