BIOL10002 Lecture Notes - Lecture 6: Activation Energy, Reaction Rate, Exergonic Process

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21 Jul 2018
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Catalysts - to speed up a reaction, an energy barrier must be overcome. Typically proteins (some rna molecules have enzyme activity) Speed up reactions by decreasing activation energy (ea) Exergonic reactions proceed only after the reactants are pushed over the energy barrier by some added energy. The energy barrier thus represents the amount of energy needed to start the reaction, the activation energy. In a chemical reaction, the activation energy is the energy needed to change the reactants into unstable molecular forms called transition-state intermediates. Transition-state intermediates have higher free energies than either the reactants or the products. Although the amount of activation energy needed for different reactions varies, it is often small compared with the change in free energy of the overall reaction. The activation e(cid:374)ergy put i(cid:374) to start a rea(cid:272)tio(cid:374) is re(cid:272)o(cid:448)ered duri(cid:374)g the e(cid:374)sui(cid:374)g (cid:862)do(cid:449)(cid:374)hill(cid:863) phase of the reaction, so it is not a part of the net free energy change, g.

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