15_energetics

15_energetics - Chapter 15: Bioenergetics Bioenergetics...

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Chapter 15: Bioenergetics Bioenergetics • Energy transformations in living organisms system - component under study surroundings - everything else in the universe in biochemistry: open systems the ability for systems to do work is vital to life • For reactions to be useful: spontaneous
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Free energy Δ G can be used to predict spontaneity: Δ G: (+) = endergonic, non-spontaneous energy required to reach equilibrium Δ G: (-) = exergonic, spontaneous process releases energy to reach equilibrium Δ G = 0, reaction at equilibrium Δ G of reactants = Δ G of products no change in free energy of system Δ G in biological systems • Most biological systems operate ~pH 7 Biological standard state pH = 7, [H+] = 1 × 10 -7 M • Gives rise to Δ G°´ Free energy for biochemical standard state
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Free energy and equilibrium • Concentrations of reactants and products affect Δ G Δ G°´ = - RT ln K eq Δ G°´ of ATP hydrolysis: ATP + H 2 O ADP + Pi + H + Study problem #1 Given the following reaction: glucose-6-P + H 2 O glucose + Pi Δ G ° = -14kJ/mol What is the [glucose-6-P] if [glucose] and [Pi] are both 1mM?
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This note was uploaded on 04/28/2009 for the course BCH 361 taught by Professor Fromme during the Spring '08 term at ASU.

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15_energetics - Chapter 15: Bioenergetics Bioenergetics...

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