Chapter 3 - Chapter 3 Thermodynamic Concepts o o systems:...

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Chapter 3 Thermodynamic Concepts o systems: isolated, closed, open o 1 st law: ΔE = q + w (E = internal energy, q = heat absorbed, w = work done on system) internal energy only changes via heat/work o 2 nd law: systems tend towards disorder/randomness entropy unchanged for reversible processes but increases for irreversible ones o 3 rd law: entropy of a perfectly ordered, crystalline array at 0 K is exactly 0 o Free energy: ΔG = ΔH - T ΔS (at constant T and P) for adding reactions, add ΔG std. states: pH 0; std. bio. state: pH 7, 1 M, 1 atm Couple processes so thermodynamically unfavorable rxn becomes thermodynamically favored High-energy biomolecules o characteristics not long term energy storage substances molecules aren’t unstable ATP can change K eq by 10 8 o high (PEP, 1,3-BPG created in course of glucose breakdown, give energy to ADP to form ATP), intermediate (ATP), low (sugar phosphates) o why hydrolysis of high-energy bonds are favorable:
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This note was uploaded on 02/09/2010 for the course BIOL 3361 taught by Professor Zhang/spiro during the Fall '08 term at Dallas.

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Chapter 3 - Chapter 3 Thermodynamic Concepts o o systems:...

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