Enthalpy change
•Download as PPTX, PDF•
2 likes•948 views
This document summarizes different types of enthalpy changes in chemical reactions. It defines exothermic reactions as releasing energy to the surroundings and endothermic reactions as absorbing energy from the surroundings. Enthalpy change is the energy exchange between a reaction and its surroundings at constant pressure. The document explains how to calculate enthalpy change and represents reaction pathways using enthalpy profile diagrams to show enthalpy changes for exothermic and endothermic reactions. It also defines standard enthalpy changes of combustion, neutralization, solution, and hydration of salts.
Report
Share
Report
Share
Recommended
Chemical Equilibrium
The document discusses chemical equilibrium, including:
- When equilibrium is reached, concentrations of reactants and products remain constant, with the forward and reverse reaction rates being equal.
- Le Chatelier's principle states that applying stress (changing temperature, concentration, volume, or pressure) causes a system at equilibrium to shift in a way that reduces the stress.
- For example, increasing temperature shifts exothermic reactions toward reactants and endothermic reactions toward products.
Properties of solutions
1) Solutions are homogeneous mixtures of two or more substances, where the solute is dispersed uniformly throughout the solvent.
2) For a solution to form, the intermolecular forces between solute and solvent particles must be strong enough to overcome those within the pure substances.
3) The energetics of dissolving involves breaking interactions within the pure substances and forming new interactions between solute and solvent particles. Even endothermic processes can occur spontaneously if they increase the disorder or entropy of the system.
Chemical energetic
Exothermic and endothermic reaction, energy level diagram, bond energy and calculatution of enthalpy change of reaction.
Oxidation & reduction
The document discusses redox reactions, including definitions of oxidation, reduction, oxidizing agents and reducing agents. It provides examples of redox reactions like magnesium burning in oxygen, bromine water oxidizing iron(II) ions, and the displacement of metals in salt solutions. It also describes how electrons are transferred during redox reactions and how redox reactions can occur at a distance using a salt bridge.
Concentration units
This document discusses various units used to express the concentration of solutions, including mass percent, molarity, molality, mole fraction, and parts per million/billion/trillion. It provides definitions and examples of calculating each type of concentration unit. Various concentration units can be interconverted, as demonstrated through examples solving for molarity, mass percent, and mole fraction in different solutions. Dilution of solutions is also discussed, with an example of calculating molarity after mixing a more concentrated solution with water.
05c reversible reactions
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.
analytical chemistry: introduction
This document provides an introduction and overview of analytical chemistry concepts:
- Analytical chemistry involves separating, identifying, and determining the relative amounts of compounds in a sample. It has two main parts: qualitative analysis to identify what is present, and quantitative analysis to determine how much is present.
- Important units of measurement in analytical chemistry include grams, milligrams, microliters, and the mole. A mole represents 6.02x1023 units of a substance and is used to relate amounts of substances.
- Calculations involving moles and millimoles allow determining the amount of a substance in a sample based on its mass, molar mass, and the chemical formula. Factor-label and dimensional analysis
Enthalpy
Enthalpy is a thermodynamic quantity equivalent to the total heat content of a system. Enthalpy changes (ΔH) can be exothermic or endothermic. Exothermic reactions release energy to surroundings while endothermic reactions absorb energy from surroundings. Standard enthalpy changes are used to compare reactions under standard conditions of temperature, pressure and states. Examples of standard enthalpy changes include formation, combustion, neutralization, atomization, solution, and hydration. These changes can be determined experimentally by measuring the temperature change of a reaction.
Recommended
Chemical Equilibrium
The document discusses chemical equilibrium, including:
- When equilibrium is reached, concentrations of reactants and products remain constant, with the forward and reverse reaction rates being equal.
- Le Chatelier's principle states that applying stress (changing temperature, concentration, volume, or pressure) causes a system at equilibrium to shift in a way that reduces the stress.
- For example, increasing temperature shifts exothermic reactions toward reactants and endothermic reactions toward products.
Properties of solutions
1) Solutions are homogeneous mixtures of two or more substances, where the solute is dispersed uniformly throughout the solvent.
2) For a solution to form, the intermolecular forces between solute and solvent particles must be strong enough to overcome those within the pure substances.
3) The energetics of dissolving involves breaking interactions within the pure substances and forming new interactions between solute and solvent particles. Even endothermic processes can occur spontaneously if they increase the disorder or entropy of the system.
Chemical energetic
Exothermic and endothermic reaction, energy level diagram, bond energy and calculatution of enthalpy change of reaction.
Oxidation & reduction
The document discusses redox reactions, including definitions of oxidation, reduction, oxidizing agents and reducing agents. It provides examples of redox reactions like magnesium burning in oxygen, bromine water oxidizing iron(II) ions, and the displacement of metals in salt solutions. It also describes how electrons are transferred during redox reactions and how redox reactions can occur at a distance using a salt bridge.
Concentration units
This document discusses various units used to express the concentration of solutions, including mass percent, molarity, molality, mole fraction, and parts per million/billion/trillion. It provides definitions and examples of calculating each type of concentration unit. Various concentration units can be interconverted, as demonstrated through examples solving for molarity, mass percent, and mole fraction in different solutions. Dilution of solutions is also discussed, with an example of calculating molarity after mixing a more concentrated solution with water.
05c reversible reactions
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.
analytical chemistry: introduction
This document provides an introduction and overview of analytical chemistry concepts:
- Analytical chemistry involves separating, identifying, and determining the relative amounts of compounds in a sample. It has two main parts: qualitative analysis to identify what is present, and quantitative analysis to determine how much is present.
- Important units of measurement in analytical chemistry include grams, milligrams, microliters, and the mole. A mole represents 6.02x1023 units of a substance and is used to relate amounts of substances.
- Calculations involving moles and millimoles allow determining the amount of a substance in a sample based on its mass, molar mass, and the chemical formula. Factor-label and dimensional analysis
Enthalpy
Enthalpy is a thermodynamic quantity equivalent to the total heat content of a system. Enthalpy changes (ΔH) can be exothermic or endothermic. Exothermic reactions release energy to surroundings while endothermic reactions absorb energy from surroundings. Standard enthalpy changes are used to compare reactions under standard conditions of temperature, pressure and states. Examples of standard enthalpy changes include formation, combustion, neutralization, atomization, solution, and hydration. These changes can be determined experimentally by measuring the temperature change of a reaction.
