## 15.65 (c)

$K = \frac{k_{forward}}{k_{reverse}}$

Hannah Guo 3D
Posts: 56
Joined: Fri Sep 29, 2017 7:06 am

### 15.65 (c)

Why k increases more for reaction with higher activation energy?

Thank you!

Gurshaan Nagra 2F
Posts: 49
Joined: Thu Jul 27, 2017 3:01 am

### Re: 15.65 (c)

The reasoning is better explained in section 15.11, but I believe it is due to the reaction having Arrhenius behavior, which allowed for the conclusion to be made about the k relating to activation energy.

Emily Oren 3C
Posts: 50
Joined: Fri Sep 29, 2017 7:07 am

### Re: 15.65 (c)

This can be seen in the Arrhenius equation: ln(k)=-Ea/RT+ln(A) where Ea is the activation energy. The slope of the line plotted on a ln(k) vs 1/T graph is -Ea/R. This means that for higher activation energies, the slope is more steeply negative so the ln(k) value, and also the k value, changes more rapidly with time than for lower activation energies.