Relation between k and activation energy

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

Relation between k and activation energy

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

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

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

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

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

Re: Relation between k and activation energy

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

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!

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