5.4 exothermic and endothermic reactions
This document discusses exothermic and endothermic reactions. Exothermic reactions release heat, while endothermic reactions absorb heat. Combustion reactions of hydrocarbons like methane and propane are exothermic, producing carbon dioxide, water vapor, and large amounts of heat. The heat of reaction, ΔH, indicates whether a reaction is exothermic (negative ΔH) or endothermic (positive ΔH). Bond energies represent the energy required to break bonds, while heat of combustion measures the heat released from complete combustion. A bomb calorimeter is used to accurately measure heats of combustion by igniting samples in excess oxygen. Hess's law states that the heat change of a reaction depends only on
Lecture-02.Classifications of Qualitative and Quantitative Analysis
https://www.youtube.com/watch?v=wObwXIt1ZQc&t=123s
Basic Concept of Analytical Chemistry
Meaning: The word analytical comes from the Ancient Greek ana- "up, and lysis "a loosening"). Collectively it means breaking-up" or "an untying.
Definition: The branch of chemistry which deals with the analysis of matter, its identification, and its components. Thus, the process of chemical analysis are of two type;
(1) Qualitative Analysis (2) Quantitative Analysis
Classifications of Analytical Techniques
There are two types of techniques
(1) Classical technique (2) Instrumental techniques
The classical techniques are qualitative as well as quantitative. The qualitative analysis is based on identifying and determining the analyte based on some properties specific to the analyte like boiling point, melting point, optical activities or refractive index, solubilities, and color. E.g., the Boling point of water is 100oC, the melting point of sugar is 186 °C, the refractive index of water is 1.333, test color of K is purple or the color of litmus. paper indicating the acidity or basicity of a compound. When sulphuretted hydrogen (H2S) is passed through a solution containing Arsenic, a yellowish precipitate is formed indicating the presence of arsenic. If the precipitate is brown, is brown, it indicates Tin.
The quantitative analysis is based on the quantity of the analyte. Like determining the volume of the analyte ( volumetric and gasometric analysis) and weight of the analyte (gravimetric analysis.
2) Instrumental methods can be both qualitative and quantitative. The qualitative analysis likewise relies on detecting and determining the analyte based on certain characteristics. Elements (C, H, N, S) of organic compounds using a CHNS analyzer, heavy metals using an atomic absorption spectrophotometer, and alkali and alkaline earth metals (K, Na, Ca, Mg) using a flame photometer. At the molecular level, infrared (IR) spectroscopy, Nuclear magnetic resonance (NMR) spectroscopy, mass spectrometry, and thin-layer chromatography are used to examine substances. These techniques tell us the nature of a compound. Some of these techniques can also be used for quantitative purposes as well.
Reference Books:
Skoog, D. A., West, P. M., Holler, F. J., Crouch, S. R., Fundamentals of Analytical Chemistry, 9th ed., Brooks Cole Publishing Company, (2013).
Christian, G. D., Analytical Chemistry. 6th ed., John-Wiley & Sons, New York, (2006).
Harris, D. C., Quantitative Chemical Analysis, 8th ed., W. H. Freeman and Company, New York, USA, (2011).
Bender, G.T. 1987. “Principles of Chemical Instrumentation” W.B. Saunders Co., London.
Reilley, C. 1993. Laboratory Manual of Analytical Chemistry. Allyn& Bacon, London.
Hargis, L.G. 1988. “Analytical Chemistry: Printice Hall Publishers, London.
Empirical and molecular formulas
The document discusses empirical and molecular formulas. It defines molecular formulas as showing the exact number of each type of atom in a compound, while empirical formulas show the simplest whole number ratio of elements in a compound. It provides examples of molecular and empirical formulas being the same or different. The document also provides steps for calculating empirical formulas from elemental composition percentages and determining the molecular formula from the empirical formula and molar mass.
Difference between organic and inorganic compounds
This document describes an experiment to classify compounds as organic or inorganic based on their physical and chemical properties. Students observed the structure of various compounds under a microscope, noting differences such as cube or hexagonal shapes. They then heated compounds and observed whether they burned or underwent other reactions. Testing solubility in water and benzene showed differences between organic and inorganic compounds. Examining reactions with litmus paper identified one solvent as acidic. The goal was to understand relationships between molecular structure and properties to distinguish organic from inorganic substances.
Method of expressing of concentration
This presentation describes different expressing of concentration like normality, molarity, molality, formality.PPM, PPB etc.
Concentration of Solution
Concentration of solution refers to the relative amounts of solute and solvent. It can be expressed as percent by volume, which is the amount of solute in a given volume of solution in grams per 100 mL. It can also be expressed as percent by mass, which is the amount of solute in a given mass of solvent in grams per 100 grams of solution. Sample problems are provided to demonstrate how to calculate the concentration of a solution by determining the mass or volume of solute present using the total mass or volume of the solution and the given percentage concentration. Formulas are also provided to calculate mass percent and volume percent concentration.
Chapter 1 Rate of Reactions
The document discusses rate of reaction and factors that affect it. It defines rate of reaction as the change in amount of reactants or products per unit time. It describes several factors that affect rate based on collision theory, including surface area, concentration, temperature, catalysts, and pressure. It gives examples of how scientific understanding of rate of reaction enhances quality of life, such as refrigeration, pressure cooking, cutting food into smaller pieces, making margarine, and burning coal.
8.2 types of oxides
This document discusses different types of oxides:
- Acidic oxides are formed from nonmetals and produce acidic solutions. Basic oxides are formed from metals and produce basic solutions.
- Neutral oxides do not react with acids or bases. Amphoteric oxides can behave as either acids or bases depending on the other reactants.
- Common acidic oxides include SO2 and SiO2. Sodium oxide (Na2O) and calcium oxide (CaO) are examples of basic oxides. Zinc oxide and aluminum oxide are amphoteric oxides that can react as either acids or bases.
Enthalpy Hess's Law
Hess's law states that the enthalpy change of a reaction is independent of the pathway taken and depends only on the initial and final states. ∆Hrxn is calculated by adding individual reaction enthalpies that convert reactants to products. For example, if reaction A is A → B with ∆H = x kJ and reaction B is B → C with ∆H = y kJ, the direct reaction A → C has ∆H = x + y kJ by Hess's law. Hess's law allows calculating enthalpy changes for complex reactions by summing enthalpies of simpler constituent reactions.
Catalyst
Catalysis is the process by which a catalyst increases the rate of a chemical reaction without undergoing any permanent chemical change. A catalyst works by providing an alternative reaction pathway or mechanism that has a lower activation energy. There are two main types of catalysis: homogeneous catalysis where the catalyst is in the same phase as the reactants, and heterogeneous catalysis where the catalyst is in a different phase. Catalysts can be classified as positive or negative depending on whether they increase or decrease the reaction rate.
