Sir Cyril Hinshelwood and Nikolaevich received the 1956 Nobel Prize in Chemistry for their research on chemical reaction mechanisms. Hinshelwood modified Lindemann's explanation for unimolecular reactions by proposing that energized molecules (A*) may store energy in various molecular bonds and vibrational degrees of freedom, rather than immediately reacting. This statistical distribution of energy among s degrees of freedom leads to a modified rate constant expression containing an additional term of 1/(s-1) that can account for much higher observed reaction rates. However, Hinshelwood's theory does not fully explain some experimental observations such as the temperature dependence of rate constants and nonlinear plots of 1/k1 versus concentration.
This document discusses ligand substitution reactions in octahedral complexes. It describes the main mechanisms of ligand substitution including dissociative (SN1), associative (SN2), and concerted (interchange) pathways. It also discusses hydrolysis reactions and anation reactions as types of ligand substitutions. Specific examples are provided of acid and base hydrolysis in octahedral cobalt complexes, and factors that influence the reaction mechanisms and rates are outlined.
The Lindemann-Hinshelwood mechanism explains how first-order unimolecular gas-phase reactions can occur through collisions. It proposes that: (1) A reactant molecule A becomes energized through a collision with another A molecule, forming the excited species A*. (2) A* then either loses its excess energy through another collision or undergoes unimolecular decay to form products P. (3) If the unimolecular decay is the slowest step, the overall reaction appears first-order. The mechanism predicts a transition to second-order kinetics at low pressures when bimolecular collisions become rate-determining.
The document discusses various factors that affect the stability of metal complexes. It explains that complexes formed with ligands having higher charge and smaller size are generally more stable. It also discusses the Irving-Williams order of stability and the factors of charge to radius ratio, electronegativity, and basicity of ligands. The chelate effect is described as an important ligand effect where multidentate ligands form more stable complexes due to entropy gains. Kinetic and thermodynamic stability are distinguished from reactivity concepts of labile and inert complexes.
The document discusses charge transfer complexes and the different types of charge transfer that can cause color in transition metal complexes. It explains that ligand to metal charge transfer and metal to ligand charge transfer can produce color when pi donor or accepting ligands are present with metals lacking or having low oxidation state d-electrons, respectively. As an example, it describes the metal to ligand charge transfer observed in the spectra of the tris(bipyridine)ruthenium(II) dichloride complex.
This document discusses the trans effect phenomenon in square planar metal complexes. It defines the trans effect as the tendency of a coordinated group to direct an incoming ligand to occupy the position trans to that group. This effect is explained by both the polarization and pi bonding theories. The document also provides examples of how the trans effect principle is applied in the synthesis of various platinum complexes to selectively form the cis or trans isomers.
Sir Cyril Hinshelwood and Nikolaevich received the 1956 Nobel Prize in Chemistry for their research on chemical reaction mechanisms. Hinshelwood modified Lindemann's explanation for unimolecular reactions by proposing that energized molecules (A*) may store energy in various molecular bonds and vibrational degrees of freedom, rather than immediately reacting. This statistical distribution of energy among s degrees of freedom leads to a modified rate constant expression containing an additional term of 1/(s-1) that can account for much higher observed reaction rates. However, Hinshelwood's theory does not fully explain some experimental observations such as the temperature dependence of rate constants and nonlinear plots of 1/k1 versus concentration.
This document discusses ligand substitution reactions in octahedral complexes. It describes the main mechanisms of ligand substitution including dissociative (SN1), associative (SN2), and concerted (interchange) pathways. It also discusses hydrolysis reactions and anation reactions as types of ligand substitutions. Specific examples are provided of acid and base hydrolysis in octahedral cobalt complexes, and factors that influence the reaction mechanisms and rates are outlined.
The Lindemann-Hinshelwood mechanism explains how first-order unimolecular gas-phase reactions can occur through collisions. It proposes that: (1) A reactant molecule A becomes energized through a collision with another A molecule, forming the excited species A*. (2) A* then either loses its excess energy through another collision or undergoes unimolecular decay to form products P. (3) If the unimolecular decay is the slowest step, the overall reaction appears first-order. The mechanism predicts a transition to second-order kinetics at low pressures when bimolecular collisions become rate-determining.
The document discusses various factors that affect the stability of metal complexes. It explains that complexes formed with ligands having higher charge and smaller size are generally more stable. It also discusses the Irving-Williams order of stability and the factors of charge to radius ratio, electronegativity, and basicity of ligands. The chelate effect is described as an important ligand effect where multidentate ligands form more stable complexes due to entropy gains. Kinetic and thermodynamic stability are distinguished from reactivity concepts of labile and inert complexes.
The document discusses charge transfer complexes and the different types of charge transfer that can cause color in transition metal complexes. It explains that ligand to metal charge transfer and metal to ligand charge transfer can produce color when pi donor or accepting ligands are present with metals lacking or having low oxidation state d-electrons, respectively. As an example, it describes the metal to ligand charge transfer observed in the spectra of the tris(bipyridine)ruthenium(II) dichloride complex.
