Chemical reactions occurs when the colliding reactants have energy that is

Chemical reactions occur when the colliding reactants have energy that is greater than the activation energy. Activation energy is the minimum amount of energy required for a chemical reaction to occur. If the colliding reactants do not have enough energy to meet or exceed the activation energy, the reaction will not take place. In other words, the activation energy acts as a barrier that needs to be overcome for the reaction to proceed. Once the reactants have enough energy to surpass this barrier, they can form new products with a lower energy state than the reactants, which releases energy in the form of heat, light, or other forms of energy. Therefore, only when the colliding reactants have energy greater than the activation energy can they overcome this barrier and form new products with a lower energy state, resulting in a chemical reaction.