Relation between k and activation energy

Moderators: Chem_Mod, Chem_Admin

Mishta Stanislaus 1H
Posts: 45
Joined: Fri Sep 29, 2017 7:04 am

Relation between k and activation energy

Postby Mishta Stanislaus 1H » Sun Mar 11, 2018 11:01 pm

What exactly is the relationship between k and activation energy?

Lily Sperling 1E
Posts: 49
Joined: Tue Oct 10, 2017 7:14 am

Re: Relation between k and activation energy

Postby Lily Sperling 1E » Sun Mar 11, 2018 11:22 pm

You can observe the relationship through the Arrhenius Equation - basically, the formula implies that the rate constant increases exponentially as the activation energy decreases.

Christina Cen 2J
Posts: 53
Joined: Sat Jul 22, 2017 3:01 am

Re: Relation between k and activation energy

Postby Christina Cen 2J » Sun Mar 11, 2018 11:44 pm

Reactions generally speed up when temperature increases and slow down when temperature decreases. This means that k increases with increasing temperature, which in turn increases the overall rate of the reaction.

diangelosoriano
Posts: 49
Joined: Fri Sep 29, 2017 7:07 am

Re: Relation between k and activation energy

Postby diangelosoriano » Mon Mar 12, 2018 4:01 pm

If a catalyst were added, how would this also affect k or activation energy?

Johann Park 2B
Posts: 51
Joined: Thu Jul 27, 2017 3:01 am
Been upvoted: 1 time

Re: Relation between k and activation energy

Postby Johann Park 2B » Mon Mar 12, 2018 4:36 pm

diangelosoriano wrote:If a catalyst were added, how would this also affect k or activation energy?


When you add a catalyst, the reaction is sped up - k is increased and Ea is lowered. The new pathway has a lower activation energy.

Nehal Banik
Posts: 64
Joined: Thu Jul 13, 2017 3:00 am

Re: Relation between k and activation energy

Postby Nehal Banik » Mon Mar 12, 2018 4:41 pm

As activation energy decreases, it reduces the energy barrier required for the reaction to proceed therefore the rate constant increases, causes the overall rate of the reaction to increase. Also, if the activation energy is higher, the dependence of the rate constant on temperature increases, meaning at higher temperatures the rate constant is most likely going to be higher. These are a couple of the relationships that can be understood from the Arrhenius equation in the textbook.
Hope that helps!


Return to “*Free Energy of Activation vs Activation Energy”

Who is online

Users browsing this forum: No registered users and 2 guests