《生物化学》课程PPT教学课件（英文版）Chapter 14 Principles of Bioenergetics

Chapter- Principles of Bioenergetics

Chapter 14 Principles of Bioenergetics

1. Cells need energy to do all theirs work To generate and maintain its highly ordered structure(biosynthesis of macromolecules To generate all kinds of movement. To generate concentration and electrical gradients s across cell membranes.h To maintain a body temperature To generate light in some animals The energy industry(production, storage and use is central to the economy of the cell society!

1. Cells need energy to do all their work • To generate and maintain its highly ordered structure (biosynthesis of macromolecules). • To generate all kinds of movement. • To generate concentration and electrical gradients across cell membranes. • To maintain a body temperature. • To generate light in some animals. • The “energy industry”(production, storage and use) is central to the economy of the cell society!

the quantitative study of energy transductions in living cells and the chemical nature underlying these processes

• Bioenergetics (生物能学）: the quantitative study of energy transductions in living cells and the chemical nature underlying these processes

2. Cells have to use chemical energy to do all their work Antoine Lavoisier s insight on animal respiration in the 18th century: it is nothing but a slow combustion of carbon and hydrogen( the same nature as a lighting candle)5 Living cells are generally held at constant temperature and pressure: chemical energy(free energy) has to be used by living organisms, no thermal energy neither mechanical energy is available to do work in cells

2. Cells have to use chemical energy to do all their work • Antoine Lavoisier`s insight on animal respiration in the 18th century: it is nothing but a slow combustion of carbon and hydrogen (the same nature as a lighting candle). • Living cells are generally held at constant temperature and pressure: chemical energy (free energy) has to be used by living organisms, no thermal energy, neither mechanical energy is available to do work in cells

Biological energy transformation obey the two basic laws of thermodynamics revealed by physicists and chemists in the 19th century: energy can neither be created nor be destroyed(but conserved); energy conversion is never 100% efficient (some will always be wasted in increasing the disorder or entropy of the universe) The free energy concept of thermodynamic is more important to biochemists than to chemists (who can always increase the temperature and pressure to make a reaction to occur!)

• Biological energy transformation obey the two basic laws of thermodynamics revealed by physicists and chemists in the 19th century: energy can neither be created nor be destroyed (but conserved); energy conversion is never 100% efficient (some will always be wasted in increasing the disorder or “entropy” of the universe). • The free energy concept of thermodynamic is more important to biochemists than to chemists (who can always increase the temperature and pressure to make a reaction to occur!)

3. Application of the free energy ( concept to biochemical reactions. G): the amount of energy available to do work during a reaction at a constant temperature and pressure: change, not absolute value can be measured The free energy difference between the products and the reactants Gibbs observation: under constant temperature and pressure, all systems change in such a way that free energy is minimized(products should have less free energy than reactants for a reaction to occur spontaneously, i. e, 4G has a negative o value

3. Application of the free energy (G) concept to biochemical reactions • Free energy (G): the amount of energy available to do work during a reaction at a constant temperature and pressure; change, not absolute value can be measured. • Free energy change (G): The free energy difference between the products and the reactants. • Gibbs observation: under constant temperature and pressure, all systems change in such a way that free energy is minimized (products should have less free energy than reactants for a reaction to occur spontaneously, i.e., G has a negative value )

ta neit has nothing to do with rate in biochemist ) value of the change in free energy under conditions of 298K(25 C), I atm pressure, pH 7.0(chemists use pH O, 1.e, the concentration of H they use is IM not 10-7M as biochemists use here) and initial concentrations of 1 M for all reactants and products(except H The depends on 4G"o, temperature, ratio of product and reactant concentrations(Q): FO.LG- AGo+ RTIn Q Enzymes only speed up thermodynamical favorable reactions(having a negative 4G

• Spontaneity has nothing to do with rate! • Standard free energy change in biochemistry (G' o ): value of the change in free energy under conditions of 298 K (25oC), 1 atm pressure, pH 7.0 (chemists use pH 0, i.e., the concentration of H+ they use is 1M, not 10-7 M as biochemists use here) and initial concentrations of 1 M for all reactants and products (except H+ ). • The actual free energy chang (G )depends on G' o , temperature, ratio of product and reactant concentrations (Q): • G = G' o + RT ln Q • Enzymes only speed up thermodynamically favorable reactions (having a negative G) !

AG"o is related to the equilibrium constant (the prime again indicates its biochemical transformation): at equilibrium, 4G=0, Q=K thus AGo--RTIn Ke The G and Go values are additive when reactions are coupled (1. e, sharing common intermediates), thus a thermodynamically unfavorable reaction can be driven by a favorable one The overall K ea is multiplicative(the product of wo,两值相乘), although AG o is additive (the algebraic sum of two 两值相如)

• G' o is related to the equilibrium constant K' eq (the prime again indicates its biochemical transformation): at equilibrium, G = 0, Q = K` eq , thus • G' o = -RT ln K' eq • The G and G' o values are additive when reactions are coupled (i.e., sharing common intermediates), thus a thermodynamically unfavorable reaction can be driven by a favorable one. • The overall K` eq is multiplicative (the product of two,两值相乘), although G' o is additive (the algebraic sum of two，两值相加)

4. ATP is the universal currency for biologiealenergy This was first perceived by Fritz Lipmann and Herman Kalckar in 194 1 when studying glycolysis Hydrolysis of the two phosphoanhydride(磷酸酐鍵 bonds in atp generate more stable products releasing large amount of free energy (4G is.5 kJ/mol: 4G in cells is-50 to -65 kJ/mol) The ATP molecule is kinetically stable at pH 7 (i.e it has a high activation energy, 4G* for hydrolysis) and enzyme catalysis is needed for its hydrolysis

4. ATP is the universal currency for biological energy • This was first perceived by Fritz Lipmann and Herman Kalckar in 1941 when studying glycolysis. • Hydrolysis of the two phosphoanhydride (磷酸酐键) bonds in ATP generate more stable products releasing large amount of free energy (G' o is -30.5 kJ/mol; G in cells is -50 to -65 kJ/mol). • The ATP molecule is kinetically stable at pH 7 (i.e., it has a high activation energy, G‡ for hydrolysis) and enzyme catalysis is needed for its hydrolysis

atP is not a long-term storage form of free energy in living cells, being consumed within a minute following its formation (phosphocreatine 磷酸肌酸, act as a energy storage form for longer term) A resting human consumes about 40 kg of ATP in 24 hours A provides energy by group transfer (donating ap PP or AMP to form covalent intermediates), not by simple hydrolysis atp has an intermediate A, thus ADP can accept and ATP can donate phosphoryl groups

• ATP is not a long-term storage form of free energy in living cells, being consumed within a minute following its formation (phosphocreatine, 磷酸肌酸, act as a energy storage form for longer term). • A resting human consumes about 40 kg of ATP in 24 hours! • ATP provides energy by group transfer (donating a Pi , PPi or AMP to form covalent intermediates), not by simple hydrolysis. • ATP has an intermediate phosphoryl group transfer potential, thus ADP can accept and ATP can donate phosphoryl groups