This document discusses the trans effect phenomenon in square planar metal complexes. It defines the trans effect as the tendency of a coordinated group to direct an incoming ligand to occupy the position trans to that group. This effect is explained by both the polarization and pi bonding theories. The document also provides examples of how the trans effect principle is applied in the synthesis of various platinum complexes to selectively form the cis or trans isomers.
This document presents information on the Tanabe-Sugano diagram, which is used in coordination chemistry to predict absorptions in the UV-visible and IR spectra of coordination compounds. It was developed by Yukito Tanabe and Satoru Sugano in 1954 to explain the absorption spectra of octahedral complex ions. The diagram plots orbital energy as a function of the Racah parameter B versus the ligand field splitting parameter Δo/B. It can be used to determine the ordering of electronic states and predict possible electronic transitions based on parameters like Δo, Racah parameters B and C, symmetry rules, and term symbols of electronic configurations. The diagram has advantages over earlier Orgel diagrams in that it can be applied to
The document discusses the Linear Free Energy Relationship known as the Hammett Equation. It describes how the Hammett Equation can be used to investigate organic reaction mechanisms by studying the effects of substituents on reaction rates. The key aspects are:
1) The Hammett Equation relates the logarithm of reaction rates or equilibrium constants to substituent constants (σ) using the reaction constant (ρ).
2) σ values describe electronic properties of substituents, with electron-withdrawing groups having positive σ and electron-donating groups having negative σ.
3) ρ indicates how sensitive a reaction is to substituents, relating the electronic demand of the reaction transition state. Its sign and magnitude provide insight into
1. The von Richter reaction involves reacting aromatic nitro compounds with potassium cyanide, which results in the displacement of the nitro group and addition of a carboxyl group in the ortho position through cine substitution.
2. The reaction mechanism eluded chemists for almost 100 years before the currently accepted one was proposed.
3. This reaction is an example of cine aromatic nucleophilic substitution where the nitro group is replaced by a carboxylic group, which is always in the ortho position. However, the reaction has limited application and poor yields.
The document discusses the trans effect in inorganic chemistry. It defines the trans effect as the effect of a ligand trans to the leaving ligand on the rate of substitution reactions in square planar complexes. It presents the trans effect series and explains that ligands at the low end of the series are more polarizable while those at the high end are better π-acceptors. The document also summarizes the polarization theory and π-bonding theory that have been proposed to explain the trans effect. It concludes by noting that the trans effect depends on both the π-bonding ability and polarizability of ligands.
1) 1,3-Dithiane is a heterocyclic disulfide compound that is prepared through the reaction of dithiols with carbonyl compounds.
2) It has many synthetic applications and is used to synthesize ketones, aldehydes, and cyclic ketones through reactions such as addition of organolithium reagents to the dithiane ring.
3) Specifically, the document discusses how lithiated 1,3-dithiane can react with alkyl halides, aryl halides, alkyl dihalides, aldehydes and ketones to form substituted dithiane derivatives that can then be hydrolyzed to form various ketones and aldehydes.
Dioxygen complexes, dioxygen as ligand Geeta Tewari
This presentation describes about the preparation, properties, bonding modes, classification and applications of metal Dinitrogen Complexes. Also explains the MO diagram of molecular nitrogen.
Definition - Mechanism - Effect of dielectric constant on the rate of reactions in solutions - Salt effect - Primary salt effect - Bronsted – Bjerrum equation - Secondary salt effect - Effect of pressure on rate of reaction in solution - Volume of activation - Significance
1. The trans effect refers to the observation that certain ligands increase the rate of ligand substitution when positioned trans to the departing ligand.
2. This effect was first discovered in 1926 when studying platinum complexes, where it was found that ammonia preferentially substituted the chloride ligand cis rather than trans to the nitrite ligand in Pt(NO2)Cl3 complexes.
3. Two main theories have been proposed to explain the trans effect - the polarization theory involving electrostatic weakening of the trans metal-ligand bond, and the pi-bonding theory involving back-donation of electron density from the metal into the pi* orbitals of ligands like NO2 weakening the trans bond.
This document discusses theories of unimolecular reaction kinetics, including the Lindemann-Christiansen theory, Hinshelwood theory, RRK theory, and RRKM theory. It notes limitations of earlier theories in explaining experimental data. The RRKM theory, developed by Marcus in 1951-1952, redefined the RRK treatment and addressed prior limitations. RRKM theory is now widely used to interpret thermal and photochemical reactions and allows calculating reaction rates from known vibrational frequencies of molecules.
The Lindemann theory provides an explanation for unimolecular gas-phase reactions. It proposes that:
1) A molecule A acquires sufficient vibrational energy from collisions with other A molecules to form an energized molecule A*.
2) A* can then either lose its energy and revert to A, or it can decompose or isomerize in a subsequent reaction.
3) This process leads to first-order kinetics for the overall reaction rate, consistent with experimental observations of unimolecular reactions.
However, the Lindemann theory has some limitations, as the predicted rate constant versus concentration relationship is hyperbolic rather than linear as observed experimentally. More advanced theories like RRK and Slater were developed to
IR spectroscopy . P.K.Mani, BCKV, West Bengal, IndiaP.K. Mani
This document provides an introduction to infrared (IR) spectroscopy, including:
1. IR spectra originate from the vibrational and rotational motions of molecules, which can absorb IR radiation if there is a change in dipole moment.
