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Major Pathways in Cells • Metabolic fuels Three major nutrients consumed by mammals: (1) Carbohydrates - provide energy (2) Proteins - provide amino acids for protein synthesis and some energy (3) Fats - triacylglycerols provide energy and also lipids for membrane synthesis Prentice Hall c2002 Chapter 10 1 • Overview of catabolic pathways Prentice Hall c2002 Chapter 10 2 Catabolism produces compounds for energy utilization • Three types of compounds are produced that mediate the release of energy (1) Acetyl CoA (2) Nucleoside triphosphates (e.g. ATP) (3) Reduced coenzymes (NADH, FADH2, QH2) Prentice Hall c2002 Chapter 10 3 Reducing Power • Electrons of reduced coenzymes flow toward O2 • This produces a proton flow and a transmembrane potential • Oxidative phosphorylation is the process by which the potential is coupled to the reaction: ADP + Pi ATP Prentice Hall c2002 Chapter 10 4 Compartmentation of metabolic processes Prentice Hall c2002 Chapter 10 5 Thermodynamics and Metabolism A. Free-Energy Change • Free-energy change (DG) is a measure of the chemical energy available from a reaction DG = Gproducts - Greactants • DH = change in enthalpy • DS = change in entropy Prentice Hall c2002 Chapter 10 6 Relationship between energy and entropy • Both entropy and enthalpy contribute to DG DG = DH - TDS (T = degrees Kelvin) -DG = a spontaneous reaction in the direction written +DG = the reaction is not spontaneous DG = 0 the reaction is at equilibrium Prentice Hall c2002 Chapter 10 7 Prentice Hall c2002 Chapter 10 8 The Standard State (DGo) Conditions • Reaction free-energy depends upon conditions • Standard state (DGo) - defined reference conditions Standard Temperature = 298K (25oC) Standard Pressure = 1 atmosphere Standard Solute Concentration = 1.0M • Biological standard state = DGo’ or DG’o Standard [H+] = 10-7 M (pH = 7.0) rather than 1.0M (pH = 1.0); [H2O]=55.5M; [Mg2+]=1mM Prentice Hall c2002 Chapter 10 9 B. Equilibrium Constants and Standard Free-Energy Change • For the reaction: A + B C+D DGreaction = DGo’reaction + RT ln([C][D]/[A][B]) • At equilibrium: Keq = [C][D]/[A][B] and DGreaction = 0, so that: DGo’reaction = -RT ln Keq Prentice Hall c2002 Chapter 10 10 C. Actual Free-Energy Change Determines Spontaneity of Cellular Reactions • When a reaction is not at equilibrium, the actual free energy change (DG) depends upon the ratio of products to substrates • Q = the mass action ratio DG = DG’o + RT ln Q Where Q = [C]’[D]’ / [A]’[B]’ Prentice Hall c2002 Chapter 10 11 Prentice Hall c2002 Chapter 10 12 The Free Energy of ATP • Energy from oxidation of metabolic fuels is largely recovered in the form of ATP Prentice Hall c2002 Chapter 10 13 Prentice Hall c2002 Chapter 10 14 Prentice Hall c2002 Chapter 10 15 Prentice Hall c2002 Chapter 10 16 • Hydrolysis of ATP Prentice Hall c2002 Chapter 10 17 Complexes between ATP and Mg2+ Prentice Hall c2002 Chapter 10 18 ATP is an “energy-rich” compound • A large amount of energy is released in the hydrolysis of the phosphoanhydride bonds of ATP (and UTP, GTP, CTP) • All nucleoside phosphates have nearly equal standard free energies of hydrolysis Prentice Hall c2002 Chapter 10 19