Search results
Results From The WOW.Com Content Network
In chemical thermodynamics, an endergonic reaction (from Greek ἔνδον (endon) 'within' and ἔργον (ergon) 'work'; 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 ...
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.
and they have positive (endergonic) or negative (exergonic) Gibbs free energies of reaction . As Marcus calculations refer exclusively to the electrostatic properties in the solvent (outer sphere) Δ G ∘ {\displaystyle \Delta G^{\circ }} and λ 0 {\displaystyle \lambda _{0}} are independent of one another and therefore can just be added up.
[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 .
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.
Image source: Getty Images. 1. The stock looks like a bargain. Dollar General is currently being priced as a no-growth company in secular decline.
The change of Gibbs free energy (ΔG) in an exergonic reaction (that takes place at constant pressure and temperature) is negative because energy is lost (2). In chemical thermodynamics, an exergonic reaction is a chemical reaction where the change in the free energy is negative (there is a net release of free energy). [1]
From January 2008 to December 2012, if you bought shares in companies when John L. Hennessy joined the board, and sold them when he left, you would have a -8.3 percent return on your investment, compared to a -2.8 percent return from the S&P 500.