Chemistry, 22.02.2021 18:40, danbat3023
The rate constant for a certain reaction is measured at two different temperatures:
temperature k
376.0 °C 4.8 x 10^8
280.0 °C 2.3 x 10^8
Assuming the rate constant obeys the Arrhenius equation, calculate the activation energy Ea for this reaction.
Answers: 1
![ln \frac{k_{2}}{k_{1}} = \frac{-E_{a}}{R}[\frac{1}{T_{2}} - \frac{1}{T_{1}}]](/tpl/images/1136/3217/c502b.png)
= rate constant at temperature 
= 
= rate constant at temperature 
= 
= activation energy = ?
![ln \frac{4.8\times 10^8}{2.3\times 10^8} = \frac{-E_{a}}{8.314}[\frac{1}{649} - \frac{1}{553}]](/tpl/images/1136/3217/fcab8.png)
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The rate constant for a certain reaction is measured at two different temperatures:
temperature k
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