If the bond dissociation energy for reactants is high then activation energy required for the reaction also will be high.
Activation energy is the minimum energy required for a chemical reaction to occur. It is related to bond energy because breaking chemical bonds and forming new bonds requires energy, which contributes to the activation energy of a reaction. Bonds with higher bond energy are more stable and require more energy to break, hence increasing the activation energy of the reaction.
The strength of a covalent bond is directly related to its bond dissociation energy. The higher the bond dissociation energy, the stronger the covalent bond will be. This energy represents the amount of energy required to break the bond between two atoms.
The activation energy of an endothermic reaction is at least as large as its enthalpy change because the reactants require a minimum amount of energy to reach the transition state where bond-breaking and bond-forming occur. The enthalpy change represents the overall energy difference between reactants and products but does not account for the energy needed to overcome the energy barrier (activation energy) for the reaction to proceed.
The energy required to break a chemical bond and form neutral isolated atoms is called bond dissociation energy or bond energy. It represents the amount of energy needed to break a specific chemical bond in a molecule into its isolated atoms.
The energy needed to break existing chemical bonds during the initiation of a chemical reaction is called the activation energy. This energy is required to overcome the energy barrier between reactants and products, allowing the reaction to proceed. Once the activation energy is reached, the bonds can be broken and new bonds can form.
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.
The activation energy of an endothermic reaction is at least as large as its enthalpy change because the reactants require a minimum amount of energy to reach the transition state where bond-breaking and bond-forming occur. The enthalpy change represents the overall energy difference between reactants and products but does not account for the energy needed to overcome the energy barrier (activation energy) for the reaction to proceed.
They are the same
The energy required to break a chemical bond and form neutral isolated atoms is called bond dissociation energy or bond energy. It represents the amount of energy needed to break a specific chemical bond in a molecule into its isolated atoms.
The strength of a covalent bond is directly related to its bond dissociation energy. The higher the bond dissociation energy, the stronger the covalent bond will be. This energy represents the amount of energy required to break the bond between two atoms.
If the activation energy elated to travelling is high, then a large amount of energy is required to start a chemical reaction. After the reaction is initiated, less energy is needed.
Generally speaking, the lower the activation energy, the more successful collision between molecules will happen.
The relation is:k is the reaction rate coefficient.
An exergonic reaction is activation energy (or energy of activation). An endergonic reaction is essentially the opposite of an exergonic reaction.
The energy needed to break existing chemical bonds during the initiation of a chemical reaction is called the activation energy. This energy is required to overcome the energy barrier between reactants and products, allowing the reaction to proceed. Once the activation energy is reached, the bonds can be broken and new bonds can form.
Greater the bond strength, greater is the bond dissociation energy. (So they are proportional to each other).
In chemistry, activation energy is a term introduced in 1889 by the Swedish scientist Svante Arrhenius that means the minimum energy that must be input to a chemical system with potential reactants to cause a chemical reaction. Activation energy may also be defined as the minimum energy required to start a chemical reaction.The activation energy of a reaction is usually denoted by Ea and given in units of kilojoules per mole
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.