(Microsoft PowerPoint - ATP angl.ppt [Re\236im kompatibility])

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Free enthalpy∆G G = ∆G 0 ‘ +RT·ln[products]/[reactants]∆G 0 … all concentrations 1 mol/l∆G 0 ‘ … + aquaeous sol., pH = 7,0∆G 0 = - RT·ln K‘

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Free enthalpyinclinationto react=decreasein energyof system+increase inrandomness ofsystem∆G G < 0 … reaction runs spontaneously∆G G = 0 … equilibrium∆G G > 0 … need for energy

Free enthalpy∆G G = ∆G 0 ‘ +RT·ln[products]/[reactants]∆G 0 … all concentrations 1 mol/l∆G 0 ‘ … + aquaeous sol., pH = 7,0∆G 0 = - RT·ln K‘

Page 1 and 2: The role of ATP in metabolismMUDr.
Page 3 and 4: ATP, ADP, AMP a cAMP Macroergic com
Page 5 and 6: Thermodynamics Two axioms Abstract
Page 7 and 8: Enthalpy Constant volume:∆U U = Q
Page 9: Free enthalpy A portion of enthalpy
Page 13 and 14: Course of reaction∆G G = ∆G 0
Page 15 and 16: ATP Hydrolysis of ATP is stronglyex
Page 17 and 18: Coupling of reactionsheatModified f
Page 19 and 20: Irreversible reactions
Page 21 and 22: How to make ATPoxidation of fuelsmi
Page 23 and 24: Other properties of ATP A complex w

(Microsoft PowerPoint - ATP angl.ppt [Re\236im kompatibility])

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