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Endergonic reactions can be achieved if they are either pulled or pushed by an exergonic (stability increasing, negative change in free energy) process. Of course, in all cases the net reaction of the total system (the reaction under study plus the puller or pusher reaction) is exergonic.
[1] [2] These reactions require energy, known also as an endergonic process. [3] Anabolism is the building-up aspect of metabolism, whereas catabolism is the breaking-down aspect. Anabolism is usually synonymous with biosynthesis.
An endergonic reaction is an anabolic chemical reaction that consumes energy. [3] It is the opposite of an exergonic reaction. It has a positive ΔG because it takes more energy to break the bonds of the reactant than the energy of the products offer, i.e. the products have weaker bonds than the reactants.
The chain of redox reactions driving the flow of electrons through the electron transport chain, from electron donors such as NADH to electron acceptors such as oxygen and hydrogen (protons), is an exergonic process – it releases energy, whereas the synthesis of ATP is an endergonic process, which requires an input of energy.
An exergonic reaction (such as cellular respiration) is a reaction that releases free energy in the process of the reaction. The progress of the reaction is shown by the line. Activation energy (1) slows down the reaction.
For exergonic and endergonic reactions, see the separate articles: Endergonic reaction; Exergonic reaction; See also. Exergonic process; Endergonic;
The reaction will only be allowed if the total entropy change of the universe is zero or positive. This is reflected in a negative ΔG, and the reaction is called an exergonic process. If two chemical reactions are coupled, then an otherwise endergonic reaction (one with positive ΔG) can be made to happen.
The reaction products of the combustion of methane are carbon dioxide and water. Products are the species formed from chemical reactions. [1] During a chemical reaction, reactants are transformed into products after passing through a high energy transition state. This process results in the consumption of the reactants.