Activation Energy

[Kayley Steele 3D]

How are the activation energy of the forward and reverse reactions affected when a catalyst is added?

[Kaleigh Olla 1L]

Catalysts decrease the activation energy for both the forward and the reverse reactions.

[Gianna Greco 1G]

Hi! Catalysts decrease activation energy whether a reaction is proceeding in the forward or backward direction.

[105740916]

Catalysts speeds up a chemical reaction, or lowers the temperature or pressure needed to start one, without itself being consumed during the reaction

[Benicio Rivera 1F]

Catalysts lower the activation energy for the reaction. Catalysts will not alter the equilibrium of the reaction. Catalysts do not alter the energy change between the products and reactants. Catalysts increase the forward rate, while reducing the reverse rate.

[Talia Tam 3L]

Catalysts lower the activation energy for both forward and reverse reactions.

[Tammy Shen 2L]

Catalysts or enzymes speed up the forward rate of the reaction by lowering the activation rate. They are also not consumed during the reaction. However, it's also important to note that when its in the reaction, the rate of the reaction is independent of the concentration of R.

[Om Patel]

catalysts decrease the activation and reverse reactions while increasing the forward reactions

[Neelaj Das 3I]

Catalysts tend to speed up the rate of a reaction as they lower the activation energy.

[krish shah]

For both forward and reverse processes, catalysts reduce the activation energy.

[Celine Khuu 2F]

When a catalyst is added, the activation energy of a reaction, regardless of its direction, decreases.

[Vanessa Wiratmo 3k]

Activation energy is the energy needed to facilitate a chemical reaction. The addition of a catalyst lowers the activation energy needed for a reaction to undergo. This works in the forward and reverse direction.

[Henry_2A]

A catalyst decreases the activation energy, which thus increases the rate of the forward and reverse reactions. It's important to note that this does not mean there's an energy change between products and reactants.

[Anubhav_Chandla1G]

Catalysts boost forward rates while lowering reverse rates. The activation energy of forward and reverse processes is reduced by using a catalyst, which raises the pace of the reactions.

[Evonne Chau 2I]

Hi Kayley,

Catalysts can be used to speed up the forward rate of the reaction, so when it's added, it lowers/decreases the activation energy. In addition, it reduces the reverse rate.

[Anish_Marripati_2F]

Catalysts reduce the activation energies for both the reverse and forward reaction.

[Charly Ng 1K]

Catalysts speed up reactions by lowering the activation energy needed, and they can do this for both the forward and reverse reactions.

[305589333]

Whether a reaction is in the forward or backward direction, catalysts decrease the activation energy

[BriannaDis2C]

Catalysts will speed up the forward rate of the reaction by decreasing the activation rate.

[Skylar Lo 2C]

Catalysts will lower the activation energy.

[14b_student 2E]

The catalysts decrease the activation energy in both circumstances.

[Praveena Ratnavel - 1A]

Catalysts lower the activation energy for both, which means that a catalyst can decrease the reaction rate (you can see this mathematically in the Arrhenius equation).

[WedaadDis3k]

The activation energy for both are decreased by a catalyst

[Ashrita Singh 2F]

The activation energy is always decreased when there is a catalyst, speeding up the forward and reverse reactions.

[Ryan Blaydon 1K]

As everyone has mentioned a catalyst lowers the activation energy for both the forward and reverse reactions. I do also believe that the forward and reverse reactions will speed up equally.

[Sidharth Paparaju 3B]

I believe catalysts reduce activation energy in general.

[Mara Crooks 1F]

Catalysts increase the rate of reaction by decreasing the activation energy. This speeds it in both forward and reverse.

[Bailey Herbert 2L]

For a forward and reverse reaction, a catalyst will decrease the amount of energy needed to initiate the reaction.

[Aaron Li 1D]

Catalysts will decrease the activation energy.

[Misha_Khan_2H]

Catalysts always work to decrease the activation energy of both forward and reverse reactions.

[Achyutha Kodavatikanti_3H]

adding a catalyst --> activation energy for the reaction is reduced

[Mari Masunaga 1G]

Hi!! I think catalysts decrease activation energy for forward and reverse reactions. this is why catalysts do what they do! hope this helps

[Mari Masunaga 1G]

Hi!! I think catalysts decrease activation energy for forward and reverse reactions. this is why catalysts do what they do! hope this helps

[Zoe Dhalla 3I]

Catalysts lower the activation energy for the reaction. Catalysts increase the forward rate, while reducing the reverse rate. Correct answer: Catalysts increase the forward rate, while reducing the reverse rate.

[Rebekah Jung 1C]

The reverse and forward reaction rate is faster when a catalyst is present because it lowers activation energy required for the reaction to take place.