C2.3.3 quantitative chemistry
Farmer Giles wants to determine which fertilizer contains more nitrogen. To do this, he needs to calculate the percentage of nitrogen by mass in each fertilizer. KNO3 has a higher percentage of nitrogen than NaNO3 because KNO3 has a lower molar mass and therefore more of its mass is made up of nitrogen. Calculating percentage by mass involves using relative atomic masses and molar masses. For example, the percentage of nitrogen in ammonia is calculated by taking the mass of nitrogen atoms, dividing by the molar mass of ammonia, and multiplying by 100.
Properties and Formation of Ionic Compounds Powerpoint
Ionic compounds form when ions bond through electrostatic attraction. Metals form cations by losing electrons to achieve a full outer shell, while nonmetals form anions by gaining electrons. Cations and anions are attracted due to their opposite charges. Ionic compounds have high melting points, are crystalline solids, and dissolve in water due to the separation of ions. They do not conduct electricity as solids but do so as liquids or dissolved solutions.
CONCENTRATION OF SOLUTIONS
Here are the key steps to solve this problem:
1) Convert grams of NH3 to moles using molar mass (65.3 g / 17 g/mol = 3.83 mol NH3)
2) Use balanced equation to determine moles of other substances (3.83 mol NH3 x 4/1 = 15.32 mol NO)
3) Use heat of reaction and moles of limiting reactant to determine heat (ΔH = -904 kJ/mol NH3 x 3.83 mol NH3 = -3,459 kJ)
Calorimetry
Calorimetry is a technique used to measure heat transfer during chemical or physical processes by relating temperature changes. There are two main types: bomb calorimetry, which maintains constant volume to directly measure the internal energy change; and constant pressure calorimetry, which measures the enthalpy change. Calorimetry experiments involve relating the heat absorbed or released by a reaction to the temperature change it induces in a calorimeter of known heat capacity.
Naming Compounds
This document provides an overview of basic chemistry concepts related to naming and writing formulas for ionic compounds. It discusses:
1) How to name ionic compounds by writing the cation first followed by the anion with "-ide" ending, except for polyatomic ions.
2) How to write formulas for ionic compounds by ensuring charges are balanced between cations and anions using subscripts.
3) Special rules for writing formulas involving polyatomic ions and d-block metal cations, which can have multiple oxidation states requiring specifying the oxidation number.
4) How to calculate formula masses of compounds by multiplying the number of atoms of each element by the atomic mass and summing the products.
Tang 01d bond energy
This document discusses bond energy and how it relates to chemical reactions. It states that bond breaking is endothermic while bond formation is exothermic. Bond energies can be used to calculate the change in enthalpy (ΔH°) of a reaction. A table of average bond energies is provided. Examples are given showing how to use bond energies to calculate ΔH° for different reactions, recognizing that bond energies may vary depending on neighboring bonds. Bond dissociation energy is also introduced as another measure of bond strength.
Hess's law
Hess's law states that the total enthalpy change for a reaction is independent of the pathway between the initial and final states. To calculate the enthalpy change of a reaction, standard enthalpy change values can be used for the elementary steps that add up to the overall reaction through algebraic manipulation. For the reaction of 4NH3(g) + 5O2(g) → 4NO(g) + 6H2O(g), using standard enthalpy change values for the elementary steps gives an overall exothermic enthalpy change of -906.3 kJ.
Le Chatelier's Principle
Le Chatelier's Principle states that if conditions of a system at equilibrium are changed, the equilibrium will shift to counteract the imposed change. Specifically:
- Increasing the concentration of a reactant will shift the equilibrium towards products.
- Decreasing the concentration of a reactant will shift equilibrium towards reactants.
- Increasing pressure of a gaseous reaction will shift equilibrium towards the side with fewer moles of gas.
- Increasing temperature of an endothermic reaction shifts equilibrium towards reactants, while an exothermic reaction shifts towards products.
Types of chemical reactions
Introduces the 5 types of chemical reactions: synthesis, decomposition, single and double replacement, and combustion.
oxidation numbers
Oxidation numbers reflect the gain or loss of electrons by an atom in a compound. They are assigned according to a set of rules, such as hydrogen being +1, oxygen being -2, and the sum of oxidation numbers in a neutral compound being 0. Oxidation numbers track the change in electrons during oxidation-reduction reactions where oxidation is a loss of electrons and reduction is a gain.
null.pptx
This document discusses bioenergetics, which describes how living organisms capture, transform, store, and utilize energy. It defines endergonic and exergonic reactions, and explains that ATP is used to transport energy in cells. When ATP is hydrolyzed, energy is released to power cellular work in an exergonic reaction. This hydrolysis is coupled to endergonic reactions through common intermediates like ATP to drive biochemical pathways.
bioenergetics.pptx
- Free energy (G) allows prediction of reaction direction and equilibrium. Cells acquire free energy from nutrients (heterotrophs) or sunlight (photosynthesizers).
- At equilibrium, forward and reverse reaction rates are equal. The equilibrium constant (Keq) defines concentrations of reactants and products at equilibrium.
- Biochemical reactions mainly occur through carbon-carbon bond formation/cleavage, isomerizations, free radical reactions, group transfers, and oxidation-reductions. Common functional groups and leaving groups facilitate these reactions.
More Related Content
What's hot
5.4 exothermic and endothermic reactions
This document discusses exothermic and endothermic reactions. Exothermic reactions release heat, while endothermic reactions absorb heat. Combustion reactions of hydrocarbons like methane and propane are exothermic, producing carbon dioxide, water vapor, and large amounts of heat. The heat of reaction, ΔH, indicates whether a reaction is exothermic (negative ΔH) or endothermic (positive ΔH). Bond energies represent the energy required to break bonds, while heat of combustion measures the heat released from complete combustion. A bomb calorimeter is used to accurately measure heats of combustion by igniting samples in excess oxygen. Hess's law states that the heat change of a reaction depends only on
Lecture-02.Classifications of Qualitative and Quantitative Analysis
https://www.youtube.com/watch?v=wObwXIt1ZQc&t=123s
Basic Concept of Analytical Chemistry
Meaning: The word analytical comes from the Ancient Greek ana- "up, and lysis "a loosening"). Collectively it means breaking-up" or "an untying.
Definition: The branch of chemistry which deals with the analysis of matter, its identification, and its components. Thus, the process of chemical analysis are of two type;
(1) Qualitative Analysis (2) Quantitative Analysis
Classifications of Analytical Techniques
There are two types of techniques
(1) Classical technique (2) Instrumental techniques
The classical techniques are qualitative as well as quantitative. The qualitative analysis is based on identifying and determining the analyte based on some properties specific to the analyte like boiling point, melting point, optical activities or refractive index, solubilities, and color. E.g., the Boling point of water is 100oC, the melting point of sugar is 186 °C, the refractive index of water is 1.333, test color of K is purple or the color of litmus. paper indicating the acidity or basicity of a compound. When sulphuretted hydrogen (H2S) is passed through a solution containing Arsenic, a yellowish precipitate is formed indicating the presence of arsenic. If the precipitate is brown, is brown, it indicates Tin.
