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What else can I help you with?
What is the minimum energy requirement for a collision with proper alignment to be successful?
The minimum energy requirement for a collision to be successful depends on the specific reaction and molecules involved. Generally, colliding particles need to surpass the activation energy barrier to initiate a successful reaction. This energy is determined by the specific chemical bonds involved and the reaction mechanism.
What statements about activation energy is correct?
Activation energy is the minimum amount of energy required for a chemical reaction to occur. An increase in activation energy leads to a decrease in reaction rate. Catalysts lower the activation energy required for a reaction to proceed, increasing the reaction rate. Activation energy does not affect the overall energy change of a reaction, only the speed at which it occurs.
What are two components of collision theory?
Two components of collision theory are the activation energy, which is the minimum energy required for a reaction to occur, and the orientation of reactant molecules, which dictates the proper alignment needed for effective collisions to take place.
What are two characteristics of an effective collision?
It could be momentum and energy, but I am not 100% sure.
What energy is the energy needed to start a reaction?
Activation Energy.
Does activation energy depend on collision frequency?
No, activation energy is a fixed value for a specific reaction and does not depend on collision frequency. Activation energy is the minimum amount of energy required for a reaction to occur, while collision frequency relates to the number of collisions that occur in a given time period.
A collision may have energy in excess of the activation energy reaction may not occur?
"Collisions may have enough energy to react yet not react if the orientation of the molecules is incorrect. Difficult to explain here without graphics, but basically of the molecules are facing the wrong way it won't happen."
What is it called when energy is required to start a chemical reaction?
An exergonic reaction is activation energy (or energy of activation). An endergonic reaction is essentially the opposite of an exergonic reaction.
When will a collision lead to a chemical reaction?
When the collision is hard and fast enough. Increasing the kinetic energy will increase the likelihood of hard and fast collisions, which will ultimately increase the rate of the reaction. (This is called collision theory.)
What is the collision energy needed to break bonds of an existing one and make new bonds?
I think the term you're looking for might be "activation energy", but if so that's a pretty poor way of describing it, so I'm reluctant to say definitively that that's the answer (there really isn't an answer to the question as written).
What it the term used to describe the energy needed to get a reaction started?
The energy needed to get a reaction started is called activation energy.
Is activation energy added or just there?
Activation energy is the amount of energy that should be gained by potential reactants, for a reaction to occur. A reaction can be occurred by reducing the activation energy of the reaction or increasing the activation energy of the reactants. Activation energy should be added.
What is activation energy How does a catalyst affect activation energy?
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.
What is the minimum energy requirement for a collision with proper alignment to be successful?
The minimum energy requirement for a collision to be successful depends on the specific reaction and molecules involved. Generally, colliding particles need to surpass the activation energy barrier to initiate a successful reaction. This energy is determined by the specific chemical bonds involved and the reaction mechanism.
What does the activation energy for a reaction represent?
Activation energy is the amount of energy needed to start a reaction.
What is the relationship between an energy diagram and activation energy in a chemical reaction?
An energy diagram shows the energy changes that occur during a chemical reaction. Activation energy is the minimum amount of energy required for a reaction to occur. In the energy diagram, the activation energy is the energy barrier that must be overcome for the reaction to proceed. A higher activation energy means a slower reaction, while a lower activation energy means a faster reaction.
What is the minimum amount of energy needed to start a chemical reaction?
The minimum amount of energy needed to start a chemical reaction is called the activation energy. It is the energy required to break the bonds in reactant molecules and initiate the reaction. Once this energy barrier is overcome, the reaction proceeds without additional energy input.