[Heba Bounar 3K]

Hi! Catalysts increase the rate of the forward reaction by lowering the activation energy. You should also know that when a catalyst is required in a reaction, the rate of the reaction is independent of the concentration of reactants. Hope that helps!

[Dillon Taing 3H]

Regardless of the direction of the reaction, a catalyst will function by reducing the activation energy of the reaction. The rate of the forward reaction increases while the reverse reaction decreases, but the reaction has the same equilibrium constant.

[Windell Viste 1K]

Catalysts decrease the activation energy for both

[105740916]

catalysts decrease the activation energy for the reaction in both the forward and reverse.

[Andrewtrung Le 3A]

Catalysts decrease the activation energy for both the forward and reverse reactions!

Remember that they lower the "hill" that is the activation energy, so no matter which direction you go along the graph, the hill will be less steeper!

[Alice Weber 3I]

Hi, catalysts decrease activation energy for forward and reverse reactions.

[Ashley Presnell 1C]

Catalysts can lower the barrier of activation energy, to make it easier for a reaction to start. This means a catalyst can lower the activation energy necessary for a reaction to start, speeding up the reaction overall and requiring less energy.

[Saatvika Nair]

Basically, the main job of catalysts is to lower the activation energy of a reaction and speed it up. This is because if the activation energy is lowered, it takes up less time for the system to build up enough energy to initiate the reaction (hence speeding it up!). One important thing to note though is that catalysts don't impact the equilibrium constant in any way.

[Chelsea Tran 3H]

Catalysts lower the activation energy for both forward and reverse reactions so that it is easier for the reaction to start.

[Emily Quill 2H]

Hi! Catalysts decrease the activation energy in both forward and reverse reactions.

[Eric Sun 2G]

Catalysts lower the activation energy of a reaction.

[Adithi Ayyala 2G]

Hello! Essentially the reaction follows the same pathway (same reactant and product concentrations) but the energy required to produce these products is lowered by the catalyst.

[HemangD 3K]

When a catalyst is added, the activation energy of both the forward and reverse reactions is lowered. Hence, both the forward and reverse reactions occur at a faster rate.

[Mia Orr 3B]

The activation energy for both the forward and reverse reactions decreases when a catalyst is added. Hope this helps!

[Jieun 2C]

The activation energy required will decrease for both forward and reverse reactions.

[Debie_Morales1D]

Catalysts increase the forward rate, while reducing the reverse rate.Catalysts also lower the activation energy need to complete the reaction

[Caitlin_Doak_2H]

Catalysts decrease activation energies moving toward the products or reactants

[madeleine_lim_2A]

Catalysts decrease the activation energy required to start a reaction in both the forward and reverse directions.

[105784203]

How are the activation energy of the forward and reverse reactions affected when a catalyst is added?

The activation energy is the same with or without a catalyst, but the rxn rate is different.

[Mahika Saoji 3K]

Hi! Catalysts actually decrease the activation energy that is required to start a reaction in the forward and reverse directions. I hope that helped!

[Rachel Yu 3K]

Catalysts increase the rate of both the forward and reverse reactions by decreasing the activation energy of both the forward and reverse reactions.

[Sydney Ngao 3I]

Catalysts lower the activation energy so they would help to increase the rates!

[Jacob_Eberson_2D]

catalysts reduce the activation energy no matter the direction of the reaction which increases the rate

[Helen Ringley 2E]

catalysts decrease the energy barrier of the reaction, which is how it speeds up the reaction.

[Morgan Micallef 1A]

Adding a catalyst lowers the activation energy for both the forward and reverse reactions

[Hannah Carsey 1B]

When a catalyst is added to a reaction, the activation energy (Ea) for both the forward and reverse reactions is decreased. The activation energy (Ea) of a reaction is the minimum amount of energy that is required to activate atoms or molecules to a condition in which they can undergo a chemical reaction.

[Ivy Vo Dis 1C]

Adding a catalyst to a reaction will decrease the activation energy for the forward and reverse reactions. By decreasing the activation energy, the reaction is able to happen at a lower energy, meaning it can happen faster.

[Konmal Ali 1G]

For both forward and reverse processes, catalysts lower the activation energy.

[WS405590915]

When a catalyst is added to a reaction, the activation energy (Ea) for both the forward and reverse reactions is decreased. The activation energy (Ea) of a reaction is the minimum amount of energy that is required to activate atoms or molecules to a condition in which they can undergo a chemical reaction.

This was really helpful and clarified the topic for me.

Thanks

[davis sandberg 2H]

Catalysts decrease the activation energy of the forward reaction.

[Matthew Li 1B]

the activation energy is decreased

[205819952]

Catalysts reduce activation energy in both forward and reverse reactions.

[205819952]

Catalysts reduce activation energy in both forward and reverse reactions.

