## Quiz 3 question

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

danielashirazi_1L
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Joined: Fri Sep 25, 2015 3:00 am

### Quiz 3 question

On the Friday Quiz there was a question asking about how k affects affects activation energy.

the course reader says that a higher k will cause lower activation energy but i got this wrong on the quiz. anybody know why?

Jake Ney lecture 1 discussion 1F
Posts: 26
Joined: Fri Sep 25, 2015 3:00 am

### Re: Quiz 3 question

On page 76 the course reader notes that as activation energy increases k decreases. According to the Arrhenius equation k=A*e^(-E/RT) however there can be multiple factors that change if k increases. It is possible that Ea increases as k decreases however this is not definitive. The increase in k can also be caused by an increase in concentration A or an increase in temperature T. Therefore to say higher k will always cause lower activation energy is incorrect.

danielashirazi_1L
Posts: 11
Joined: Fri Sep 25, 2015 3:00 am

### Re: Quiz 3 question

Thank you!

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