Arrhenius Equation:

Moderators: Chem_Mod, Chem_Admin

Abigail Volk 1F
Posts: 52
Joined: Fri Sep 29, 2017 7:07 am
Been upvoted: 1 time


Postby Abigail Volk 1F » Tue Mar 06, 2018 10:22 am

Can someone explain how a catalyst can lower activation energy but increase the rate of a reaction? I need help with the conceptual understanding of this

David Minasyan 1C
Posts: 54
Joined: Thu Jul 13, 2017 3:00 am

Re: Catalysts

Postby David Minasyan 1C » Tue Mar 06, 2018 10:27 am

AS far as I know, lowering the activation energy of the reaction means the reaction has less of a barrier to overcome so the reaction would proceed faster.

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

Re: Catalysts

Postby Hannah Guo 3D » Tue Mar 06, 2018 10:28 am

The catalyst lowers the activation energy by providing the reaction an alternative energy pathway. With a catalyst, more collisions result in a reaction because the reactants need less energy to get to the transition state (with the highest energy), so the rate of reaction increases.

Hope it helps!

Mary Becerra 2D
Posts: 53
Joined: Fri Sep 29, 2017 7:06 am

Re: Catalysts

Postby Mary Becerra 2D » Fri Mar 09, 2018 11:08 am

The concept part of it would be that there is an inverse relationship between the activation energy and the rate of a reaction: the lower the activation energy, the higher the rate of the reaction. A catalyst offers an alternative pathway with a lower activation energy, therefore, the reaction goes faster.

JamesAntonios 1E
Posts: 70
Joined: Fri Sep 29, 2017 7:04 am

Re: Catalysts

Postby JamesAntonios 1E » Fri Mar 09, 2018 12:01 pm

The activation energy determines the rate of reaction. To increase the rate of reaction, the activation energy or energy barrier must be lowered. For example, when rolling a ball up a hill and then letting it roll down, the get up the hill is the activation energy. A catalyst just builds a tunnel through the hill to get to the other side.

Yu Chong 2H
Posts: 30
Joined: Fri Sep 29, 2017 7:05 am

Re: Catalysts

Postby Yu Chong 2H » Fri Mar 09, 2018 5:57 pm

Since the rate of reaction and also activation energy depends on successful collision of molecules in the correct orientation, we can think of catalysts as things that helps the reactants collide more frequently in the correct orientation. Some catalyst such as many metals actually allow reactants to adhere to itself. So the reaction takes place on the surface of the catalyst. If you think about it this way, it will be easier for a reactant to collide with another reactant that is already adhere to the surface of the catalyst, thus the catalyst will lower the activation energy and increase the rate of reaction.

Return to “Arrhenius Equation, Activation Energies, Catalysts”

Who is online

Users browsing this forum: No registered users and 1 guest