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In chemistry and physics, activation energy is the minimum amount of energy needed to start a chemical reaction. Reactants often get activation energy from heat, but sometimes energy comes from light or energy released by other chemical reactions.
Activation energy, in chemistry, the minimum amount of energy that is required to activate atoms or molecules to a condition in which they can undergo chemical transformation or physical transport. Activation energies are determined from experimental rate constants or diffusion coefficients.
In the Arrhenius model of reaction rates, activation energy is the minimum amount of energy that must be available to reactants for a chemical reaction to occur. [1] The activation energy (E a) of a reaction is measured in kilojoules per mole (kJ/mol) or kilocalories per mole (kcal/mol). [2]
In chemistry, activation energy is the minimum amount of energy required for a chemical reaction. The activation energy can be thought of as the magnitude of a potential barrier that the reacting molecules need to overcome to initiate a reaction and convert into products.
The activation energy (Ea), labeled ΔG ‡ in Figure 2, is the energy difference between the reactants and the activated complex, also known as transition state. In a chemical reaction, the transition state is defined as the highest-energy state of the system.
Activation energy is defined as the minimum amount of extra energy required by a reacting molecule to get converted into a product. It can also be described as the minimum amount of energy needed to activate or energise molecules or atoms so that they can undergo a chemical reaction or transformation.
Activation energy is the minimum amount of energy required to initiate a reaction. It is the height of the potential energy barrier between the potential energy minima of the reactants and products. Activation energy is denoted by E a and typically has units of kilojoules per mole (kJ/mol) or kilocalories per mole (kcal/mol).
Activation energy refers to the amount of energy required to initiate a reaction. Activation energy, commonly represented as Ea, is usually measured in joules (J) and or kilojoules per mole (kJ/mol) or kilocalories per mole (kcal/mol). Activation energy depends on two factors.
The activation energy is the minimum energy required for a reaction to occur. This means that the reactant molecules have enough kinetic energy to collide successfully and...
The activation energy for a reaction is the minimum energy that colliding particles must have in order to undergo a reaction. Some reactions occur readily at room temperature because the reacting particles already have the requisite activation energy at that temperature.