Achemist sets up a chemical reaction but finds that none of the reactant molecules have a required activation energy. what is the result ? a.) products will form with less energy input b.) no products with be formed c.) the products will form to quickly d.) products will convert to reactants

Activation energy is the minimum amount of energy that the colliding reactant molecules must possess for the formation of products. Lower the activation energy, higher will be chance of formation of products. So activation energy is the minimum energy requirement that has to overcome for the reaction to be completed. Therefore, when in a chemical reaction the reactant molecules do not collide with required activation energy, the collisions will not be fruitful even if they are properly oriented which means that the products will not form.

Hence the correct answer will be B.) no products will be formed

i think its 5049.

i hope this !