BIOENERGETICS Δ G Gibbs Free Energy- maximum amount of useful work at constant T and P Δ G o ’-biochemical standard state Gibbs Free Energy; all concs = 1 M, partial P = 1 atm, but pH=7 EXERGONIC REACTIONS- Δ G is negative, reaction can be used to do work ENDERGONIC REACTIONS- Δ G is positive, energy must be supplied for reaction to go REVERSIBLE REACTIONS- Δ G is small, ratio of [products]/[reactants] determine direction IRREVERSIBLE REACTIONS- Δ G is large, only direction is with negative Δ G REACTION COUPLING- an exergonic reaction drives an endergonic reaction, both reactions have a common intermediate HIGH ENERGY BONDS-coupled with catabolic reactions to save energy (condensation) -coupled with anabolic reactions to supply energy (hydrolysis) ATP + H 2 O ⇔ ADP + P i Δ G o ’= -7.3 kcal/mole ATP + H 2 O ⇔
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This note was uploaded on 11/27/2011 for the course CHM 365 taught by Professor Thomaszamis during the Spring '06 term at FSU.