Lecture 05; Energy

Lecture 05; Energy - Lecture 5: Bioenergetics Reading...

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Lecture 5: Bioenergetics Wednesday, September 2 nd Reading assignment: Chapter 4 Overview - Conservation of energy in biological systems - Physical chemistry concepts Enthalpy, entropy, Gibbs free energy - Free energy storage ATP, redox reactions - Coupled reactions
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Concepts Energy is constant in system plus surroundings Released energy in a biological system is used for: - work - to heat the surroundings - to form higher energy chemical bonds Oxidation of carbon releases energy ATP is energy currency - hydrolyzed to release energy - synthesized when extra energy is available
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First Law: Conservation of Energy Enthalpy change, ΔH: - heat released or absorbed for a chemical reaction - at constant volume and pressure no work done ΔH converts chemical bond energy and heat - negative ΔH: heat released (exothermic) - positive ΔH: heat absorbed (endothermic) Both exothermic and endothermic reactions can occur spontaneously - i.e., ΔH by itself does not determine direction
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Second Law: Disorder Increases Disorder of the universe always increases - system can become more ordered if surroundings become
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This note was uploaded on 09/09/2011 for the course BBMB 301 taught by Professor Girton during the Spring '07 term at Iowa State.

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Lecture 05; Energy - Lecture 5: Bioenergetics Reading...

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