The quantitative analysis is based on the quantity of the analyte. Like determining the volume of the analyte ( volumetric and gasometric analysis) and weight of the analyte (gravimetric analysis.
2) Instrumental methods can be both qualitative and quantitative. The qualitative analysis likewise relies on detecting and determining the analyte based on certain characteristics. Elements (C, H, N, S) of organic compounds using a CHNS analyzer, heavy metals using an atomic absorption spectrophotometer, and alkali and alkaline earth metals (K, Na, Ca, Mg) using a flame photometer. At the molecular level, infrared (IR) spectroscopy, Nuclear magnetic resonance (NMR) spectroscopy, mass spectrometry, and thin-layer chromatography are used to examine substances. These techniques tell us the nature of a compound. Some of these techniques can also be used for quantitative purposes as well.
Reference Books:
Skoog, D. A., West, P. M., Holler, F. J., Crouch, S. R., Fundamentals of Analytical Chemistry, 9th ed., Brooks Cole Publishing Company, (2013).
Christian, G. D., Analytical Chemistry. 6th ed., John-Wiley & Sons, New York, (2006).
Harris, D. C., Quantitative Chemical Analysis, 8th ed., W. H. Freeman and Company, New York, USA, (2011).
Bender, G.T. 1987. “Principles of Chemical Instrumentation” W.B. Saunders Co., London.
Reilley, C. 1993. Laboratory Manual of Analytical Chemistry. Allyn& Bacon, London.
Hargis, L.G. 1988. “Analytical Chemistry: Printice Hall Publishers, London.
Empirical and molecular formulas
The document discusses empirical and molecular formulas. It defines molecular formulas as showing the exact number of each type of atom in a compound, while empirical formulas show the simplest whole number ratio of elements in a compound. It provides examples of molecular and empirical formulas being the same or different. The document also provides steps for calculating empirical formulas from elemental composition percentages and determining the molecular formula from the empirical formula and molar mass.
Difference between organic and inorganic compounds
This document describes an experiment to classify compounds as organic or inorganic based on their physical and chemical properties. Students observed the structure of various compounds under a microscope, noting differences such as cube or hexagonal shapes. They then heated compounds and observed whether they burned or underwent other reactions. Testing solubility in water and benzene showed differences between organic and inorganic compounds. Examining reactions with litmus paper identified one solvent as acidic. The goal was to understand relationships between molecular structure and properties to distinguish organic from inorganic substances.
Method of expressing of concentration
This presentation describes different expressing of concentration like normality, molarity, molality, formality.PPM, PPB etc.
Concentration of Solution
Concentration of solution refers to the relative amounts of solute and solvent. It can be expressed as percent by volume, which is the amount of solute in a given volume of solution in grams per 100 mL. It can also be expressed as percent by mass, which is the amount of solute in a given mass of solvent in grams per 100 grams of solution. Sample problems are provided to demonstrate how to calculate the concentration of a solution by determining the mass or volume of solute present using the total mass or volume of the solution and the given percentage concentration. Formulas are also provided to calculate mass percent and volume percent concentration.
Chapter 1 Rate of Reactions
The document discusses rate of reaction and factors that affect it. It defines rate of reaction as the change in amount of reactants or products per unit time. It describes several factors that affect rate based on collision theory, including surface area, concentration, temperature, catalysts, and pressure. It gives examples of how scientific understanding of rate of reaction enhances quality of life, such as refrigeration, pressure cooking, cutting food into smaller pieces, making margarine, and burning coal.
8.2 types of oxides
This document discusses different types of oxides:
- Acidic oxides are formed from nonmetals and produce acidic solutions. Basic oxides are formed from metals and produce basic solutions.
- Neutral oxides do not react with acids or bases. Amphoteric oxides can behave as either acids or bases depending on the other reactants.
- Common acidic oxides include SO2 and SiO2. Sodium oxide (Na2O) and calcium oxide (CaO) are examples of basic oxides. Zinc oxide and aluminum oxide are amphoteric oxides that can react as either acids or bases.
Enthalpy Hess's Law
Hess's law states that the enthalpy change of a reaction is independent of the pathway taken and depends only on the initial and final states. ∆Hrxn is calculated by adding individual reaction enthalpies that convert reactants to products. For example, if reaction A is A → B with ∆H = x kJ and reaction B is B → C with ∆H = y kJ, the direct reaction A → C has ∆H = x + y kJ by Hess's law. Hess's law allows calculating enthalpy changes for complex reactions by summing enthalpies of simpler constituent reactions.
Catalyst
Catalysis is the process by which a catalyst increases the rate of a chemical reaction without undergoing any permanent chemical change. A catalyst works by providing an alternative reaction pathway or mechanism that has a lower activation energy. There are two main types of catalysis: homogeneous catalysis where the catalyst is in the same phase as the reactants, and heterogeneous catalysis where the catalyst is in a different phase. Catalysts can be classified as positive or negative depending on whether they increase or decrease the reaction rate.
C2.3.3 quantitative chemistry
Farmer Giles wants to determine which fertilizer contains more nitrogen. To do this, he needs to calculate the percentage of nitrogen by mass in each fertilizer. KNO3 has a higher percentage of nitrogen than NaNO3 because KNO3 has a lower molar mass and therefore more of its mass is made up of nitrogen. Calculating percentage by mass involves using relative atomic masses and molar masses. For example, the percentage of nitrogen in ammonia is calculated by taking the mass of nitrogen atoms, dividing by the molar mass of ammonia, and multiplying by 100.
Properties and Formation of Ionic Compounds Powerpoint
Ionic compounds form when ions bond through electrostatic attraction. Metals form cations by losing electrons to achieve a full outer shell, while nonmetals form anions by gaining electrons. Cations and anions are attracted due to their opposite charges. Ionic compounds have high melting points, are crystalline solids, and dissolve in water due to the separation of ions. They do not conduct electricity as solids but do so as liquids or dissolved solutions.
CONCENTRATION OF SOLUTIONS
Here are the key steps to solve this problem:
1) Convert grams of NH3 to moles using molar mass (65.3 g / 17 g/mol = 3.83 mol NH3)
2) Use balanced equation to determine moles of other substances (3.83 mol NH3 x 4/1 = 15.32 mol NO)
3) Use heat of reaction and moles of limiting reactant to determine heat (ΔH = -904 kJ/mol NH3 x 3.83 mol NH3 = -3,459 kJ)
Calorimetry
Calorimetry is a technique used to measure heat transfer during chemical or physical processes by relating temperature changes. There are two main types: bomb calorimetry, which maintains constant volume to directly measure the internal energy change; and constant pressure calorimetry, which measures the enthalpy change. Calorimetry experiments involve relating the heat absorbed or released by a reaction to the temperature change it induces in a calorimeter of known heat capacity.
