Activation Energy
Activation energy is the minimum amount of energy needed to start a chemical reaction. Think of it like a hill that reactants must climb to transform into products. Even if a reaction is favorable, it won’t happen until enough energy is provided to reach the top of this hill. This energy can come from heat, light, or other sources. Once the reaction begins, it can continue on its own, similar to how a ball rolls down a hill. Understanding activation energy helps explain why some reactions occur quickly while others take longer.
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Activation energy is the minimum energy required for a chemical reaction to occur. Think of it as the energy needed to "push" reactants over a barrier to transform into products. This barrier prevents reactions from happening spontaneously at lower energy levels. Imagine trying to roll a ball up a hill: you need a certain amount of energy to get it over the top. Once it's over, it can roll down easily. Similarly, once enough energy is supplied to overcome the activation energy, reactions can proceed more readily, leading to the formation of new substances.