Activation Energy
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Activation Energy
How are the activation energy of the forward and reverse reactions affected when a catalyst is added?
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Re: Activation Energy
Catalysts decrease the activation energy for both the forward and the reverse reactions.
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Re: Activation Energy
Hi! Catalysts decrease activation energy whether a reaction is proceeding in the forward or backward direction.
Re: Activation Energy
Catalysts speeds up a chemical reaction, or lowers the temperature or pressure needed to start one, without itself being consumed during the reaction
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Re: Activation Energy
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.
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Re: Activation Energy
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.
Re: Activation Energy
catalysts decrease the activation and reverse reactions while increasing the forward reactions
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Re: Activation Energy
Catalysts tend to speed up the rate of a reaction as they lower the activation energy.
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Re: Activation Energy
For both forward and reverse processes, catalysts reduce the activation energy.
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Re: Activation Energy
When a catalyst is added, the activation energy of a reaction, regardless of its direction, decreases.
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Re: Activation Energy
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.
Re: Activation Energy
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.
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Re: Activation Energy
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.
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Re: Activation Energy
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.
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.
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Re: Activation Energy
Catalysts reduce the activation energies for both the reverse and forward reaction.
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Re: Activation Energy
Catalysts speed up reactions by lowering the activation energy needed, and they can do this for both the forward and reverse reactions.
Re: Activation Energy
Whether a reaction is in the forward or backward direction, catalysts decrease the activation energy
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Re: Activation Energy
Catalysts will speed up the forward rate of the reaction by decreasing the activation rate.
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Re: Activation Energy
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).
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Re: Activation Energy
The activation energy is always decreased when there is a catalyst, speeding up the forward and reverse reactions.
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Re: Activation Energy
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.
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Re: Activation Energy
Catalysts increase the rate of reaction by decreasing the activation energy. This speeds it in both forward and reverse.
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Re: Activation Energy
For a forward and reverse reaction, a catalyst will decrease the amount of energy needed to initiate the reaction.
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Re: Activation Energy
Catalysts always work to decrease the activation energy of both forward and reverse reactions.
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Re: Activation Energy
Hi!! I think catalysts decrease activation energy for forward and reverse reactions. this is why catalysts do what they do! hope this helps
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Re: Activation Energy
Hi!! I think catalysts decrease activation energy for forward and reverse reactions. this is why catalysts do what they do! hope this helps
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Re: Activation Energy
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.
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Re: Activation Energy
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.
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Re: Activation Energy
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!
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Re: Activation Energy
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.
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Re: Activation Energy
catalysts decrease the activation energy for the reaction in both the forward and reverse.
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Re: Activation Energy
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!
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!
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Re: Activation Energy
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.
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Re: Activation Energy
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.
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Re: Activation Energy
Catalysts lower the activation energy for both forward and reverse reactions so that it is easier for the reaction to start.
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Re: Activation Energy
Hi! Catalysts decrease the activation energy in both forward and reverse reactions.
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Re: Activation Energy
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.
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Re: Activation Energy
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.
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Re: Activation Energy
The activation energy for both the forward and reverse reactions decreases when a catalyst is added. Hope this helps!
Re: Activation Energy
The activation energy required will decrease for both forward and reverse reactions.
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Re: Activation Energy
Catalysts increase the forward rate, while reducing the reverse rate.Catalysts also lower the activation energy need to complete the reaction
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Re: Activation Energy
Catalysts decrease activation energies moving toward the products or reactants
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Re: Activation Energy
Catalysts decrease the activation energy required to start a reaction in both the forward and reverse directions.
Re: Activation Energy
Kayley Steele 3D wrote: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.
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Re: Activation Energy
Hi! Catalysts actually decrease the activation energy that is required to start a reaction in the forward and reverse directions. I hope that helped!
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Re: Activation Energy
Catalysts increase the rate of both the forward and reverse reactions by decreasing the activation energy of both the forward and reverse reactions.
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Re: Activation Energy
Catalysts lower the activation energy so they would help to increase the rates!
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Re: Activation Energy
catalysts reduce the activation energy no matter the direction of the reaction which increases the rate
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Re: Activation Energy
catalysts decrease the energy barrier of the reaction, which is how it speeds up the reaction.
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Re: Activation Energy
Adding a catalyst lowers the activation energy for both the forward and reverse reactions
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Re: Activation Energy
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.
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Re: Activation Energy
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.
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Re: Activation Energy
For both forward and reverse processes, catalysts lower the activation energy.
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Re: Activation Energy
Hannah Carsey 1B wrote: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
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Re: Activation Energy
Hello! Basically, a catalyst works to decrease the amount of activation energy needed in order for the reaction to occur.
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Re: Activation Energy
Catalysts decrease the activation energy for both the forward and reverse directions in a reaction.
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Re: Activation Energy
Hi! In simple terms, catalysts tend to increase the forward rate, and they also reduce the reverse rate. Hope this helped! :)
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Re: Activation Energy
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!
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Re: Activation Energy
Kayley Steele 3D wrote: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.
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Re: Activation Energy
Catalysts decrease the activation energy in both the forward and reverse reactions.
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Re: Activation Energy
When a catalyst is added, the activation energies of both the forward and reverse reactions are lowered.
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Re: Activation Energy
Catalysts have the ability to decrease the activation energy in the forward and reverse reaction.
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Re: Activation Energy
A catalyst lowers the activation energy of both the forward and reverse reactions, because a catalyst changes the mechanism of the reaction.
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Re: Activation Energy
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!
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Re: Activation Energy
The activation energy for the reaction is lowered to the same threshold for both directions.
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Re: Activation Energy
catalysts speed up the reaction process by lowering the activation energy required.
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Re: Activation Energy
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.
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Re: Activation Energy
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.
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Re: Activation Energy
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.
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Re: Activation Energy
Catalysts affect reactions by reducing the amount of activation energy needed for a reaction.
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Re: Activation Energy
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.
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Re: Activation Energy
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.
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Re: Activation Energy
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!
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!
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