2. Molecules absorb specific frequencies that correspond to their natural vibrational frequencies. Stretching and bending vibrations within different functional groups absorb in characteristic regions of the IR spectrum.
3. IR spectroscopy can be used to identify molecules based on their absorption fingerprints between 400-1300 cm-1, which are influenced by the whole molecular structure.
Part 2, Substitution reactions in square planar complexes, Factors.pptxGeeta Tewari
Dr. Geeta Tewari discusses factors that affect the rates of substitution reactions in square planar complexes.
(1) The nature of the entering and leaving ligands impacts the rate, with more polarizable and soft ligands being better nucleophiles for Pt(II) complexes, and the leaving group bond strength determining the rate.
(2) Steric effects of non-leaving ligands can slow the rate, as bulky ligands create hindrance.
(3) For associative mechanisms common in square planar complexes, the charge on the metal center does not impact the rate.
Theories of coordination compounds, CFSE, Bonding in octahedral and tetrahedral complex, color of transition metal complex, magnetic properties, selection rules, Nephelxeuatic effect, angular overlap model
The document summarizes the dienone-phenol rearrangement, which is the acid- or base-catalyzed migration of alkyl groups in cyclohexadienones, resulting in highly substituted phenols. It was first described in 1893 for the rearrangement of santonin to desmotroposantonin under acidic conditions, but was more fully characterized in 1930. The rearrangement requires only moderately strong acids and is exothermic. It proceeds by a [1,3] sigmatropic migration of C-C bonds, which actually occurs through two subsequent [1,2] alkyl shifts. Depending on the migrating group, other rearrangements such as [1,2], [1,3], [
This document summarizes aromatic nucleophilic substitution reactions. It discusses the SNAr, SN1, and benzyne mechanisms. For SNAr, a strong withdrawing group is needed for reactivity. SN1 is rare for aromatics. In the benzyne mechanism, elimination of H forms benzyne which then adds the nucleophile, producing either ortho or para substituted products. Radiocarbon labeling is used to identify the products. In summary, the document outlines different aromatic nucleophilic substitution reaction mechanisms and factors affecting their reactivity.
The coupling constant is the distance between peaks in a multiplet in NMR spectroscopy. It is measured in Hertz and does not depend on external magnetic field strength. The value of the coupling constant provides information to distinguish multiplets and can indicate structural features like cis/trans isomers. Coupling occurs between protons close in space, known as geminal, vicinal, and sometimes long-range coupling over several bonds. The coupling constant is affected by factors like bond angle, dihedral angle, and electronegativity of substituents.
This document summarizes the aromatic nucleophilic substitution (SNAr) reaction mechanism. It involves the formation of a carbanion intermediate called the Meisenheimer intermediate through an addition-elimination process. Aryl halides are relatively unreactive toward nucleophilic substitution, but reactivity increases in the presence of electron-withdrawing groups due to stabilization of the carbanion. Under highly forcing conditions, aryl halides can undergo substitution through a benzyne intermediate that has been trapped using Diels-Alder reactions.
The Paternò-Büchi reaction involves the photochemical reaction between a carbonyl compound and an alkene to form an oxetane ring. This reaction was first reported in 1909 by Paternò and Chieffi. Several mechanisms are possible, including those involving a diradical intermediate or photoinduced electron transfer. The reaction shows regioselectivity, site selectivity, and stereoselectivity that depend on factors such as the solvent, substituents on the carbonyl compound or alkene, and temperature. The Paternò-Büchi reaction has been used to synthesize various natural products and allows formation of oxetane rings, which are present in several biologically active compounds.
Pyrolytic elimination reactions involve the application of heat to induce an elimination reaction in an organic substrate without the need for an external base or solvent. This type of elimination proceeds through a concerted, syn-elimination via a cyclic transition state that allows for an intramolecular proton transfer and the formation of a new carbon-carbon double bond. Specific examples of pyrolytic eliminations discussed in the document include the conversion of esters to carboxylic acids and alkenes, eliminations in alicyclic systems, Cope eliminations, sulfoxide eliminations, xanthate pyrolysis, and selenoxide eliminations.
CHAPTER 6- CHEMICAL REACTIAN EQUILIBRIA.PPTDelight26
This chapter discusses chemical reaction equilibria, focusing on how temperature, pressure, and initial composition affect the equilibrium conversions of chemical reactions. It introduces the reaction coordinate, which characterizes the extent of a reaction, and explains how the numbers of moles and mole fractions of reaction species relate to the coordinate. It also covers the equilibrium constant K, how it depends on temperature based on the standard Gibbs energy change, and how to evaluate K values from thermodynamic data.
Chemical equilibrium is a state where the rates of the forward and reverse reactions are equal and the concentrations of reactants and products remain constant. Equilibrium is achieved when these conditions are met. The equilibrium constant, K, provides a quantitative measure of the position of equilibrium and can be expressed in terms of concentrations or pressures depending on whether the reaction involves gases or solutions. Factors such as concentration, pressure, temperature, and catalysis can influence the position of equilibrium based on Le Chatelier's principle.