Naming Compounds
This document provides an overview of basic chemistry concepts related to naming and writing formulas for ionic compounds. It discusses:
1) How to name ionic compounds by writing the cation first followed by the anion with "-ide" ending, except for polyatomic ions.
2) How to write formulas for ionic compounds by ensuring charges are balanced between cations and anions using subscripts.
3) Special rules for writing formulas involving polyatomic ions and d-block metal cations, which can have multiple oxidation states requiring specifying the oxidation number.
4) How to calculate formula masses of compounds by multiplying the number of atoms of each element by the atomic mass and summing the products.
Tang 01d bond energy
This document discusses bond energy and how it relates to chemical reactions. It states that bond breaking is endothermic while bond formation is exothermic. Bond energies can be used to calculate the change in enthalpy (ΔH°) of a reaction. A table of average bond energies is provided. Examples are given showing how to use bond energies to calculate ΔH° for different reactions, recognizing that bond energies may vary depending on neighboring bonds. Bond dissociation energy is also introduced as another measure of bond strength.
Hess's law
Hess's law states that the total enthalpy change for a reaction is independent of the pathway between the initial and final states. To calculate the enthalpy change of a reaction, standard enthalpy change values can be used for the elementary steps that add up to the overall reaction through algebraic manipulation. For the reaction of 4NH3(g) + 5O2(g) → 4NO(g) + 6H2O(g), using standard enthalpy change values for the elementary steps gives an overall exothermic enthalpy change of -906.3 kJ.
Le Chatelier's Principle
Le Chatelier's Principle states that if conditions of a system at equilibrium are changed, the equilibrium will shift to counteract the imposed change. Specifically:
- Increasing the concentration of a reactant will shift the equilibrium towards products.
- Decreasing the concentration of a reactant will shift equilibrium towards reactants.
- Increasing pressure of a gaseous reaction will shift equilibrium towards the side with fewer moles of gas.
- Increasing temperature of an endothermic reaction shifts equilibrium towards reactants, while an exothermic reaction shifts towards products.
Types of chemical reactions
Introduces the 5 types of chemical reactions: synthesis, decomposition, single and double replacement, and combustion.
oxidation numbers
Oxidation numbers reflect the gain or loss of electrons by an atom in a compound. They are assigned according to a set of rules, such as hydrogen being +1, oxygen being -2, and the sum of oxidation numbers in a neutral compound being 0. Oxidation numbers track the change in electrons during oxidation-reduction reactions where oxidation is a loss of electrons and reduction is a gain.
What's hot (20)
Lecture-02.Classifications of Qualitative and Quantitative Analysis
Lecture-02.Classifications of Qualitative and Quantitative Analysis
Difference between organic and inorganic compounds
Difference between organic and inorganic compounds
Properties and Formation of Ionic Compounds Powerpoint
Properties and Formation of Ionic Compounds Powerpoint
Similar to Enthalpy change
null.pptx
This document discusses bioenergetics, which describes how living organisms capture, transform, store, and utilize energy. It defines endergonic and exergonic reactions, and explains that ATP is used to transport energy in cells. When ATP is hydrolyzed, energy is released to power cellular work in an exergonic reaction. This hydrolysis is coupled to endergonic reactions through common intermediates like ATP to drive biochemical pathways.
bioenergetics.pptx
- Free energy (G) allows prediction of reaction direction and equilibrium. Cells acquire free energy from nutrients (heterotrophs) or sunlight (photosynthesizers).
- At equilibrium, forward and reverse reaction rates are equal. The equilibrium constant (Keq) defines concentrations of reactants and products at equilibrium.
- Biochemical reactions mainly occur through carbon-carbon bond formation/cleavage, isomerizations, free radical reactions, group transfers, and oxidation-reductions. Common functional groups and leaving groups facilitate these reactions.
Energy Consuming & Energy Releasing Reactions.pptx
Here's a basic presentation on what endergonic and exergonic reactions mean and their relevance in the field on enzyme engineering
Photosynthesis 02_11-02_14.pptx
This document provides an overview and outline of a lesson on photosynthesis. It includes:
1. A do now activity asking students to define terms and discuss with a neighbor.
2. An outline of the chapter sections on photosynthesis including the light and dark reactions, chloroplasts, and alternative plants.
3. A series of slides explaining key concepts like autotrophs, the food web, photosynthesis formula, and why plants are green due to chloroplasts and pigment absorption.
4. Directions for students to complete worksheets, readings, and online practice questions on photosynthesis as part of their homework.
5.1 autotrophic nutrition UEC Senior 1 Biology
The document provides information about different types of photosynthesis pathways:
- C3 plants fix carbon dioxide into a 3-carbon compound. C4 plants and CAM plants have evolved pathways to concentrate carbon dioxide around rubisco to reduce photorespiration.
- C4 plants separate the initial fixation from the Calvin cycle between mesophyll and bundle sheath cells. CAM plants separate fixation temporally by fixing at night and running the Calvin cycle during the day.
- The pathways allow C4 and CAM plants to thrive in hot, dry environments where C3 plants are disadvantaged by their higher rates of photorespiration.
Redoxtherm
Oxidation-reduction reactions are an important type of reaction in biochemistry that involve the transfer of electrons. Oxidation involves the loss of electrons and reduction involves the gain of electrons. These two processes must occur simultaneously. Thermodynamics is the study of energy and is important for understanding biochemistry. The first law of thermodynamics states that energy is conserved, while the second law states that spontaneous reactions result in an increase in the randomness or entropy of the universe. For a reaction to be spontaneous, the change in entropy of the universe must be positive.
Redoxtherm
Oxidation-reduction reactions are an important type of reaction in biochemistry that involve the transfer of electrons. Oxidation involves the loss of electrons and reduction involves the gain of electrons. These two processes must occur simultaneously. Thermodynamics is the study of energy and is important for understanding biochemistry. The first law of thermodynamics states that energy is conserved, while the second law states that spontaneous reactions result in an increase in the randomness or entropy of the universe. For a reaction to be spontaneous, the change in entropy of the universe must be positive.
