Activation energy is the minimum amount of energy required for a chemical reaction to occur. It is the energy needed to break the bonds of reactant molecules so that they can form new products.
Activation energy is important because it determines the rate of a chemical reaction. Reactions with high activation energy require more energy to occur, and therefore, happen at a slower rate. It also helps to ensure that reactions are not spontaneous and out of control, which could be dangerous.
The activation energy of a reaction can be determined experimentally by measuring the reaction rate at different temperatures and using the Arrhenius equation. It can also be estimated using computational methods and theoretical models.
Yes, activation energy can be changed. Increasing the temperature can lower the activation energy, making the reaction happen faster. Catalysts can also lower the activation energy by providing an alternate pathway for the reaction to occur.
When the activation energy is too high, the reaction will not occur at a significant rate, or it may not occur at all. This can be problematic in industrial processes where reactions need to happen quickly. High activation energy can also make a reaction more difficult to control and lead to unwanted byproducts.