If the activation energy of a reaction is high, then it requires a large amount of energy to initiate the reaction. The situation arising when a spontaneous reaction has a large activation energy is similar to rolling a ball over a hill. At first, energy must be expended to move the ball to the crest of the hill (or, in the case of a reaction, impart enough energy to the molecules so that their bonds can be sufficiently weakened). However, once the ball is at the top of the hill, it rolls down on its own. This is analogous to the reforming of chemical bonds, which releases energy. High activation energies are typical when a reaction involves molecules whose bonds are strong.
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.
This energy is called "energy of activation", it is used to overcame the energy barrier between reactants and products.
Activation energy is the amount of energy needed to start a reaction.
Activation Energy is the required energy needed in order for a chemical reaction to start.
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.
activation energy
An exergonic reaction is activation energy (or energy of activation). An endergonic reaction is essentially the opposite of an exergonic 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.
That is called the activation energy or energy of activation (Ea).
The energy needed to get a reaction started is called 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.
Activation energy describes the energy that is required to get chemical reactions started.
Activation energy is energy or power conducted that can be instantly activated for use when flick a light switch you used activation energy.
This energy is called "energy of activation", it is used to overcame the energy barrier between reactants and products.
Enzymes reduce activation energy, which is the energy required to start a chemical reaction. By lowering the activation energy, enzymes make reactions occur more readily and at a faster pace.
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.
Enzymes function when they lower the activation energy. That means it takes less energy for the reaction to work.