Chapter 8 metabolism
KEY CONCEPTS
8.1 An organism’s metabolism transforms matter and
energy, subject to the laws of thermodynamics
8.2 The free-energy change of a reaction tells us whether or not the reaction occurs
spontaneously
8.3 ATP powers cellular work by coupling exergonic reactions to endergonic reactions
8.4 Enzymes speed up metabolic reactions by lowering energy barriers
8.5 Regulation of enzyme activity helps control metabolism
Chapter8 metabolism-151125142235-lva1-app6892
This document provides an overview of metabolism and bioenergetics. It discusses how cells extract energy from reactions to perform work, and how metabolism involves thousands of chemical reactions catalyzed by enzymes. Metabolic pathways convert molecules through a series of steps, with catabolic pathways releasing energy and anabolic pathways requiring energy. The energy of reactions is discussed in terms of free energy, and how ATP powers cellular work by coupling exergonic reactions to endergonic processes through phosphorylation. Enzymes lower the activation energy of reactions to speed up metabolism.
Chapter8 metabolism-151125142235-lva1-app6892
Metabolism is the set of chemical reactions that occur in living organisms to sustain life. Energy from food fuels these reactions through the intermediary ATP. Enzymes catalyze reactions by lowering their activation energy. Regulation of enzyme activity controls metabolic pathways and maintains cellular homeostasis.
Organic Reaction Mechanism
Organic Reaction Mechanism : This topic is very-very important for CSIR-NET, GATE, IIT-JAM and other Competitive exams for Chemistry and Chemical Sciences.
Types of chemical reactions
This document discusses classifying chemical reactions into synthesis, decomposition, or replacement reactions and defines exothermic and endothermic reactions. It also addresses factors that affect the rate of reactions such as temperature, surface area, stirring, concentration, and catalysts. Photosynthesis is used as an example of an endothermic reaction requiring light as a catalyst.
metabolism, anabolism and catabolism.ppt
Metabolism involves anabolic and catabolic pathways that build up or break down molecules. These pathways are coupled so that energy released in catabolism can drive energy-requiring anabolism. Thermodynamics studies energy transformations, with the first law stating energy is conserved and the second law that entropy always increases. Free energy indicates what reactions are spontaneous as it decreases for such reactions, allowing maximal work. Metabolism maintains order by using exergonic reactions to power endergonic ones, keeping cells from equilibrium and alive.
Enthalpy Change
The document discusses enthalpy changes and exothermic and endothermic reactions. It defines exothermic reactions as reactions where heat energy is released to the surroundings, giving a negative enthalpy change. Endothermic reactions absorb heat from the surroundings, having a positive enthalpy change. Bond breaking requires energy and is endothermic, while bond forming releases energy and is exothermic. Whether a reaction is exothermic or endothermic depends on if more energy is released or absorbed during bond breaking and forming.
C13 enthalpy change
The document discusses enthalpy changes and exothermic and endothermic reactions. It defines exothermic reactions as reactions where heat energy is given out to the surroundings, while endothermic reactions absorb heat from the surroundings. It explains that the enthalpy change (ΔH) is negative for exothermic reactions and positive for endothermic reactions. The document also discusses how bond breaking requires energy input and is endothermic, while bond forming releases energy and is exothermic.
Biological oxidation L1
The document discusses biological oxidation and the electron transport chain. It covers topics like the stages of foodstuff oxidation, redox potentials, enzymes and co-enzymes in biological oxidation, high energy compounds, the organization of the electron transport chain, oxidative phosphorylation, and ATP synthesis. It notes that food is broken down and oxidized to generate reducing equivalents like NADH and FADH2, which then enter the electron transport chain to release energy that is used to synthesize ATP through oxidative phosphorylation.
Catalysis
This document discusses the topic of catalysis through an experiment demonstrating the Haber process for ammonia production. It describes how inserting an iron rod or powdered iron increases the reaction rate between nitrogen and hydrogen gases, and adding molybdenum further increases the rate. A catalyst is defined as a substance that increases the rate of a chemical reaction without being consumed itself, and properties of catalysts are that they provide an alternative reaction pathway requiring lower activation energy. Common industrial applications of catalysis include chemical production and catalytic converters.
Aqib behzad (1767,21332)catalysis1
Catalysts accelerate chemical reactions without being consumed. There are two types of catalysts: homogeneous, where the catalyst is in the same phase as the reactants, and heterogeneous, where the catalyst is in a different phase. In heterogeneous catalysis, the catalyst is typically a solid and the reactants are gases or liquids. The catalyst provides alternative reaction pathways with lower activation energies. Enzymes are biological catalysts that work by binding reactants in cavities on their surfaces, forming activated complexes that decompose into products.
Similar to Enthalpy change (20)
Energy Consuming & Energy Releasing Reactions.pptx
Energy Consuming & Energy Releasing Reactions.pptx
Chemistry_Energetics_Lecture_1.Chemistry_Energetics_Lecture
Chemistry_Energetics_Lecture_1.Chemistry_Energetics_Lecture
Chem7JD;SLKGJSDLKJSKGJSFLKJG;LASDKGASLGLA250p2.ppt
Chem7JD;SLKGJSDLKJSKGJSFLKJG;LASDKGASLGLA250p2.ppt
More from Rania S Seoudi
Moles and Concentration Calculations Course
This course covers the fundamentals of chemistry including atomic and molecular masses, calculating relative atomic mass using a mass spectrometer, formula mass and relative molecular mass, amount of substances, Avogadro's constant, chemical formulas and equations, empirical and molecular formulas, balancing chemical equations, mole calculations, stoichiometry, solutions and concentrations, titration experiments, gas volume calculations, and exercises to practice these concepts. The goal is to learn essential chemistry topics through this comprehensive high school or introductory college chemistry course.
Writing in Science and Research
This 4-section course aims to help undergraduate and graduate science students at any stage of their research to write effectively. The course covers starting a research project, collecting and writing up data, using writing tools to report results, and editing drafts.
Principles of Polymer Chemistry
This document discusses different types of polymers including natural, synthetic, and semi-synthetic polymers. It describes methods of polymerization such as step-growth, chain-growth, ring-opening, and coordination polymerization. Specific polymers are also mentioned including polyesters, polycarbonates, polyamides, polyurethane, nylon 6, polyethylene oxide, and polypropylene oxide. The document provides an overview of polymer chemistry concepts like molecular weight calculation, crystalline structures, glass transition and melt temperatures, and different polymerization reactions.
Writing in Science and Research
Academic writing and Editing Course
Enrollment link:
https://www.udemy.com/course/writing-in-science-and-research
Corona virus what went wrong
This document discusses the failures in addressing past epidemics like SARS and MERS that contributed to the spread of COVID-19. It argues that governments and industries prioritized other areas like cancer research and extending lifespan over researching epidemic diseases. This left few experienced researchers behind to confront new diseases rapidly. It also criticizes overpopulation, urbanization, and a reliance on experienced employees rather than training new graduates. The document warns that if we do not learn from past mistakes and find cures for animal-borne diseases, future pandemics may be even more severe.
Corona virus the new panademic
Coronavirus SARS-CoV-2 (COVID-19)
What is the difference between pandemic and epidemic?