This document presents information on the Tanabe-Sugano diagram, which is used in coordination chemistry to predict absorptions in the UV-visible and IR spectra of coordination compounds. It was developed by Yukito Tanabe and Satoru Sugano in 1954 to explain the absorption spectra of octahedral complex ions. The diagram plots orbital energy as a function of the Racah parameter B versus the ligand field splitting parameter Δo/B. It can be used to determine the ordering of electronic states and predict possible electronic transitions based on parameters like Δo, Racah parameters B and C, symmetry rules, and term symbols of electronic configurations. The diagram has advantages over earlier Orgel diagrams in that it can be applied to
The document discusses the Linear Free Energy Relationship known as the Hammett Equation. It describes how the Hammett Equation can be used to investigate organic reaction mechanisms by studying the effects of substituents on reaction rates. The key aspects are:
1) The Hammett Equation relates the logarithm of reaction rates or equilibrium constants to substituent constants (σ) using the reaction constant (ρ).
2) σ values describe electronic properties of substituents, with electron-withdrawing groups having positive σ and electron-donating groups having negative σ.
3) ρ indicates how sensitive a reaction is to substituents, relating the electronic demand of the reaction transition state. Its sign and magnitude provide insight into
1. The von Richter reaction involves reacting aromatic nitro compounds with potassium cyanide, which results in the displacement of the nitro group and addition of a carboxyl group in the ortho position through cine substitution.
2. The reaction mechanism eluded chemists for almost 100 years before the currently accepted one was proposed.
3. This reaction is an example of cine aromatic nucleophilic substitution where the nitro group is replaced by a carboxylic group, which is always in the ortho position. However, the reaction has limited application and poor yields.
The document discusses the trans effect in inorganic chemistry. It defines the trans effect as the effect of a ligand trans to the leaving ligand on the rate of substitution reactions in square planar complexes. It presents the trans effect series and explains that ligands at the low end of the series are more polarizable while those at the high end are better π-acceptors. The document also summarizes the polarization theory and π-bonding theory that have been proposed to explain the trans effect. It concludes by noting that the trans effect depends on both the π-bonding ability and polarizability of ligands.
1) 1,3-Dithiane is a heterocyclic disulfide compound that is prepared through the reaction of dithiols with carbonyl compounds.
2) It has many synthetic applications and is used to synthesize ketones, aldehydes, and cyclic ketones through reactions such as addition of organolithium reagents to the dithiane ring.
3) Specifically, the document discusses how lithiated 1,3-dithiane can react with alkyl halides, aryl halides, alkyl dihalides, aldehydes and ketones to form substituted dithiane derivatives that can then be hydrolyzed to form various ketones and aldehydes.
Dioxygen complexes, dioxygen as ligand Geeta Tewari
This presentation describes about the preparation, properties, bonding modes, classification and applications of metal Dinitrogen Complexes. Also explains the MO diagram of molecular nitrogen.
Definition - Mechanism - Effect of dielectric constant on the rate of reactions in solutions - Salt effect - Primary salt effect - Bronsted – Bjerrum equation - Secondary salt effect - Effect of pressure on rate of reaction in solution - Volume of activation - Significance
1. The trans effect refers to the observation that certain ligands increase the rate of ligand substitution when positioned trans to the departing ligand.
2. This effect was first discovered in 1926 when studying platinum complexes, where it was found that ammonia preferentially substituted the chloride ligand cis rather than trans to the nitrite ligand in Pt(NO2)Cl3 complexes.
3. Two main theories have been proposed to explain the trans effect - the polarization theory involving electrostatic weakening of the trans metal-ligand bond, and the pi-bonding theory involving back-donation of electron density from the metal into the pi* orbitals of ligands like NO2 weakening the trans bond.
This document discusses theories of unimolecular reaction kinetics, including the Lindemann-Christiansen theory, Hinshelwood theory, RRK theory, and RRKM theory. It notes limitations of earlier theories in explaining experimental data. The RRKM theory, developed by Marcus in 1951-1952, redefined the RRK treatment and addressed prior limitations. RRKM theory is now widely used to interpret thermal and photochemical reactions and allows calculating reaction rates from known vibrational frequencies of molecules.
The Lindemann theory provides an explanation for unimolecular gas-phase reactions. It proposes that:
1) A molecule A acquires sufficient vibrational energy from collisions with other A molecules to form an energized molecule A*.
2) A* can then either lose its energy and revert to A, or it can decompose or isomerize in a subsequent reaction.
3) This process leads to first-order kinetics for the overall reaction rate, consistent with experimental observations of unimolecular reactions.
However, the Lindemann theory has some limitations, as the predicted rate constant versus concentration relationship is hyperbolic rather than linear as observed experimentally. More advanced theories like RRK and Slater were developed to
IR spectroscopy . P.K.Mani, BCKV, West Bengal, IndiaP.K. Mani
This document provides an introduction to infrared (IR) spectroscopy, including:
1. IR spectra originate from the vibrational and rotational motions of molecules, which can absorb IR radiation if there is a change in dipole moment.
2. Molecules absorb specific frequencies that correspond to their natural vibrational frequencies. Stretching and bending vibrations within different functional groups absorb in characteristic regions of the IR spectrum.
3. IR spectroscopy can be used to identify molecules based on their absorption fingerprints between 400-1300 cm-1, which are influenced by the whole molecular structure.
