What is the Difference Between Endergonic and Exergonic?

The main difference between endergonic and exergonic reactions lies in the release or absorption of free energy.

• Exergonic reactions release free energy and are considered spontaneous reactions, meaning they can occur without the addition of energy. These reactions have a negative Gibbs free energy (∆G) value, indicating that the reactants have more free energy than the products.
• Endergonic reactions absorb free energy and require an input of energy to occur. These reactions have a positive Gibbs free energy (∆G) value, indicating that the products have more free energy than the reactants.

In summary:

Exergonic reactions occur in various organisms, such as the synthesis and breakdown of adenosine triphosphate (ATP), which is the "energy currency" of the cell. On the other hand, endergonic reactions require energy to proceed, and they are essential for various biological processes, including the synthesis of complex molecules.

Comparative Table: Endergonic vs Exergonic

Here is a table comparing endergonic and exergonic reactions:

Endergonic reactions have a positive Gibbs free energy (ΔG), meaning that energy is stored in the products, while exergonic reactions have a negative ΔG, indicating that energy is released to the environment. Endergonic reactions are non-spontaneous and require additional energy to proceed, whereas exergonic reactions are spontaneous and occur without the addition of energy.