What is Coronavirus?
Watch the full video: https://youtu.be/y9zr7M8mBIY
Vitamin D
This document discusses vitamin D, including what it is, how the body processes and activates it, its functions, sources, and requirements. Vitamin D is a fat-soluble vitamin synthesized in the skin upon exposure to sunlight and found in some foods. It is activated through two hydroxylation steps in the liver and kidneys. Vitamin D promotes calcium absorption and bone mineralization and supports immune function. While sunlight is the major source, many factors impact skin synthesis, so dietary sources and supplements are also important to meet daily requirements.
Naming compounds and Balancing chemical equations using oxidation numbers
1) The document discusses naming compounds and balancing chemical equations using oxidation numbers. It provides examples of naming metal and non-metal compounds as well as oxide compounds.
2) Methods for determining oxidation numbers from compound names and formulas are explained. Examples are given for nitrate compounds and working out formulas from compound names.
3) The document demonstrates balancing chemical equations using oxidation numbers, giving examples of copper (II) oxide reacting with ammonia and manganate (VII) ions reacting with iron (II) ions.
Electronegativity and electropositivity trends in periodic table
Electronegativity and electropositivity trends in periodic table
Video link:
https://youtu.be/_ojmwCHhuJM
Calorimeter and enthalpy measurements
1) Calorimetry can be used to measure the enthalpy change of reactions by using either a constant pressure calorimeter or a bomb calorimeter.
2) The enthalpy change is calculated using the formula: ΔH=-mcΔT, where m is the mass of the calorimeter contents, c is the specific heat capacity, and ΔT is the temperature change.
3) For example, a student measured a 6.5°C temperature increase when mixing 50mL of 1M HCl and 50mL of 1M NaOH. Using the calorimetry equation, the enthalpy change for the neutralization reaction of 1 mole of HCl with NaOH
Atomic structure electronic configuration - ib
Atomic structure and electronic configuration
Ionization energy and ionization energy trend in periodic table
Video link:
https://youtu.be/C-xhuw9ZN6U
stoichiometric relations
Stoichiometric relations
For more materials subscribe to channel:
https://www.youtube.com/channel/UCzXxV4xER9NIWt316gfeO1w
Acid base eqm and solubility equilibrium
This chapter talks about:
Acid –base equilibria
solubility equilibria
Buffer solution
Acid-base titration
Molar solubility and solubility
pH and Solubility
For more materials subscribe to channel:
https://www.youtube.com/channel/UCzXxV4xER9NIWt316gfeO1w
Acid and bases
Acid- base
pH, The ion product of water
For more materials subscribe to channel:
https://www.youtube.com/channel/UCzXxV4xER9NIWt316gfeO1w
More from Rania S Seoudi (14)
Naming compounds and Balancing chemical equations using oxidation numbers
Naming compounds and Balancing chemical equations using oxidation numbers
Electronegativity and electropositivity trends in periodic table
Electronegativity and electropositivity trends in periodic table
Recently uploaded
How to deliver Powerpoint Presentations.pptx
"How to make and deliver dynamic presentations by making it more interactive to captivate your audience attention"
BÀI TẬP DẠY THÊM TIẾNG ANH LỚP 7 CẢ NĂM FRIENDS PLUS SÁCH CHÂN TRỜI SÁNG TẠO ...
BÀI TẬP DẠY THÊM TIẾNG ANH LỚP 7 CẢ NĂM FRIENDS PLUS SÁCH CHÂN TRỜI SÁNG TẠO ...Nguyen Thanh Tu Collection
https://app.box.com/s/qhtvq32h4ybf9t49ku85x0n3xl4jhr15BBR 2024 Summer Sessions Interview Training
Qualitative research interview training by Professor Katrina Pritchard and Dr Helen Williams
Level 3 NCEA - NZ: A Nation In the Making 1872 - 1900 SML.ppt
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,
A Visual Guide to 1 Samuel | A Tale of Two Hearts
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.
Lifelines of National Economy chapter for Class 10 STUDY MATERIAL PDF
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.
Philippine Edukasyong Pantahanan at Pangkabuhayan (EPP) Curriculum
(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.
LAND USE LAND COVER AND NDVI OF MIRZAPUR DISTRICT, UP
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.
Mule event processing models | MuleSoft Mysore Meetup #47
Mule event processing models | MuleSoft Mysore Meetup #47
Event Link:- https://meetups.mulesoft.com/events/details/mulesoft-mysore-presents-mule-event-processing-models/
Agenda
● What is event processing in MuleSoft?
● Types of event processing models in Mule 4
● Distinction between the reactive, parallel, blocking & non-blocking processing
For Upcoming Meetups Join Mysore Meetup Group - https://meetups.mulesoft.com/mysore/YouTube:- youtube.com/@mulesoftmysore
Mysore WhatsApp group:- https://chat.whatsapp.com/EhqtHtCC75vCAX7gaO842N
Speaker:-
Shivani Yasaswi - https://www.linkedin.com/in/shivaniyasaswi/
Organizers:-
Shubham Chaurasia - https://www.linkedin.com/in/shubhamchaurasia1/
Giridhar Meka - https://www.linkedin.com/in/giridharmeka
Priya Shaw - https://www.linkedin.com/in/priya-shaw
Chapter wise All Notes of First year Basic Civil Engineering.pptx
Chapter wise All Notes of First year Basic Civil Engineering
Syllabus
Chapter-1
Introduction to objective, scope and outcome the subject
Chapter 2
Introduction: Scope and Specialization of Civil Engineering, Role of civil Engineer in Society, Impact of infrastructural development on economy of country.
Chapter 3
Surveying: Object Principles & Types of Surveying; Site Plans, Plans & Maps; Scales & Unit of different Measurements.
Linear Measurements: Instruments used. Linear Measurement by Tape, Ranging out Survey Lines and overcoming Obstructions; Measurements on sloping ground; Tape corrections, conventional symbols. Angular Measurements: Instruments used; Introduction to Compass Surveying, Bearings and Longitude & Latitude of a Line, Introduction to total station.
Levelling: Instrument used Object of levelling, Methods of levelling in brief, and Contour maps.
Chapter 4
Buildings: Selection of site for Buildings, Layout of Building Plan, Types of buildings, Plinth area, carpet area, floor space index, Introduction to building byelaws, concept of sun light & ventilation. Components of Buildings & their functions, Basic concept of R.C.C., Introduction to types of foundation
Chapter 5
Transportation: Introduction to Transportation Engineering; Traffic and Road Safety: Types and Characteristics of Various Modes of Transportation; Various Road Traffic Signs, Causes of Accidents and Road Safety Measures.