Part 2, Substitution reactions in square planar complexes, Factors.pptxGeeta Tewari
Dr. Geeta Tewari discusses factors that affect the rates of substitution reactions in square planar complexes.
(1) The nature of the entering and leaving ligands impacts the rate, with more polarizable and soft ligands being better nucleophiles for Pt(II) complexes, and the leaving group bond strength determining the rate.
(2) Steric effects of non-leaving ligands can slow the rate, as bulky ligands create hindrance.
(3) For associative mechanisms common in square planar complexes, the charge on the metal center does not impact the rate.
Theories of coordination compounds, CFSE, Bonding in octahedral and tetrahedral complex, color of transition metal complex, magnetic properties, selection rules, Nephelxeuatic effect, angular overlap model
The document summarizes the dienone-phenol rearrangement, which is the acid- or base-catalyzed migration of alkyl groups in cyclohexadienones, resulting in highly substituted phenols. It was first described in 1893 for the rearrangement of santonin to desmotroposantonin under acidic conditions, but was more fully characterized in 1930. The rearrangement requires only moderately strong acids and is exothermic. It proceeds by a [1,3] sigmatropic migration of C-C bonds, which actually occurs through two subsequent [1,2] alkyl shifts. Depending on the migrating group, other rearrangements such as [1,2], [1,3], [
This document summarizes aromatic nucleophilic substitution reactions. It discusses the SNAr, SN1, and benzyne mechanisms. For SNAr, a strong withdrawing group is needed for reactivity. SN1 is rare for aromatics. In the benzyne mechanism, elimination of H forms benzyne which then adds the nucleophile, producing either ortho or para substituted products. Radiocarbon labeling is used to identify the products. In summary, the document outlines different aromatic nucleophilic substitution reaction mechanisms and factors affecting their reactivity.
The coupling constant is the distance between peaks in a multiplet in NMR spectroscopy. It is measured in Hertz and does not depend on external magnetic field strength. The value of the coupling constant provides information to distinguish multiplets and can indicate structural features like cis/trans isomers. Coupling occurs between protons close in space, known as geminal, vicinal, and sometimes long-range coupling over several bonds. The coupling constant is affected by factors like bond angle, dihedral angle, and electronegativity of substituents.
This document summarizes the aromatic nucleophilic substitution (SNAr) reaction mechanism. It involves the formation of a carbanion intermediate called the Meisenheimer intermediate through an addition-elimination process. Aryl halides are relatively unreactive toward nucleophilic substitution, but reactivity increases in the presence of electron-withdrawing groups due to stabilization of the carbanion. Under highly forcing conditions, aryl halides can undergo substitution through a benzyne intermediate that has been trapped using Diels-Alder reactions.
The Paternò-Büchi reaction involves the photochemical reaction between a carbonyl compound and an alkene to form an oxetane ring. This reaction was first reported in 1909 by Paternò and Chieffi. Several mechanisms are possible, including those involving a diradical intermediate or photoinduced electron transfer. The reaction shows regioselectivity, site selectivity, and stereoselectivity that depend on factors such as the solvent, substituents on the carbonyl compound or alkene, and temperature. The Paternò-Büchi reaction has been used to synthesize various natural products and allows formation of oxetane rings, which are present in several biologically active compounds.
Pyrolytic elimination reactions involve the application of heat to induce an elimination reaction in an organic substrate without the need for an external base or solvent. This type of elimination proceeds through a concerted, syn-elimination via a cyclic transition state that allows for an intramolecular proton transfer and the formation of a new carbon-carbon double bond. Specific examples of pyrolytic eliminations discussed in the document include the conversion of esters to carboxylic acids and alkenes, eliminations in alicyclic systems, Cope eliminations, sulfoxide eliminations, xanthate pyrolysis, and selenoxide eliminations.
CHAPTER 6- CHEMICAL REACTIAN EQUILIBRIA.PPTDelight26
This chapter discusses chemical reaction equilibria, focusing on how temperature, pressure, and initial composition affect the equilibrium conversions of chemical reactions. It introduces the reaction coordinate, which characterizes the extent of a reaction, and explains how the numbers of moles and mole fractions of reaction species relate to the coordinate. It also covers the equilibrium constant K, how it depends on temperature based on the standard Gibbs energy change, and how to evaluate K values from thermodynamic data.
Chemical equilibrium is a state where the rates of the forward and reverse reactions are equal and the concentrations of reactants and products remain constant. Equilibrium is achieved when these conditions are met. The equilibrium constant, K, provides a quantitative measure of the position of equilibrium and can be expressed in terms of concentrations or pressures depending on whether the reaction involves gases or solutions. Factors such as concentration, pressure, temperature, and catalysis can influence the position of equilibrium based on Le Chatelier's principle.
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.
This document discusses chemical equilibrium. It defines irreversible and reversible reactions, and explains that reversible reactions can proceed in both the forward and backward directions and never reach completion. It also defines the state of equilibrium as when the rates of the forward and reverse reactions are equal and concentrations remain constant. The document then discusses the law of mass action and how it relates to the rate and equilibrium constants (Kc and Kp). It provides examples to illustrate these concepts and relationships between Kc and Kp.
