This document discusses a live online tutorial for CSIR NET life sciences. It covers topics of bioenergetics including standard free energy change of chemical reactions, energy coupling, ATP hydrolysis, and high-energy phosphate bonds. The tutorial is led by Dr. Sheelendra and covers units on bioenergetics, ATP, and energy coupling reactions. It provides equations and examples to explain energetic concepts in biochemistry.
This reading assignment covers chemical equilibrium, including:
- Systems reach equilibrium when the forward and reverse reaction rates are equal
- The equilibrium constant, Keq, is a ratio of products to reactants at equilibrium and is constant at a given temperature
- Catalysts do not change equilibrium concentrations, though they speed both reaction directions
- Heterogeneous equilibria involve solids/liquids, which do not change concentration and are omitted from Keq expressions
This document discusses key concepts in bioenergetics including the first and second laws of thermodynamics. It defines bioenergetics as the study of energy changes that accompany biochemical reactions. The first law states that energy cannot be created or destroyed, only transformed between forms. The second law introduces the concept of entropy, which is a measure of disorder or randomness in a system. The document also defines other important energy terms such as free energy, entropy, and enthalpy.
1. The document discusses cellular metabolism and bioenergetics. It covers topics like catabolism, anabolism, metabolic pathways, and energy relationships.
2. A key point is that catabolism breaks down nutrients to extract energy, which is converted to ATP through electron transport. ATP then fuels anabolic reactions.
3. Thermodynamics principles like Gibbs free energy, entropy, and redox potentials govern metabolic reactions and determine whether they release or require energy. Electron carriers in the electron transport chain facilitate energy release.
The document discusses reversible reactions and chemical equilibrium. It defines reversible reactions as those that can proceed in both the forward and reverse directions simultaneously. It explains that a reversible reaction reaches equilibrium when the rates of the forward and reverse reactions are equal. It introduces Le Chatelier's principle, which states that if a stress is applied to a system at equilibrium, the system will respond in a way to counteract the stress and re-establish a new equilibrium state. The document also discusses how temperature, concentration, pressure, and catalysts can affect the position of equilibrium by altering reaction rates based on Le Chatelier's principle. Finally, it introduces equilibrium expressions and the equilibrium constant (Keq), explaining how these relate the concentrations of
1. The document describes a chapter on chemical equilibrium, including defining chemical equilibrium as a dynamic state reached when the rates of the forward and reverse reactions are equal.
2. It discusses the equilibrium constant expression and calculating equilibrium concentrations by applying stoichiometry to reaction mixtures.
3. Heterogeneous and homogeneous equilibria are described, as well as how the equilibrium constant expression is modified for reactions involving pure solids or liquids.
Introduction
Basis
Importance
Classification
Homogeneous catalysis
Mechanism
Example
Heterogeneous catalysis
Mechanism
Examples
Promoters
Catalytic Poisoning
Autocatalysis
Enzyme catalysis
Enzymes
References
Catalyst: -
The substances that alter the rate of a reaction but itself remains chemically unchanged at the end of the reaction is called a Catalyst.
The process is called Catalysis.
prop-
A catalyst cannot start the reaction by itself.
Catalytic activity increases as surface area of catalyst increases.
Catalysts are thermolabile, this effect is very well pronounced in enzymes.
Catalytic activity is maximum at a catalyst’s optimum temperature.
A catalyst does not alter the position of the equilibrium, instead it helps in achieving the equilibrium faster.
This unit includes: rate of a chemical reaction, graphs,, unit of rate, average rate& instantaneous rate,. factors influuncing rate of a reaction, Rate expression & rate constant, Order & molecularity of a reaction,, initiall rate method & integrated rate law equations, numerical problems,, Half life period, Pseudo first order reaction, Temperature of rate of reaction, Activation energy, collision frequency & effective collision, Collision theory, Arrhenius equation,, effect of catalyst on rate of reaction, numerical problems
The document discusses bioenergetics, which is the study of energy transformations that occur within living cells. It covers several key topics:
- Bioenergetics obeys the laws of thermodynamics, particularly the first law of conservation of energy and the second law regarding entropy.
- Key thermodynamic concepts discussed include entropy, enthalpy, free energy, and how biological reactions are either exergonic (releasing energy) or endergonic (requiring energy).
- For a reaction to be spontaneous, the change in free energy (ΔG) must be negative. However, many essential biological reactions are non-spontaneous (endergonic).
- Cells overcome
This reading assignment covers chemical equilibrium, including:
- Systems reach equilibrium when the forward and reverse reaction rates are equal
- The equilibrium constant, Keq, is a ratio of products to reactants at equilibrium and is constant at a given temperature
- Catalysts do not change equilibrium concentrations, though they speed both reaction directions
- Heterogeneous equilibria involve solids/liquids, which do not change concentration and are omitted from Keq expressions
This document discusses key concepts in bioenergetics including the first and second laws of thermodynamics. It defines bioenergetics as the study of energy changes that accompany biochemical reactions. The first law states that energy cannot be created or destroyed, only transformed between forms. The second law introduces the concept of entropy, which is a measure of disorder or randomness in a system. The document also defines other important energy terms such as free energy, entropy, and enthalpy.
1. The document discusses cellular metabolism and bioenergetics. It covers topics like catabolism, anabolism, metabolic pathways, and energy relationships.
2. A key point is that catabolism breaks down nutrients to extract energy, which is converted to ATP through electron transport. ATP then fuels anabolic reactions.
3. Thermodynamics principles like Gibbs free energy, entropy, and redox potentials govern metabolic reactions and determine whether they release or require energy. Electron carriers in the electron transport chain facilitate energy release.
The document discusses reversible reactions and chemical equilibrium. It defines reversible reactions as those that can proceed in both the forward and reverse directions simultaneously. It explains that a reversible reaction reaches equilibrium when the rates of the forward and reverse reactions are equal. It introduces Le Chatelier's principle, which states that if a stress is applied to a system at equilibrium, the system will respond in a way to counteract the stress and re-establish a new equilibrium state. The document also discusses how temperature, concentration, pressure, and catalysts can affect the position of equilibrium by altering reaction rates based on Le Chatelier's principle. Finally, it introduces equilibrium expressions and the equilibrium constant (Keq), explaining how these relate the concentrations of
1. The document describes a chapter on chemical equilibrium, including defining chemical equilibrium as a dynamic state reached when the rates of the forward and reverse reactions are equal.
2. It discusses the equilibrium constant expression and calculating equilibrium concentrations by applying stoichiometry to reaction mixtures.
3. Heterogeneous and homogeneous equilibria are described, as well as how the equilibrium constant expression is modified for reactions involving pure solids or liquids.
Introduction
Basis
Importance
Classification
Homogeneous catalysis
Mechanism
Example
Heterogeneous catalysis
Mechanism
Examples
Promoters
Catalytic Poisoning
Autocatalysis
Enzyme catalysis
Enzymes
References
Catalyst: -
The substances that alter the rate of a reaction but itself remains chemically unchanged at the end of the reaction is called a Catalyst.
The process is called Catalysis.
prop-
A catalyst cannot start the reaction by itself.
Catalytic activity increases as surface area of catalyst increases.
Catalysts are thermolabile, this effect is very well pronounced in enzymes.
Catalytic activity is maximum at a catalyst’s optimum temperature.
A catalyst does not alter the position of the equilibrium, instead it helps in achieving the equilibrium faster.
This unit includes: rate of a chemical reaction, graphs,, unit of rate, average rate& instantaneous rate,. factors influuncing rate of a reaction, Rate expression & rate constant, Order & molecularity of a reaction,, initiall rate method & integrated rate law equations, numerical problems,, Half life period, Pseudo first order reaction, Temperature of rate of reaction, Activation energy, collision frequency & effective collision, Collision theory, Arrhenius equation,, effect of catalyst on rate of reaction, numerical problems
The document discusses bioenergetics, which is the study of energy transformations that occur within living cells. It covers several key topics:
- Bioenergetics obeys the laws of thermodynamics, particularly the first law of conservation of energy and the second law regarding entropy.
- Key thermodynamic concepts discussed include entropy, enthalpy, free energy, and how biological reactions are either exergonic (releasing energy) or endergonic (requiring energy).
- For a reaction to be spontaneous, the change in free energy (ΔG) must be negative. However, many essential biological reactions are non-spontaneous (endergonic).
- Cells overcome
The effect of dielectric constant on the kinetics of reaction between plasm...Alexander Decker
This document summarizes a study that investigated the effect of increasing ethanol concentration on the rate of reaction between plasma albumin and formaldehyde. The rate constant was determined at various dielectric constants and temperatures by measuring absorption in ethanol-water mixtures containing plasma albumin and formaldehyde. The rate constant decreased with increasing ethanol concentration. Activation energy and other thermodynamic parameters also decreased with decreasing dielectric constant (increasing ethanol proportion). A linear relationship was observed between the log of the rate constant and the reciprocal of dielectric constant, indicating three mechanistic changes. The rate increased in water but decreased in ethanol, suggesting reaction rates were slowed by progressive ethanol addition. In conclusion, the reaction was second-order and its rate decreased with increasing ethanol concentration in accordance with
1. The document discusses chemical kinetics, which is the study of reaction rates and their mechanisms. It defines the average and instantaneous rates of reactions in terms of changes in reactant or product concentrations over time.
2. Reaction rates depend on factors like concentration, temperature, and catalysts. The rate law expresses how the rate of a reaction varies with changes in concentration. Generally, reaction rates increase with higher reactant concentrations and decrease over time as concentrations decrease.
3. For reactions where stoichiometric coefficients are not equal to one, the rates of appearance/disappearance must be divided by the appropriate coefficients to make the rates equal. This allows rates to be expressed consistently in terms of changes in concentrations of
Reaction of aniline with ammonium persulphate and concentrated hydrochloric a...Maciej Przybyłek
In this paper, the reaction of aniline with ammonium persulphate and concentrated HCl was studied. As a result of our experimental studies, 2,4,6-trichlorophenylamine was identified as the main product. This shows that a high concentration of HCl does not favour oxidative polymerisation of phenylamine, even though the ammonium persulphate/HCl system is widely used in polyaniline synthesis. On the basis of the experimental data and density functional theory for reaction path modelling, we proposed a mechanism for oxidative chlorination of aniline. We assumed that this reaction proceeded in three cyclically repeated steps; protonation of aniline, formation of singlet ground state phenylnitrenium cation, and nucleophilic substitution. In order to confirm this mechanism, kinetic, thermochemical, and natural bond orbital population analyses were performed.
