March 14th, 2018, 04:34 AM  #1 
Member Joined: Mar 2016 From: Sweden Posts: 34 Thanks: 4  Activation energy
I'm suppose to find the activation energy based on this given information: When double the temperature the rate constant increases with 2.11%. The Arrhenius equation is valid. I did this: k1 is the rate constant when T1=T k2=1.0211k1 is the rate constant when T2=2T Then I used the Arrhenius for both kvalues and divided the two expressions and got k1/k2=1/1.0211=exp(E/R(1/2T1/T)=exp(E/R(1/2T)) but then T is unknown and I don't know how to come up with a solution for E. 
March 14th, 2018, 08:36 AM  #2  
Math Team Joined: Jul 2011 From: Texas Posts: 2,767 Thanks: 1422  Quote:
$k_1 = Ae^{\dfrac{E}{RT_1}}$ $k_2 = 1.0211 \cdot k_1 = Ae^{\dfrac{E}{R \cdot 2T_1}}$ $\dfrac{k_2}{k_1} = 1.0211 = e^{\dfrac{E}{R \cdot 2T_1} + \dfrac{E}{RT_1}} = e^{\dfrac{E}{R \cdot 2T_1}}$ $\log(1.0211) = \dfrac{E}{R \cdot 2T_1}$ $R \cdot 2T_1 \cdot \log(1.0211) = E$ that's as far as you can go ... obviously values for $R$ and $T_1$ are required to determine a numerical value for $E$.  
March 14th, 2018, 11:14 AM  #3 
Member Joined: Mar 2016 From: Sweden Posts: 34 Thanks: 4 
Thanks! I thought so, maybe there's something more in the question I don't understand. But thanks a lot for for taking your time to answer


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