Chapter 6
Environmental Engineering: Environmental Pollution, Environmental Acts and Regulations, Functional Concepts of Ecology, Basics of Species, Biodiversity, Ecosystem, Hydrological Cycle; Chemical Cycles: Carbon, Nitrogen & Phosphorus; Energy Flow in Ecosystems.
Water Pollution: Water Quality standards, Introduction to Treatment & Disposal of Waste Water. Reuse and Saving of Water, Rain Water Harvesting. Solid Waste Management: Classification of Solid Waste, Collection, Transportation and Disposal of Solid. Recycling of Solid Waste: Energy Recovery, Sanitary Landfill, On-Site Sanitation. Air & Noise Pollution: Primary and Secondary air pollutants, Harmful effects of Air Pollution, Control of Air Pollution. . Noise Pollution Harmful Effects of noise pollution, control of noise pollution, Global warming & Climate Change, Ozone depletion, Greenhouse effect
Text Books:
1. Palancharmy, Basic Civil Engineering, McGraw Hill publishers.
2. Satheesh Gopi, Basic Civil Engineering, Pearson Publishers.
3. Ketki Rangwala Dalal, Essentials of Civil Engineering, Charotar Publishing House.
4. BCP, Surveying volume 1
Gender and Mental Health - Counselling and Family Therapy Applications and In...
A proprietary approach developed by bringing together the best of learning theories from Psychology, design principles from the world of visualization, and pedagogical methods from over a decade of training experience, that enables you to: Learn better, faster!
BÀI TẬP BỔ TRỢ TIẾNG ANH 8 CẢ NĂM - GLOBAL SUCCESS - NĂM HỌC 2023-2024 (CÓ FI...
BÀI TẬP BỔ TRỢ TIẾNG ANH 8 CẢ NĂM - GLOBAL SUCCESS - NĂM HỌC 2023-2024 (CÓ FI...Nguyen Thanh Tu Collection
https://app.box.com/s/y977uz6bpd3af4qsebv7r9b7s21935vdHYPERTENSION - SLIDE SHARE PRESENTATION.
IT WILL BE HELPFULL FOR THE NUSING STUDENTS
IT FOCUSED ON MEDICAL MANAGEMENT AND NURSING MANAGEMENT.
HIGHLIGHTS ON HEALTH EDUCATION.
Recently uploaded (20)
spot a liar (Haiqa 146).pptx Technical writhing and presentation skills
spot a liar (Haiqa 146).pptx Technical writhing and presentation skills
BÀI TẬP DẠY THÊM TIẾNG ANH LỚP 7 CẢ NĂM FRIENDS PLUS SÁCH CHÂN TRỜI SÁNG TẠO ...
BÀI TẬP DẠY THÊM TIẾNG ANH LỚP 7 CẢ NĂM FRIENDS PLUS SÁCH CHÂN TRỜI SÁNG TẠO ...
B. Ed Syllabus for babasaheb ambedkar education university.pdf
B. Ed Syllabus for babasaheb ambedkar education university.pdf
Film vocab for eal 3 students: Australia the movie
Film vocab for eal 3 students: Australia the movie
SWOT analysis in the project Keeping the Memory @live.pptx
SWOT analysis in the project Keeping the Memory @live.pptx
Level 3 NCEA - NZ: A Nation In the Making 1872 - 1900 SML.ppt
Level 3 NCEA - NZ: A Nation In the Making 1872 - 1900 SML.ppt
Lifelines of National Economy chapter for Class 10 STUDY MATERIAL PDF
Lifelines of National Economy chapter for Class 10 STUDY MATERIAL PDF
Philippine Edukasyong Pantahanan at Pangkabuhayan (EPP) Curriculum
Philippine Edukasyong Pantahanan at Pangkabuhayan (EPP) Curriculum
LAND USE LAND COVER AND NDVI OF MIRZAPUR DISTRICT, UP
LAND USE LAND COVER AND NDVI OF MIRZAPUR DISTRICT, UP
Mule event processing models | MuleSoft Mysore Meetup #47
Mule event processing models | MuleSoft Mysore Meetup #47
Chapter wise All Notes of First year Basic Civil Engineering.pptx
Chapter wise All Notes of First year Basic Civil Engineering.pptx
Gender and Mental Health - Counselling and Family Therapy Applications and In...
Gender and Mental Health - Counselling and Family Therapy Applications and In...
BÀI TẬP BỔ TRỢ TIẾNG ANH 8 CẢ NĂM - GLOBAL SUCCESS - NĂM HỌC 2023-2024 (CÓ FI...
BÀI TẬP BỔ TRỢ TIẾNG ANH 8 CẢ NĂM - GLOBAL SUCCESS - NĂM HỌC 2023-2024 (CÓ FI...
Enthalpy change
- 1. Enthalpy Changes Chapter 6 Part 1 YouTube: Chemistry bright minds https://www.youtube.com/channel/UCzXxV4xER9NIWt316gfeO1w Visit us on Blog: http://chemistrybrightminds.blogspot.com Facebook: https://www.facebook.com/BrightMinds 1
- 2. Exothermic and endothermic reactions: • Exothermic reaction: chemical reaction that release energy to the surroundings • Example: reaction of magnesium and sulfuric acid to produce magnesium sulfide • Endothermic reaction: chemical reaction that absorb energy from the surrounding • Example dissolving of ammonium chloride in water 2
- 3. Enthalpy change: Enthalpy change is the energy exchange between a chemical reaction and its surroundings at constant pressure. Enthalpy (H): total energy associated with the materials that react 3
- 4. How to calculate enthalpy change? 4 Unit of enthalpy change is kilojoules per mole (kJ mol-1)
- 5. Reaction pathway (enthalpy profile diagram): • Y-axis: enthalpy of reactants and products • X-axis: reaction pathway with reactant on the left and product on the right. 5
- 6. Exothermic reaction: • Energy is released to the surrounding • Enthalpy of reactants is higher than products • H Products – H Reactants is negative • Example: 6
- 7. Endothermic reaction: • Energy is absorbed from the surrounding • Enthalpy of reactants is lower than products • H Products – H Reactants is positive • Example: 7
- 8. Standard enthalpy change of combustion ΔHO c • Substance that is combusted can be element or compound • Enthalpy always exothermic and have negative value 8
- 9. Standard enthalpy change of neutralisation, ΔHO n • Is the enthalpy change when one mole of water is formed by the reaction of an acid with alkali under standard conditions • Example: • Cl- and Na+ are spectator ions 9
- 10. Standard enthalpy change of solution, ΔHO sol • Is enthalpy change when one mole of solute is dissolved in a solvent to form an infinitely dilute solution under standard conditions. 10
- 11. Standard enthalpy change of hydration of an anhydrous salt: 11
- 12. End of Video 12