The document discusses chemical kinetics and factors that affect the rate of chemical reactions. It provides an introduction to kinetics, defines reaction rates, outlines rate laws and rate constants, and describes six key factors that influence reaction rates: the nature of reactants and products, concentration, temperature, catalysts, surface area, and light radiation. Specific examples are given to illustrate concepts like reaction stoichiometry and how different factors alter reaction rates.
Concept of rate of reaction.
Factors effecting rate of reaction.
Concept of order of reaction.
Methods for the determination of order of reaction.
Pharmaceutical importance and applications of rate and order of reaction.
Kinetics in UP
This document discusses chemical kinetics and reaction rates. It defines key kinetics concepts like reaction order, rate laws, and rate constants. Specific examples covered include first-order, second-order, and zero-order reactions. The effects of temperature, catalysts, and physical conditions on reaction rates are also explained. Several industrial reaction mechanisms are summarized, such as the chlorination of methane, hydrolysis, nitration of benzene, and sulfonation of benzene.
This document discusses spontaneous and nonspontaneous reactions. It explains that a spontaneous reaction favors the formation of products under specified conditions, while a nonspontaneous reaction does not favor the formation of products under the same conditions. It provides the example that photosynthesis is a nonspontaneous reaction that requires an input of energy. The document also discusses entropy, enthalpy, and Gibbs free energy in the context of spontaneous reactions.
This document provides an overview of the key concepts covered in 5 sections of a chapter on energy and chemical change:
Section 15.1 defines energy and distinguishes between potential and kinetic energy. It relates chemical potential energy to heat released or absorbed in chemical reactions.
Section 15.2 describes how calorimetry is used to measure energy changes and defines enthalpy and enthalpy changes.
Section 15.3 explains how to write thermochemical equations and describes energy changes during state changes.
Section 15.4 discusses calculating enthalpy changes using Hess's law and standard enthalpies of formation.
Section 15.5 differentiates between spontaneous and nonspontaneous processes and explains how entropy
This document provides an overview of three sections on chemical equilibrium from a chemistry textbook. Section 17.1 discusses the definition of chemical equilibrium as a state where forward and reverse reactions occur at equal rates. It also defines equilibrium constants and expressions. Section 17.2 explains how temperature, pressure, and concentration changes affect equilibrium based on Le Châtelier's principle. Section 17.3 discusses using equilibrium constants to determine concentrations and solubility products, and how the common ion effect impacts solubility.
This document contains a chapter menu and outline for a chapter on reaction rates. The chapter is divided into 4 main sections:
1) A Model for Reaction Rates - discusses calculating reaction rates from data and relating rates to collisions between particles.
2) Factors Affecting Reaction Rates - identifies factors like concentration, temperature, surface area, and catalysts that affect reaction rates.
3) Reaction Rate Laws - expresses the relationship between reaction rate and concentration, and how to determine reaction orders.
4) Instantaneous Reaction Rates and Reaction Mechanisms - discusses calculating instantaneous rates, complex reactions having multiple steps, and relating rates to reaction mechanisms.
This document discusses reversible chemical reactions and chemical equilibrium. It defines key terms like activation energy, exothermic and endothermic reactions, and how factors like temperature, concentration, and catalysts affect the rate and direction of reversible reactions. Specifically, it explains that at chemical equilibrium, the rates of the forward and reverse reactions are equal and application of Le Chatelier's principle describes how the system responds to changes to relieve stress.
This document discusses chemical kinetics, which is the study of reaction rates. It defines kinetics and lists some of its applications in pharmaceutical sciences like drug stability, dissolution, and pharmacokinetics. It then describes the molecularity and common types of reactions like unimolecular, bimolecular, and termolecular. The rest of the document discusses factors that influence reaction rates such as temperature, solvents, ionic strength, and dielectric constant. It also covers reaction orders, methods for determining order, and concepts like half-life. Catalysis is mentioned as another factor that can increase reaction rates.
1. The document discusses irreversible and reversible reactions. Irreversible reactions proceed in only the forward direction, while reversible reactions can proceed in both directions.
2. It defines chemical equilibrium as the state where the rates of the forward and reverse reactions are equal, resulting in constant concentrations of reactants and products. At equilibrium, the reaction is dynamic rather than stopped.
3. It explains the law of mass action, which states that the rate of a reaction is directly proportional to the active masses or concentrations of reactants. The equilibrium constant K is derived from the law of mass action.
The document discusses chemical kinetics and reaction rates. It provides information on:
- The study of rates of chemical reactions and reaction mechanisms (chemical kinetics).
- How reaction rates are expressed in terms of changes in reactant/product concentrations over time.
- Factors that influence reaction rates such as concentration, temperature, and surface area.
- Collision theory and how effective collisions between reactant particles lead to reactions.
- Reaction orders, rate laws, and how to determine the order of reactions based on experimental rate data.
This document contains an outline for a chapter on redox reactions with the following sections:
1. Section 19.1 covers oxidation and reduction processes, defining oxidation numbers and identifying oxidizing and reducing agents.
2. Section 19.2 discusses balancing redox equations using the oxidation-number method and splitting reactions into half-reactions.
3. The document provides assessment questions to test understanding and links to additional resources like study guides, concept illustrations, and standardized test practice questions.
Dra Núria López - IN SITU SURFACE COVERAGE ANALYSIS OF RUO2-CATALYSED HCL OXI...xrqtchemistry
IN SITU SURFACE COVERAGE ANALYSIS OF RUO2-CATALYSED HCL OXIDATION REVEALS THE ENTROPIC ORIGIN OF COMPENSATION IN HETEROGENEOUS CATALYSIS - Nature Chemistry (29 July 2012)
This document provides an overview of stoichiometry concepts covered in 11 sections. It defines stoichiometry and discusses mole ratios from balanced equations. It describes how to perform stoichiometric calculations using mole-to-mole, mole-to-mass, and mass-to-mass conversions. It also covers limiting reactants, excess reactants, and calculating products. Finally, it defines theoretical yield, actual yield, and percent yield for chemical reactions. The document provides learning objectives, examples, and self-assessment questions for each section.
The Influence of Solvent on the Solvolysis of Ethyl Cinnamate in Water Aceton...IJEACS
The kinetic of alkaline hydrolysis of Ethyl Cinnamate was investigated at different percentage of aqua-organic solvent mixture with Acetone (30 to 70% v/v) over the temperature range of 20o C to 40 o C. The specific rate constant was found to be decreased with increasing proportion of solvent (Acetone) at all the temperature range. The Iso-composition Activation energy (EC) was also evaluated which decreases with solvent composition in (water-Acetone) system. The number of water molecule associated with the activated complex is found to be increase (0.7003to 0.786) in water-Acetone system. The Thermodynamic Activation Parameter such as Enthalpy of Activation (H*), Entropy of Activation (S*) and Gibb's free energy of activation (G*) were also calculated
1) Bioenergetics examines the energy flow in living organisms using concepts like entropy, enthalpy, and free energy.
2) ATP acts as the energy currency of cells, being produced through exergonic reactions and consumed to power endergonic reactions.
3) Standard free energy changes can be added for coupled reactions and actual free energy depends on reactant and product concentrations, driving reactions towards or away from equilibrium.
Bioenergetics describes the transfer and use of energy in biological systems using concepts from thermodynamics like free energy. The change in free energy (ΔG) of a reaction predicts whether it can occur spontaneously. ATP acts as an energy carrier in cells by storing free energy in its phosphate bonds. During oxidative phosphorylation, electrons are passed through an electron transport chain in the mitochondrial inner membrane, with their energy used to synthesize ATP from ADP and inorganic phosphate.
The document summarizes key topics in biochemistry including metabolism, bioenergetics, and biochemical pathways. Specifically, it discusses [1] the principles of bioenergetics including thermodynamics, phosphoryl group transfers, and oxidation-reduction reactions; [2] how ATP and other phosphorylated compounds are used to drive cellular processes; and [3] how electrons flow through metabolic pathways and soluble electron carriers to provide energy for biological work. It concludes by outlining topics to be covered in the next chapter on glycolysis and carbohydrate catabolism.
The document discusses Gibbs free energy and its relationship to chemical equilibrium. It defines Gibbs free energy and how it can be used to predict the spontaneity of reactions. The Gibbs free energy change, ΔG, is related to the standard Gibbs free energy change, ΔG°, and the reaction quotient, Q, by the equation ΔG = ΔG° + RTlnQ. At equilibrium when ΔG = 0, Q equals the equilibrium constant, K. Expressions are provided for calculating K for different types of reactions, such as gas phase, liquid phase, and liquid-solid reactions. The key points are that a reaction will only proceed spontaneously if ΔG is negative and that a reaction will reach equilibrium when ΔG equals
The effect of dielectric constant on the kinetics of reaction between plasm...Alexander Decker
This document summarizes a study that investigated the effect of increasing ethanol concentration on the rate of reaction between plasma albumin and formaldehyde. The rate constant was determined at various dielectric constants and temperatures by measuring absorption in ethanol-water mixtures containing plasma albumin and formaldehyde. The rate constant decreased with increasing ethanol concentration. Activation energy and other thermodynamic parameters also decreased with decreasing dielectric constant (increasing ethanol proportion). A linear relationship was observed between the log of the rate constant and the reciprocal of dielectric constant, indicating three mechanistic changes. The rate increased in water but decreased in ethanol, suggesting reaction rates were slowed by progressive ethanol addition. In conclusion, the reaction was second-order and its rate decreased with increasing ethanol concentration in accordance with
1. The document discusses chemical kinetics, which is the study of reaction rates and their mechanisms. It defines the average and instantaneous rates of reactions in terms of changes in reactant or product concentrations over time.
2. Reaction rates depend on factors like concentration, temperature, and catalysts. The rate law expresses how the rate of a reaction varies with changes in concentration. Generally, reaction rates increase with higher reactant concentrations and decrease over time as concentrations decrease.
