BIO_211_Ch6.__MetabolismBB

BIO_211_Ch6.__MetabolismBB - Introduction to Metabolism K...

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    Introduction to Metabolism K. Sathasivan Basic Energy concepts Thermodynamic laws  Entropy, enthalpy, free energy,   Chemical reaction, equilibrium constant ATP and Energy Coupling Enzymes Activation energy - Ea, Vmax, Km,  Factors affecting and regulating enzyme activity
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    Basic  Terms Metabolism Catabolism Anabolism Potential energy Kinetic energy Chemical bond   energy Enthalpy, Entropy Free energy Exergonic reaction Endergonic reaction Exothermic reaction Endothermic reaction Equilibrium constant
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    Types of Energy  Potential energy Kinetic energy
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    Laws of Thermodynamics First Law Total energy in the universe is constant Energy can neither be created nor  destroyed Energy can be transferred or transformed Second Law Every energy transfer or transformation  results in increased randomness in the  universe.
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    Concept Enthalpy ( H): Total potential energy or heat  content Entropy ( S): Measure of randomness or  disorderliness Free energy ( G). The energy available to do  work under uniform temperature. G = H – T S where T = Absolute temperature in Kelvin (K= C + 273 )
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    Spontaneous Reactions
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    Chemical Reaction Examples of bond energy in kcal/mol C-C = 83, C-H = 99, C-O 84, C=0 = 174, O-H = 111, O=O = 118 Example of a chemical reaction CH 4 + 2 O 2 CO 2 + 2 H 2 O Bond energy (4 X 99) + (2 X 118) (2 X 174) + (4 X 111) H = H (reactants) 632 kcal/mol - H (products)792 kcal/mol = -162 kcal/mol (for gas phase reactions only) Note : All other reactions H = H (products) – H (reactants)
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