Energy and Metabolism

ID #1092

If a reaction requires an input of energy to proceed, does that mean that it is energetically unfavorable to begin with?

Typically, if a reaction requires a lot of energy to proceed (an endergonic reaction), that is an indication that the substrate molecule is pretty stable to begin with. This would be considered an energetically favorable state, since the molecule is "happier" and therefore less reactive. If you put enough energy into the system, you can make it reactive, yielding a product that is at a higher energy level. This makes the product more reactive. So yes, a reaction that requires energy is energetically unfavorable.

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