## Reaction Graphs

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

Joyce Gu 1E
Posts: 29
Joined: Tue Nov 24, 2015 3:00 am

### Reaction Graphs

When looking at a reaction graph, how do you determine which reactants have the smallest/greatest rate in the forward/reverse direction?

Virpal Gill 1B
Posts: 32
Joined: Thu Jul 27, 2017 3:00 am

### Re: Reaction Graphs

The greater the activation energy of each step, the slower the rate. So the curves with smaller hills/height (whatever you'd like to call them) have lower activation rates and are therefore faster (have greater rates).

Tim Nguyen 2J
Posts: 31
Joined: Sat Jul 22, 2017 3:00 am

### Re: Reaction Graphs

Higher peaks should indicate a slower rate since it takes more energy to overcome the higher activation energy. Lower peaks are easier to overcome thus indicating a lower activation energy.

Guangyu Li 2J
Posts: 50
Joined: Fri Sep 29, 2017 7:07 am
Been upvoted: 1 time

### Re: Reaction Graphs

The greater the activation energy, the longer reactants cost to reach the energy barrier, and the slower the reaction rate. For the endothermic reactions, since products need to overcome a higher energy barrier, the forward reaction is slower than the reverse reaction; For the exothermic reactions, since products need to overcome a lower energy barrier, the reverse reaction is faster than the reverse reaction.

Hope this helps! Good luck in the Final!