3. For reactions where stoichiometric coefficients are not equal to one, the rates of appearance/disappearance must be divided by the appropriate coefficients to make the rates equal. This allows rates to be expressed consistently in terms of changes in concentrations of
Reaction of aniline with ammonium persulphate and concentrated hydrochloric a...Maciej Przybyłek
In this paper, the reaction of aniline with ammonium persulphate and concentrated HCl was studied. As a result of our experimental studies, 2,4,6-trichlorophenylamine was identified as the main product. This shows that a high concentration of HCl does not favour oxidative polymerisation of phenylamine, even though the ammonium persulphate/HCl system is widely used in polyaniline synthesis. On the basis of the experimental data and density functional theory for reaction path modelling, we proposed a mechanism for oxidative chlorination of aniline. We assumed that this reaction proceeded in three cyclically repeated steps; protonation of aniline, formation of singlet ground state phenylnitrenium cation, and nucleophilic substitution. In order to confirm this mechanism, kinetic, thermochemical, and natural bond orbital population analyses were performed.
The document discusses chemical kinetics and factors that affect the rate of chemical reactions. It provides an introduction to kinetics, defines reaction rates, outlines rate laws and rate constants, and describes six key factors that influence reaction rates: the nature of reactants and products, concentration, temperature, catalysts, surface area, and light radiation. Specific examples are given to illustrate concepts like reaction stoichiometry and how different factors alter reaction rates.
Concept of rate of reaction.
Factors effecting rate of reaction.
Concept of order of reaction.
Methods for the determination of order of reaction.
Pharmaceutical importance and applications of rate and order of reaction.
Kinetics in UP
This document discusses chemical kinetics and reaction rates. It defines key kinetics concepts like reaction order, rate laws, and rate constants. Specific examples covered include first-order, second-order, and zero-order reactions. The effects of temperature, catalysts, and physical conditions on reaction rates are also explained. Several industrial reaction mechanisms are summarized, such as the chlorination of methane, hydrolysis, nitration of benzene, and sulfonation of benzene.
This document discusses spontaneous and nonspontaneous reactions. It explains that a spontaneous reaction favors the formation of products under specified conditions, while a nonspontaneous reaction does not favor the formation of products under the same conditions. It provides the example that photosynthesis is a nonspontaneous reaction that requires an input of energy. The document also discusses entropy, enthalpy, and Gibbs free energy in the context of spontaneous reactions.
This document provides an overview of the key concepts covered in 5 sections of a chapter on energy and chemical change:
Section 15.1 defines energy and distinguishes between potential and kinetic energy. It relates chemical potential energy to heat released or absorbed in chemical reactions.
Section 15.2 describes how calorimetry is used to measure energy changes and defines enthalpy and enthalpy changes.
Section 15.3 explains how to write thermochemical equations and describes energy changes during state changes.
Section 15.4 discusses calculating enthalpy changes using Hess's law and standard enthalpies of formation.
Section 15.5 differentiates between spontaneous and nonspontaneous processes and explains how entropy
This document provides an overview of three sections on chemical equilibrium from a chemistry textbook. Section 17.1 discusses the definition of chemical equilibrium as a state where forward and reverse reactions occur at equal rates. It also defines equilibrium constants and expressions. Section 17.2 explains how temperature, pressure, and concentration changes affect equilibrium based on Le Châtelier's principle. Section 17.3 discusses using equilibrium constants to determine concentrations and solubility products, and how the common ion effect impacts solubility.
This document contains a chapter menu and outline for a chapter on reaction rates. The chapter is divided into 4 main sections:
1) A Model for Reaction Rates - discusses calculating reaction rates from data and relating rates to collisions between particles.
2) Factors Affecting Reaction Rates - identifies factors like concentration, temperature, surface area, and catalysts that affect reaction rates.
3) Reaction Rate Laws - expresses the relationship between reaction rate and concentration, and how to determine reaction orders.
4) Instantaneous Reaction Rates and Reaction Mechanisms - discusses calculating instantaneous rates, complex reactions having multiple steps, and relating rates to reaction mechanisms.
This document discusses reversible chemical reactions and chemical equilibrium. It defines key terms like activation energy, exothermic and endothermic reactions, and how factors like temperature, concentration, and catalysts affect the rate and direction of reversible reactions. Specifically, it explains that at chemical equilibrium, the rates of the forward and reverse reactions are equal and application of Le Chatelier's principle describes how the system responds to changes to relieve stress.
This document discusses chemical kinetics, which is the study of reaction rates. It defines kinetics and lists some of its applications in pharmaceutical sciences like drug stability, dissolution, and pharmacokinetics. It then describes the molecularity and common types of reactions like unimolecular, bimolecular, and termolecular. The rest of the document discusses factors that influence reaction rates such as temperature, solvents, ionic strength, and dielectric constant. It also covers reaction orders, methods for determining order, and concepts like half-life. Catalysis is mentioned as another factor that can increase reaction rates.
1. The document discusses irreversible and reversible reactions. Irreversible reactions proceed in only the forward direction, while reversible reactions can proceed in both directions.
2. It defines chemical equilibrium as the state where the rates of the forward and reverse reactions are equal, resulting in constant concentrations of reactants and products. At equilibrium, the reaction is dynamic rather than stopped.
3. It explains the law of mass action, which states that the rate of a reaction is directly proportional to the active masses or concentrations of reactants. The equilibrium constant K is derived from the law of mass action.
The document discusses chemical kinetics and reaction rates. It provides information on:
- The study of rates of chemical reactions and reaction mechanisms (chemical kinetics).
- How reaction rates are expressed in terms of changes in reactant/product concentrations over time.
- Factors that influence reaction rates such as concentration, temperature, and surface area.
- Collision theory and how effective collisions between reactant particles lead to reactions.
- Reaction orders, rate laws, and how to determine the order of reactions based on experimental rate data.
This document contains an outline for a chapter on redox reactions with the following sections:
1. Section 19.1 covers oxidation and reduction processes, defining oxidation numbers and identifying oxidizing and reducing agents.
2. Section 19.2 discusses balancing redox equations using the oxidation-number method and splitting reactions into half-reactions.
3. The document provides assessment questions to test understanding and links to additional resources like study guides, concept illustrations, and standardized test practice questions.
Dra Núria López - IN SITU SURFACE COVERAGE ANALYSIS OF RUO2-CATALYSED HCL OXI...xrqtchemistry
IN SITU SURFACE COVERAGE ANALYSIS OF RUO2-CATALYSED HCL OXIDATION REVEALS THE ENTROPIC ORIGIN OF COMPENSATION IN HETEROGENEOUS CATALYSIS - Nature Chemistry (29 July 2012)
This document provides an overview of stoichiometry concepts covered in 11 sections. It defines stoichiometry and discusses mole ratios from balanced equations. It describes how to perform stoichiometric calculations using mole-to-mole, mole-to-mass, and mass-to-mass conversions. It also covers limiting reactants, excess reactants, and calculating products. Finally, it defines theoretical yield, actual yield, and percent yield for chemical reactions. The document provides learning objectives, examples, and self-assessment questions for each section.
The Influence of Solvent on the Solvolysis of Ethyl Cinnamate in Water Aceton...IJEACS
The kinetic of alkaline hydrolysis of Ethyl Cinnamate was investigated at different percentage of aqua-organic solvent mixture with Acetone (30 to 70% v/v) over the temperature range of 20o C to 40 o C. The specific rate constant was found to be decreased with increasing proportion of solvent (Acetone) at all the temperature range. The Iso-composition Activation energy (EC) was also evaluated which decreases with solvent composition in (water-Acetone) system. The number of water molecule associated with the activated complex is found to be increase (0.7003to 0.786) in water-Acetone system. The Thermodynamic Activation Parameter such as Enthalpy of Activation (H*), Entropy of Activation (S*) and Gibb's free energy of activation (G*) were also calculated
1) Bioenergetics examines the energy flow in living organisms using concepts like entropy, enthalpy, and free energy.
2) ATP acts as the energy currency of cells, being produced through exergonic reactions and consumed to power endergonic reactions.
3) Standard free energy changes can be added for coupled reactions and actual free energy depends on reactant and product concentrations, driving reactions towards or away from equilibrium.
Bioenergetics describes the transfer and use of energy in biological systems using concepts from thermodynamics like free energy. The change in free energy (ΔG) of a reaction predicts whether it can occur spontaneously. ATP acts as an energy carrier in cells by storing free energy in its phosphate bonds. During oxidative phosphorylation, electrons are passed through an electron transport chain in the mitochondrial inner membrane, with their energy used to synthesize ATP from ADP and inorganic phosphate.
The document summarizes key topics in biochemistry including metabolism, bioenergetics, and biochemical pathways. Specifically, it discusses [1] the principles of bioenergetics including thermodynamics, phosphoryl group transfers, and oxidation-reduction reactions; [2] how ATP and other phosphorylated compounds are used to drive cellular processes; and [3] how electrons flow through metabolic pathways and soluble electron carriers to provide energy for biological work. It concludes by outlining topics to be covered in the next chapter on glycolysis and carbohydrate catabolism.
The document discusses Gibbs free energy and its relationship to chemical equilibrium. It defines Gibbs free energy and how it can be used to predict the spontaneity of reactions. The Gibbs free energy change, ΔG, is related to the standard Gibbs free energy change, ΔG°, and the reaction quotient, Q, by the equation ΔG = ΔG° + RTlnQ. At equilibrium when ΔG = 0, Q equals the equilibrium constant, K. Expressions are provided for calculating K for different types of reactions, such as gas phase, liquid phase, and liquid-solid reactions. The key points are that a reaction will only proceed spontaneously if ΔG is negative and that a reaction will reach equilibrium when ΔG equals
Biochemical Thermodynamics for Biotechnologyssusere9cd97
This document provides an overview of biochemical thermodynamics. It discusses biochemical stoichiometry, including stoichiometric coefficients and ratios. It also covers limiting and excess reactants. The document defines equilibrium constants and describes how Gibbs free energy relates to whether reactions are spontaneous. It discusses how growth stoichiometry relates to biomass and product yields. Laws of thermodynamics are applied to biochemical reactions, specifically how coupling reactions can drive reactions that individually are non-spontaneous. Gibbs free energy changes are used to determine reaction spontaneity.
This document discusses bioenergetics and the role of ATP in living systems. It explains that ATP stores and transports chemical energy within cells, which is released through its hydrolysis into ADP and phosphate. The hydrolysis of ATP is highly exergonic, with a large negative standard free energy change of -30.5 kJ/mol. This energy from ATP hydrolysis drives endergonic biochemical reactions and processes, such as the synthesis of glucose-6-phosphate from glucose and phosphate. The energy from ATP hydrolysis is efficiently coupled to these endergonic reactions through a cyclic process of ATP synthesis and breakdown.
