BIOCHEM 420 Lecture Notes - Lecture 6: Exergonic Reaction, Exergonic Process, Endergonic Reaction
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15 Jan 2017
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Lecture 6 and 7: draw a concept map using the terms: free energy, enthalpy, entropy, standard free energy, exergonic, endergonic, k, and, free energy (g): maximum potential usable energy. The change in gibbs free energy during a reaction provides information about the reaction energetics and spontaneity. Difference between the g of reactants & g of products. G indicates whether the reaction releases or requires energy: negative g: products are at a lower energy than the reactants = exergonic. Exergonic reactions: - g, releases energy, spontaneous & favorable. These reactions can proceed without an input of energy: positive g: products are at a higher energy than the reactants = endergonic. Endergonic reactions: + g, consumes free energy (requires energy input in order to proceed) Nonspontaneous & not favorable: enthalpy (h): measure of the internal energy (heat) of the system. Change in internal energy going from reactants to products is measured by the heat absorbed or released.
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1. An exergonic reaction is one that _______.
An exergonic reaction is one that
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is at equilibrium. | ||||||||||||||||||||||||||||||||||||||
is not spontaneous. 2. Enzymes accelerate the rate of reactions by______.
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