This document presents information about chain reactions. It begins with definitions of chain reactions and examples of stationary and non-stationary chain reactions. It then uses the reaction between hydrogen and bromine as a specific example of a chain reaction. It shows the initiation, propagation, inhibition, and termination steps of this reaction and derives rate equations based on the steady-state hypothesis. The final rate law equation indicates that the initial rate of formation of HBr is first order in hydrogen and half order in bromine.
This document discusses heat transfer via forced convection in pipes and ducts. It provides correlations to calculate heat transfer coefficients for laminar and turbulent flow in circular pipes, as well as the transition region. It also discusses forced convection in external flow over flat plates, cylinders, and spheres, providing correlations for calculating heat transfer coefficients in these situations. Several examples are provided to demonstrate the use of the correlations.
1. The document contains an unsolved chemistry practice test with 43 multiple choice questions and answers related to topics like atomic structure, chemical bonding, thermodynamics, kinetics and equilibrium.
2. The questions cover concepts such as Bohr model, de Broglie wavelength, Lewis structures, IUPAC naming, acid-base reactions, salt solubility, electrolysis, redox reactions, colligative properties, rate laws, free energy and entropy changes.
3. The document tests understanding of fundamental chemistry principles as well as the ability to apply these principles to solve quantitative problems.
1. The document contains an unsolved chemistry practice test with 43 multiple choice questions and answers related to topics like atomic structure, chemical bonding, thermodynamics, kinetics and equilibrium.
2. The questions cover concepts such as Bohr model, de Broglie wavelength, Lewis structures, IUPAC naming, acid-base reactions, salt solubility, electrochemistry and more.
3. The document provides the questions and answer options but does not include the correct answers. It is intended as a practice test for students or as a reference for teachers.
1. This document contains an unsolved chemistry exam paper from 2003 with 43 multiple choice questions covering topics like atomic structure, chemical bonding, thermodynamics, kinetics and equilibrium.
2. The questions test understanding of concepts like Bohr model, de Broglie wavelength, Lewis structures, IUPAC naming, acid-base reactions, salt solubility, electrolysis, redox reactions and more.
3. The document provides the questions and multiple choice answers but no solutions, making it a challenging practice exam for reviewing core chemistry topics.
This document contains a chemistry exam with multiple choice questions. It tests concepts related to redox reactions, gas laws, organic chemistry reactions, transition metals, acid-base chemistry, and more. There are 65 total questions with 4 possible answers for each question labeled A, B, C, or D. The questions cover a wide range of chemistry topics and concepts at an undergraduate level.
This document discusses oxidation-reduction (redox) reactions and electrochemistry.
1. It explains how to identify redox reactions by checking if the oxidation number (O.N.) of any species changes in the reaction. An example reaction between permanganate and oxalic acid is given.
2. Balancing redox reactions is important, and the document outlines the step-by-step process for balancing both acidic and basic redox reactions.
3. Electrochemical cells are described as either galvanic cells that generate potential or electrolytic cells that consume potential. The standard hydrogen electrode is used as a reference electrode with a standard potential of 0 V.
1. Mert's room was 20°F while Mort's room was -5°C. Converting to Celsius, Mert's room was -6.7°C, which is colder than Mort's room.
2. As a gas is compressed from point A to point B while keeping the temperature constant, the pressure of the gas increases according to the ideal gas law.
3. For an ideal gas, halving both the temperature and volume leaves the pressure constant.
The document provides notes on homework problems involving chemical equilibrium. It states that problems may use different pressure units and that negatives are possible. It also advises not rounding when doing online homework. Key concepts covered include reversible reactions reaching equilibrium when forward and reverse reaction rates are equal. The equilibrium constant K is defined using concentrations or pressures and describes the position of equilibrium. K is constant at a given temperature but the concentrations or pressures at equilibrium can vary.
1) The document discusses heat transfer by conduction through plane walls and cylindrical pipes. It presents the general heat conduction equations and derives the equations for the temperature distribution in plane walls and cylindrical pipes.
2) It also discusses heat transfer by convection and defines the overall heat transfer coefficient (U) for a plane wall subjected to convection on both sides. Expressions are developed for the surface temperatures and overall heat transfer coefficient.
3) An example problem is presented to calculate the surface temperatures and overall heat transfer coefficient for a plane wall subjected to a uniform heat flux on one side and convection on the other.
Basic chemistry in school for student to learnwidhyahrini1
The document discusses chemical equilibrium, including:
- Equilibrium is achieved when the rates of the forward and reverse reactions are equal and concentrations remain constant.
- The equilibrium constant, K, relates concentrations or pressures of reactants and products at equilibrium.
- Le Châtelier's principle states that if a stress is applied to a system at equilibrium, it will shift in a way to partially offset the stress and reestablish a new equilibrium.
This document contains 15 multiple choice questions related to thermodynamics and gases. Each question has 4 possible answer choices labeled A, B, C, or D. After each question is a "Solution" section that provides the reasoning for the correct answer(s). Some questions have a single correct answer, while others are marked as having multiple correct answers. The questions cover topics such as the Maxwell distribution of molecular speeds, the van der Waals equation of state, compressibility factors, and pressure-volume relationships for real gases.
