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  2. Activation energy - Wikipedia

    en.wikipedia.org/wiki/Activation_energy

    Activation energy can be thought of as the magnitude of the potential barrier (sometimes called the energy barrier) separating minima of the potential energy surface pertaining to the initial and final thermodynamic state. For a chemical reaction to proceed at a reasonable rate, the temperature of the system should be high enough such that ...

  3. Activation - Wikipedia

    en.wikipedia.org/wiki/Activation

    The energy of activation [1] specifies the amount of free energy the reactants must possess (in addition to their rest energy) in order to initiate their conversion into corresponding products—that is, in order to reach the transition state for the reaction. The energy needed for activation can be quite small, and often it is provided by the ...

  4. Activated complex - Wikipedia

    en.wikipedia.org/wiki/Activated_complex

    The activation energy is the minimum amount of energy to initiate a chemical reaction and form the activated complex. [6] The energy serves as a threshold that reactant molecules must surpass to overcome the energy barrier and transition into the activated complex.

  5. Collision theory - Wikipedia

    en.wikipedia.org/wiki/Collision_theory

    The activation energy is often predicted using the Transition state theory. Increasing the concentration of the reactant brings about more collisions and hence more successful collisions. Increasing the temperature increases the average kinetic energy of the molecules in a solution, increasing the number of collisions that have enough energy.

  6. Transition state theory - Wikipedia

    en.wikipedia.org/wiki/Transition_state_theory

    The free energy of activation, ΔG ‡, is defined in transition state theory to be the energy such that ‡ = ⁡ ‡ ′ holds. The parameters ΔH ‡ and ΔS ‡ can then be inferred by determining ΔG ‡ = ΔH ‡ – TΔS ‡ at different temperatures.

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  8. Chemical reaction - Wikipedia

    en.wikipedia.org/wiki/Chemical_reaction

    Activation energy, which is defined as the amount of energy required to make the reaction start and carry on spontaneously. Higher activation energy implies that the reactants need more energy to start than a reaction with lower activation energy.

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