CHP 13 Bioenergetics (4pp) - Chapter 13 Homework Assignment...

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1 Chapter 13 1 Chapter 13 Homework Assignment • I have decided to alter the homework assignment for Chapter 13. • These problems will NOT collected but if I were to want some practice, I would look at these problems: 2, 4, 6, 8, 9, 10, 14, 18, 19, 22 Chapter 13 Bioenergetics Chapter 13 3 Metabolism is a highly coordinated cellular activity in which many multienzyme systems (pathways) cooperate to: – Obtain chemical energy by capturing solar energy or degrading energy-rich nutrients – Convert nutrients into raw materials for the production of macromolecules – Polymerize monomeric precursors into macromolecules – Synthesize and degrade biomolecules required for specialized cellular functions • Metabolism includes hundreds of varied pathways, but we will be focusing on the central metabolic pathways that are common to all forms of life Chapter 13 4 Fig 3, page 483 • In a metabolic pathway, each step brings about a small chemical change, usually the removal, transfer or addition of an atom or functional group. – These intermediates are metabolites Catabolism is the degradative phase in which nutrients are converted into smaller end products – These pathways release energy as either ATP or reduced electron carriers (NADH, FADH 2 , NADPH) Anabolism is the biosynthetic phase where small precursors are built into macromolecules – These pathways require energy, usually in the form of ATP or the reduced electron carriers
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2 Chapter 13 5 Categories of Pathway Chapter 13 6 Complexity is Vast, but Fundamental Principles are Not • Four simple types of weak interactions • Five basic classes of chemical reactions • Five common high-energy intermediates • A few basic types of enzyme mechanism • A few basic classes of reaction kinetics • A few basic principles of thermodynamics • Energy coupling drives unfavorable reactions Bioenergetics Chapter 13 7 Primer of Thermodynamic Terms G = [Energy] products –[Energy] reactants Negative if reaction is spontaneous and energy is released ( exergonic ) H = [Heat content] products – [Heat content] reactants Negative if heat is released ( exothermic ) S = [Entropy] products –[Entropy] reactants Positive if products are “simpler” ( i.e. more disordered) Overall: G = H - T S Chapter 13 8 Recall from previously: Free Energy Nomenclature G o : used by the chemist for reactions under “standard conditions” of pressure, temperature, and solutes at 1M… VERSUS G’ o : used by the biochemist for reactions under “standard conditions” of pressure, temperature, and pH 7 (because we can’t work at 1M H + !) Bioenergetics & Thermodynamics
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3 Chapter 13 9 Recall the 2 nd REALLY IMPORTANT Equation • There is a direct relationship between net free energy change and the equilibrium constant •W
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This note was uploaded on 06/03/2008 for the course BIO 150 taught by Professor Kore during the Spring '08 term at Abraham Baldwin Agricultural College.

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CHP 13 Bioenergetics (4pp) - Chapter 13 Homework Assignment...

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