Thermogravimetric analysis (TGA) was used to screen various metal (II) chlorides as potential destabilizing agents for solid-state hydrazine borane (N2H4BH3) for chemical hydrogen storage applications. TGA showed that: (1) Copper chloride (CuCl2) alone was not very effective at destabilizing hydrazine borane, while nickel chloride (NiCl2) greatly lowered the decomposition temperature when combined with CuCl2; (2) The combination of CuCl2 and NiCl2 caused hydrazine borane to decompose starting at 30°C with reduced gaseous byproducts, indicating it was one of the most effective destabil
1) The document discusses heat transfer through conduction and convection in a finned tube system. Heat is transferred from a hot liquid to fins through convection, and through the fins by conduction.
2) An analysis is presented for one-dimensional heat transfer through a fin into a surrounding fluid. Three cases are considered for different boundary conditions at the ends of the fin.
3) Expressions are derived for the temperature distribution and heat lost by the fin for each case. The heat lost can be calculated from the temperature distribution or from an energy balance at the fin.
Similar to Mechanism of the reaction between hydrogen and bromine (20)
The debris of the ‘last major merger’ is dynamically youngSérgio Sacani
The Milky Way’s (MW) inner stellar halo contains an [Fe/H]-rich component with highly eccentric orbits, often referred to as the
‘last major merger.’ Hypotheses for the origin of this component include Gaia-Sausage/Enceladus (GSE), where the progenitor
collided with the MW proto-disc 8–11 Gyr ago, and the Virgo Radial Merger (VRM), where the progenitor collided with the
MW disc within the last 3 Gyr. These two scenarios make different predictions about observable structure in local phase space,
because the morphology of debris depends on how long it has had to phase mix. The recently identified phase-space folds in Gaia
DR3 have positive caustic velocities, making them fundamentally different than the phase-mixed chevrons found in simulations
at late times. Roughly 20 per cent of the stars in the prograde local stellar halo are associated with the observed caustics. Based
on a simple phase-mixing model, the observed number of caustics are consistent with a merger that occurred 1–2 Gyr ago.
We also compare the observed phase-space distribution to FIRE-2 Latte simulations of GSE-like mergers, using a quantitative
measurement of phase mixing (2D causticality). The observed local phase-space distribution best matches the simulated data
1–2 Gyr after collision, and certainly not later than 3 Gyr. This is further evidence that the progenitor of the ‘last major merger’
did not collide with the MW proto-disc at early times, as is thought for the GSE, but instead collided with the MW disc within
the last few Gyr, consistent with the body of work surrounding the VRM.
PPT on Direct Seeded Rice presented at the three-day 'Training and Validation Workshop on Modules of Climate Smart Agriculture (CSA) Technologies in South Asia' workshop on April 22, 2024.
ESA/ACT Science Coffee: Diego Blas - Gravitational wave detection with orbita...Advanced-Concepts-Team
Presentation in the Science Coffee of the Advanced Concepts Team of the European Space Agency on the 07.06.2024.
Speaker: Diego Blas (IFAE/ICREA)
Title: Gravitational wave detection with orbital motion of Moon and artificial
Abstract:
In this talk I will describe some recent ideas to find gravitational waves from supermassive black holes or of primordial origin by studying their secular effect on the orbital motion of the Moon or satellites that are laser ranged.
Authoring a personal GPT for your research and practice: How we created the Q...Leonel Morgado
Thematic analysis in qualitative research is a time-consuming and systematic task, typically done using teams. Team members must ground their activities on common understandings of the major concepts underlying the thematic analysis, and define criteria for its development. However, conceptual misunderstandings, equivocations, and lack of adherence to criteria are challenges to the quality and speed of this process. Given the distributed and uncertain nature of this process, we wondered if the tasks in thematic analysis could be supported by readily available artificial intelligence chatbots. Our early efforts point to potential benefits: not just saving time in the coding process but better adherence to criteria and grounding, by increasing triangulation between humans and artificial intelligence. This tutorial will provide a description and demonstration of the process we followed, as two academic researchers, to develop a custom ChatGPT to assist with qualitative coding in the thematic data analysis process of immersive learning accounts in a survey of the academic literature: QUAL-E Immersive Learning Thematic Analysis Helper. In the hands-on time, participants will try out QUAL-E and develop their ideas for their own qualitative coding ChatGPT. Participants that have the paid ChatGPT Plus subscription can create a draft of their assistants. The organizers will provide course materials and slide deck that participants will be able to utilize to continue development of their custom GPT. The paid subscription to ChatGPT Plus is not required to participate in this workshop, just for trying out personal GPTs during it.