[Nathan Morgan 2C]

Hello! Basically, a catalyst works to decrease the amount of activation energy needed in order for the reaction to occur.

[Neha Mukund]

Catalysts decrease the activation energy for both the forward and reverse directions in a reaction.

[Alejandra Hernandez 2A]

Hi! In simple terms, catalysts tend to increase the forward rate, and they also reduce the reverse rate. Hope this helped! :)

[Sophia Hartwell 1F]

Hi! Catalysts can be used to increase the forward rate of the reaction, which lowers/increases the activation energy when applied. Furthermore, it lowers the reversal rate. Hope that this was helpful!

[Claire Kim 1F]

How are the activation energy of the forward and reverse reactions affected when a catalyst is added?

When a catalyst is added to a reaction, it helps the reaction take place, therefore decreasing the required amount of activation energy. Knowing this, the activation energy of the forward and reverse reactions should both be decreased.

[Rachel Bartley 2B]

Catalysts decrease the activation energy in both the forward and reverse reactions.

[elliemehrara]

When a catalyst is added, the activation energies of both the forward and reverse reactions are lowered.

[sidneypalacios]

Catalysts have the ability to decrease the activation energy in the forward and reverse reaction.

[isabella garcia - 1G]

A catalyst lowers the activation energy of both the forward and reverse reactions, because a catalyst changes the mechanism of the reaction.

[Phoebe Ko 3E]

Hi, catalysts decrease the activation energies for both forward and reverse reactions, so that rates of both reactions will be increased. I hope this was helpful!

[Andrew_Ramirez]

The activation energy for the reaction is lowered to the same threshold for both directions.

[Polo Morales 3C]

Catalysts decrease the activation energy in both directions. Hope this helps!

[405690892]

catalysts speed up the reaction process by lowering the activation energy required.

[Audric Banuelos 1A]

The purpose of a catalyst is to speed up the reaction. Therefore, the activation energy would decrease when a catalyst is added for both the forward and reverse reactions.

[Akilah Beatty 2k]

In both situations, the activation energy will decrease.

[Shubhreet Bhullar 3C]

Now, in order for a reaction to occur, their must be a minimum activation energy and the particles must collide in a certain orientation. The catalyst helps to do this by binding with a reactant in order to make it easier for the other reactant(s) to collide. The catalyst also decreases the minimum activation energy that is needed in the collision for the reaction to occur (on a molecular, micro level). Now, the catalyst decreases The activation energy of both the forward and backward (reverse) reaction by the same amount/factor. This means that activation energy doesn't affect the K value in equilibrium.

[Jarod Miller 2E]

Catalysts affect reactions by decreasing the activation energy in both the forward and reverse reactions. Due to the decrease in activation energy the catalysts help speed up reactions.

[Student805]

Catalysts affect reactions by reducing the amount of activation energy needed for a reaction.

[Trinabh Khera Sahni]

A catalyst lowers the activation energy for both the forward and reverse reactions. The activation energy is the minimum energy required for a reaction to occur. Higher activation energy means that fewer molecules have the required energy to undergo the reaction. By lowering the activation energy, a catalyst increases the number of molecules with sufficient energy to react this increases the rate of the reaction. The effect of a catalyst on the activation energy is due to its ability to provide an alternative pathway for the reaction to occur. This alternative pathway has lower activation energy than the original pathway meaning that more molecules can overcome the energy barrier. Because the catalyst provides a lower-energy pathway for both the forward and reverse reactions, the equilibrium position of the reaction is not affected by the addition of a catalyst. This means that the equilibrium constant remains the same but the reaction rate is increased.

[Saba Honarvar 3A]

Catalysts would be lowering the activation energy for the reaction. Catalysts do not alter the energy change between the products and reactants but rather increase the forward rate, while reducing the reverse rate. The higher the activation energy, the slower the chemical reaction will be. This is because molecules can only complete the reaction once they have reached the top of the activation energy barrier. But by lowering the activation energy, what you are doing is adding a catalyst, which would increase the number of molecules with energy to react and increases the rate of the reaction.

[Kimberly_Wu_3H]

Catalysts lower the activation energy for forward and reverse reactions.

[AliciaRoice_1K]

Hello!

Catalysts work in the same way, whether a forward or reverse reaction is occurring. This is because a reaction itself is still occurring, whether it is going in the the forward direction or the reverse direction, so it will complete its function regardless of what direction the reaction is doing in.

As for what catalysts do to the activation energy, catalysts are responsible for decreasing the activation energy for a reaction. The activation energy is the energy that the reaction must reach in order for a specific reaction to occur. Therefore, reactions with a high activation energy may take a longer time to occur that reactions with lower activation energies. Hence, by decreasing the activation energy, catalysts help speed up the rate of a chemical reaction, allowing it to occur faster with less expenditure in energy.

Hope this helps!