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7 de mar. de 2021 · 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.
- The Editors of Encyclopaedia Britannica
The activation energy of a chemical reaction is closely related to its rate. Specifically, the higher the activation energy, the slower the chemical reaction will be. This is because molecules can only complete the reaction once they have reached the top of the activation energy barrier.
- The official definition of activation energy is a bit complicated and involves some calculus. But to simplify it: Activation energy is the minimum...
- Exothermic and endothermic refer to specifically heat. Exergonic and endergonic refer to energy in general.
- Endothermic and exothermic refers to sign of the enthalpy of a reaction. Whether the net enthalpy change is positive or negative respectively. Wher...
- yeah, like amathakbari said-activation energy is the amount of energy needed to activate the complex that ocurrs at the transition state. it isn't...
- Theoretically yes, but practically no. So this concept can be visualized with combustion or fire. While wood does not spontaneously burst into flam...
- In an exothermic reaction, the energy is released in the form of heat, and in an industrial setting, this may save on heating bills, though the eff...
- Activation energy is the amount of energy needed to initiate a reaction.
La energía de activación de una reacción química es como esa "barrera" que tienes que superar para levantarte de la cama. Incluso las reacciones que liberan energía (exergónicas) requieren cierto aporte de energía para comenzar antes de que puedan proceder con sus pasos de liberación de energía.
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. The activation energy (E a) of a reaction is measured in kilojoules per mole (kJ/mol) or kilocalories per mole (kcal/mol).
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.
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.
