The presence of a catalyst affects the activation energy of a reaction by lowering the activation energy, helping the reaction go faster and making it so the reaction does not have to use as much energy to fulfill the products.
it speeds up the process :)
A catalyst changes the reaction mechanism to one with a lower activation energy; activation energy is lowered when a catalyst is added
Activation energy is the energy required by a reaction for the reaction to occur. The catalyst lowers the activation energy, making it easier for the reaction to happen.Improvement:A catalyst don't lowers the activation energy. A catalyst creates a alternative route (*) for the same reaction with a lower activation energy.* = as a result of the interaction of the reagents with the catalyst.
Catalysts doesn't affect the energy of reactions
The activation energy is reduced.
it speeds up the process :)
It lowers it, so the reaction is faster.
It lowers it, so the reaction is faster.
It lowers it, so the reaction is faster.
A catalyst changes the reaction mechanism to one with a lower activation energy; activation energy is lowered when a catalyst is added
Activation energy is the energy required by a reaction for the reaction to occur. The catalyst lowers the activation energy, making it easier for the reaction to happen.Improvement:A catalyst don't lowers the activation energy. A catalyst creates a alternative route (*) for the same reaction with a lower activation energy.* = as a result of the interaction of the reagents with the catalyst.
Catalysts doesn't affect the energy of reactions
The activation energy is reduced.
yes. lowers it.
The presence of a hydrogen peroxide catalyst can increase the rate of a chemical reaction by providing an alternative pathway with lower activation energy, allowing the reaction to occur more quickly.
Catalysts greatly reduce the amount of activation energy needed to begin a reaction.
A catalyst affects a reaction by speeding it up. A catalyst, remember, does not participate as a reactant or product in the reaction. It facilitates the reaction by lowering its activation energy, making the reaction easier to happen.