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Activation energy describes the energy that is required to get chemical reactions started.
The energy needed to get a reaction started is called activation energy.
Activation energy describes the energy that is required to get chemical reactions started.
Activation energy, usually from a strong oxidizer.
Activation energy is the energy barrier that must be overcome for a chemical reaction to occur. It represents the minimum amount of energy needed to initiate a reaction. A lower activation energy makes a reaction proceed more quickly, while a higher activation energy slows down the reaction.
Activation energy is the term used to describe the energy required to start a chemical reaction by breaking the initial bonds between atoms or molecules. This energy barrier must be overcome in order for the reaction to proceed.
Activation energy describes the energy that is required to get chemical reactions started.
The energy needed to get a reaction started is called activation energy.
ACTIVATION ENERGY IS THE ENERGY WHICH IS REQUIRED FOR INITIALIZING OF ANY TYPE OF REACTION.
activation energy
Activation energy describes the energy that is required to get chemical reactions started.
To get a reaction started, the activation energy must be overcome. This energy barrier is necessary to break the bonds in the reactant molecules and initiate the reaction. Once the activation energy is surpassed, the reaction can proceed on its own.
Even though exothermic reactions release energy overall, they still require an initial input of energy to overcome the activation energy barrier. This energy is needed to initiate the reaction by breaking the existing bonds in the reactant molecules. Once this barrier is crossed, the reaction proceeds spontaneously and releases energy in the form of heat.
Activation energy
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activation energy
The amount of energy needed to start a chemical reaction is known as the activation energy. This energy is required to break the existing bonds in the reactants before new bonds can be formed in the products.