1. The document discusses chemical equilibrium, describing reversible reactions that can proceed in both the forward and backward directions under the same conditions until equilibrium is reached.
2. Key factors that affect chemical equilibrium are discussed, including concentration, pressure, and temperature based on Le Chatelier's principle. The principle states that if a system at equilibrium experiences a change, the equilibrium shifts to counteract the change.
3. Examples of industrial processes that utilize chemical equilibrium principles are described briefly, including the Haber process for ammonia synthesis and the contact process for sulfur trioxide production.
* Adenosine triphosphate (ATP) is energy currency in our body.
*ATP contains
1.A nitrogenous base – Adenine
2.A sugar – Ribose
3.Three Phosphate Groups
*Whenever a body needs energy beta – gamma phosphate bonds of ATP is hydrolyzed to create the ADP and a free phosphate molecule.
*ATP forms by the processes – Citric acid cycle and Glycolysis.
This document summarizes Chapter 20 from the textbook "Prentice-Hall General Chemistry" by Petrucci, Harwood, and Herring. The chapter discusses spontaneous change, entropy, free energy, and their relationships to determining the spontaneity of chemical reactions. It defines key concepts such as entropy, the Boltzmann equation, and Gibbs free energy. It also explains how these quantities can be used to evaluate spontaneity based on the second law of thermodynamics and establish equilibrium using the equilibrium constant Keq. Examples are provided for calculating entropy changes during phase transitions as well as determining temperature dependence of free energy and equilibrium. The chapter concludes by discussing how coupled reactions can be used to drive nonspontaneous processes.
Cellular processes are driven by exergonic reactions that generate high-energy compounds like ATP. ATP can undergo exergonic reactions to donate phosphate groups or AMP, driving other endergonic reactions like glucose phosphorylation. Cells couple unfavorable reactions to favorable ones through ATP to drive cellular synthesis and transport against gradients. The hydrolysis of ATP and other high-energy compounds provides the energy for these critical energy-requiring cellular processes.
Bioenergetics is the quantitative study of energy transformations that occur in living cells. It concerns the initial and final energy states of biochemical reactions, not reaction rates. The goal is to describe how organisms acquire and transform energy to perform biological work. Reactions are classified as exergonic (energy releasing) or endergonic (energy consuming). Gibbs free energy determines the direction of reactions. It is related to enthalpy, entropy, and temperature based on the equation ΔG = ΔH - TΔS. Redox potential is a quantitative measure of an element or compound's ability to oxidize or reduce. It indicates the tendency of chemical species to gain or lose electrons in redox reactions.
This document contains 27 practice questions related to bioenergetics and oxidative phosphorylation. The questions cover topics like standard free energy changes in multi-step reactions, identification of high-energy compounds, components of the electron transport chain, the chemiosmotic hypothesis, and the effects of uncoupling agents. For each question, multiple choice options for the answer are provided.
Thermodynamics of Biological Systems
The chapter outlines key thermodynamic concepts including:
1) Systems can exchange energy but not matter (closed systems) or both energy and matter (open systems)
2) The first law relates changes in internal energy (ΔE) to heat (q) and work (w)
3) The second law introduces entropy (S) as a measure of disorder
4) Gibbs free energy (ΔG) determines spontaneity and is related to ΔH and TΔS
The chapter discusses coupled processes that drive unfavorable reactions, energy transduction via ATP and NADPH, and high-energy molecules like phosphates. Hydrolysis of high-energy bonds
- ∆G represents the change in free energy for a chemical reaction and can be used to predict spontaneity. Enzymes accelerate reactions but do not change equilibrium.
- Free energy is harvested from oxidation reactions in the form of electrons carried by NADH/FADH2 and used to generate a proton gradient for ATP synthesis.
- ATP is the universal energy currency in cells. Its hydrolysis is highly exergonic and allows energetically unfavorable reactions to proceed.
lecture slide on:
Gibbs free energy and Nernst Equation, Faradaic Processes and Factors Affecting Rates of Electrode Reactions, Potentials and Thermodynamics of Cells, Kinetics of Electrode Reactions, Kinetic controlled reactions,Essentials of Electrode Reactions,BUTLER-VOLMER MODEL FOR THE ONE-STEP, ONE-ELECTRON PROCESS,Current-overpotential curves for the system, Mass Transfer by Migration And Diffusion,MASS-TRANSFER-CONTROLLED REACTIONS,
This document discusses bioenergetics, which is the study of energy changes that accompany biochemical reactions. It examines exergonic and endergonic reactions, and how bioenergetics can predict the feasibility and rate of reactions based on initial and final energy states. Modern organisms use chemical energy from fuels like carbohydrates and lipids to power metabolic reactions and generate concentration gradients, motion, heat, and light. A doctor's understanding of bioenergetics is important for diseases related to nutrition, metabolism, hormones, growth, and molecular processes involving energy. The document outlines the first and second laws of thermodynamics, Gibbs free energy, redox couples, ATP as the energy currency, electron carriers, substrate-level phosphorylation
IRJET- Compressibility of a Periodic Lattice of Atomic HydrogenIRJET Journal
This study uses density functional theory to model the behavior of atomic hydrogen arranged in a pseudo-cubic lattice under extreme pressures of up to 3000 GPa. The results show that the lattice compression does not fit the Murnaghan equation well and exhibits a sharp increase near 2500 GPa. The bulk modulus also shows anomalous behavior, peaking at 282 GPa then dropping sharply at 283 GPa. A critical transition is observed between 2515-2525 GPa where the hydrogen-hydrogen distance collapses from 0.902 to 0.743 Angstroms, corresponding to the transition from solid to atomic hydrogen.
Introduction
• Review of thermodynamic principles
• Ellingham diagrams
a. Graphical representation of free energy data with temperature of oxides
b. Calculation of oxygen pressures in equilibrium with a metal and its
oxide at a given temperature
Thermodynamic principles of extraction
c. Use of oxygen scale
d. Use of CO/CO2 scale
e. Use of H2/H2O scale
• Free energies of formation of sulphides
• Thermo-chemical data bank
Assignment chemical equilibrium_jh_sir-4168NEETRICKSJEE
This document provides information about chemical equilibrium. It begins with defining types of chemical reactions as irreversible or reversible. For reversible reactions, the document states that the reactants and products can interconvert under equilibrium conditions. Several examples of homogeneous and heterogeneous equilibrium reactions are given. The key characteristics of chemical equilibrium are then outlined, including the dynamic nature of equilibrium and the role of Le Chatelier's principle in affecting the equilibrium position. The concepts of equilibrium constants Kp and Kc are introduced, along with how to use them to predict reaction direction and extent. Factors that influence the equilibrium position like concentration, pressure, temperature and catalysts are also discussed.
Enzyme Kinetics and thermodynamic analysisKAUSHAL SAHU
Introduction
Kinetics and thermodynamicSG
Thermodynamic in enzymatic reactions
balanced equations in chemical reactions
changes in free energy determine the direction & equilibrium state of chemical reactions
the rates of reactions
Factors effecting enzymatic activity
(i) Enzyme concentration.
(ii) Substrate concentration.
(iii)Temperature
(iv) pH.
(v) Activators.
(vi)Inhibitors
Michaelis-menten equation
CONCLUSIONS
REFERENECES
Level 3 NCEA - NZ: A Nation In the Making 1872 - 1900 SML.pptHenry Hollis
The History of NZ 1870-1900.
Making of a Nation.
From the NZ Wars to Liberals,
Richard Seddon, George Grey,
Social Laboratory, New Zealand,
Confiscations, Kotahitanga, Kingitanga, Parliament, Suffrage, Repudiation, Economic Change, Agriculture, Gold Mining, Timber, Flax, Sheep, Dairying,
LAND USE LAND COVER AND NDVI OF MIRZAPUR DISTRICT, UPRAHUL
This Dissertation explores the particular circumstances of Mirzapur, a region located in the
core of India. Mirzapur, with its varied terrains and abundant biodiversity, offers an optimal
environment for investigating the changes in vegetation cover dynamics. Our study utilizes
advanced technologies such as GIS (Geographic Information Systems) and Remote sensing to
analyze the transformations that have taken place over the course of a decade.
The complex relationship between human activities and the environment has been the focus
of extensive research and worry. As the global community grapples with swift urbanization,
population expansion, and economic progress, the effects on natural ecosystems are becoming
more evident. A crucial element of this impact is the alteration of vegetation cover, which plays a
significant role in maintaining the ecological equilibrium of our planet.Land serves as the foundation for all human activities and provides the necessary materials for
these activities. As the most crucial natural resource, its utilization by humans results in different
'Land uses,' which are determined by both human activities and the physical characteristics of the
land.
The utilization of land is impacted by human needs and environmental factors. In countries
like India, rapid population growth and the emphasis on extensive resource exploitation can lead
to significant land degradation, adversely affecting the region's land cover.
Therefore, human intervention has significantly influenced land use patterns over many
centuries, evolving its structure over time and space. In the present era, these changes have
accelerated due to factors such as agriculture and urbanization. Information regarding land use and
cover is essential for various planning and management tasks related to the Earth's surface,
providing crucial environmental data for scientific, resource management, policy purposes, and
diverse human activities.
Accurate understanding of land use and cover is imperative for the development planning
of any area. Consequently, a wide range of professionals, including earth system scientists, land
and water managers, and urban planners, are interested in obtaining data on land use and cover
changes, conversion trends, and other related patterns. The spatial dimensions of land use and
cover support policymakers and scientists in making well-informed decisions, as alterations in
these patterns indicate shifts in economic and social conditions. Monitoring such changes with the
help of Advanced technologies like Remote Sensing and Geographic Information Systems is
crucial for coordinated efforts across different administrative levels. Advanced technologies like
Remote Sensing and Geographic Information Systems
9
Changes in vegetation cover refer to variations in the distribution, composition, and overall
structure of plant communities across different temporal and spatial scales. These changes can
occur natural.
The chapter Lifelines of National Economy in Class 10 Geography focuses on the various modes of transportation and communication that play a vital role in the economic development of a country. These lifelines are crucial for the movement of goods, services, and people, thereby connecting different regions and promoting economic activities.
