The minimum amount of energy required for effective collisions between reacting particles is known as
Answer Details
Activation energy is the minimum amount of energy required for effective collisions between reacting particles.
In a chemical reaction, reactant molecules must collide with a certain minimum amount of kinetic energy in order for the reaction to occur. The reactant molecules must also collide with the correct orientation in order for the reaction to take place. The minimum amount of energy required for these effective collisions is known as the activation energy.
Activation energy is a barrier that must be overcome for a reaction to occur. This barrier can be overcome by increasing the temperature of the reaction, since this increases the kinetic energy of the reactant molecules, making them more likely to collide with sufficient energy to react. Alternatively, a catalyst can be used to lower the activation energy barrier and increase the rate of the reaction.
In summary, the correct option in the question is activation energy, which is the minimum amount of energy required for effective collisions between reacting particles.