ESPP presentation to EU Waste Water Network, 4th June 2024 “EU policies driving nutrient removal and recycling
and the revised UWWTD (Urban Waste Water Treatment Directive)”
Describing and Interpreting an Immersive Learning Case with the Immersion Cub...Leonel Morgado
Current descriptions of immersive learning cases are often difficult or impossible to compare. This is due to a myriad of different options on what details to include, which aspects are relevant, and on the descriptive approaches employed. Also, these aspects often combine very specific details with more general guidelines or indicate intents and rationales without clarifying their implementation. In this paper we provide a method to describe immersive learning cases that is structured to enable comparisons, yet flexible enough to allow researchers and practitioners to decide which aspects to include. This method leverages a taxonomy that classifies educational aspects at three levels (uses, practices, and strategies) and then utilizes two frameworks, the Immersive Learning Brain and the Immersion Cube, to enable a structured description and interpretation of immersive learning cases. The method is then demonstrated on a published immersive learning case on training for wind turbine maintenance using virtual reality. Applying the method results in a structured artifact, the Immersive Learning Case Sheet, that tags the case with its proximal uses, practices, and strategies, and refines the free text case description to ensure that matching details are included. This contribution is thus a case description method in support of future comparative research of immersive learning cases. We then discuss how the resulting description and interpretation can be leveraged to change immersion learning cases, by enriching them (considering low-effort changes or additions) or innovating (exploring more challenging avenues of transformation). The method holds significant promise to support better-grounded research in immersive learning.
2. • Mechanism is comparatively simple.
• The results could be fitted into the following expression for the
rate of consumption of H2 and Br2
• m and k are constants; m value is about 10 and is independent
of temperature .
1
1
2
2
1
22
Brm
HBr
BrHk
vt
4. Applying the steady state hypothesis for H is :
For Br:
When you add these equations:
2022322 HBrHkBrHkHBrk
dt
Hd
30
2
12232221 BrkHBrHkBrHkBrHkBrk
dt
Brd
0
2
121 BrkBrk
42
1
2
2
1
1
1
Br
k
k
Br
30
2
12232221 BrkHBrHkBrHkBrHkBrk
dt
Brd
5. (4) Gives the equilibrium concentration of Br atoms.
An expression for [H] can be obtained by inserting this
expression for [Br] into (2) or(3). Inserting into (2) becomes,
So that
502232
2
1
2
2
1
1
1
2
HBrHkBrHkHBr
k
k
k
6
223
2
1
22
2
1
1
1
2
HBrkBrk
BrH
k
kk
H
6. The rate of reaction is the rate of consumption of H2, which is ,
Subtraction of eqn. (2) gives,
Insertion of the expression for [H] gives,
7222 HBrHkHBrkvt
823 BrHkvt
9
223
2
3
22
2
1
1
1
32
HBrkBrk
BrH
k
k
kk
vt
7. Also given by,
This is of the same form as the empirical equation (1) where k is
equal to k2(k1/k-1)½ and m = k3/k-2
10
/1 2
3
2
5.0
22
2
1
1
1
2
BrHBr
k
k
BrH
k
kk
vt
8. All the constants k1,k2,k3,k-2 and k-1 have been evaluated.
k which is experimental , together with k1/k-1 leads to k2.
From the temperature of k2 dependence E2 can be obtained
Reaction -2 is the reverse of reaction 2, so that from the
equilibrium constant k2/k-2 and from thermochemistry for the
reaction, k-2 and E-2 can be obtained.
The values of k3 and E3 can be found from the value of m: since
this is temperature independent, E3 is equal to E-2.
The values of k1 and k-1 were obtained by comparing the thermal
and photochemical reactions of H2-Br2
9. It was found that the photochemical reaction proceeds
according to the equation:
K’, m’ are constants and I is the intensity of light absorbed.
Similarity with (1) shows that mechanisms are similar.
Difference being that initiation reaction in the photochemical
reaction is absorption of a photon by a bromine molecule.
11
'
1
'
2
2
1
2
Brm
HBr
IHk
vp
BrhBr 22
10. This process is followed by the same four reactions as in the
thermal reaction. The steady state equation for bromine atoms
is now,
Eqn (2) is still the steady state equation for H, and addition of eqns
2 and 12 gives,
Or,
1202
2
122322 BrkHBrHkBrHkBrHkI
dt
Brd
)13(02
2
1 BrkI
14
2 2
1
1
k
I
Br
11. The rate equation is obtained from (10) by replacing k1[Br2] with 2I
Which is in agreement with eqn. 11.
15
/1
2
2
3
2
2
1
2
2
1
1
2
BrHBr
k
k
IH
k
k
vp
12. SOME FEATURES ABOUT THE REACTION:
Br. atom concentration in the thermal
reaction is the same with or without the
presence of hydrogen. (why ?)
Change in nature of surface or its area
cannot affect the rate of reaction.(why ?)
Presence of third bodies has no effect.
nterminatio21
21
2
2
MBrMBr
InitiationMBrMBr
13. It follows from 10 and 15 that the ratio of the photochemical and
thermal rates is
At the same concentrations of H2 and Br2. Therefore if vp/vt is
measured at known values of I and [Br2] , the rate k1 can be
obtained.
If the experiments are repeated at different temperatures, the
parameters A1 and E1 are obtained.
16
2
2
2
12
1
1
Br
I
kv
v
t
p
14. # Using the activation energies estimate the overall activation
energy of thermal hydrogen-bromine reaction under the
following conditions
a. At the beginning of the reaction
b. In the presence of large excess of HBr.
Also estimate the overall activation energy for the photochemical
reaction under the same conditions.
0
5
5
72
192
nterminatio21
2
3
2
21
2
2
2
2
2
BrBr
BrHHBrH
npropagatiochain
BrHBrBrH
HHBrHBr
InitiationBrBr
Editor's Notes
The presence of third bodies which may accelerate the formation of atoms cannot affect their concentration.