A Visual Guide to 1 Samuel | A Tale of Two HeartsSteve Thomason
These slides walk through the story of 1 Samuel. Samuel is the last judge of Israel. The people reject God and want a king. Saul is anointed as the first king, but he is not a good king. David, the shepherd boy is anointed and Saul is envious of him. David shows honor while Saul continues to self destruct.
This presentation was provided by Rebecca Benner, Ph.D., of the American Society of Anesthesiologists, for the second session of NISO's 2024 Training Series "DEIA in the Scholarly Landscape." Session Two: 'Expanding Pathways to Publishing Careers,' was held June 13, 2024.
Temple of Asclepius in Thrace. Excavation resultsKrassimira Luka
The temple and the sanctuary around were dedicated to Asklepios Zmidrenus. This name has been known since 1875 when an inscription dedicated to him was discovered in Rome. The inscription is dated in 227 AD and was left by soldiers originating from the city of Philippopolis (modern Plovdiv).
Philippine Edukasyong Pantahanan at Pangkabuhayan (EPP) CurriculumMJDuyan
(𝐓𝐋𝐄 𝟏𝟎𝟎) (𝐋𝐞𝐬𝐬𝐨𝐧 𝟏)-𝐏𝐫𝐞𝐥𝐢𝐦𝐬
𝐃𝐢𝐬𝐜𝐮𝐬𝐬 𝐭𝐡𝐞 𝐄𝐏𝐏 𝐂𝐮𝐫𝐫𝐢𝐜𝐮𝐥𝐮𝐦 𝐢𝐧 𝐭𝐡𝐞 𝐏𝐡𝐢𝐥𝐢𝐩𝐩𝐢𝐧𝐞𝐬:
- Understand the goals and objectives of the Edukasyong Pantahanan at Pangkabuhayan (EPP) curriculum, recognizing its importance in fostering practical life skills and values among students. Students will also be able to identify the key components and subjects covered, such as agriculture, home economics, industrial arts, and information and communication technology.
𝐄𝐱𝐩𝐥𝐚𝐢𝐧 𝐭𝐡𝐞 𝐍𝐚𝐭𝐮𝐫𝐞 𝐚𝐧𝐝 𝐒𝐜𝐨𝐩𝐞 𝐨𝐟 𝐚𝐧 𝐄𝐧𝐭𝐫𝐞𝐩𝐫𝐞𝐧𝐞𝐮𝐫:
-Define entrepreneurship, distinguishing it from general business activities by emphasizing its focus on innovation, risk-taking, and value creation. Students will describe the characteristics and traits of successful entrepreneurs, including their roles and responsibilities, and discuss the broader economic and social impacts of entrepreneurial activities on both local and global scales.
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CSIR NET LIFE
unit-1
Bioenergetics and Biochemical
Reaction Types
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WELCOME
MERIT LIFE SCIENCESMERIT LIFE SCIENCES
e-TUTORIALe-TUTORIAL
NEET/NET JRF CSIR EXAM /JAM/DBT
DR SHEELENDRA Ph.D. FROM BHU
FACULTY: DR SHEELENDRA BHATT
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UNIT-1
BIOENERGETICS-2
TIME 8:00-10:00PM
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• Heat energy can be used to do work
only through a change of temperature.
Bioenergetics & ATPBioenergetics & ATP
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Standard free energy change (∆G°) of a
chemical reaction:
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• When a reaction results in release of energy
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The free-energy change of a reaction (ΔG) divided
into 3 types:
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Standard free energy change (∆G°) of a
chemical reaction:
For every reaction ∆G can be calculated using:-
∆G° = - 2.303 RT log Keq
While:
R = Gas constant
T = AbsoluteTemp.
Keq = Equilibrium constant
Note:
∆G° indicates constant temperature & pressure and physiological pH 7.2
for cells.
Unites of free energy = calorie (cal) or kilocalorie (kcal) /mole
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Units of energy
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• ΔG° is the free energy change for this reaction under
standard conditions that is, when each of the
reactants A, B, C, and D is present at a concentration
of 1.0 M (for a gas, the standard state is usually chosen
to be 1 atmosphere).
• Thus, the ΔG of a reaction depends on the nature of
the reactants (expressed in the ΔG° term of equation
1) and on their concentrations (expressed in the
logarithmic term of equation 1).
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•The ΔG of a reaction depends only on the free energy
of the products (the final state) minus the free energy
of the reactants (the initial state).
•The ΔG of a reaction is independent of the path (or
molecular mechanism) of the transformation. The
mechanism of a reaction has no effect on ΔG.
•The ΔG provides no information about the rate of a
reaction.
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∆G values of pathways can be
calculated
The ∆G value of an overall pathway can be calculated as
the algebraic sum of the ∆G values of the individual
reactions making the pathway:-
∆Gpathway= ∆G1 + ∆G2 + ∆G3 + ∆G4 + ∆G5
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Free energy of a reaction
The free energy change (∆G) of a reaction determines
its spontaneity. A reaction is spontaneous if ∆G is
negative (if the free energy of products is less than
that of reactants).
∆Go
' = standard free energy change (at pH 7, 1M
reactants & products); R = gas constant; T = temp.
For a reaction A + B C + D
∆G = ∆Go
' + RT ln
[C] [D]
[A] [B]
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∆Go
' of a reaction may be positive, & ∆G negative,
depending on cellular concentrations of reactants and
products.
Many reactions for which ∆Go
' is positive are
spontaneous because other reactions cause depletion
of products or maintenance of high substrate
concentration.
For a reaction A + B C + D
∆G = ∆Gº' + RT ln
[A] [B]
[C] [D]
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At equilibrium
∆G = 0.
K'eq, the ratio [C][D]/[A]
[B] at equilibrium, is the
equilibrium constant.
An equilibrium constant
(K'eq) greater than one
indicates a spontaneous
reaction (negative ∆G°').
∆G = ∆Gº' + RT ln
0 = ∆Gº' + RT ln
∆Gº' = - RTln
defining K'eq =
∆Gº' = - RT ln K'eq
[C] [D]
[A] [B]
[C] [D]
[A] [B]
[C] [D]
[A] [B]
[C] [D]
[A] [B]
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K'eq
∆G º'
kJ/mol
Starting with 1 M reactants &
products, the reaction:
104
- 23 proceeds forward (spontaneous)
102
- 11 proceeds forward (spontaneous)
100
= 1 0 is at equilibrium
10
-2 + 11 reverses to form “reactants”
10
-4 + 23 reverses to form “reactants”
∆Go
' = − RT ln K'eq
Variation of equilibrium constant with ∆Go
‘ (25 o
C)
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Energy coupling
A spontaneous reaction may drive a non-spontaneous reaction.
Free energy changes of coupled reactions are additive.
A. Some enzyme-catalyzed reactions are
interpretable as two coupled half-reactions, one
spontaneous and the other non-spontaneous.
At the enzyme active site, the coupled reaction is kinetically
facilitated, while individual half-reactions are prevented.
Free energy changes of half reactions may be summed, to yield the
free energy of the coupled reaction.
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For example, in the reaction catalyzed by the Glycolysis
enzyme Hexokinase, the half-reactions are:
ATP + H2O ↔ ADP + Pi ∆Go
' = −31 kJ/mol
Pi + glucose ↔ glucose-6-P + H2O ∆Go
' = +14 kJ/mol
Coupled reaction:
ATP + glucose ↔ ADP + glucose-6-P ∆Go
' = −17 kJ/mol
The structure of the enzyme active site, from which H2O
is excluded, prevents the individual hydrolytic reactions,
while favoring the coupled reaction.
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B.Two separate reactions, occurring in the same cellular compartment, one
spontaneous and the other not, may be coupled by a common intermediate
(reactant or product).
A hypothetical, but typical, example involving PPi:
Enzyme 1:
A + ATP ↔ B + AMP + PPi ∆Go
' = + 15 kJ/mol
Enzyme 2:
PPi + H2O ↔ 2Pi ∆Go
' = – 33 kJ/mol
Overall spontaneous reaction:
A + ATP + H2O ↔ B + AMP + 2Pi ∆Go
' = – 18 kJ/mol
Pyrophosphate (PPi) is often the product of a reaction that needs a driving
force.
Its spontaneous hydrolysis, catalyzed by Pyrophosphatase enzyme, drives
the reaction for which PPi is a product.
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Ion Transport may be coupled
to a chemical reaction, e.g.,
hydrolysis or synthesis of ATP.
In this diagram & below,
water is not shown. It should
be recalled that the ATP
hydrolysis/synthesis reaction
is: ATP + H2O ↔ ADP + Pi.
S1 S2
ATP
ADP + Pi
Side 1 Side 2
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The free energy change (electrochemical potential
difference) associated with transport of an ion S
across a membrane from side 1 to side 2 is:
R = gas constant, T = temperature, Z = charge on the ion,
F = Faraday constant, ∆Ψ = voltage.
∆G = R T ln + Z F ∆Ψ
[S]1
[S]2
S1 S2
Side 1 Side 2
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∆G for ion flux - varies with ion gradient & voltage.
∆G for chemical reaction - negative ∆Go
' for ATP
hydrolysis; ∆G depends also on [ATP], [ADP], [Pi].
Since free energy changes
are additive, the
spontaneous direction
for the coupled reaction
will depend on relative
magnitudes of:
S1 S2
ATP
ADP + Pi
Side 1 Side 2
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Two examples:
ActiveTransport: Spontaneous ATP hydrolysis
(negative ∆G) is coupled to (drives) ion flux against a
gradient (positive ∆G).
ATP synthesis: Spontaneous H+
flux (negative ∆G) is
coupled to (drives) ATP synthesis (positive ∆G).
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“High energy” bonds
Phosphoanhydride bonds (formed by splitting out H2O
between 2 phosphoric acids or between carboxylic &
phosphoric acids) have a large negative ∆G of hydrolysis.
N
NN
N
NH2
O
OHOH
HH
H
CH2
H
OPOPOP-O
O
O- O-
O O
O-
adenine
ribose
ATP
adenosine triphosphate
phosphoanhydride
bonds (~)
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N
NN
N
NH2
O
OHOH
HH
H
CH2
H
OPOPOP-O
O
O- O-
O O
O-
adenine
ribose
ATP
adenosine triphosphate
phosphoanhydride
bonds (~)
Phosphoanhydride linkages are said to be "high energy"
bonds. Bond energy is not high, just ∆G of hydrolysis.
"High energy" bonds are represented by the "~" symbol.
