[Answer] What is the basic difference between exergonic and endergonic reactions?

Answer: Exergonic reactions release energy; endergonic reactions absorb it.

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What is the basic difference between exergonic and endergonic reactions? In chemical thermodynamics an endergonic reaction (also called a heat absorbing nonspontaneous reaction or an unfavorable reaction) is a chemical reaction in which the standard change in free energy is positive and an additional driving force is needed to perform this reaction. In layman's terms the total amount of useful energy is negative (it takes more energy to start the reaction than what is rec… In chemical thermodynamics an endergonic reaction (also called a heat absorbing nonspontaneous reaction or an unfavorable reaction) is a chemical reaction in which the standard change in free energy is positive and an additional driving force is needed to perform this reaction. In layman's terms the total amount of useful energy is negative (it takes more energy to start the reaction than what is received out of it) so the total energy is a negative net result. For an overall gain in the net result see exergonic reaction. Another way to phrase this is that useful energy must be absorbed from the surroundings into the workable system for the reaction to happen. Under constant temperature and constant pressure conditions this means that the change in the standard Gibbs free energy would be positive ${\displaystyle \Delta G^{\circ }>0}$for the reaction at standard state (i.e. at standard pressure (1 bar) and standard concentrations (1 molar) of all the reagents). In metabolism an endergonic process is anabolic meaning that energy is stored; in many such anabolic processes energy is supplied by coupling the reaction to adenosine triphosphate (ATP) and consequently resulting in a high energy negatively charged organic phosphate and positive adenosine diphosphate. The equilibrium constant for the reaction is related to ΔG° by the relation: ${\displaystyle K=e^{-{\frac {\Delta G^{\circ }}{RT}}}}$ where T is the absolute temperature and R is the gas constant . A positive value of ΔG° therefore implies The equilibrium constant for the reaction is related to ΔG° by the relation: ${\displaystyle K=e^{-{\frac {\Delta G^{\circ }}{RT}}}}$ where T is the absolute temperature and R is the gas constant . A positive value of ΔG° therefore implies ${\displaystyle K<1\ }$ so that starting from molar stoichiometric quantities such a reaction would move backwards toward equilibrium not forwards. Nevertheless endergonic reactions are quite common in nature especially in biochemistry and physiology . Examples of endergonic reactions in cells include protein synthesis and the Na /K pump which drives nerve conduction and muscle contraction . Mon Sep 13 2004 · An exergonic process is one which there is a positive flow of energy from the system to the surroundings. This is in contrast with an endergonic process. Constant pressure constant temperature reactions are exergonic if and only if the Gibbs free energy change is negative (∆G < 0). " Exergonic " (from the prefix exo- derived for the Greek word ἔξω exō "outside" and the suffix … ...

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