## Equations for activation energy

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

Wendy_Liu_3A
Posts: 27
Joined: Wed Sep 21, 2016 2:55 pm

### Equations for activation energy

I thought ln(k) = -Ea/RT +ln(A) and k = Ae^(-Ea/RT) are equivalent equations. On the course reader, ln(k) = -Ea/RT +ln(A) shows linear but the other k = Ae^(-Ea/RT) does not. I understand that if we plot them one would obviously be linear and the other is not, but what is the significance of pointing out the difference between the two?

Grace_Bower_2B
Posts: 13
Joined: Wed Sep 21, 2016 2:58 pm

### Re: Equations for activation energy

The significance of pointing out the difference between the two is it's sometimes useful to have the linear equation. It makes it easy to see how temperature affects the reaction constant K from an equation or a plot. If you were given a plot of the non-linear Arrhenius equation it would be a lot more difficult to tease out how the temperature is affecting the reaction constant.
If you're wondering why they're both on the equation sheet, it's just because Mr. Lavelle is nice. Technically speaking, you don't need both because it's very easy to derive the linear version from the non-linear version, but it's nice to not have an extra step to do on tests and quizzes.