~P represents a phosphate group with a large negative
∆G of hydrolysis.
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Compounds with “high energy bonds” are said to
have high group transfer potential.
For example, Pi may be spontaneously cleaved from
ATP for transfer to another compound (e.g., to a
hydroxyl group on glucose).
“High energy” bonds
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Example: AMPPNP.
Such analogs have been used to study the dependence of
coupled reactions onATP hydrolysis.
In addition, they have made it possible to crystallize an
enzyme that catalyzes ATP hydrolysis with an ATP analog
at the active site.
AMPPNP (ADPNP) ATP analog
N
NN
N
NH2
O
OHOH
HH
H
CH2
H
OPOPNP-O
O
O- O-
O O
O-
H
Artificial ATP
analogs have
been designed
that are resistant
to cleavage of
the terminal
phosphate by
hydrolysis.
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A reaction important for equilibrating ~P among
adenine nucleotides within a cell is that catalyzed by
Adenylate Kinase:
ATP + AMP ↔ 2 ADP
The Adenylate Kinase reaction is also important because
the substrate for ATP synthesis, e.g., by mitochondrial
ATP Synthase, is ADP, while some cellular reactions
dephosphorylate ATP all the way to AMP.
The enzyme Nucleoside Diphosphate Kinase (NuDiKi)
equilibrates ~P among the various nucleotides that are
needed, e.g., for synthesis of DNA & RNA.
NuDiKi catalyzes reversible reactions such as:
ATP + GDP ↔ ADP + GTP,
ATP + UDP ↔ ADP + UTP, etc.
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Inorganic polyphosphate
Many organisms store energy as inorganic
polyphosphate, a chain of many phosphate residues
linked by phosphoanhydride bonds:
P~P~P~P~P...
Hydrolysis of Pi residues from polyphosphate may be
coupled to energy-dependent reactions.
Depending on the organism or cell type, inorganic
polyphosphate may have additional functions.
E.g., it may serve as a reservoir for Pi
, a chelator of
metal ions, a buffer, or a regulator.
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Why do phosphoanhydride linkages have a high ∆G
of hydrolysis? Contributing factors for ATP & PPi
include:
Resonance stabilization of products of hydrolysis exceeds resonance
stabilization of the compound itself.
Electrostatic repulsion between negatively charged phosphate
oxygen atoms favors separation of the phosphates.
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Creatine Kinase catalyzes:
Phosphocreatine + ADP ↔ ATP + creatine
This is a reversible reaction, though the equilibrium
constant slightly favors phosphocreatine formation.
Phosphocreatine is produced when ATP levels are high.
When ATP is depleted during exercise in muscle, phosphate is transferred
from phosphocreatine to ADP, to replenish ATP.
−
O P
H
N C
O
O−
N
NH2
+
CH2
CH3
C
O
O−
phosphocreatine
Phosphocreatine (creatine
phosphate), another
compound with a "high
energy" phosphate linkage,
is used in nerve & muscle
for storage of ~P bonds.
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Phosphoenolpyruvate (PEP), involved in ATP synthesis
in Glycolysis, has a very high ∆G of Pi hydrolysis.
Removal of Pi from ester linkage in PEP is spontaneous
because the enol spontaneously converts to a ketone.
The ester linkage in PEP is an exception.
C
C
O O−
OPO3
2−
CH2
C
C
O O−
O
CH3
C
C
O O−
OH
CH2
ADP ATP
H+
PEP enolpyruvate pyruvate
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Generally phosphate esters, formed by splitting out
water between a phosphoric acid and an OH group,
have a low but negative ∆G of hydrolysis. Examples:
the linkage between the first phosphate and the ribose hydroxyl of ATP.
N
NN
N
NH2
O
OHOH
HH
H
CH2
H
OPOPOP-O
O
O- O-
O O
O-
adenine
ribose
ATP (adenosine triphosphate)
ester linkage
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Other examples of phosphate esters with low but
negative ∆G of hydrolysis:
the linkage between phosphate & a hydroxyl group in glucose-6-
phosphate or glycerol-3-phosphate.
glycerol-3-phosphate
CH2
CH
CH2
OH
HO
O P
O
O−
O−
H O
OH
H
OHH
OH
CH2
H
OH
H
1
6
5
4
3 2
O P
O
OH
OH
glucose-6-phosphate
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the linkage between phosphate and the hydroxyl group of an amino
acid residue in a protein (serine, threonine or tyrosine).
Regulation of proteins by phosphorylation and dephosphorylation will
be discussed later.
Protein OH + ATP Protein O P
O
O−
O−
+ ADP
Pi H2O
Protein Kinase
Protein Phosphatase
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ATP has special roles in energy coupling & Pi transfer.
∆G of phosphate hydrolysis from ATP is intermediate
among examples below.
ATP can thus act as a Pi donor, & ATP can be synthesized
by Pi transfer, e.g., from PEP.
Compound
∆Go
' of phosphate
hydrolysis, kJ/mol
Phosphoenolpyruvate (PEP) −61.9
Phosphocreatine −43.1
Pyrophosphate −33.5
ATP (to ADP) −30.5
Glucose-6-phosphate −13.8
Glycerol-3-phosphate −9.2
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Coenzyme A-SH + HO C
O
R
Coenzyme A-S C
O
R + H2O
A thioester forms between a carboxylic acid & a thiol
(SH), e.g., the thiol of coenzyme A (abbreviated CoA-SH).
Thioesters are ~ linkages. In contrast to phosphate esters,
thioesters have a large negative ∆G of hydrolysis.
Some other
“high energy”
bonds:
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The thiol of coenzyme A can react with a carboxyl
group of acetic acid (yielding acetyl-CoA) or a fatty
acid (yielding fatty acyl-CoA).
The spontaneity of thioester cleavage is essential to the
role of coenzyme A as an acyl group carrier.
Like ATP, CoA has a high group transfer potential.
Coenzyme A-SH + HO C
O
CH3
Coenzyme A-S C
O
CH3 + H2O
acetic acid
acetyl-CoA
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Coenzyme A includes
β-mercaptoethylamine,
in amide linkage to the
carboxyl group of the B
vitamin pantothenate.
The hydroxyl of
pantothenate is in ester
linkage to a phosphate
of ADP-3'-phosphate.
The functional group is
the thiol (SH) of
β-mercaptoethylamine.
N
N N
N
NH2
O
OHO
HH
H
CH2
H
OPOPOH2C
O−
O O
O−
P
O
O−−
O
C
C
C
NH
CH2
CH2
C
NH
CH3H3C
HHO
O
CH2
CH2
SH
O
β-mercaptoethylamine
pantothenate
ADP-3'-phosphate
Coenzyme A
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3',5'-Cyclic AMP (cAMP), is used by
cells as a transient signal.
Adenylate Cyclase catalyzes cAMP
synthesis: ATP → cAMP + PPi.
The reaction is highly spontaneous
due to the production of PPi, which
spontaneously hydrolyzes.
Phosphodiesterase catalyzes
hydrolytic cleavage of one Pi ester
(red), converting cAMP → 5'-AMP.
N
N N
N
NH2
O
OHO
HH
H
H2
C
H
O
P
O
O-
1'
3'
5' 4'
2'
cAMP
This is a highly spontaneous reaction, because cAMP is
sterically constrained by having a phosphate with ester
links to 2 hydroxyls of the same ribose. The lability of
cAMP to hydrolysis makes it an excellent transient signal.
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List compounds exemplifying the following roles
of "high energy" bonds:
Energy transfer or storage
ATP, PPi, polyphosphate, phosphocreatine
Group transfer
ATP, Coenzyme A
Transient signal
cyclic AMP
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Kinetics vsThermodynamics:
A high activation energy barrier usually causes
hydrolysis of a “high energy” bond to be very slow in
the absence of an enzyme catalyst.
This kinetic stability is essential to the role of ATP and
other compounds with ~ bonds.
If ATP would rapidly hydrolyze in the absence of a
catalyst, it could not serve its important roles in energy
metabolism and phosphate transfer.
Phosphate is removed from ATP only when the
reaction is coupled via enzyme catalysis to some other
reaction useful to the cell, such as transport of an ion,
phosphorylation of glucose, or regulation of an enzyme
by phosphorylation of a serine residue.
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Oxidation & reduction
Oxidation & reduction will be covered in more detail later.
The evolution of photosynthesis, and the generation of
the oxygen that is now plentiful in our environment,
allowed development of metabolic pathways that derive
energy from transfer of electrons from various
reductants ultimately to molecular oxygen.
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Oxidation of an iron atom involves loss of an electron
(to an acceptor): Fe++
(reduced) Fe+++
(oxidized) + e-
Since electrons in a C-O bond are associated more with
O, increased oxidation of a C atom means increased
number of C-O bonds.
Oxidation of carbon is spontaneous (energy-yielding).
Two important e−
carriers in metabolism: NAD+
& FAD.
Increasing oxidation of carbon
H
CH H
H
H
CH OH
H
H
C
H
O
O
C
O
OH
C
H
O
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NAD+
, Nicotinamide
Adenine Dinucleotide,
is an electronacceptor
in catabolic pathways.
The nicotinamide ring,
derived from the vitamin
niacin, accepts 2 e-
& 1 H+
(a hydride) in going to
the reduced state,
NADH.
NADP+
/NADPH is
similar except for Pi.
NADPH is e−
donor in
synthetic pathways.
H
C
NH2
O
CH2
H
N
H
OH OH
H H
O
OP
O
HH
OH OH
H H
O
CH2
N
N
N
NH2
OP
O
O
−
O
+
N−
O
nicotinamide
adenine
esterified to
Pi in NADP+
Nicotinamide
Adenine
Dinucleotide
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NAD+
/NADH
The electron transfer reaction may be summarized
as :
NAD+
+ 2e−
+ H+
↔ NADH.
It may also be written as:
NAD+
+ 2e−
+ 2H+
↔ NADH + H+
N
R
H
C
NH2
O
N
R
C
NH2
O
H H
+
+ 2 e−
+ H+
NAD+
NADH
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FAD (Flavin Adenine Dinucleotide), derived from the
vitamin riboflavin, functions as an e−
acceptor.
The dimethylisoalloxazine ring undergoes
reduction/oxidation.
FAD accepts 2e−
+ 2H+
in going to its reduced state:
FAD + 2e−
+ 2H+
↔ FADH2
C
C
C
H
C
C
H
C
N
C
C
N
N
C
NH
C
H3C
H3C
O
O
CH2
HC
HC
HC
H2C
OH
O P O P O
O
O-
O
O-
Ribose
OH
OH
Adenine
C
C
C
H
C
C
H
C
N
C
C
H
N
N
H
C
NH
C
H3C
H3C
O
O
CH2
HC
HC
HC
H2C
OH
O P O P O
O
O-
O
O-
Ribose
OH
OH
Adenine
FAD FADH2
2 e−
+ 2 H+
dimethylisoalloxazine
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NAD+
is a coenzyme, that reversibly binds to
enzymes.
FAD is a prosthetic group, that remains tightly
bound at the active site of an enzyme.
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Chemistry of ATP (Adenosine – tri –
phosphate):ATP is a nucleotide type molecule made of the following
components:-
1.The nitrogenous base adenine
2.The pentose sugar ribose
3.Three phosphate groups
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Chemistry of ATP (Adenosine – tri –
phosphate)
Thus:-Thus:-
ATP ADP + Pi ∆G = -7.3 kcal/mole
ADP AMP + Pi ∆G = -7.2 kcal/mole
AMP Adenosine + Pi ∆G = -3.2 kcal/mole
ATP, ADP and AMP are present in all forms of life. They
occur not only in the cytosol of cells but also in the
mitochondria & nucleus. In normal respiring cells ATP
makes up 80% of the three ribonucleotides. ADP & AMP
account for 20%.
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Chemistry of ATP (Adenosine – tri –
phosphate):
At pH 7, ATP occurs as the multiply charged anion ATP4-
whereas ADP
occurs as ADP3-
. This is because their phosphate groups are completely
ionized at the intracellular PH. ATP and ADP occur inside cells as
magnesium complexes:-
ATP4-
+ Mg2+
(ATP-Mg)2-
ADP3-
+ Mg2+
(ADP-Mg)
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Chemistry of ATP (Adenosine – tri –
phosphate):
Inside cells the concentration of ATP remains normally relatively
constantly high. It’s rate of formation equals it’s rate of
hydrolysis. Thus the terminal phosphate group of ATP
undergoes continuous removal & replacement from the pool of
inorganic phosphate during cell metabolism.
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∆G values for some characteristic
reactions
Super high energy compounds are compounds generated during
catabolism. They are phosphorylated compounds. Once formed along a
catabolic pathway, they undergo immediate hydrolysis
(dephosphorylation). As a result a large amount of energy is released
this is used by the cell to synthesize ATP from ADP and the hydrolyzed
inorganic phosphate.
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∆G values for some characteristic
reactions
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The Bioenergetics of Muscle Contraction
The contraction of muscle requires a large amount of energy that
cannot be fulfilled by the ATP stored inside muscle tissue. In
addition to ATP there is a super-high energy compound stored in
muscle cells that plays a major role in the energetics of muscle. This
super-high energy compound is also present in large concentrations
in other contractile tissues such as brain & nerve tissue.
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The Bioenergetics of Muscle Contraction
This compound is PHOSPHOCREATINE. It serves as a storage
form of high energy phosphate groups. The ∆G value for the
hydrolytic reaction of phosphocreatine is highly negative (-10.3
kcal/mole). This is greater than that of ATP. The energy released is
sufficient to allow coupled synthesis of ATP from ADP:-
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The Bioenergetics of Muscle
Contraction
Phosphocreatine thus functions to keep the ATP
concentration in muscle cells at constantly high level
whenever some of the ATP of muscle cells is used for
contraction, ADP is formed. Through the action of
creatine kinase phosphocreatine is quickly hydrolyzed
and donates its phosphate group to ADP to form ATP.
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The phosphocreatine level inside muscle is 3-4 times greater
than that of ATP and thus stores enough high energy phosphate
groups to keep the ATP level constantly high during short
periods of intense muscular contraction.
The Bioenergetics of Muscle
Contraction
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The Bioenergetics of Muscle
Contraction:
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Bioenergetics
• Bioenergetics
• The quantitative study of…
• Cellular energy transduction
• Nature and function of the chemical processes for energy
transductions
• Fundamental laws in thermodynamics governing
bioenergetics
• First law : Energy conservation
• Second law: Increase in entropy
Living Orgamism
1. Metabolism
2. Reproduction
Energy: work to survive and reproduce
Energy transduction in biological system
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Free Energy Change for Biological Reactions
• Thermodynamic quantities describing the energy changes in chemical
reaction
• Gibbs free energy, G
• The amount of energy capable of doing work during a reaction at constant
T and P
• Positive ∆G : endergonic
• Negative ∆G : exergonic, spontaneous reaction
• Enthalpy, H
• The heat content of the reacting system
• Number & kinds of chemical bonds in the reactants and products
• Positive ∆H : endothermic
• Negative ∆H : exothermic
• Entropy, S
• Quantitative expression for the randomness or disorder in a system
• ∆G = ∆H –T∆S
• Cells use free energy for reactions
• Energy source
• Heterotrope :Nutrient
• Autotrope: Solar energy
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Standard Free Energy Change vs. Equilibrium Constant
• aA + bB cC + dD
• Equilibrium constant [Ceq]c
[Deq]d
[Aeq]a
[Beq]b
• ∆Go
: standard free energy change (J/mol)
• 298K=25o
C, 1M of initial reactants and products,1 atm (101.3 kPa)
• Standard transformed constants
• pH 7, 55.5M water, 1mM Mg2+
(ATP as reactant)
• ∆G’o
,K’eq
• ∆G’o
= -RT ln K’eq
• Spontaneous reaction
• K’’
eq >1
• ∆Go
: negative
Keq =
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∆G’o
for some representative chemical reactions
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∆G’o
are additive
• Sequential chemical reactions
• (1) A B : ∆G’1
o
,K’eq1
glucose + Pi G-6P + H2O ; ∆G’o
= 13.8 kJ/mol
• (2) B C : ∆G’2
o
,K’eq2
ATP + H2O ADP + Pi ;∆G’o
= -30.5 kJ/mol
• (1) + (2) : A C : ∆G’1
o
+ ∆G’1
o
,K’eq1 X K’eq2
ATP + glucose ADP + Pi ; ∆G’o
= -16.7 kJ/mol
• Coupling of endergonic and exergonic reaction to make exergonic
reaction
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The ΔG of a Reaction Depends on
Changes in Enthalpy (Bond Energy) and
Entropy
At any constant temperature and pressure, two factors determine
the ΔG of a reaction and thus whether the reaction will tend to
occur:
the change in bond energy between reactants and products and
the change in the randomness of the system. Gibbs showed that
free energy can be defined as
where H is the bond energy, or enthalpy, of the system; T is its
temperature in degrees Kelvin (K); and S is a measure of
randomness, called entropy.
If temperature remains
constant, a reaction proceeds
spontaneously only if the
free energy change ΔG in the
following equation is
negative:
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In an exothermic reaction, the products contain less bond energy than the
reactants, the liberated energy is usually converted to heat (the energy of
molecular motion), and ΔH is negative.
In an endothermic reaction, the products contain more bond energy than the
reactants, heat is absorbed, and ΔH is positive.
Reactions tend to proceed if they liberate energy (if ΔH < 0), but this is only
one of two important parameters of free energy to consider; the other is
entropy.
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Entropy S is a measure of the degree of
randomness or disorder of a system.
Entropy increases as a system becomes more
disordered and decreases as it becomes more
structured.
Consider, for example, the diffusion of solutes from one
solution into another one in which their concentration is
lower.
This important biological reaction is driven only by an
increase in entropy; in such a process ΔH is near zero.
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suppose that a 0.1 M solution of glucose is
separated from a large volume of water by a
membrane through which glucose can diffuse.
Diffusion of glucose molecules across the
membrane will give them more room in which
to move, with the result that the randomness, or
entropy, of the system is increased.
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Common Biochemical Reaction
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Common Biochemical Reaction
Two basic chemical principle
1. A covalent bond can be broken in two general way: homolytic cleavage
and heterolytic cleavge
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2. Biochemical reactions involve interactions between nucleophiles and
electrophiles
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Most of the reactions in living cells fall into one of five general
categories
1.Reaction that make or break carbon-carbon bond
2.Internal rearrangements, isomerization, and elimination
3.Free-radical reaction
4.Group transfer: acyl, glycosyl, phosphoryl
5.Oxidation-reduction
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Reaction that make or break carbon-carbon bond
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Internal rearrangements, isomerization, and
elimination
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Internal rearrangements, isomerization, and
elimination
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Free-radical-mediated decarboxylation
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Acyl group transfer
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Phosphoryl group transfer
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The oxidation states of carbon in biomolecules
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Oxidation-Reduction
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Phosphoryl group transfers and ATP
The free energy change for ATP hydrolysis is large negative
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Other phosphorylated compounds also have large free
energies of hydrolysis
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For hydrolysis reactions with large negative free-energy changes, the
products are more stable than the reactants for one or more of the
following reasons
1.The bond strain is relieved by charge separation (ATP).
2.The products are stabilized by ionization (ATP, 3-phosphoglycerate,
thioester) .
3.The products are stabilized by isomerization (PEP)
4.The products are stabilized by resonance (creatin, inorganic phosphate,
thioester)
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ATP provides energy by group transfer
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ATP serve as the universal energy currency in
all living cells Because of its intermediate
position on the scale of group transfer
potential.
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ATP donates phosphoryl, pyrophosphoryl,
and adenyl group
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Transphosphorylation between nucleotide by
nucleotide diphosphate kinase
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Inorganic phosphate may serve as a reservoir
of phosphoryl group with high energy
transfer potential
Polyphosphate kinase-1 (in bacterial)
Polyphosphate kinase-2
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Biological oxidation-reduction reaction
1.The transfer of phosphoryl groups is a central feature of metabolism
2.Electron transfer in oxidation-reduction reaction is another important
transfer in living cells.
3.The flow of electrons is responsible for all work done by living organism
4.In heterotroph, the source of electron are reduced compounds (food)
5.In autotroph, the source of electron is a chemical species excited by the
absorption of light (e.g. H2O).
6.Cells contain a variety of molecular energy transducers, which convert
the every of electron flow into useful work
7.Biological oxidation often involve dehydrogenation
- alkane (-CH2-CH2-) convert to alkene (-CH=CH-)
- oxidation is coincident with the loss of hydrogen
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Oxidation states of carbon in the biosphere
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A Few Types of Coenzymes and Proteins Serve as Universal Electron
1.Electrons from hundreds of different substrates into a few types of
universal electron carriers
2.NAD, NADP, FMN, and FAD are water soluble coenzymes that undergo
reversible oxidation and reduction in many of the electron-transfer
reactions of metabolism
3.Lipid-soluble quinones, such as ubiquinone, act as electorn carriers and
proton donors in membrane
4.Iron-sulfur proteins and cytochromes that undergo reversible oxidation-
reduction reaction
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Editor's Notes
FIGURE 13-2 Common nucleophiles and electrophiles in biochemical reactions. Chemical reaction mechanisms, which trace the formation and breakage of covalent bonds, are communicated with dots and curved arrows, a convention known informally as &quot;electron pushing.&quot; A covalent bond consists of a shared pair of electrons. Nonbonded electrons important to the reaction mechanism are designated by dots. Curved arrows represent the movement of electron pairs. For movement of a single electron (as in a free radical reaction), a single-headed (fishhook-type) arrow is used. Most reaction steps involve an unshared electron pair.
FIGURE 13-4 Some common reactions that form and break C—C bonds in biological systems. For both the aldol condensation and the Claisen condensation, a carbanion serves as nucleophile and the carbon of a carbonyl group serves as electrophile. The carbanion is stabilized in each case by another carbonyl at the adjoining carbon. In the decarboxylation reaction, a carbanion is formed on the carbon shaded blue as the CO2 leaves. The reaction would not occur at an appreciable rate without the stabilizing effect of the carbonyl adjacent to the carbanion carbon. Wherever a carbanion is shown, a stabilizing resonance with the adjacent carbonyl, as shown in Figure 13-3b, is assumed. An imine (Figure 13-3c) or other electron-withdrawing group (including certain enzymatic cofactors such as pyridoxal) can replace the carbonyl group in the stabilization of carbanions.
FIGURE 13-6a Isomerization and elimination reactions. (a) The conversion of glucose 6-phosphate to fructose 6-phosphate, a reaction of sugar metabolism catalyzed by phosphohexose isomerase.
FIGURE 13-7 A free radicalミinitiated decarboxylation reaction. The biosynthesis of heme (see Figure 22-24) in Escherichia coli includes a decarboxylation step in which propionyl side chains on the coproporphyrinogen III intermediate are converted to the vinyl side chains of protoporphyrinogen IX. When the bacteria are grown anaerobically, the enzyme oxygen-independent coproporphyrinogen III oxidase, also called HemN protein, promotes decarboxylation via the free-radical mechanism shown here. The acceptor of the released electron is not known. For simplicity, only the relevant portions of the large coproporphyrinogen III and protoporphyrinogen molecules are shown; the entire structures are given in Figure 22-24. When E. coli are grown in the presence of oxygen, this reaction is an oxidative decarboxylation and is catalyzed by a different enzyme.
FIGURE 13-8c Alternative ways of showing the structure of inorganic orthophosphate. (c) When a nucleophile Z (in this case, the —OH on C-6 of glucose) attacks ATP, it displaces ADP (W). In this SN2 reaction, a pentacovalent intermediate (d) forms transiently.
FIGURE 13-9 The oxidation states of carbon in biomolecules. Each compound is formed by oxidation of the red carbon in the compound shown immediately above. Carbon dioxide is the most highly oxidized form of carbon found in living systems.
FIGURE 13-10 An oxidation-reduction reaction. Shown here is the oxidation of lactate to pyruvate. In this dehydrogenation, two electrons and two hydrogen ions (the equivalent of two hydrogen atoms) are removed from C-2 of lactate, an alcohol, to form pyruvate, a ketone. In cells the reaction is catalyzed by lactate dehydrogenase and the electrons are transferred to the cofactor nicotinamide adenine dinucleotide (NAD). This reaction is fully reversible; pyruvate can be reduced by electrons transferred from the cofactor.
FIGURE 13-11 Chemical basis for the large free-energy change associated with ATP hydrolysis. 1 The charge separation that results from hydrolysis relieves electrostatic repulsion among the four negative charges on ATP. 2 The product inorganic phosphate (Pi) is stabilized by formation of a resonance hybrid, in which each of the four phosphorusミoxygen bonds has the same degree of double-bond character and the hydrogen ion is not permanently associated with any one of the oxygens. (Some degree of resonance stabilization also occurs in phosphates involved in ester or anhydride linkages, but fewer resonance forms are possible than for Pi.) 3 The product ADP2– immediately ionizes, releasing a proton into a medium of very low [H+] (pH 7). A fourth factor (not shown) that favors ATP hydrolysis is the greater degree of solvation (hydration) of the products Pi and ADP relative to ATP, which further stabilizes the products relative to the reactants.
FIGURE 13-13 Hydrolysis of phosphoenolpyruvate (PEP). Catalyzed by pyruvate kinase, this reaction is followed by spontaneous tautomerization of the product, pyruvate. Tautomerization is not possible in PEP, and thus the products of hydrolysis are stabilized relative to the reactants. Resonance stabilization of Pi also occurs, as shown in Figure 13-11.
FIGURE 13-14 Hydrolysis of 1,3-bisphosphoglycerate. The direct product of hydrolysis is 3-phosphoglyceric acid, with an undissociated carboxylic acid group, but dissociation occurs immediately. This ionization and the resonance structures it makes possible stabilize the product relative to the reactants. Resonance stabilization of Pi further contributes to the negative free-energy change.
FIGURE 13-15 Hydrolysis of phosphocreatine. Breakage of the P—N bond in phosphocreatine produces creatine, which is stabilized by formation of a resonance hybrid. The other product, Pi, is also resonance stabilized.
FIGURE 13-16 Hydrolysis of acetyl-coenzyme A. Acetyl-CoA is a thioester with a large, negative, standard free energy of hydrolysis. Thioesters contain a sulfur atom in the position occupied by an oxygen atom in oxygen esters. The complete structure of coenzyme A (CoA, or CoASH) is shown in Figure 8-38.
FIGURE 13-17 Free energy of hydrolysis for thioesters and oxygen esters. The products of both types of hydrolysis reaction have about the same free-energy content (G), but the thioester has a higher free-energy content than the oxygen ester. Orbital overlap between the O and C atoms allows resonance stabilization in oxygen esters; orbital overlap between S and C atoms is poorer and provides little resonance stabilization.
FIGURE 13-18 ATP hydrolysis in two steps. (a) The contribution of ATP to a reaction is often shown as a single step, but is almost always a twostep process. (b) Shown here is the reaction catalyzed by ATP-dependent glutamine synthetase. 1 A phosphoryl group is transferred from ATP to glutamate, then 2 the phosphoryl group is displaced by NH3 and released as Pi.
FIGURE 13-19 Ranking of biological phosphate compounds by standard free energies of hydrolysis. This shows the flow of phosphoryl groups, represented by P, from high-energy phosphoryl group donors via ATP to acceptor molecules (such as glucose and glycerol) to form their low-energy phosphate derivatives. This flow of phosphoryl groups, catalyzed by kinases, proceeds with an overall loss of free energy under intracellular conditions. Hydrolysis of low-energy phosphate compounds releases Pi, which has an even lower phosphoryl group transfer potential (as defined in the text).
FIGURE 13-20 Nucleophilic displacement reactions of ATP. Any of the three P atoms (α, β, or γ) may serve as the electrophilic target for nucleophilic attack—in this case, by the labeled nucleophile R—18O:. The nucleophile may be an alcohol (ROH), a carboxyl group (RCOO–), or a phosphoanhydride (a nucleoside mono- or diphosphate, for example). (a) When the oxygen of the nucleophile attacks the γ position, the bridge oxygen of the product is labeled, indicating that the group transferred from ATP is a phosphoryl (—PO32–), not a phosphate (—OPO32–). (b) Attack on the β position displaces AMP and leads to the transfer of a pyrophosphoryl (not pyrophosphate) group to the nucleophile. (c) Attack on the α position displaces PPi and transfers the adenylyl group to the nucleophile.
BOX 13-1 FIGURE 1a The firefly, a beetle of the Lampyridae family.
BOX 13-1 FIGURE 1b Important components in the firefly bioluminescence cycle.
FIGURE 13-21 Ping-Pong mechanism of nucleoside diphosphate kinase. The enzyme binds its first substrate (ATP in our example), and a phosphoryl group is transferred to the side chain of a His residue. ADP departs, and another nucleoside (or deoxynucleoside) diphosphate replaces it, and this is converted to the corresponding triphosphate by transfer of the phosphoryl group from the phosphohistidine residue.
FIGURE 13-22 Oxidation states of carbon in the biosphere. The oxidation states are illustrated with some representative compounds. Focus on the red carbon atom and its bonding electrons. When this carbon is bonded to the less electronegative H atom, both bonding electrons (red) are assigned to the carbon. When carbon is bonded to another carbon, bonding electrons are shared equally, so one of the two electrons is assigned to the red carbon. When the red carbon is bonded to the more electronegative O atom, the bonding electrons are assigned to the oxygen. The number to the right of each compound is the number of electrons &quot;owned&quot; by the red carbon, a rough expression of the oxidation state of that carbon. As the red carbon undergoes oxidation (loses electrons), the number gets smaller. Thus the oxidation state increases from top to bottom of the list.
FIGURE 13-24 NAD and NADP. (a) Nicotinamide adenine dinucleotide, NAD+, and its phosphorylated analog NADP+ undergo reduction to NADH and NADPH, accepting a hydride ion (two electrons and one proton) from an oxidizable substrate. The hydride ion is added to either the front (the A side) or the back (the B side) of the planar nicotinamide ring (see Table 13-8). (b) The UV absorption spectra of NAD+ and NADH. Reduction of the nicotinamide ring produces a new, broad absorption band with a maximum at 340 nm. The production of NADH during an enzyme-catalyzed reaction can be conveniently followed by observing the appearance of the absorbance at 340 nm (molar extinction coefficient ε340 = 6,200 M–1cm–1).
FIGURE 13-27 Oxidized and reduced FAD and FMN. FMN consists of the structure above the dashed line on the FAD (oxidized form). The flavin nucleotides accept two hydrogen atoms (two electrons and two protons), both of which appear in the flavin ring system. When FAD or FMN accepts only one hydrogen atom, the semiquinone, a stable free radical, forms.